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Research ArticleLiquid-Phase Ethanol Oxidation and Gas-Phase CO OxidationReactions over M Doped (M = Ag Au Pd and Ni) and MM1015840
Codoped CeO2 Nanoparticles
Yohan Park1 Yulri Na1 Debabrata Pradhan2 and Youngku Sohn1
1Department of Chemistry Yeungnam University Gyeongsan 38541 Republic of Korea2Materials Science Centre Indian Institute of Technology Kharagpur 721302 India
Correspondence should be addressed to Youngku Sohn youngkusohnynuackr
Received 14 October 2016 Revised 13 November 2016 Accepted 22 November 2016
Academic Editor Stojan Stavber
Copyright copy 2016 Yohan Park et al This is an open access article distributed under the Creative Commons Attribution Licensewhich permits unrestricted use distribution and reproduction in any medium provided the original work is properly cited
Transition metal doped metal oxides have been studied extensively for potential applications to environments and chemicalindustry HereinMdoped (M=Ag Au Pd andNi) andMM1015840 codopedCeO
2nanoparticles (NPs) were prepared by a hydrothermal
method and their liquid-phase ethanol and gas-phase CO oxidation performances were examined by UV-visible absorptionspectroscopy and temperature programmed mass spectrometry respectively The ethanol and CO oxidation performances wereenhanced greatly by metal-doping and were dependent on the relative concentration of codoped metals For ethanol oxidationthe concentration of acetaldehyde became saturated at low levels while that of ethyl acetate continuously increased to become afinal major product For M doped CeO
2NPs the ethanol oxidation performance showed an order of Ni lt Ag lt Pd ≪ Au For
MM1015840 codoped CeO2NPs the activity of Au doped CeO
2deteriorated drastically upon adding other metals (Ag Ni and Pd) as a
cocatalyst
1 Introduction
The hybridization of metal oxides with transition metals hasbeen performed extensively to increase the catalytic (eg COoxidation) efficiency of the oxides [1ndash12] Among the manymetal oxides a reducible CeO
2support has been studied
extensively as a model oxidation catalyst because of its con-vertible redox states (Ce4+Ce3+) and oxygen releasestorageproperties [13ndash17] Doped transition metals include Au andAg [1 5 18ndash32] Because Au and Ag have the same crystalstructure as well as similar lattice constants and metallicbond lengths they can easily form alloys which can promotecatalytic activity [18 19 21] For CO oxidation over AuCeO
2
catalysts Chen et al reported that the oxidation reactivityof adsorbed CO was independent of the Au particle sizewhereas the decomposition reactivity of carbonate bicarbon-ate and formate species was dependent on the particle size itwas higher for larger Au particles [20] To identify the activesites for AuCO
2 Nie et al prepared thiol-protected Au and
observed enhanced CO oxidation activity compared to bareAu [1] Based on this result they concluded that the activesite was the perimeter of Au Au nanoparticles aggregateeasily by sintering at high temperature which can resultin deactivation of Au To avoid the aggregation of Au Qiet al synthesized core-shell AuCeO
2nanocomposites and
observed remarkably enhanced CO oxidation activity [5]Liu et al prepared Ag
119909Au1minus119909
CeO2coreshell nanospheres
by galvanic replacement and observed the catalytic COoxidation activity in the order of AuCeO
2lt AgCeO
2≪
Ag041
Au059
CeO2ltAg064
Au036
CeO2[21] No catalyst
shows the best performance in all reaction systems Fiorenzaet al tested AuCeO
2 AgCeO
2 CuCeO
2 AuAgCeO
2
and AuCuCeO2
catalysts on the oxidation of volatileorganic compounds (2-propanol ethanol and toluene)Theyreported that AuCeO
2was most active for the oxidation
of alcohols AgCeO2showed the best efficiency for total
toluene oxidation and AuAgCeO2and AuCuCeO
2showed
the highest selectivity to partial oxidation [24] Studying
Hindawi Publishing CorporationJournal of ChemistryVolume 2016 Article ID 2176576 11 pageshttpdxdoiorg10115520162176576
2 Journal of Chemistry
alcohol oxidation is very important to understanding of thereaction mechanisms involved in many industrial organicsynthetic processes because of its importance as a fuel [3233] Zhang et al prepared plum-pudding type PdCeO
2
and used it as a visible light photocatalyst for selectiveoxidation of benzylic alcohols to corresponding aldehydesin a process in which photogenerated electron producedsuperoxide radicals thereby facilitating the oxidation [34]Maldotti et al emphasized that Au-H species is an importantintermediate for alcohol oxidation when Au-CeO
2catalyst is
used [32]Motivated by these studies this study examined the
catalytic activity of M doped (M = Ag Au Pd and Ni) andMM1015840 codoped CeO
2for both liquid ethanol and gas-phase
COoxidation reactionsThe catalysts were reacted in a streamof gas-phase CO and liquid-phase ethanol CO oxidation isthe simplest model system understood by a simplified CO +[O]lowast rarr CO
2mechanism while for CH
3CH2OH oxidation
on an oxide support the reactions are very complicatedCH3CH2OH rarr CH
3CH2O(ad) + H(ad) CH
3CH2O(ad) +
[O]lowast rarr CH3CHO CH
3CHO + [O]lowast rarr CH
3COOH and
ethyl acetate (CH3COOCH
2CH3) formation via aldehyde
and hemiacetal (CH3CH(OH)OC
2H5) Because the two oxi-
dation reactions have different mechanisms two systemstogether were investigated to determine the role of dopedmetals and the relative concentrations of two differentmetals
2 Experimental
Cerium oxide (CeO2) nanoparticles (NPs) were synthesized
by a hydrothermal method which is described briefly asfollows 10mL of 01M Ce(NO
3)3sdot6H2O (Sigma-Aldrich
99) was added to 15mL of deionized water in a Teflonbottle Subsequently 20mL of ammonia (28sim30) solutionwas added The solution was fully mixed and the bottlewas tightly capped and placed in an oven (120∘C) for 12 hrsFor the synthesis of metal (Ag Au Pd and Ni) doped andcodoped CeO
2 stoichiometric amounts (MM1015840 = 50mol
14mol 2525mol 41mol and 05mol relative toCe ions) of two differentmetal solutions were added to the Cenitrate solution before capping the bottle and placing it intothe oven Upon the reaction for 12 hrs the final products werecooled naturally and washed repeatedly with deionized waterand ethanol several times The finally collected samples werefully dried in a conventional oven (80∘C)
The morphologies of the samples were examined bytransmission electron microscopy (TEM Hitachi H-7600)operated at 100 kV For this the samples were mountedonto carbon-coated Cu grids X-ray diffraction (XRD PAN-alytical XrsquoPert Pro MPD) was performed to examine thecrystal structures of the dried powder samples using CuK120572 radiation at 40 kV and 30mA The UV-visible (UV-VisSCINCO Neosys-2000) absorption spectra of the powdersamples were recorded The Fourier transform infrared (FT-IR) spectra were obtained using a Thermo Scientific NicoletiS10 spectrometer in ZnSe attenuated total reflection mode
Temperature programmed reduction (TPR) was per-formed to examine the reducibility of the catalyst powder
samples using a Quantachrome CHEMBET equipped with athermal conductivity detector The samples were degassed at150∘C for 2 hrs under nitrogen before being tested by TPRTPR was performed at a heating rate of 20∘Cmin and aflow rate of 40mLmin under 5 H
2N2gas stream CO
oxidation tests were performed in a U-tube (inner diameterof 40mm) quartz reactor loaded with 10mg of the catalystThe temperature heating rate was set to 10∘CminThemixedCO(10)O
2(25)N
2gas was fed to the reactor at a flow
rate of 40mLmin The final gas reaction products weremonitored using a RGA 200 quadrupole mass spectrometer(Stanford Research Systems USA)
The liquid-phase ethanol oxidation reaction was per-formed as follows 10mg of the catalyst and 15mL of ethanolsolvent were mixed in a test tube after which the tube wastightly capped The test tube was then placed in an oven at80∘C (or 40∘C) without stirring Since we tightly capped thetube the oxygen supply will be limited at a certain reactionlevel After a desired reaction time in the oven we took theUV-visible absorption spectrum of the solution in the testtube To detect the final products after the ethanol oxidationwe introduced the solution via a leak valve into the UHVchamber and recorded a mass spectrum
3 Results and Discussion
The metal (Ag Au Pd and Ni) codoped (M and M1015840 = 25and 25mol resp) CeO
2catalysts were examined by TEM
Figure 1 reveals two different (big and small) size distribu-tions one was lt20 nm and the other was lt5 nm The largerand smaller particles could be attributed to bulk CeO
2and
doped metal nanoparticles which could be further clearlyidentified by energy dispersive X-ray spectroscopy and highresolution transmissionmicroscopyThe smaller metal parti-cles could be active sites for the catalytic reactions The AgAu doped sample showed much higher aggregation and theaggregation was found to be in the order of AgAu gtAuNi simAuPd gt NiPd
Material characterization and CO oxidation were focusedonly for Ag and Au doped and codoped CeO
2NPs Figure 2
presents the powder XRD patterns of undoped CeO2and
Au and Ag doped and codoped (05 41 2525 14 and50mol resp) CeO
2catalysts For undoped Ce oxide
several major peaks (red filled circles) were observed at 2120579 =285∘ 330∘ 474∘ 563∘ 590∘ and 693∘ which were assignedto the (111) (200) (220) (311) (222) and (400) planes of thecubic (Fm-3m) structure (JCPDS 034-0394) of CeO
2 respec-
tively [11 12] The major peak at 2120579 = 285∘ showed no criticaldifference in peak position for all the samples This meansthat the crystal lattice of the CeO
2support was not critically
affected by metal-doping On the other hand the broadnessof the peak was somewhat different indicating a differencein particle size The particle sizes of the undoped 5molAg 41mol of AgAu 2525mol of AgAu 14mol ofAgAu and 5mol of Au doped CeO
2were calculated
(using the peak at 2120579 = 285∘) using Scherrerrsquos equation tobe 130 140 124 80 100 and 86 nm respectively For themetal doped samples new peaks (green filled circles) were
Journal of Chemistry 3
Ag 25 Au 25 25mol
Au 25 Ni 2520nm 20nm
20nm20nm mol Nimol Au 25 mol
mol Pd 25 mol mol Pd 25 mol
Figure 1 Typical TEM image of AuAg AuNi AuPd and NiPd codoped (25 and 25mol resp) CeO2catalysts
Cou
nt ra
te (a
rb u
nit)
(111
)(200
)
(111
)
(002
)(220
)
(311
)(222
)
(022
)
(400
)
= 5 0
4 1
25 25
1 4
= 0 5
CeO2
2120579 (degree)70605040302010
Ag Au
Ag Au
Ag Au (mol)Doped
Figure 2 Power X-ray diffraction patterns of undoped CeO2and Au and Ag doped and codoped (05 41 2525 14 and 50mol resp)
CeO2catalysts The red and green filled circles are of cubic CeO
2and Au phases respectively
4 Journal of Chemistry
Abso
rban
ce (a
rb u
nit)
CeO2Ag = 5mol
Au = 5mol
Wavelength (nm)800600400200
1mol 4mol25 mol 25 mol
4mol 1mol
Doped Ag Au
Figure 3 UV-visible diffuse reflectance spectra (expressed in termsof KubelkandashMunk absorbance arbitrary unit) of undoped CeO
2and
Au and Ag doped and codoped (50 05 41 2525 and 14mol)CeO2catalysts Optical microscopy images (inset) show the colors
of the corresponding samples
observed at 2120579 = 381∘ 443∘ and 646∘ corresponding tothe (111) (002) and (022) planes of cubic phase metallic Au[5] The new peaks were the most intense for the AgAu(14mol) doped sample which was attributed to the highercrystallinity No Ag peaks were observed indicating well-dispersed small amorphous states
TheUV-Vis diffuse reflectance characteristics of themetaldoped samples were examined to determine the metal-doping states as shown in Figure 3 For undoped CeO
2
no significant visible light absorption was observed and theabsorption edge was positioned at sim29 eV Upon metal-doping the absorption in the visible region was increasedsignificantly For Ag (5mol) doped CeO
2 the color of the
powder sample became yellow The color became reddish asthe amount of Au was increased and the UV-Vis absorp-tion in the visible region also increased For Au (5mol)doped CeO
2 a broad absorption peak was observed at
approximately 530 nm which was attributed to the surfaceplasmon resonance absorption of Au nanoparticles [30] Forthe AgAu (41 2525 and 14mol) doped samples theabsorption in the longer wavelength region was attributed tothe formation of larger particles
Figure 4 presents the FT-IR spectra of undopedCeO2and
Au and Ag doped and codoped (50 05 41 2525 and 14mol) CeO
2nanoparticles A broad peak was commonly
observed at 3400 cmminus1 which was attributed to the adsorbedsurface OH andor H
2O species The maximum of the broad
peak was shifted to a shorter wavenumber with increasing theamount of Au The complicated vibrational peaks observed
Tran
smitt
ance
(arb
uni
t)
CeO2
Ag = 5mol
Au = 5mol
Wavenumber (cmminus1)1000200030004000
Doped Ag Au
1mol 4mol
25 mol 25 mol
4mol 1mol
Figure 4 FT-IR spectra of undoped CeO2and Au and Ag doped
and codoped (50 05 41 2525 and 14mol) CeO2
H2
cons
umpt
ion
(arb
uni
t)
CeO2
Au = 5mol
H2-TPR
100800600400200
Temperature (∘C)
1mol 4mol
25 mol 25 mol
4mol 1mol
Doped Ag Au
Ag = 5mol
Figure 5 TPR profiles of undoped CeO2and Au and Ag doped and
codoped (50 05 41 2525 and 14mol) CeO2catalysts
between 1300 and 1800 cmminus1 were assigned to C=O C=C andCOO- functional groups [5] which were dependent on thesample states
Figure 5 shows the temperature programmed hydrogenreduction (TPR) profiles of the bare and metal doped CeO
2
catalysts For bare CeO2 two broad peaks were observed at
around 550 and 900∘C The higher temperature peak wasattributed to the reduction of bulk oxygen of CeO
2 The
lower temperature peak was assigned to the reduction ofsurface oxygen The reduction peak for bulk oxygen is
Journal of Chemistry 5
commonly observed for metal doped CeO2 but at a lower
temperature (by sim50∘C) In addition the strong peaks newlyappeared below 400∘C for the metal doped CeO
2 The peak
intensityposition and broadness were dependent on theinteractions between the dopedmetal and the lattice of CeO
2
Because doped Ag and Au are present as the metallic statethe doped metallic nanoparticles could cause the spillover oflattice oxygen by forming AundashOndashCe state to result in easyreduction [19 24] Ce3+ can be formed from Ce4+ by formingAundashO bond and charge transfer from Au to Ce [27] For Au(5mol) doped CeO
2 the lower TPR peak was observed at
approximately 300∘C For AgAu (14 and 2525mol)doped CeO
2 the peak was observed at a somewhat
higher temperature with different intensities For AgAu(41 and 50mol) doped CeO
2 the peak was observed
at lower temperatures indicating stronger interactions withCeO2
Figure 6 presents the 1st and 2nd run CO oxidationconversion profiles for undoped CeO
2and Au and Ag
doped and codoped (50 05 41 2525 and 14mol)CeO2catalysts The CO conversion () was calculated using
([CO]inndash[CO]out)[CO]in times 100 [35 36] T10 is definedas the temperature corresponding to CO conversion of 10As seen in the spectra the CO oxidation onset position wasdramatically different in all samples For the 1st and 2nd runsof bare CeO
2 T10 was observed at 405∘C Upon metal-
dopingT10 was lowered dramatically In the 1st runT
10 ofthe 5mol Au and Ag doped samples was observed at240∘C and 352∘C respectively Compared to that of bareCeO2 T10 was lowered by 165∘C and 53∘C respectively
(bottom left of Figure 6) As the amount of Au was increasedT10 was observed at a lower temperature The order of
catalytic activity was found to be bare CeO2lt AgAu
(50mol) lt AgAu (41mol) lt AgAu (2525mol)lt AgAu (14mol) lt AgAu (05mol) In the 2nd runT10 was drastically changed for the metal doped samples
T10 of the 5mol Au and Ag doped samples was observed
at 295∘C and 262∘C respectively The Au doped sampleshowed a 55∘C increase in T
10 while Ag doped sampleshowed a 90∘C decrease in T
10 The order of the catalyticactivity was bare CeO
2lt AgAu (2525mol) lt AgAu
(05mol) asymp AgAu (41mol) lt AgAu (50mol) ltAgAu (14mol)The AgAu (14mol) showed the high-est activity Compared to T
10 in the 1st run the AgAu(50mol) and AgAu (14mol) samples showed a lowerT10 while other samples showed a higher T
10 in the 2ndrun as shown in the bottom right of Figure 6 In the 2nd runboth the sintering of Au nanoparticles and alloying of twodifferent metals were expected to play a role in determiningthe activity because the sample had already experienced ahigh temperature up to 700∘C The colors of the sampleswere significantly changed after the CO oxidation reactionsParticularly the colors of the AgAu (41mol) AgAu(2525mol) andAgAu (05mol) became dark grey (orblack) after the CO oxidation unlike other three samplesThe corresponding catalysts showed catalyst deactivation inthe 2nd run compared with the 1st run (Figure 6(d)) Thisindicates that change in oxidation state carbon residues
after reaction and sinteringalloying of loaded metals areimportant factors for the determination of catalytic activitySasirekha et al examined CO oxidation under hydrogen-rich conditions for Au and Ag doped and codoped CeO
2
catalysts and reported that the Ag-Ag (5 5) doped sampleshowed the highest CO conversion and selectivity [19] Theenhancement was attributed to bimetallic alloy formation[19 24] On the other hand in the present study the AgAu(2525mol) sample showed the poorest activity amongthe metal doped samples in the 2nd run This suggests thatother factors (eg size and relative distributions) are alsoimportant for determining the activity CO oxidation hascommonly been understood by CO(ad) + [O]lowast rarr CO
2(g)
where [O]lowast is the active surface oxygen The surface oxygenis replenished by molecular oxygen present in air AdsorbedCO is plausibly present at the interface of doped metal andCeO2 on top of metal andor defect sites [31]The crystalline
size (reflecting the surface area) of the samples was estimatedusing the full width at half maximum of the (111) peak andScherrerrsquos equation [12] The order of the size was found tobe AgAu (2525mol) 80 nm lt AgAu (05mol)86 nm lt AgAu (14mol) 100 nm lt AgAu (41mol)124 nm lt bare CeO
2 130 nm lt AgAu (50mol) and
140 nm Based on this the size was not linearly related withthe catalytic activity For this reason the metal-loading isimportant and themetal-support interactions play significantroles in the catalytic activity [37] In the present study T
50for all the samples was observed to be gt300∘C Zhang et alreported significantly lower T
50 for AuCeO2prepared by a
deposition-precipitation method [37] They reported T50 of
63 35 and 17∘C for untreatedH2 andH
2-O2treated samples
respectively They concluded that the surface interactionbetween Au and CeO
2was the most important factor for
the catalytic activity Li et al reported T50 of lt150∘C for
crystalline Cu-CeO2(5ndash8 nm) nanopowders synthesized by a
hydrothermal method [38] The formic acid-treated Co3O4-
CeO2catalysts were reported to show T
50 at 695∘C for COoxidation [39]The CO oxidation catalytic activities for otherCeO2-based catalysts were summarized elsewhere [11]
Ethanol oxidation reaction performances were fullyexamined for all M doped (M=Ag Au Pd andNi) andMM1015840codoped CeO
2NPs by UV-visible absorption spectroscopy
Figure 7 shows the UV-Vis absorption spectra of the ethanolsolutions reacted at 80∘C for 5 days with and without cat-alysts and with different metal-doping concentration statesTwo broad absorption peaks were commonly observed ataround 220 and 280 nm which were tentatively attributedto ethyl acetate (CH
3COOCH
2CH3 EA) and acetaldehyde
(CH3CHO AcA) respectively for the oxidation products
of ethanol Further details were discussed below The EApeak became stronger and increased more sharply than theAcA peak with reaction time The AcA absorption peakintensity increased slightly gradually reaching a certain lowconcentration levelThe presence of EA as amajor andAcA asaminor productwas further confirmedbymass spectrometry(or UV-visible absorption) as discussed in detail belowTo examine the temperature effect we conducted ethanoloxidation experiments at 40∘C and 80∘C As expected theabsorbance of the two peaks was dramatically enhanced upon
6 Journal of Chemistry
1st run
CeO2
Ag = 5molAu = 5mol
Temperature (∘C)700600500400300200100
00
20
40
60
80
100CO
conv
ersio
n (
)
1 mol 4 mol25 mol 25 mol
4 mol 1molDoped Ag Au
(a)
2nd run
Temperature (∘C)700600500400300200100
00
20
40
60
80
100
CO co
nver
sion
()
CeO2
Ag = 5molAu = 5mol1 mol 4 mol25 mol 25 mol
4 mol 1molDoped Ag Au
(b)
1st run2nd run
Au=
5mol
14m
ol
25
25m
ol
41m
ol
Ag
=5m
ol
0
minus50
minus100
minus150
T10
(MC
eO2)
minusT
10(b
are)
(c)
Au = 5 mol
14 mol
2525 mol
41 mol
Ag = 5mol
T10
(2nd
)minusT
10
minus100
minus50
0
50
100
(1st)
(d)
Au = 5 mol14 mol2525 mol41 molAg = 5molCeO2
bf C
O o
xaf
CO
ox
(e)
Figure 6 1st (a) and 2nd (b) run temperature programmed CO oxidation conversion () profiles (a b) of undoped CeO2and Au and Ag
doped and codoped (50 05 41 2525 and 14mol) CeO2catalysts The difference (c) in T
10 between the metal doped and bare CeO2
for the 1st and 2nd runs The difference (d) in T10 between the 1st and 2nd runs for the metal doped CeO
2catalysts Optical microscope
images showed the color of the powder samples before and after CO oxidation reactions
Journal of Chemistry 7
Rxn in 5 daysat 80∘C
Wavelength (nm)350300250
Wavelength (nm)
350300250Wavelength (nm)
350300250
Doped Ag AuAb
sorb
ance
(arb
uni
t)
10
05
00
15
00
01
02
03
04
Abso
rban
ce (a
rb u
nit)
0
1
2
3
4
5
Abso
rban
ce (a
rb u
nit)
With reaction timeat 80
∘C5 days4 days3 days2 days1 day (24h)8 h4hAu-(5mol) CeO2
Au = 5molNo catalyst
Ag = 5 molCeO21 mol 4 mol
25 mol 25 mol
4 mol 1 mol
O
O
O
(a)
O
O
O
Au = 5mol
Rxn in 5 daysat 80∘C
at 80∘C
0
1
2
3
4
5
Abso
rban
ce (a
rb u
nit)
Wavelength (nm)350300250
Wavelength (nm)
350300250
Doped Ni Au
Rxn in 24 hrs
Abso
rban
ce (a
rb u
nit)
10
05
00
15
1 mol 4 mol25 mol 25 mol
Ni = 5 mol4 mol 1 mol
(b)
O
O
O
Au = 5mol
Rxn in 5 daysat 80∘C
at 80∘C
0
1
2
3
4
5
Abso
rban
ce (a
rb u
nit)
Wavelength (nm)350300250
Wavelength (nm)
350300250
Doped Pd Au
Rxn in 24 hrs
Abso
rban
ce (a
rb u
nit)
10
05
00
15
1 mol 4 mol25 mol 25 mol
Pd = 5 mol4 mol 1 mol
(c)
O
O
O
Au = 5mol
Rxn in 5 daysat 80∘C
at 80∘C
Wavelength (nm)350300250
Wavelength (nm)
350300250
Doped Ni Pd
Rxn in 24 hrs
Abso
rban
ce (a
rb u
nit)
10
05
00
15
0
1
2
3
4
5
Abso
rban
ce (a
rb u
nit)
1 mol 4 mol25 mol 25 mol
Pd = 5 molNi = 5 mol
4 mol 1 mol
(d)
Figure 7 UV-visible absorption spectra of the ethanol oxidation with no catalyst undoped CeO2 M doped (M = Ag Au Pd and Ni) and
MM1015840 codoped (AgAu (a) NiAu (b) PdAu (c) and NiPd (d)) CeO2catalysts at 80∘C for 5 days The left inset in (a) shows the magnified
spectra of the grey shadowed region The right inset in (a) shows the UV-Vis absorption spectra of ethanol oxidation with the 5mol Audoped CeO
2catalyst at 80∘C according to the reaction time
increasing reaction temperatureWithout catalysts no signif-icant ethanol oxidation occurred even at high temperatureFor further ethanol oxidation experiments we selected areaction temperature of 80∘C and a total metal-doping levelof 5mol
For Ag and Au doped and codoped samples (Figure 7(a))a strong absorption peak (below 250 nm) was observed forthe Au (5mol) and AuAg (14mol) doped CeO
2cata-
lysts Without a catalyst no significant absorption peak was
observed even after 5 days The absorption peak (shown inthe right inset of Figure 7(a)) increased with increasingreaction time This was attributed to an increase in reactionproducts that contain C=C andor C=O functional groupsFor the other metal doped samples the absorption peakswere much weaker In addition to the strong absorptionpeak a weaker peak at 280 nm was also observed (in theleft inset of Figure 7) The results suggest that at least tworeaction products (EA and AcA as mentioned above) were
8 Journal of Chemistry
present in the ethanol solution The catalytic activity wasobserved to be in the order of bare CeO
2asymp 2525 lt 41 lt
50 ≪ 14 lt 05 (AgAumol) When the concentration ofAu was the same as or lower than that of Ag the activitydeteriorated drastically For Au and Ni doped and codopedsamples (Figure 7(b)) the catalytic activity was decreasedupon adding Ni as a cocatalyst The activity was found to bein the order of 50 lt 41≪ 2525 lt 14 lt 05 (NiAumol)For Au and Pd doped and codoped samples (Figure 7(c))the oxidation performance was more greatly decreased uponadding Pd as a cocatalyst and found to be in the order of 41 le2525asymp 14asymp 50≪ 05 (PdAumol) ForNi and Pd dopedand codoped samples (Figure 7(d)) the catalytic activity wasobserved to be in the order of 50 lt 05≪ 41 asymp 14 le 2525(NiPdmol) The catalytic activity of the NiPd codopedsamples showed much higher catalytic activity than those ofthe single M- (Ni and Pd) doped samples For comparisonof the catalytic activities of single M doped CeO
2NPs the
ethanol oxidation performance showed an order of undopedasympNi ltAg lt Pd≪Au Interestingly the Ni-doping showed noincrease in catalytic activity for ethanol oxidation
For ethanol oxidation on a metal doped CeO2power
sample since the reaction mechanism was much more com-plicated than expected on a single crystal surface we proposethe following simplified mechanisms which are discussed ingreater detail below [32]
Acetaldehyde hemiacetal and ethyl acetate formationfrom ethanol is as follows
CH3CH2OndashH 997888rarr CH
3CH2O (ad) +H (ad) (1)
CH3CH2O (ad) +O species
997888rarr CH3CHO (ad) +OH (ad)
(2)
CH3CH2O (ad) ndashM
997888rarr CH3CHO (minor) +MH hydride shift
(3)
CH3CHO +O (ad) 997888rarr CH
3COO (ad) +H (ad)
997888rarr CH3COOH
(4)
CH3COOH (ad) + CH3CH2OH (ad)
997888rarr CH3COOCH
2CH3+H2O
(5)
2CH3CHO (ad) 997888rarr CH
3COOCH
2CH3 (6)
CH3CHO (ad) + CH3CH2OH (ad)
997888rarr CH3CH (OH)OC
2H5 (hemiacetal)
997888rarr CH3COOCH
2CH3(major) +H
2
(7)
The rate constant for each step is controlled by the surfacearea and metal-support interaction (or surface activity) Inreaction (1) the OndashH bond of ethanol dissociates to formCH3CH2O which may be mainly adsorbed onto the doped
metal siteThis then turns into adsorbedCH3CHOvia nearby
active oxygen species in (2) or the adsorbed CH3CH2O on
metal desorbs as CH3CHO (acetaldehyde) in response to a
hydride shift reaction in (3) [32 40] Although we have nodirect evidence of the hydride shift reaction the reactionprocess is highly plausible The acetaldehyde in (4) furtherprecedes oxidation reactions to form CH
3COOH (acetic
acid) if active oxygen species are available nearby Otherwisethe CH
3COOH with ethanol in (5) and 2CH
3CHO in (6)
react to form CH3COOCH
2CH3(ethyl acetate) In reaction
(7) CH3CHO and ethanol formCH
3CH(OH)OC
2H5(hemi-
acetal) which is converted to ethyl acetate Consequentlyethyl acetate (CH
3COOCH
2CH3) is formed as a final oxi-
dation product which was confirmed by mass spectrometryIn the present UV-Vis spectra two products of ethyl acetate(major) and acetaldehyde (minor) were observed For alcoholoxidation on the Au-CeO
2catalyst Maldotti et al reported
that the Au-H species is an important intermediate [32] Thisindicates that the hydride shift reaction is facilitated by activedopedmetalsThe present study showed that the Au-rich cat-alyst produced much higher oxidation products and the Auspecies is more active than other metal species (Ag Ni andPd)The reference UV-Vis spectra (Figure 8(a)) were checkedfor four plausible ethanol oxidation products acetaldehydeethyl acetate acetone and acetic acid and the stronger andweaker peak positions near 220 and 280 nm were assignedto the UV-Vis absorptions of ethyl acetate and acetaldehyderespectively Figure 8(b) displays the mass spectrum of thesolution sample after reaction relative to those of the referencesolvents (ethyl acetate and ethanol) As shown in the massspectrum the oxidation product in ethanol matched thatof the reference ethyl acetate well In addition the smell ofthe two samples was very similar As a result we concludedthat the final major product was ethyl acetate For someother extra mass fragmentation signals (59 73 and 75 amu)although no reference data were available the fragmentationsappeared to form from the hemiacetal as shown in reaction(7) Abad et al extensively studied oxidation of alcoholscatalyzed by AuCeO
2[40] and proposed a reaction of (7)
mentioned above in which hemiacetal was detected by H-NMR We have excluded diethyl ether as a major producteven though it could be formed by 2C
2H5OHrarrC
2H5OC2H5
+ H2O because the UV-visible absorption intensity (even
measuredwith 50 solution) was extremely low (Figure 8(a))when compared with that of the sample We also detected nofragmentation signals of diethyl ether by mass spectrometryThe acetone formation reaction 2CH
3CHOrarr CH
3COCH
3
(acetone) + CO2+ H2 was excluded due to absence of the
mass signal Acetic acid as a major product was also excludedbecause the solution is not acidic the mass signal is absentand it did not smell like acetic acid Table 1 summarizes thesizes of the metal-loaded CeO
2estimated using Scherrerrsquos
equation As for the CO oxidation the ethanol oxidationactivity was also found to be more loaded metal (and therelative concentrations) dependent than the size-dependent
4 Conclusion
To increase the catalytic activity of bare CeO2 the CeO
2
matrix was doped and codoped with Ag Au Pd and Ni bya hydrothermal method The novelty of the present study
Journal of Chemistry 9
Table 1 Particles sizes of the metal-loaded CeO2estimated using Scherrerrsquos equation
Loaded MM1015840 50mol (nm) 41mol (nm) 2525mol (nm) 14mol (nm) 05mol (nm)Ag Au 140 124 80 100 86Ni Au 152 123 106 82 86Pd Au 151 127 121 90 86Ni Pd 152 111 147 121 151
Catalysts without stirring
Tightly capped
OOH
O
O
O
lowast
lowast
O
OH
OHO
OO
Abso
rban
ce
10
05
00
Diethyl ether 50
Different smellAcetaldehyde sim1
Acetone sim1
Different smellAcetic acid 01
Ethyl acetate 01
Wavelength (nm)400350300250
(a)
Ethyl acetate(reference)
O
O
Mass (amu)1009080706050M
ass s
igna
l (au
)
OH Before reaction(ETOH)
50 60
Mass (amu)70 80 90 100M
ass s
igna
l (au
)
Afterreaction
01234
UV-VisO
O
Mass (amu)1009080706050M
ass s
igna
l (au
)
Abso
rban
ce
250 300Wavelength (nm)
(b)
Figure 8 UV-Vis absorption spectra (a) of standard samples of acetaldehyde (1) acetone (1) acetic acid (01) and ethyl acetate (01)Mass spectra (b) of reference samples (ethyl acetate and ethanol) and the solution sample after reactionThe inset shows theUV-Vis absorptionspectrum of the corresponding sample solution Blue and red lowast indicate the peak positions for acetaldehyde and ethyl acetate respectively
was that the catalytic efficiency of doped and codoped CeO2
was tested for both gas-phase CO and liquid-phase ethanoloxidation reactions For the 1st and 2nd runs of bare CeO
2
T10 was observed at 405∘C T
10 of bare CeO2for CO oxi-
dation was lowered significantly by 165∘C uponmetal (AgAu= 14mol) doping There were some synergic effects uponcodoping for the CO oxidation The CO oxidation activityvaries with the relative concentrations of two differentmetalsSintering and alloying of two different metals were found toplay important roles in the CO oxidation activity
For liquid-phase ethanol oxidation two liquid productsof ethyl acetate (major 120582max = 220 nm) and acetaldehyde(minor 120582max = 280 nm) were observed by UV-Vis absorptionspectroscopyThe concentration of acetaldehyde (CH
3CHO)
reached a saturation point while that of ethyl acetate(CH3COOCH
2CH3) dramatically increased with reaction
time These findings indicate that acetaldehyde speciespromptly undergo further reaction to form a major productethyl acetate whichwas confirmed bymass spectrometry andUV-visible absorption Undoped CeO
2produces negligible
acetaldehyde which is direct evidence that a hydride shiftreaction CH
3CH2O(ad)-MrarrCH
2CHO+MH is an impor-
tant step for acetaldehyde production for metal-loaded CeO2
catalysts For M- (single) doped CeO2NPs the ethanol
oxidation performance showed an order of Ni lt Ag lt Pd ≪Au For MM1015840 codoped CeO
2NPs the activity of Au doped
CeO2deteriorated drastically upon adding another metals
(Ag Ni and Pd) as cocatalyst The Au-rich CeO2catalyst
showed higher catalytic activity On the other hand the NiPd codoped sample showed much higher catalytic activitycompared with the single M- (Ni and Pd) doped samplesThis study provides further insights into the development ofcatalysts applicable to a range of oxidation reactions
Competing Interests
The authors declare no conflict of interests
Acknowledgments
This study was supported by the 2015 Yeungnam UniversityResearch Grant
References
[1] X Nie H Qian Q Ge H Xu and R Jin ldquoCO oxidationcatalyzed by oxide-supported Au
25(SR)18
nanoclusters and
10 Journal of Chemistry
identification of perimeter sites as active centersrdquo ACS Nanovol 6 no 7 pp 6014ndash6022 2012
[2] H-F Li N Zhang P Chen M-F Luo and J-Q Lu ldquoHigh sur-face area AuCeO
2catalysts for low temperature formaldehyde
oxidationrdquoApplied Catalysis B Environmental vol 110 pp 279ndash285 2011
[3] K Y Ho and K L Yeung ldquoEffects of ozone pretreatment on theperformance of AuTiO
2catalyst for CO oxidation reactionrdquo
Journal of Catalysis vol 242 no 1 pp 131ndash141 2006[4] K Y Ho and K L Yeung ldquoProperties of TiO
2support and the
performance of AuTiO2catalyst for CO oxidation reactionrdquo
Gold Bulletin vol 40 no 1 pp 15ndash30 2007[5] J Qi J Chen G Li S Li Y Gao and Z Tang ldquoFacile
synthesis of core-shell AuCeO2nanocomposites with remark-
ably enhanced catalytic activity for CO oxidationrdquo Energy andEnvironmental Science vol 5 no 10 pp 8937ndash8941 2012
[6] D Jiang W Wang L Zhang Y Zheng and Z Wang ldquoInsightsinto the surface-defect dependence of photoreactivity overCeO2nanocrystals with well-defined crystal facetsrdquo ACS Catal-
ysis vol 5 no 8 pp 4851ndash4858 2015[7] W Lei T Zhang L Gu et al ldquoSurface-structure sensitivity
of CeO2nanocrystals in photocatalysis and enhancing the
reactivity with nanogoldrdquo ACS Catalysis vol 5 no 7 pp 4385ndash4393 2015
[8] B Li T Gu T Ming J Wang P Wang and J C Yu ldquoGoldcore)(ceria shell) nanostructures for plasmon-enhanced cat-alytic reactions under visible lightrdquo ACS Nano vol 8 no 8 pp8152ndash8162 2014
[9] P Lu B Qiao N Lu et al ldquoPhotochemical deposition of highlydispersed Pt nanoparticles on porous CeO
2nanofibers for the
water-gas shift reactionrdquoAdvanced FunctionalMaterials vol 25no 26 pp 4153ndash4162 2015
[10] L Meng A-P Jia J-Q Lu L-F Luo W-X Huang and M-FLuo ldquoSynergetic effects of PdO species on CO oxidation overPdO-CeO
2catalystsrdquo Journal of Physical Chemistry C vol 115
no 40 pp 19789ndash19796 2011[11] Y Park S K Kim D Pradhan and Y Sohn ldquoThermal H
2-
treatment effects on COCO2conversion over Pd-doped CeO
2
comparison with Au and Ag-doped CeO2rdquo Reaction Kinetics
Mechanisms and Catalysis vol 113 no 1 pp 85ndash100 2014[12] Y Park S K Kim D Pradhan and Y Sohn ldquoSurface treatment
effects on CO oxidation reactions over Co Cu and Ni-dopedand codopedCeO
2catalystsrdquoChemical Engineering Journal vol
250 pp 25ndash34 2014[13] B Xu Q Zhang S YuanM Zhang and T Ohno ldquoMorphology
control and photocatalytic characterization of yttrium-dopedhedgehog-like CeO
2rdquo Applied Catalysis B Environmental vol
164 pp 120ndash127 2015[14] W Huang and Y Gao ldquoMorphology-dependent surface chem-
istry and catalysis of CeO2nanocrystalsrdquo Catalysis Science and
Technology vol 4 no 11 pp 3772ndash3784 2014[15] Y Gao W Wang S Chang and W Huang ldquoMorphology
effect of CeO2support in the preparation metal-support
interaction and catalytic performance of PtCeO2catalystsrdquo
ChemCatChem vol 5 no 12 pp 3610ndash3620 2013[16] Y Zhang N Zhang Z-R Tang and Y-J Xu ldquoA unique
silk mat-like structured PdCeO2as an efficient visible light
photocatalyst for green organic transformation in waterrdquo ACSSustainable Chemistry amp Engineering vol 1 no 10 pp 1258ndash1266 2013
[17] W G Shin H J Jung H G Sung H S Hyun and YSohn ldquoSynergic CO oxidation activities of boron-CeO
2hybrid
materials prepared by dry and wet milling methodsrdquo CeramicsInternational vol 40 no 8 pp 11511ndash11517 2014
[18] H Wu P Wang H He and Y Jin ldquoControlled synthesisof porous AgAu bimetallic hollow nanoshells with tunableplasmonic and catalytic propertiesrdquo Nano Research vol 5 no2 pp 135ndash144 2012
[19] N Sasirekha P Sangeetha and Y-W Chen ldquoBimetallic AundashAgCeO
2catalysts for preferential oxidation ofCO inhydrogen-
rich stream effect of calcination temperaturerdquo The Journal ofPhysical Chemistry C vol 118 no 28 pp 15226ndash15233 2014
[20] S Chen L Luo Z Jiang and W Huang ldquoSize-dependent reac-tion pathways of low-temperature CO oxidation on AuCeO
2
catalystsrdquo ACS Catalysis vol 5 no 3 pp 1653ndash1662 2015[21] D LiuW Li X Feng andY Zhang ldquoGalvanic replacement syn-
thesis of Ag119909Au1minus119909
CeO2(0 le x le 1) coreshell nanospheres
with greatly enhanced catalytic performancerdquoChemical Sciencevol 6 pp 7015ndash7019 2015
[22] Y Kang M Sun and A Li ldquoStudies of the catalytic oxidationof CO over AgCeO
2catalystrdquo Catalysis Letters vol 142 no 12
pp 1498ndash1504 2012[23] S Chang M Li Q Hua et al ldquoShape-dependent inter-
play between oxygen vacancies and AgndashCeO2interaction in
AgCeO2catalysts and their influence on the catalytic activityrdquo
Journal of Catalysis vol 293 pp 195ndash204 2012[24] R Fiorenza C Crisafulli G G Condorelli F Lupo and S Scire
ldquoAu-AgCeO2and Au-CuCeO
2Catalysts for volatile organic
compounds oxidation and CO preferential oxidationrdquo CatalysisLetters vol 145 no 9 pp 1691ndash1702 2015
[25] J Zhang L Li X Huang and G Li ldquoFabrication of AgndashCeO2
core-shell nanospheres with enhanced catalytic performancedue to strengthening of the interfacial interactionsrdquo Journal ofMaterials Chemistry vol 22 no 21 pp 10480ndash10487 2012
[26] A Leyva-Perez D Combita-Merchan J R Cabrero-AntoninoS I Al-Resayes and A Corma ldquoOxyhalogenation of activatedarenes with nanocrystalline ceriardquo ACS Catalysis vol 3 no 2pp 250ndash258 2013
[27] Y Liu H Li J Yu DMao andG Lu ldquoElectronic storage capac-ity of ceria role of peroxide inAux supported onCeO
2(111) facet
and CO adsorptionrdquo Physical Chemistry Chemical Physics vol17 no 41 pp 27758ndash27768 2015
[28] D Jiang WWang S Sun L Zhang and Y Zheng ldquoEquilibrat-ing the plasmonic and catalytic roles of metallic nanostructuresin photocatalytic oxidation over Au-modified CeO
2rdquo ACS
Catalysis vol 5 no 2 pp 613ndash621 2015[29] M M Khan S A Ansari M O Ansari B K Min J Lee and
M H Cho ldquoBiogenic fabrication of AuCeO2nanocomposite
with enhanced visible light activityrdquo Journal of Physical Chem-istry C vol 118 no 18 pp 9477ndash9484 2014
[30] A Tanaka K Hashimoto and H Kominami ldquoPreparation ofAuCeO
2exhibiting strong surface plasmon resonance effective
for selective or chemoselective oxidation of alcohols to alde-hydes or ketones in aqueous suspensions under irradiation bygreen lightrdquo Journal of the American Chemical Society vol 134no 35 pp 14526ndash14533 2012
[31] H Y Kim H M Lee and G Henkelman ldquoCO oxidationmechanism on CeO
2-supported Au nanoparticlesrdquo Journal of
the American Chemical Society vol 134 no 3 pp 1560ndash15702012
[32] A Maldotti A Molinari R Juarez and H Garcia ldquoPhotoin-duced reactivity of AundashH intermediates in alcohol oxidation by
Journal of Chemistry 11
gold nanoparticles supported on ceriardquoChemical Science vol 2no 9 pp 1831ndash1834 2011
[33] L Vivier andDDuprez ldquoCeria-based solid catalysts for organicchemistryrdquo ChemSusChem vol 3 no 6 pp 654ndash678 2010
[34] N Zhang S Liu X Fu and Y-J Xu ldquoA simple strategy forfabrication of ldquoplum-puddingrdquo type PdCeO
2semiconductor
nanocomposite as a visible-light-driven photocatalyst for selec-tive oxidationrdquo Journal of Physical Chemistry C vol 115 no 46pp 22901ndash22909 2011
[35] Y Sohn ldquoSiO2nanospheres modified by Ag nanoparticles sur-
face charging and CO oxidation activityrdquo Journal of MolecularCatalysis A Chemical vol 379 pp 59ndash67 2013
[36] W J Kim D Pradhan and Y Sohn ldquoFundamental natureand CO oxidation activities of indium oxide nanostructures1D-wires 2D-plates and 3D-cubes and donutsrdquo Journal ofMaterials Chemistry A vol 1 no 35 pp 10193ndash10202 2013
[37] R-R Zhang L-H Ren A-H Lu and W-C Li ldquoInfluence ofpretreatment atmospheres on the activity of AuCeO
2catalyst
for low-temperature CO oxidationrdquo Catalysis Communicationsvol 13 no 1 pp 18ndash21 2011
[38] Y Li Y Cai X Xing N Chen D Deng and YWang ldquoCatalyticactivity for CO oxidation of CundashCeO
2composite nanoparticles
synthesized by a hydrothermal methodrdquo Analytical Methodsvol 7 no 7 pp 3238ndash3245 2015
[39] R Shang Y Duan X Zhong W Xie Y Luo and L HuangldquoFormic acid modified Co
3O4-CeO
2catalysts for CO oxida-
tionrdquo Catalysts vol 6 no 3 p 48 2016[40] A Abad P Concepcion A Corma and H Garcıa ldquoA collab-
orative effect between gold and a support induces the selectiveoxidation of alcoholsrdquo Angewandte ChemiemdashInternational Edi-tion vol 44 no 26 pp 4066ndash4069 2005
Submit your manuscripts athttpwwwhindawicom
Hindawi Publishing Corporationhttpwwwhindawicom Volume 2014
Inorganic ChemistryInternational Journal of
Hindawi Publishing Corporation httpwwwhindawicom Volume 2014
International Journal ofPhotoenergy
Hindawi Publishing Corporationhttpwwwhindawicom Volume 2014
Carbohydrate Chemistry
International Journal of
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Journal of
Chemistry
Hindawi Publishing Corporationhttpwwwhindawicom Volume 2014
Advances in
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Analytical Methods in Chemistry
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Bioinorganic Chemistry and ApplicationsHindawi Publishing Corporationhttpwwwhindawicom Volume 2014
SpectroscopyInternational Journal of
Hindawi Publishing Corporationhttpwwwhindawicom Volume 2014
The Scientific World JournalHindawi Publishing Corporation httpwwwhindawicom Volume 2014
Medicinal ChemistryInternational Journal of
Hindawi Publishing Corporationhttpwwwhindawicom Volume 2014
Chromatography Research International
Hindawi Publishing Corporationhttpwwwhindawicom Volume 2014
Applied ChemistryJournal of
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Analytical ChemistryInternational Journal of
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Quantum Chemistry
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ElectrochemistryInternational Journal of
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Hindawi Publishing Corporationhttpwwwhindawicom Volume 2014
CatalystsJournal of
2 Journal of Chemistry
alcohol oxidation is very important to understanding of thereaction mechanisms involved in many industrial organicsynthetic processes because of its importance as a fuel [3233] Zhang et al prepared plum-pudding type PdCeO
2
and used it as a visible light photocatalyst for selectiveoxidation of benzylic alcohols to corresponding aldehydesin a process in which photogenerated electron producedsuperoxide radicals thereby facilitating the oxidation [34]Maldotti et al emphasized that Au-H species is an importantintermediate for alcohol oxidation when Au-CeO
2catalyst is
used [32]Motivated by these studies this study examined the
catalytic activity of M doped (M = Ag Au Pd and Ni) andMM1015840 codoped CeO
2for both liquid ethanol and gas-phase
COoxidation reactionsThe catalysts were reacted in a streamof gas-phase CO and liquid-phase ethanol CO oxidation isthe simplest model system understood by a simplified CO +[O]lowast rarr CO
2mechanism while for CH
3CH2OH oxidation
on an oxide support the reactions are very complicatedCH3CH2OH rarr CH
3CH2O(ad) + H(ad) CH
3CH2O(ad) +
[O]lowast rarr CH3CHO CH
3CHO + [O]lowast rarr CH
3COOH and
ethyl acetate (CH3COOCH
2CH3) formation via aldehyde
and hemiacetal (CH3CH(OH)OC
2H5) Because the two oxi-
dation reactions have different mechanisms two systemstogether were investigated to determine the role of dopedmetals and the relative concentrations of two differentmetals
2 Experimental
Cerium oxide (CeO2) nanoparticles (NPs) were synthesized
by a hydrothermal method which is described briefly asfollows 10mL of 01M Ce(NO
3)3sdot6H2O (Sigma-Aldrich
99) was added to 15mL of deionized water in a Teflonbottle Subsequently 20mL of ammonia (28sim30) solutionwas added The solution was fully mixed and the bottlewas tightly capped and placed in an oven (120∘C) for 12 hrsFor the synthesis of metal (Ag Au Pd and Ni) doped andcodoped CeO
2 stoichiometric amounts (MM1015840 = 50mol
14mol 2525mol 41mol and 05mol relative toCe ions) of two differentmetal solutions were added to the Cenitrate solution before capping the bottle and placing it intothe oven Upon the reaction for 12 hrs the final products werecooled naturally and washed repeatedly with deionized waterand ethanol several times The finally collected samples werefully dried in a conventional oven (80∘C)
The morphologies of the samples were examined bytransmission electron microscopy (TEM Hitachi H-7600)operated at 100 kV For this the samples were mountedonto carbon-coated Cu grids X-ray diffraction (XRD PAN-alytical XrsquoPert Pro MPD) was performed to examine thecrystal structures of the dried powder samples using CuK120572 radiation at 40 kV and 30mA The UV-visible (UV-VisSCINCO Neosys-2000) absorption spectra of the powdersamples were recorded The Fourier transform infrared (FT-IR) spectra were obtained using a Thermo Scientific NicoletiS10 spectrometer in ZnSe attenuated total reflection mode
Temperature programmed reduction (TPR) was per-formed to examine the reducibility of the catalyst powder
samples using a Quantachrome CHEMBET equipped with athermal conductivity detector The samples were degassed at150∘C for 2 hrs under nitrogen before being tested by TPRTPR was performed at a heating rate of 20∘Cmin and aflow rate of 40mLmin under 5 H
2N2gas stream CO
oxidation tests were performed in a U-tube (inner diameterof 40mm) quartz reactor loaded with 10mg of the catalystThe temperature heating rate was set to 10∘CminThemixedCO(10)O
2(25)N
2gas was fed to the reactor at a flow
rate of 40mLmin The final gas reaction products weremonitored using a RGA 200 quadrupole mass spectrometer(Stanford Research Systems USA)
The liquid-phase ethanol oxidation reaction was per-formed as follows 10mg of the catalyst and 15mL of ethanolsolvent were mixed in a test tube after which the tube wastightly capped The test tube was then placed in an oven at80∘C (or 40∘C) without stirring Since we tightly capped thetube the oxygen supply will be limited at a certain reactionlevel After a desired reaction time in the oven we took theUV-visible absorption spectrum of the solution in the testtube To detect the final products after the ethanol oxidationwe introduced the solution via a leak valve into the UHVchamber and recorded a mass spectrum
3 Results and Discussion
The metal (Ag Au Pd and Ni) codoped (M and M1015840 = 25and 25mol resp) CeO
2catalysts were examined by TEM
Figure 1 reveals two different (big and small) size distribu-tions one was lt20 nm and the other was lt5 nm The largerand smaller particles could be attributed to bulk CeO
2and
doped metal nanoparticles which could be further clearlyidentified by energy dispersive X-ray spectroscopy and highresolution transmissionmicroscopyThe smaller metal parti-cles could be active sites for the catalytic reactions The AgAu doped sample showed much higher aggregation and theaggregation was found to be in the order of AgAu gtAuNi simAuPd gt NiPd
Material characterization and CO oxidation were focusedonly for Ag and Au doped and codoped CeO
2NPs Figure 2
presents the powder XRD patterns of undoped CeO2and
Au and Ag doped and codoped (05 41 2525 14 and50mol resp) CeO
2catalysts For undoped Ce oxide
several major peaks (red filled circles) were observed at 2120579 =285∘ 330∘ 474∘ 563∘ 590∘ and 693∘ which were assignedto the (111) (200) (220) (311) (222) and (400) planes of thecubic (Fm-3m) structure (JCPDS 034-0394) of CeO
2 respec-
tively [11 12] The major peak at 2120579 = 285∘ showed no criticaldifference in peak position for all the samples This meansthat the crystal lattice of the CeO
2support was not critically
affected by metal-doping On the other hand the broadnessof the peak was somewhat different indicating a differencein particle size The particle sizes of the undoped 5molAg 41mol of AgAu 2525mol of AgAu 14mol ofAgAu and 5mol of Au doped CeO
2were calculated
(using the peak at 2120579 = 285∘) using Scherrerrsquos equation tobe 130 140 124 80 100 and 86 nm respectively For themetal doped samples new peaks (green filled circles) were
Journal of Chemistry 3
Ag 25 Au 25 25mol
Au 25 Ni 2520nm 20nm
20nm20nm mol Nimol Au 25 mol
mol Pd 25 mol mol Pd 25 mol
Figure 1 Typical TEM image of AuAg AuNi AuPd and NiPd codoped (25 and 25mol resp) CeO2catalysts
Cou
nt ra
te (a
rb u
nit)
(111
)(200
)
(111
)
(002
)(220
)
(311
)(222
)
(022
)
(400
)
= 5 0
4 1
25 25
1 4
= 0 5
CeO2
2120579 (degree)70605040302010
Ag Au
Ag Au
Ag Au (mol)Doped
Figure 2 Power X-ray diffraction patterns of undoped CeO2and Au and Ag doped and codoped (05 41 2525 14 and 50mol resp)
CeO2catalysts The red and green filled circles are of cubic CeO
2and Au phases respectively
4 Journal of Chemistry
Abso
rban
ce (a
rb u
nit)
CeO2Ag = 5mol
Au = 5mol
Wavelength (nm)800600400200
1mol 4mol25 mol 25 mol
4mol 1mol
Doped Ag Au
Figure 3 UV-visible diffuse reflectance spectra (expressed in termsof KubelkandashMunk absorbance arbitrary unit) of undoped CeO
2and
Au and Ag doped and codoped (50 05 41 2525 and 14mol)CeO2catalysts Optical microscopy images (inset) show the colors
of the corresponding samples
observed at 2120579 = 381∘ 443∘ and 646∘ corresponding tothe (111) (002) and (022) planes of cubic phase metallic Au[5] The new peaks were the most intense for the AgAu(14mol) doped sample which was attributed to the highercrystallinity No Ag peaks were observed indicating well-dispersed small amorphous states
TheUV-Vis diffuse reflectance characteristics of themetaldoped samples were examined to determine the metal-doping states as shown in Figure 3 For undoped CeO
2
no significant visible light absorption was observed and theabsorption edge was positioned at sim29 eV Upon metal-doping the absorption in the visible region was increasedsignificantly For Ag (5mol) doped CeO
2 the color of the
powder sample became yellow The color became reddish asthe amount of Au was increased and the UV-Vis absorp-tion in the visible region also increased For Au (5mol)doped CeO
2 a broad absorption peak was observed at
approximately 530 nm which was attributed to the surfaceplasmon resonance absorption of Au nanoparticles [30] Forthe AgAu (41 2525 and 14mol) doped samples theabsorption in the longer wavelength region was attributed tothe formation of larger particles
Figure 4 presents the FT-IR spectra of undopedCeO2and
Au and Ag doped and codoped (50 05 41 2525 and 14mol) CeO
2nanoparticles A broad peak was commonly
observed at 3400 cmminus1 which was attributed to the adsorbedsurface OH andor H
2O species The maximum of the broad
peak was shifted to a shorter wavenumber with increasing theamount of Au The complicated vibrational peaks observed
Tran
smitt
ance
(arb
uni
t)
CeO2
Ag = 5mol
Au = 5mol
Wavenumber (cmminus1)1000200030004000
Doped Ag Au
1mol 4mol
25 mol 25 mol
4mol 1mol
Figure 4 FT-IR spectra of undoped CeO2and Au and Ag doped
and codoped (50 05 41 2525 and 14mol) CeO2
H2
cons
umpt
ion
(arb
uni
t)
CeO2
Au = 5mol
H2-TPR
100800600400200
Temperature (∘C)
1mol 4mol
25 mol 25 mol
4mol 1mol
Doped Ag Au
Ag = 5mol
Figure 5 TPR profiles of undoped CeO2and Au and Ag doped and
codoped (50 05 41 2525 and 14mol) CeO2catalysts
between 1300 and 1800 cmminus1 were assigned to C=O C=C andCOO- functional groups [5] which were dependent on thesample states
Figure 5 shows the temperature programmed hydrogenreduction (TPR) profiles of the bare and metal doped CeO
2
catalysts For bare CeO2 two broad peaks were observed at
around 550 and 900∘C The higher temperature peak wasattributed to the reduction of bulk oxygen of CeO
2 The
lower temperature peak was assigned to the reduction ofsurface oxygen The reduction peak for bulk oxygen is
Journal of Chemistry 5
commonly observed for metal doped CeO2 but at a lower
temperature (by sim50∘C) In addition the strong peaks newlyappeared below 400∘C for the metal doped CeO
2 The peak
intensityposition and broadness were dependent on theinteractions between the dopedmetal and the lattice of CeO
2
Because doped Ag and Au are present as the metallic statethe doped metallic nanoparticles could cause the spillover oflattice oxygen by forming AundashOndashCe state to result in easyreduction [19 24] Ce3+ can be formed from Ce4+ by formingAundashO bond and charge transfer from Au to Ce [27] For Au(5mol) doped CeO
2 the lower TPR peak was observed at
approximately 300∘C For AgAu (14 and 2525mol)doped CeO
2 the peak was observed at a somewhat
higher temperature with different intensities For AgAu(41 and 50mol) doped CeO
2 the peak was observed
at lower temperatures indicating stronger interactions withCeO2
Figure 6 presents the 1st and 2nd run CO oxidationconversion profiles for undoped CeO
2and Au and Ag
doped and codoped (50 05 41 2525 and 14mol)CeO2catalysts The CO conversion () was calculated using
([CO]inndash[CO]out)[CO]in times 100 [35 36] T10 is definedas the temperature corresponding to CO conversion of 10As seen in the spectra the CO oxidation onset position wasdramatically different in all samples For the 1st and 2nd runsof bare CeO
2 T10 was observed at 405∘C Upon metal-
dopingT10 was lowered dramatically In the 1st runT
10 ofthe 5mol Au and Ag doped samples was observed at240∘C and 352∘C respectively Compared to that of bareCeO2 T10 was lowered by 165∘C and 53∘C respectively
(bottom left of Figure 6) As the amount of Au was increasedT10 was observed at a lower temperature The order of
catalytic activity was found to be bare CeO2lt AgAu
(50mol) lt AgAu (41mol) lt AgAu (2525mol)lt AgAu (14mol) lt AgAu (05mol) In the 2nd runT10 was drastically changed for the metal doped samples
T10 of the 5mol Au and Ag doped samples was observed
at 295∘C and 262∘C respectively The Au doped sampleshowed a 55∘C increase in T
10 while Ag doped sampleshowed a 90∘C decrease in T
10 The order of the catalyticactivity was bare CeO
2lt AgAu (2525mol) lt AgAu
(05mol) asymp AgAu (41mol) lt AgAu (50mol) ltAgAu (14mol)The AgAu (14mol) showed the high-est activity Compared to T
10 in the 1st run the AgAu(50mol) and AgAu (14mol) samples showed a lowerT10 while other samples showed a higher T
10 in the 2ndrun as shown in the bottom right of Figure 6 In the 2nd runboth the sintering of Au nanoparticles and alloying of twodifferent metals were expected to play a role in determiningthe activity because the sample had already experienced ahigh temperature up to 700∘C The colors of the sampleswere significantly changed after the CO oxidation reactionsParticularly the colors of the AgAu (41mol) AgAu(2525mol) andAgAu (05mol) became dark grey (orblack) after the CO oxidation unlike other three samplesThe corresponding catalysts showed catalyst deactivation inthe 2nd run compared with the 1st run (Figure 6(d)) Thisindicates that change in oxidation state carbon residues
after reaction and sinteringalloying of loaded metals areimportant factors for the determination of catalytic activitySasirekha et al examined CO oxidation under hydrogen-rich conditions for Au and Ag doped and codoped CeO
2
catalysts and reported that the Ag-Ag (5 5) doped sampleshowed the highest CO conversion and selectivity [19] Theenhancement was attributed to bimetallic alloy formation[19 24] On the other hand in the present study the AgAu(2525mol) sample showed the poorest activity amongthe metal doped samples in the 2nd run This suggests thatother factors (eg size and relative distributions) are alsoimportant for determining the activity CO oxidation hascommonly been understood by CO(ad) + [O]lowast rarr CO
2(g)
where [O]lowast is the active surface oxygen The surface oxygenis replenished by molecular oxygen present in air AdsorbedCO is plausibly present at the interface of doped metal andCeO2 on top of metal andor defect sites [31]The crystalline
size (reflecting the surface area) of the samples was estimatedusing the full width at half maximum of the (111) peak andScherrerrsquos equation [12] The order of the size was found tobe AgAu (2525mol) 80 nm lt AgAu (05mol)86 nm lt AgAu (14mol) 100 nm lt AgAu (41mol)124 nm lt bare CeO
2 130 nm lt AgAu (50mol) and
140 nm Based on this the size was not linearly related withthe catalytic activity For this reason the metal-loading isimportant and themetal-support interactions play significantroles in the catalytic activity [37] In the present study T
50for all the samples was observed to be gt300∘C Zhang et alreported significantly lower T
50 for AuCeO2prepared by a
deposition-precipitation method [37] They reported T50 of
63 35 and 17∘C for untreatedH2 andH
2-O2treated samples
respectively They concluded that the surface interactionbetween Au and CeO
2was the most important factor for
the catalytic activity Li et al reported T50 of lt150∘C for
crystalline Cu-CeO2(5ndash8 nm) nanopowders synthesized by a
hydrothermal method [38] The formic acid-treated Co3O4-
CeO2catalysts were reported to show T
50 at 695∘C for COoxidation [39]The CO oxidation catalytic activities for otherCeO2-based catalysts were summarized elsewhere [11]
Ethanol oxidation reaction performances were fullyexamined for all M doped (M=Ag Au Pd andNi) andMM1015840codoped CeO
2NPs by UV-visible absorption spectroscopy
Figure 7 shows the UV-Vis absorption spectra of the ethanolsolutions reacted at 80∘C for 5 days with and without cat-alysts and with different metal-doping concentration statesTwo broad absorption peaks were commonly observed ataround 220 and 280 nm which were tentatively attributedto ethyl acetate (CH
3COOCH
2CH3 EA) and acetaldehyde
(CH3CHO AcA) respectively for the oxidation products
of ethanol Further details were discussed below The EApeak became stronger and increased more sharply than theAcA peak with reaction time The AcA absorption peakintensity increased slightly gradually reaching a certain lowconcentration levelThe presence of EA as amajor andAcA asaminor productwas further confirmedbymass spectrometry(or UV-visible absorption) as discussed in detail belowTo examine the temperature effect we conducted ethanoloxidation experiments at 40∘C and 80∘C As expected theabsorbance of the two peaks was dramatically enhanced upon
6 Journal of Chemistry
1st run
CeO2
Ag = 5molAu = 5mol
Temperature (∘C)700600500400300200100
00
20
40
60
80
100CO
conv
ersio
n (
)
1 mol 4 mol25 mol 25 mol
4 mol 1molDoped Ag Au
(a)
2nd run
Temperature (∘C)700600500400300200100
00
20
40
60
80
100
CO co
nver
sion
()
CeO2
Ag = 5molAu = 5mol1 mol 4 mol25 mol 25 mol
4 mol 1molDoped Ag Au
(b)
1st run2nd run
Au=
5mol
14m
ol
25
25m
ol
41m
ol
Ag
=5m
ol
0
minus50
minus100
minus150
T10
(MC
eO2)
minusT
10(b
are)
(c)
Au = 5 mol
14 mol
2525 mol
41 mol
Ag = 5mol
T10
(2nd
)minusT
10
minus100
minus50
0
50
100
(1st)
(d)
Au = 5 mol14 mol2525 mol41 molAg = 5molCeO2
bf C
O o
xaf
CO
ox
(e)
Figure 6 1st (a) and 2nd (b) run temperature programmed CO oxidation conversion () profiles (a b) of undoped CeO2and Au and Ag
doped and codoped (50 05 41 2525 and 14mol) CeO2catalysts The difference (c) in T
10 between the metal doped and bare CeO2
for the 1st and 2nd runs The difference (d) in T10 between the 1st and 2nd runs for the metal doped CeO
2catalysts Optical microscope
images showed the color of the powder samples before and after CO oxidation reactions
Journal of Chemistry 7
Rxn in 5 daysat 80∘C
Wavelength (nm)350300250
Wavelength (nm)
350300250Wavelength (nm)
350300250
Doped Ag AuAb
sorb
ance
(arb
uni
t)
10
05
00
15
00
01
02
03
04
Abso
rban
ce (a
rb u
nit)
0
1
2
3
4
5
Abso
rban
ce (a
rb u
nit)
With reaction timeat 80
∘C5 days4 days3 days2 days1 day (24h)8 h4hAu-(5mol) CeO2
Au = 5molNo catalyst
Ag = 5 molCeO21 mol 4 mol
25 mol 25 mol
4 mol 1 mol
O
O
O
(a)
O
O
O
Au = 5mol
Rxn in 5 daysat 80∘C
at 80∘C
0
1
2
3
4
5
Abso
rban
ce (a
rb u
nit)
Wavelength (nm)350300250
Wavelength (nm)
350300250
Doped Ni Au
Rxn in 24 hrs
Abso
rban
ce (a
rb u
nit)
10
05
00
15
1 mol 4 mol25 mol 25 mol
Ni = 5 mol4 mol 1 mol
(b)
O
O
O
Au = 5mol
Rxn in 5 daysat 80∘C
at 80∘C
0
1
2
3
4
5
Abso
rban
ce (a
rb u
nit)
Wavelength (nm)350300250
Wavelength (nm)
350300250
Doped Pd Au
Rxn in 24 hrs
Abso
rban
ce (a
rb u
nit)
10
05
00
15
1 mol 4 mol25 mol 25 mol
Pd = 5 mol4 mol 1 mol
(c)
O
O
O
Au = 5mol
Rxn in 5 daysat 80∘C
at 80∘C
Wavelength (nm)350300250
Wavelength (nm)
350300250
Doped Ni Pd
Rxn in 24 hrs
Abso
rban
ce (a
rb u
nit)
10
05
00
15
0
1
2
3
4
5
Abso
rban
ce (a
rb u
nit)
1 mol 4 mol25 mol 25 mol
Pd = 5 molNi = 5 mol
4 mol 1 mol
(d)
Figure 7 UV-visible absorption spectra of the ethanol oxidation with no catalyst undoped CeO2 M doped (M = Ag Au Pd and Ni) and
MM1015840 codoped (AgAu (a) NiAu (b) PdAu (c) and NiPd (d)) CeO2catalysts at 80∘C for 5 days The left inset in (a) shows the magnified
spectra of the grey shadowed region The right inset in (a) shows the UV-Vis absorption spectra of ethanol oxidation with the 5mol Audoped CeO
2catalyst at 80∘C according to the reaction time
increasing reaction temperatureWithout catalysts no signif-icant ethanol oxidation occurred even at high temperatureFor further ethanol oxidation experiments we selected areaction temperature of 80∘C and a total metal-doping levelof 5mol
For Ag and Au doped and codoped samples (Figure 7(a))a strong absorption peak (below 250 nm) was observed forthe Au (5mol) and AuAg (14mol) doped CeO
2cata-
lysts Without a catalyst no significant absorption peak was
observed even after 5 days The absorption peak (shown inthe right inset of Figure 7(a)) increased with increasingreaction time This was attributed to an increase in reactionproducts that contain C=C andor C=O functional groupsFor the other metal doped samples the absorption peakswere much weaker In addition to the strong absorptionpeak a weaker peak at 280 nm was also observed (in theleft inset of Figure 7) The results suggest that at least tworeaction products (EA and AcA as mentioned above) were
8 Journal of Chemistry
present in the ethanol solution The catalytic activity wasobserved to be in the order of bare CeO
2asymp 2525 lt 41 lt
50 ≪ 14 lt 05 (AgAumol) When the concentration ofAu was the same as or lower than that of Ag the activitydeteriorated drastically For Au and Ni doped and codopedsamples (Figure 7(b)) the catalytic activity was decreasedupon adding Ni as a cocatalyst The activity was found to bein the order of 50 lt 41≪ 2525 lt 14 lt 05 (NiAumol)For Au and Pd doped and codoped samples (Figure 7(c))the oxidation performance was more greatly decreased uponadding Pd as a cocatalyst and found to be in the order of 41 le2525asymp 14asymp 50≪ 05 (PdAumol) ForNi and Pd dopedand codoped samples (Figure 7(d)) the catalytic activity wasobserved to be in the order of 50 lt 05≪ 41 asymp 14 le 2525(NiPdmol) The catalytic activity of the NiPd codopedsamples showed much higher catalytic activity than those ofthe single M- (Ni and Pd) doped samples For comparisonof the catalytic activities of single M doped CeO
2NPs the
ethanol oxidation performance showed an order of undopedasympNi ltAg lt Pd≪Au Interestingly the Ni-doping showed noincrease in catalytic activity for ethanol oxidation
For ethanol oxidation on a metal doped CeO2power
sample since the reaction mechanism was much more com-plicated than expected on a single crystal surface we proposethe following simplified mechanisms which are discussed ingreater detail below [32]
Acetaldehyde hemiacetal and ethyl acetate formationfrom ethanol is as follows
CH3CH2OndashH 997888rarr CH
3CH2O (ad) +H (ad) (1)
CH3CH2O (ad) +O species
997888rarr CH3CHO (ad) +OH (ad)
(2)
CH3CH2O (ad) ndashM
997888rarr CH3CHO (minor) +MH hydride shift
(3)
CH3CHO +O (ad) 997888rarr CH
3COO (ad) +H (ad)
997888rarr CH3COOH
(4)
CH3COOH (ad) + CH3CH2OH (ad)
997888rarr CH3COOCH
2CH3+H2O
(5)
2CH3CHO (ad) 997888rarr CH
3COOCH
2CH3 (6)
CH3CHO (ad) + CH3CH2OH (ad)
997888rarr CH3CH (OH)OC
2H5 (hemiacetal)
997888rarr CH3COOCH
2CH3(major) +H
2
(7)
The rate constant for each step is controlled by the surfacearea and metal-support interaction (or surface activity) Inreaction (1) the OndashH bond of ethanol dissociates to formCH3CH2O which may be mainly adsorbed onto the doped
metal siteThis then turns into adsorbedCH3CHOvia nearby
active oxygen species in (2) or the adsorbed CH3CH2O on
metal desorbs as CH3CHO (acetaldehyde) in response to a
hydride shift reaction in (3) [32 40] Although we have nodirect evidence of the hydride shift reaction the reactionprocess is highly plausible The acetaldehyde in (4) furtherprecedes oxidation reactions to form CH
3COOH (acetic
acid) if active oxygen species are available nearby Otherwisethe CH
3COOH with ethanol in (5) and 2CH
3CHO in (6)
react to form CH3COOCH
2CH3(ethyl acetate) In reaction
(7) CH3CHO and ethanol formCH
3CH(OH)OC
2H5(hemi-
acetal) which is converted to ethyl acetate Consequentlyethyl acetate (CH
3COOCH
2CH3) is formed as a final oxi-
dation product which was confirmed by mass spectrometryIn the present UV-Vis spectra two products of ethyl acetate(major) and acetaldehyde (minor) were observed For alcoholoxidation on the Au-CeO
2catalyst Maldotti et al reported
that the Au-H species is an important intermediate [32] Thisindicates that the hydride shift reaction is facilitated by activedopedmetalsThe present study showed that the Au-rich cat-alyst produced much higher oxidation products and the Auspecies is more active than other metal species (Ag Ni andPd)The reference UV-Vis spectra (Figure 8(a)) were checkedfor four plausible ethanol oxidation products acetaldehydeethyl acetate acetone and acetic acid and the stronger andweaker peak positions near 220 and 280 nm were assignedto the UV-Vis absorptions of ethyl acetate and acetaldehyderespectively Figure 8(b) displays the mass spectrum of thesolution sample after reaction relative to those of the referencesolvents (ethyl acetate and ethanol) As shown in the massspectrum the oxidation product in ethanol matched thatof the reference ethyl acetate well In addition the smell ofthe two samples was very similar As a result we concludedthat the final major product was ethyl acetate For someother extra mass fragmentation signals (59 73 and 75 amu)although no reference data were available the fragmentationsappeared to form from the hemiacetal as shown in reaction(7) Abad et al extensively studied oxidation of alcoholscatalyzed by AuCeO
2[40] and proposed a reaction of (7)
mentioned above in which hemiacetal was detected by H-NMR We have excluded diethyl ether as a major producteven though it could be formed by 2C
2H5OHrarrC
2H5OC2H5
+ H2O because the UV-visible absorption intensity (even
measuredwith 50 solution) was extremely low (Figure 8(a))when compared with that of the sample We also detected nofragmentation signals of diethyl ether by mass spectrometryThe acetone formation reaction 2CH
3CHOrarr CH
3COCH
3
(acetone) + CO2+ H2 was excluded due to absence of the
mass signal Acetic acid as a major product was also excludedbecause the solution is not acidic the mass signal is absentand it did not smell like acetic acid Table 1 summarizes thesizes of the metal-loaded CeO
2estimated using Scherrerrsquos
equation As for the CO oxidation the ethanol oxidationactivity was also found to be more loaded metal (and therelative concentrations) dependent than the size-dependent
4 Conclusion
To increase the catalytic activity of bare CeO2 the CeO
2
matrix was doped and codoped with Ag Au Pd and Ni bya hydrothermal method The novelty of the present study
Journal of Chemistry 9
Table 1 Particles sizes of the metal-loaded CeO2estimated using Scherrerrsquos equation
Loaded MM1015840 50mol (nm) 41mol (nm) 2525mol (nm) 14mol (nm) 05mol (nm)Ag Au 140 124 80 100 86Ni Au 152 123 106 82 86Pd Au 151 127 121 90 86Ni Pd 152 111 147 121 151
Catalysts without stirring
Tightly capped
OOH
O
O
O
lowast
lowast
O
OH
OHO
OO
Abso
rban
ce
10
05
00
Diethyl ether 50
Different smellAcetaldehyde sim1
Acetone sim1
Different smellAcetic acid 01
Ethyl acetate 01
Wavelength (nm)400350300250
(a)
Ethyl acetate(reference)
O
O
Mass (amu)1009080706050M
ass s
igna
l (au
)
OH Before reaction(ETOH)
50 60
Mass (amu)70 80 90 100M
ass s
igna
l (au
)
Afterreaction
01234
UV-VisO
O
Mass (amu)1009080706050M
ass s
igna
l (au
)
Abso
rban
ce
250 300Wavelength (nm)
(b)
Figure 8 UV-Vis absorption spectra (a) of standard samples of acetaldehyde (1) acetone (1) acetic acid (01) and ethyl acetate (01)Mass spectra (b) of reference samples (ethyl acetate and ethanol) and the solution sample after reactionThe inset shows theUV-Vis absorptionspectrum of the corresponding sample solution Blue and red lowast indicate the peak positions for acetaldehyde and ethyl acetate respectively
was that the catalytic efficiency of doped and codoped CeO2
was tested for both gas-phase CO and liquid-phase ethanoloxidation reactions For the 1st and 2nd runs of bare CeO
2
T10 was observed at 405∘C T
10 of bare CeO2for CO oxi-
dation was lowered significantly by 165∘C uponmetal (AgAu= 14mol) doping There were some synergic effects uponcodoping for the CO oxidation The CO oxidation activityvaries with the relative concentrations of two differentmetalsSintering and alloying of two different metals were found toplay important roles in the CO oxidation activity
For liquid-phase ethanol oxidation two liquid productsof ethyl acetate (major 120582max = 220 nm) and acetaldehyde(minor 120582max = 280 nm) were observed by UV-Vis absorptionspectroscopyThe concentration of acetaldehyde (CH
3CHO)
reached a saturation point while that of ethyl acetate(CH3COOCH
2CH3) dramatically increased with reaction
time These findings indicate that acetaldehyde speciespromptly undergo further reaction to form a major productethyl acetate whichwas confirmed bymass spectrometry andUV-visible absorption Undoped CeO
2produces negligible
acetaldehyde which is direct evidence that a hydride shiftreaction CH
3CH2O(ad)-MrarrCH
2CHO+MH is an impor-
tant step for acetaldehyde production for metal-loaded CeO2
catalysts For M- (single) doped CeO2NPs the ethanol
oxidation performance showed an order of Ni lt Ag lt Pd ≪Au For MM1015840 codoped CeO
2NPs the activity of Au doped
CeO2deteriorated drastically upon adding another metals
(Ag Ni and Pd) as cocatalyst The Au-rich CeO2catalyst
showed higher catalytic activity On the other hand the NiPd codoped sample showed much higher catalytic activitycompared with the single M- (Ni and Pd) doped samplesThis study provides further insights into the development ofcatalysts applicable to a range of oxidation reactions
Competing Interests
The authors declare no conflict of interests
Acknowledgments
This study was supported by the 2015 Yeungnam UniversityResearch Grant
References
[1] X Nie H Qian Q Ge H Xu and R Jin ldquoCO oxidationcatalyzed by oxide-supported Au
25(SR)18
nanoclusters and
10 Journal of Chemistry
identification of perimeter sites as active centersrdquo ACS Nanovol 6 no 7 pp 6014ndash6022 2012
[2] H-F Li N Zhang P Chen M-F Luo and J-Q Lu ldquoHigh sur-face area AuCeO
2catalysts for low temperature formaldehyde
oxidationrdquoApplied Catalysis B Environmental vol 110 pp 279ndash285 2011
[3] K Y Ho and K L Yeung ldquoEffects of ozone pretreatment on theperformance of AuTiO
2catalyst for CO oxidation reactionrdquo
Journal of Catalysis vol 242 no 1 pp 131ndash141 2006[4] K Y Ho and K L Yeung ldquoProperties of TiO
2support and the
performance of AuTiO2catalyst for CO oxidation reactionrdquo
Gold Bulletin vol 40 no 1 pp 15ndash30 2007[5] J Qi J Chen G Li S Li Y Gao and Z Tang ldquoFacile
synthesis of core-shell AuCeO2nanocomposites with remark-
ably enhanced catalytic activity for CO oxidationrdquo Energy andEnvironmental Science vol 5 no 10 pp 8937ndash8941 2012
[6] D Jiang W Wang L Zhang Y Zheng and Z Wang ldquoInsightsinto the surface-defect dependence of photoreactivity overCeO2nanocrystals with well-defined crystal facetsrdquo ACS Catal-
ysis vol 5 no 8 pp 4851ndash4858 2015[7] W Lei T Zhang L Gu et al ldquoSurface-structure sensitivity
of CeO2nanocrystals in photocatalysis and enhancing the
reactivity with nanogoldrdquo ACS Catalysis vol 5 no 7 pp 4385ndash4393 2015
[8] B Li T Gu T Ming J Wang P Wang and J C Yu ldquoGoldcore)(ceria shell) nanostructures for plasmon-enhanced cat-alytic reactions under visible lightrdquo ACS Nano vol 8 no 8 pp8152ndash8162 2014
[9] P Lu B Qiao N Lu et al ldquoPhotochemical deposition of highlydispersed Pt nanoparticles on porous CeO
2nanofibers for the
water-gas shift reactionrdquoAdvanced FunctionalMaterials vol 25no 26 pp 4153ndash4162 2015
[10] L Meng A-P Jia J-Q Lu L-F Luo W-X Huang and M-FLuo ldquoSynergetic effects of PdO species on CO oxidation overPdO-CeO
2catalystsrdquo Journal of Physical Chemistry C vol 115
no 40 pp 19789ndash19796 2011[11] Y Park S K Kim D Pradhan and Y Sohn ldquoThermal H
2-
treatment effects on COCO2conversion over Pd-doped CeO
2
comparison with Au and Ag-doped CeO2rdquo Reaction Kinetics
Mechanisms and Catalysis vol 113 no 1 pp 85ndash100 2014[12] Y Park S K Kim D Pradhan and Y Sohn ldquoSurface treatment
effects on CO oxidation reactions over Co Cu and Ni-dopedand codopedCeO
2catalystsrdquoChemical Engineering Journal vol
250 pp 25ndash34 2014[13] B Xu Q Zhang S YuanM Zhang and T Ohno ldquoMorphology
control and photocatalytic characterization of yttrium-dopedhedgehog-like CeO
2rdquo Applied Catalysis B Environmental vol
164 pp 120ndash127 2015[14] W Huang and Y Gao ldquoMorphology-dependent surface chem-
istry and catalysis of CeO2nanocrystalsrdquo Catalysis Science and
Technology vol 4 no 11 pp 3772ndash3784 2014[15] Y Gao W Wang S Chang and W Huang ldquoMorphology
effect of CeO2support in the preparation metal-support
interaction and catalytic performance of PtCeO2catalystsrdquo
ChemCatChem vol 5 no 12 pp 3610ndash3620 2013[16] Y Zhang N Zhang Z-R Tang and Y-J Xu ldquoA unique
silk mat-like structured PdCeO2as an efficient visible light
photocatalyst for green organic transformation in waterrdquo ACSSustainable Chemistry amp Engineering vol 1 no 10 pp 1258ndash1266 2013
[17] W G Shin H J Jung H G Sung H S Hyun and YSohn ldquoSynergic CO oxidation activities of boron-CeO
2hybrid
materials prepared by dry and wet milling methodsrdquo CeramicsInternational vol 40 no 8 pp 11511ndash11517 2014
[18] H Wu P Wang H He and Y Jin ldquoControlled synthesisof porous AgAu bimetallic hollow nanoshells with tunableplasmonic and catalytic propertiesrdquo Nano Research vol 5 no2 pp 135ndash144 2012
[19] N Sasirekha P Sangeetha and Y-W Chen ldquoBimetallic AundashAgCeO
2catalysts for preferential oxidation ofCO inhydrogen-
rich stream effect of calcination temperaturerdquo The Journal ofPhysical Chemistry C vol 118 no 28 pp 15226ndash15233 2014
[20] S Chen L Luo Z Jiang and W Huang ldquoSize-dependent reac-tion pathways of low-temperature CO oxidation on AuCeO
2
catalystsrdquo ACS Catalysis vol 5 no 3 pp 1653ndash1662 2015[21] D LiuW Li X Feng andY Zhang ldquoGalvanic replacement syn-
thesis of Ag119909Au1minus119909
CeO2(0 le x le 1) coreshell nanospheres
with greatly enhanced catalytic performancerdquoChemical Sciencevol 6 pp 7015ndash7019 2015
[22] Y Kang M Sun and A Li ldquoStudies of the catalytic oxidationof CO over AgCeO
2catalystrdquo Catalysis Letters vol 142 no 12
pp 1498ndash1504 2012[23] S Chang M Li Q Hua et al ldquoShape-dependent inter-
play between oxygen vacancies and AgndashCeO2interaction in
AgCeO2catalysts and their influence on the catalytic activityrdquo
Journal of Catalysis vol 293 pp 195ndash204 2012[24] R Fiorenza C Crisafulli G G Condorelli F Lupo and S Scire
ldquoAu-AgCeO2and Au-CuCeO
2Catalysts for volatile organic
compounds oxidation and CO preferential oxidationrdquo CatalysisLetters vol 145 no 9 pp 1691ndash1702 2015
[25] J Zhang L Li X Huang and G Li ldquoFabrication of AgndashCeO2
core-shell nanospheres with enhanced catalytic performancedue to strengthening of the interfacial interactionsrdquo Journal ofMaterials Chemistry vol 22 no 21 pp 10480ndash10487 2012
[26] A Leyva-Perez D Combita-Merchan J R Cabrero-AntoninoS I Al-Resayes and A Corma ldquoOxyhalogenation of activatedarenes with nanocrystalline ceriardquo ACS Catalysis vol 3 no 2pp 250ndash258 2013
[27] Y Liu H Li J Yu DMao andG Lu ldquoElectronic storage capac-ity of ceria role of peroxide inAux supported onCeO
2(111) facet
and CO adsorptionrdquo Physical Chemistry Chemical Physics vol17 no 41 pp 27758ndash27768 2015
[28] D Jiang WWang S Sun L Zhang and Y Zheng ldquoEquilibrat-ing the plasmonic and catalytic roles of metallic nanostructuresin photocatalytic oxidation over Au-modified CeO
2rdquo ACS
Catalysis vol 5 no 2 pp 613ndash621 2015[29] M M Khan S A Ansari M O Ansari B K Min J Lee and
M H Cho ldquoBiogenic fabrication of AuCeO2nanocomposite
with enhanced visible light activityrdquo Journal of Physical Chem-istry C vol 118 no 18 pp 9477ndash9484 2014
[30] A Tanaka K Hashimoto and H Kominami ldquoPreparation ofAuCeO
2exhibiting strong surface plasmon resonance effective
for selective or chemoselective oxidation of alcohols to alde-hydes or ketones in aqueous suspensions under irradiation bygreen lightrdquo Journal of the American Chemical Society vol 134no 35 pp 14526ndash14533 2012
[31] H Y Kim H M Lee and G Henkelman ldquoCO oxidationmechanism on CeO
2-supported Au nanoparticlesrdquo Journal of
the American Chemical Society vol 134 no 3 pp 1560ndash15702012
[32] A Maldotti A Molinari R Juarez and H Garcia ldquoPhotoin-duced reactivity of AundashH intermediates in alcohol oxidation by
Journal of Chemistry 11
gold nanoparticles supported on ceriardquoChemical Science vol 2no 9 pp 1831ndash1834 2011
[33] L Vivier andDDuprez ldquoCeria-based solid catalysts for organicchemistryrdquo ChemSusChem vol 3 no 6 pp 654ndash678 2010
[34] N Zhang S Liu X Fu and Y-J Xu ldquoA simple strategy forfabrication of ldquoplum-puddingrdquo type PdCeO
2semiconductor
nanocomposite as a visible-light-driven photocatalyst for selec-tive oxidationrdquo Journal of Physical Chemistry C vol 115 no 46pp 22901ndash22909 2011
[35] Y Sohn ldquoSiO2nanospheres modified by Ag nanoparticles sur-
face charging and CO oxidation activityrdquo Journal of MolecularCatalysis A Chemical vol 379 pp 59ndash67 2013
[36] W J Kim D Pradhan and Y Sohn ldquoFundamental natureand CO oxidation activities of indium oxide nanostructures1D-wires 2D-plates and 3D-cubes and donutsrdquo Journal ofMaterials Chemistry A vol 1 no 35 pp 10193ndash10202 2013
[37] R-R Zhang L-H Ren A-H Lu and W-C Li ldquoInfluence ofpretreatment atmospheres on the activity of AuCeO
2catalyst
for low-temperature CO oxidationrdquo Catalysis Communicationsvol 13 no 1 pp 18ndash21 2011
[38] Y Li Y Cai X Xing N Chen D Deng and YWang ldquoCatalyticactivity for CO oxidation of CundashCeO
2composite nanoparticles
synthesized by a hydrothermal methodrdquo Analytical Methodsvol 7 no 7 pp 3238ndash3245 2015
[39] R Shang Y Duan X Zhong W Xie Y Luo and L HuangldquoFormic acid modified Co
3O4-CeO
2catalysts for CO oxida-
tionrdquo Catalysts vol 6 no 3 p 48 2016[40] A Abad P Concepcion A Corma and H Garcıa ldquoA collab-
orative effect between gold and a support induces the selectiveoxidation of alcoholsrdquo Angewandte ChemiemdashInternational Edi-tion vol 44 no 26 pp 4066ndash4069 2005
Submit your manuscripts athttpwwwhindawicom
Hindawi Publishing Corporationhttpwwwhindawicom Volume 2014
Inorganic ChemistryInternational Journal of
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Journal of
Spectroscopy
Analytical ChemistryInternational Journal of
Hindawi Publishing Corporationhttpwwwhindawicom Volume 2014
Journal of
Hindawi Publishing Corporationhttpwwwhindawicom Volume 2014
Quantum Chemistry
Hindawi Publishing Corporationhttpwwwhindawicom Volume 2014
Organic Chemistry International
ElectrochemistryInternational Journal of
Hindawi Publishing Corporation httpwwwhindawicom Volume 2014
Hindawi Publishing Corporationhttpwwwhindawicom Volume 2014
CatalystsJournal of
Journal of Chemistry 3
Ag 25 Au 25 25mol
Au 25 Ni 2520nm 20nm
20nm20nm mol Nimol Au 25 mol
mol Pd 25 mol mol Pd 25 mol
Figure 1 Typical TEM image of AuAg AuNi AuPd and NiPd codoped (25 and 25mol resp) CeO2catalysts
Cou
nt ra
te (a
rb u
nit)
(111
)(200
)
(111
)
(002
)(220
)
(311
)(222
)
(022
)
(400
)
= 5 0
4 1
25 25
1 4
= 0 5
CeO2
2120579 (degree)70605040302010
Ag Au
Ag Au
Ag Au (mol)Doped
Figure 2 Power X-ray diffraction patterns of undoped CeO2and Au and Ag doped and codoped (05 41 2525 14 and 50mol resp)
CeO2catalysts The red and green filled circles are of cubic CeO
2and Au phases respectively
4 Journal of Chemistry
Abso
rban
ce (a
rb u
nit)
CeO2Ag = 5mol
Au = 5mol
Wavelength (nm)800600400200
1mol 4mol25 mol 25 mol
4mol 1mol
Doped Ag Au
Figure 3 UV-visible diffuse reflectance spectra (expressed in termsof KubelkandashMunk absorbance arbitrary unit) of undoped CeO
2and
Au and Ag doped and codoped (50 05 41 2525 and 14mol)CeO2catalysts Optical microscopy images (inset) show the colors
of the corresponding samples
observed at 2120579 = 381∘ 443∘ and 646∘ corresponding tothe (111) (002) and (022) planes of cubic phase metallic Au[5] The new peaks were the most intense for the AgAu(14mol) doped sample which was attributed to the highercrystallinity No Ag peaks were observed indicating well-dispersed small amorphous states
TheUV-Vis diffuse reflectance characteristics of themetaldoped samples were examined to determine the metal-doping states as shown in Figure 3 For undoped CeO
2
no significant visible light absorption was observed and theabsorption edge was positioned at sim29 eV Upon metal-doping the absorption in the visible region was increasedsignificantly For Ag (5mol) doped CeO
2 the color of the
powder sample became yellow The color became reddish asthe amount of Au was increased and the UV-Vis absorp-tion in the visible region also increased For Au (5mol)doped CeO
2 a broad absorption peak was observed at
approximately 530 nm which was attributed to the surfaceplasmon resonance absorption of Au nanoparticles [30] Forthe AgAu (41 2525 and 14mol) doped samples theabsorption in the longer wavelength region was attributed tothe formation of larger particles
Figure 4 presents the FT-IR spectra of undopedCeO2and
Au and Ag doped and codoped (50 05 41 2525 and 14mol) CeO
2nanoparticles A broad peak was commonly
observed at 3400 cmminus1 which was attributed to the adsorbedsurface OH andor H
2O species The maximum of the broad
peak was shifted to a shorter wavenumber with increasing theamount of Au The complicated vibrational peaks observed
Tran
smitt
ance
(arb
uni
t)
CeO2
Ag = 5mol
Au = 5mol
Wavenumber (cmminus1)1000200030004000
Doped Ag Au
1mol 4mol
25 mol 25 mol
4mol 1mol
Figure 4 FT-IR spectra of undoped CeO2and Au and Ag doped
and codoped (50 05 41 2525 and 14mol) CeO2
H2
cons
umpt
ion
(arb
uni
t)
CeO2
Au = 5mol
H2-TPR
100800600400200
Temperature (∘C)
1mol 4mol
25 mol 25 mol
4mol 1mol
Doped Ag Au
Ag = 5mol
Figure 5 TPR profiles of undoped CeO2and Au and Ag doped and
codoped (50 05 41 2525 and 14mol) CeO2catalysts
between 1300 and 1800 cmminus1 were assigned to C=O C=C andCOO- functional groups [5] which were dependent on thesample states
Figure 5 shows the temperature programmed hydrogenreduction (TPR) profiles of the bare and metal doped CeO
2
catalysts For bare CeO2 two broad peaks were observed at
around 550 and 900∘C The higher temperature peak wasattributed to the reduction of bulk oxygen of CeO
2 The
lower temperature peak was assigned to the reduction ofsurface oxygen The reduction peak for bulk oxygen is
Journal of Chemistry 5
commonly observed for metal doped CeO2 but at a lower
temperature (by sim50∘C) In addition the strong peaks newlyappeared below 400∘C for the metal doped CeO
2 The peak
intensityposition and broadness were dependent on theinteractions between the dopedmetal and the lattice of CeO
2
Because doped Ag and Au are present as the metallic statethe doped metallic nanoparticles could cause the spillover oflattice oxygen by forming AundashOndashCe state to result in easyreduction [19 24] Ce3+ can be formed from Ce4+ by formingAundashO bond and charge transfer from Au to Ce [27] For Au(5mol) doped CeO
2 the lower TPR peak was observed at
approximately 300∘C For AgAu (14 and 2525mol)doped CeO
2 the peak was observed at a somewhat
higher temperature with different intensities For AgAu(41 and 50mol) doped CeO
2 the peak was observed
at lower temperatures indicating stronger interactions withCeO2
Figure 6 presents the 1st and 2nd run CO oxidationconversion profiles for undoped CeO
2and Au and Ag
doped and codoped (50 05 41 2525 and 14mol)CeO2catalysts The CO conversion () was calculated using
([CO]inndash[CO]out)[CO]in times 100 [35 36] T10 is definedas the temperature corresponding to CO conversion of 10As seen in the spectra the CO oxidation onset position wasdramatically different in all samples For the 1st and 2nd runsof bare CeO
2 T10 was observed at 405∘C Upon metal-
dopingT10 was lowered dramatically In the 1st runT
10 ofthe 5mol Au and Ag doped samples was observed at240∘C and 352∘C respectively Compared to that of bareCeO2 T10 was lowered by 165∘C and 53∘C respectively
(bottom left of Figure 6) As the amount of Au was increasedT10 was observed at a lower temperature The order of
catalytic activity was found to be bare CeO2lt AgAu
(50mol) lt AgAu (41mol) lt AgAu (2525mol)lt AgAu (14mol) lt AgAu (05mol) In the 2nd runT10 was drastically changed for the metal doped samples
T10 of the 5mol Au and Ag doped samples was observed
at 295∘C and 262∘C respectively The Au doped sampleshowed a 55∘C increase in T
10 while Ag doped sampleshowed a 90∘C decrease in T
10 The order of the catalyticactivity was bare CeO
2lt AgAu (2525mol) lt AgAu
(05mol) asymp AgAu (41mol) lt AgAu (50mol) ltAgAu (14mol)The AgAu (14mol) showed the high-est activity Compared to T
10 in the 1st run the AgAu(50mol) and AgAu (14mol) samples showed a lowerT10 while other samples showed a higher T
10 in the 2ndrun as shown in the bottom right of Figure 6 In the 2nd runboth the sintering of Au nanoparticles and alloying of twodifferent metals were expected to play a role in determiningthe activity because the sample had already experienced ahigh temperature up to 700∘C The colors of the sampleswere significantly changed after the CO oxidation reactionsParticularly the colors of the AgAu (41mol) AgAu(2525mol) andAgAu (05mol) became dark grey (orblack) after the CO oxidation unlike other three samplesThe corresponding catalysts showed catalyst deactivation inthe 2nd run compared with the 1st run (Figure 6(d)) Thisindicates that change in oxidation state carbon residues
after reaction and sinteringalloying of loaded metals areimportant factors for the determination of catalytic activitySasirekha et al examined CO oxidation under hydrogen-rich conditions for Au and Ag doped and codoped CeO
2
catalysts and reported that the Ag-Ag (5 5) doped sampleshowed the highest CO conversion and selectivity [19] Theenhancement was attributed to bimetallic alloy formation[19 24] On the other hand in the present study the AgAu(2525mol) sample showed the poorest activity amongthe metal doped samples in the 2nd run This suggests thatother factors (eg size and relative distributions) are alsoimportant for determining the activity CO oxidation hascommonly been understood by CO(ad) + [O]lowast rarr CO
2(g)
where [O]lowast is the active surface oxygen The surface oxygenis replenished by molecular oxygen present in air AdsorbedCO is plausibly present at the interface of doped metal andCeO2 on top of metal andor defect sites [31]The crystalline
size (reflecting the surface area) of the samples was estimatedusing the full width at half maximum of the (111) peak andScherrerrsquos equation [12] The order of the size was found tobe AgAu (2525mol) 80 nm lt AgAu (05mol)86 nm lt AgAu (14mol) 100 nm lt AgAu (41mol)124 nm lt bare CeO
2 130 nm lt AgAu (50mol) and
140 nm Based on this the size was not linearly related withthe catalytic activity For this reason the metal-loading isimportant and themetal-support interactions play significantroles in the catalytic activity [37] In the present study T
50for all the samples was observed to be gt300∘C Zhang et alreported significantly lower T
50 for AuCeO2prepared by a
deposition-precipitation method [37] They reported T50 of
63 35 and 17∘C for untreatedH2 andH
2-O2treated samples
respectively They concluded that the surface interactionbetween Au and CeO
2was the most important factor for
the catalytic activity Li et al reported T50 of lt150∘C for
crystalline Cu-CeO2(5ndash8 nm) nanopowders synthesized by a
hydrothermal method [38] The formic acid-treated Co3O4-
CeO2catalysts were reported to show T
50 at 695∘C for COoxidation [39]The CO oxidation catalytic activities for otherCeO2-based catalysts were summarized elsewhere [11]
Ethanol oxidation reaction performances were fullyexamined for all M doped (M=Ag Au Pd andNi) andMM1015840codoped CeO
2NPs by UV-visible absorption spectroscopy
Figure 7 shows the UV-Vis absorption spectra of the ethanolsolutions reacted at 80∘C for 5 days with and without cat-alysts and with different metal-doping concentration statesTwo broad absorption peaks were commonly observed ataround 220 and 280 nm which were tentatively attributedto ethyl acetate (CH
3COOCH
2CH3 EA) and acetaldehyde
(CH3CHO AcA) respectively for the oxidation products
of ethanol Further details were discussed below The EApeak became stronger and increased more sharply than theAcA peak with reaction time The AcA absorption peakintensity increased slightly gradually reaching a certain lowconcentration levelThe presence of EA as amajor andAcA asaminor productwas further confirmedbymass spectrometry(or UV-visible absorption) as discussed in detail belowTo examine the temperature effect we conducted ethanoloxidation experiments at 40∘C and 80∘C As expected theabsorbance of the two peaks was dramatically enhanced upon
6 Journal of Chemistry
1st run
CeO2
Ag = 5molAu = 5mol
Temperature (∘C)700600500400300200100
00
20
40
60
80
100CO
conv
ersio
n (
)
1 mol 4 mol25 mol 25 mol
4 mol 1molDoped Ag Au
(a)
2nd run
Temperature (∘C)700600500400300200100
00
20
40
60
80
100
CO co
nver
sion
()
CeO2
Ag = 5molAu = 5mol1 mol 4 mol25 mol 25 mol
4 mol 1molDoped Ag Au
(b)
1st run2nd run
Au=
5mol
14m
ol
25
25m
ol
41m
ol
Ag
=5m
ol
0
minus50
minus100
minus150
T10
(MC
eO2)
minusT
10(b
are)
(c)
Au = 5 mol
14 mol
2525 mol
41 mol
Ag = 5mol
T10
(2nd
)minusT
10
minus100
minus50
0
50
100
(1st)
(d)
Au = 5 mol14 mol2525 mol41 molAg = 5molCeO2
bf C
O o
xaf
CO
ox
(e)
Figure 6 1st (a) and 2nd (b) run temperature programmed CO oxidation conversion () profiles (a b) of undoped CeO2and Au and Ag
doped and codoped (50 05 41 2525 and 14mol) CeO2catalysts The difference (c) in T
10 between the metal doped and bare CeO2
for the 1st and 2nd runs The difference (d) in T10 between the 1st and 2nd runs for the metal doped CeO
2catalysts Optical microscope
images showed the color of the powder samples before and after CO oxidation reactions
Journal of Chemistry 7
Rxn in 5 daysat 80∘C
Wavelength (nm)350300250
Wavelength (nm)
350300250Wavelength (nm)
350300250
Doped Ag AuAb
sorb
ance
(arb
uni
t)
10
05
00
15
00
01
02
03
04
Abso
rban
ce (a
rb u
nit)
0
1
2
3
4
5
Abso
rban
ce (a
rb u
nit)
With reaction timeat 80
∘C5 days4 days3 days2 days1 day (24h)8 h4hAu-(5mol) CeO2
Au = 5molNo catalyst
Ag = 5 molCeO21 mol 4 mol
25 mol 25 mol
4 mol 1 mol
O
O
O
(a)
O
O
O
Au = 5mol
Rxn in 5 daysat 80∘C
at 80∘C
0
1
2
3
4
5
Abso
rban
ce (a
rb u
nit)
Wavelength (nm)350300250
Wavelength (nm)
350300250
Doped Ni Au
Rxn in 24 hrs
Abso
rban
ce (a
rb u
nit)
10
05
00
15
1 mol 4 mol25 mol 25 mol
Ni = 5 mol4 mol 1 mol
(b)
O
O
O
Au = 5mol
Rxn in 5 daysat 80∘C
at 80∘C
0
1
2
3
4
5
Abso
rban
ce (a
rb u
nit)
Wavelength (nm)350300250
Wavelength (nm)
350300250
Doped Pd Au
Rxn in 24 hrs
Abso
rban
ce (a
rb u
nit)
10
05
00
15
1 mol 4 mol25 mol 25 mol
Pd = 5 mol4 mol 1 mol
(c)
O
O
O
Au = 5mol
Rxn in 5 daysat 80∘C
at 80∘C
Wavelength (nm)350300250
Wavelength (nm)
350300250
Doped Ni Pd
Rxn in 24 hrs
Abso
rban
ce (a
rb u
nit)
10
05
00
15
0
1
2
3
4
5
Abso
rban
ce (a
rb u
nit)
1 mol 4 mol25 mol 25 mol
Pd = 5 molNi = 5 mol
4 mol 1 mol
(d)
Figure 7 UV-visible absorption spectra of the ethanol oxidation with no catalyst undoped CeO2 M doped (M = Ag Au Pd and Ni) and
MM1015840 codoped (AgAu (a) NiAu (b) PdAu (c) and NiPd (d)) CeO2catalysts at 80∘C for 5 days The left inset in (a) shows the magnified
spectra of the grey shadowed region The right inset in (a) shows the UV-Vis absorption spectra of ethanol oxidation with the 5mol Audoped CeO
2catalyst at 80∘C according to the reaction time
increasing reaction temperatureWithout catalysts no signif-icant ethanol oxidation occurred even at high temperatureFor further ethanol oxidation experiments we selected areaction temperature of 80∘C and a total metal-doping levelof 5mol
For Ag and Au doped and codoped samples (Figure 7(a))a strong absorption peak (below 250 nm) was observed forthe Au (5mol) and AuAg (14mol) doped CeO
2cata-
lysts Without a catalyst no significant absorption peak was
observed even after 5 days The absorption peak (shown inthe right inset of Figure 7(a)) increased with increasingreaction time This was attributed to an increase in reactionproducts that contain C=C andor C=O functional groupsFor the other metal doped samples the absorption peakswere much weaker In addition to the strong absorptionpeak a weaker peak at 280 nm was also observed (in theleft inset of Figure 7) The results suggest that at least tworeaction products (EA and AcA as mentioned above) were
8 Journal of Chemistry
present in the ethanol solution The catalytic activity wasobserved to be in the order of bare CeO
2asymp 2525 lt 41 lt
50 ≪ 14 lt 05 (AgAumol) When the concentration ofAu was the same as or lower than that of Ag the activitydeteriorated drastically For Au and Ni doped and codopedsamples (Figure 7(b)) the catalytic activity was decreasedupon adding Ni as a cocatalyst The activity was found to bein the order of 50 lt 41≪ 2525 lt 14 lt 05 (NiAumol)For Au and Pd doped and codoped samples (Figure 7(c))the oxidation performance was more greatly decreased uponadding Pd as a cocatalyst and found to be in the order of 41 le2525asymp 14asymp 50≪ 05 (PdAumol) ForNi and Pd dopedand codoped samples (Figure 7(d)) the catalytic activity wasobserved to be in the order of 50 lt 05≪ 41 asymp 14 le 2525(NiPdmol) The catalytic activity of the NiPd codopedsamples showed much higher catalytic activity than those ofthe single M- (Ni and Pd) doped samples For comparisonof the catalytic activities of single M doped CeO
2NPs the
ethanol oxidation performance showed an order of undopedasympNi ltAg lt Pd≪Au Interestingly the Ni-doping showed noincrease in catalytic activity for ethanol oxidation
For ethanol oxidation on a metal doped CeO2power
sample since the reaction mechanism was much more com-plicated than expected on a single crystal surface we proposethe following simplified mechanisms which are discussed ingreater detail below [32]
Acetaldehyde hemiacetal and ethyl acetate formationfrom ethanol is as follows
CH3CH2OndashH 997888rarr CH
3CH2O (ad) +H (ad) (1)
CH3CH2O (ad) +O species
997888rarr CH3CHO (ad) +OH (ad)
(2)
CH3CH2O (ad) ndashM
997888rarr CH3CHO (minor) +MH hydride shift
(3)
CH3CHO +O (ad) 997888rarr CH
3COO (ad) +H (ad)
997888rarr CH3COOH
(4)
CH3COOH (ad) + CH3CH2OH (ad)
997888rarr CH3COOCH
2CH3+H2O
(5)
2CH3CHO (ad) 997888rarr CH
3COOCH
2CH3 (6)
CH3CHO (ad) + CH3CH2OH (ad)
997888rarr CH3CH (OH)OC
2H5 (hemiacetal)
997888rarr CH3COOCH
2CH3(major) +H
2
(7)
The rate constant for each step is controlled by the surfacearea and metal-support interaction (or surface activity) Inreaction (1) the OndashH bond of ethanol dissociates to formCH3CH2O which may be mainly adsorbed onto the doped
metal siteThis then turns into adsorbedCH3CHOvia nearby
active oxygen species in (2) or the adsorbed CH3CH2O on
metal desorbs as CH3CHO (acetaldehyde) in response to a
hydride shift reaction in (3) [32 40] Although we have nodirect evidence of the hydride shift reaction the reactionprocess is highly plausible The acetaldehyde in (4) furtherprecedes oxidation reactions to form CH
3COOH (acetic
acid) if active oxygen species are available nearby Otherwisethe CH
3COOH with ethanol in (5) and 2CH
3CHO in (6)
react to form CH3COOCH
2CH3(ethyl acetate) In reaction
(7) CH3CHO and ethanol formCH
3CH(OH)OC
2H5(hemi-
acetal) which is converted to ethyl acetate Consequentlyethyl acetate (CH
3COOCH
2CH3) is formed as a final oxi-
dation product which was confirmed by mass spectrometryIn the present UV-Vis spectra two products of ethyl acetate(major) and acetaldehyde (minor) were observed For alcoholoxidation on the Au-CeO
2catalyst Maldotti et al reported
that the Au-H species is an important intermediate [32] Thisindicates that the hydride shift reaction is facilitated by activedopedmetalsThe present study showed that the Au-rich cat-alyst produced much higher oxidation products and the Auspecies is more active than other metal species (Ag Ni andPd)The reference UV-Vis spectra (Figure 8(a)) were checkedfor four plausible ethanol oxidation products acetaldehydeethyl acetate acetone and acetic acid and the stronger andweaker peak positions near 220 and 280 nm were assignedto the UV-Vis absorptions of ethyl acetate and acetaldehyderespectively Figure 8(b) displays the mass spectrum of thesolution sample after reaction relative to those of the referencesolvents (ethyl acetate and ethanol) As shown in the massspectrum the oxidation product in ethanol matched thatof the reference ethyl acetate well In addition the smell ofthe two samples was very similar As a result we concludedthat the final major product was ethyl acetate For someother extra mass fragmentation signals (59 73 and 75 amu)although no reference data were available the fragmentationsappeared to form from the hemiacetal as shown in reaction(7) Abad et al extensively studied oxidation of alcoholscatalyzed by AuCeO
2[40] and proposed a reaction of (7)
mentioned above in which hemiacetal was detected by H-NMR We have excluded diethyl ether as a major producteven though it could be formed by 2C
2H5OHrarrC
2H5OC2H5
+ H2O because the UV-visible absorption intensity (even
measuredwith 50 solution) was extremely low (Figure 8(a))when compared with that of the sample We also detected nofragmentation signals of diethyl ether by mass spectrometryThe acetone formation reaction 2CH
3CHOrarr CH
3COCH
3
(acetone) + CO2+ H2 was excluded due to absence of the
mass signal Acetic acid as a major product was also excludedbecause the solution is not acidic the mass signal is absentand it did not smell like acetic acid Table 1 summarizes thesizes of the metal-loaded CeO
2estimated using Scherrerrsquos
equation As for the CO oxidation the ethanol oxidationactivity was also found to be more loaded metal (and therelative concentrations) dependent than the size-dependent
4 Conclusion
To increase the catalytic activity of bare CeO2 the CeO
2
matrix was doped and codoped with Ag Au Pd and Ni bya hydrothermal method The novelty of the present study
Journal of Chemistry 9
Table 1 Particles sizes of the metal-loaded CeO2estimated using Scherrerrsquos equation
Loaded MM1015840 50mol (nm) 41mol (nm) 2525mol (nm) 14mol (nm) 05mol (nm)Ag Au 140 124 80 100 86Ni Au 152 123 106 82 86Pd Au 151 127 121 90 86Ni Pd 152 111 147 121 151
Catalysts without stirring
Tightly capped
OOH
O
O
O
lowast
lowast
O
OH
OHO
OO
Abso
rban
ce
10
05
00
Diethyl ether 50
Different smellAcetaldehyde sim1
Acetone sim1
Different smellAcetic acid 01
Ethyl acetate 01
Wavelength (nm)400350300250
(a)
Ethyl acetate(reference)
O
O
Mass (amu)1009080706050M
ass s
igna
l (au
)
OH Before reaction(ETOH)
50 60
Mass (amu)70 80 90 100M
ass s
igna
l (au
)
Afterreaction
01234
UV-VisO
O
Mass (amu)1009080706050M
ass s
igna
l (au
)
Abso
rban
ce
250 300Wavelength (nm)
(b)
Figure 8 UV-Vis absorption spectra (a) of standard samples of acetaldehyde (1) acetone (1) acetic acid (01) and ethyl acetate (01)Mass spectra (b) of reference samples (ethyl acetate and ethanol) and the solution sample after reactionThe inset shows theUV-Vis absorptionspectrum of the corresponding sample solution Blue and red lowast indicate the peak positions for acetaldehyde and ethyl acetate respectively
was that the catalytic efficiency of doped and codoped CeO2
was tested for both gas-phase CO and liquid-phase ethanoloxidation reactions For the 1st and 2nd runs of bare CeO
2
T10 was observed at 405∘C T
10 of bare CeO2for CO oxi-
dation was lowered significantly by 165∘C uponmetal (AgAu= 14mol) doping There were some synergic effects uponcodoping for the CO oxidation The CO oxidation activityvaries with the relative concentrations of two differentmetalsSintering and alloying of two different metals were found toplay important roles in the CO oxidation activity
For liquid-phase ethanol oxidation two liquid productsof ethyl acetate (major 120582max = 220 nm) and acetaldehyde(minor 120582max = 280 nm) were observed by UV-Vis absorptionspectroscopyThe concentration of acetaldehyde (CH
3CHO)
reached a saturation point while that of ethyl acetate(CH3COOCH
2CH3) dramatically increased with reaction
time These findings indicate that acetaldehyde speciespromptly undergo further reaction to form a major productethyl acetate whichwas confirmed bymass spectrometry andUV-visible absorption Undoped CeO
2produces negligible
acetaldehyde which is direct evidence that a hydride shiftreaction CH
3CH2O(ad)-MrarrCH
2CHO+MH is an impor-
tant step for acetaldehyde production for metal-loaded CeO2
catalysts For M- (single) doped CeO2NPs the ethanol
oxidation performance showed an order of Ni lt Ag lt Pd ≪Au For MM1015840 codoped CeO
2NPs the activity of Au doped
CeO2deteriorated drastically upon adding another metals
(Ag Ni and Pd) as cocatalyst The Au-rich CeO2catalyst
showed higher catalytic activity On the other hand the NiPd codoped sample showed much higher catalytic activitycompared with the single M- (Ni and Pd) doped samplesThis study provides further insights into the development ofcatalysts applicable to a range of oxidation reactions
Competing Interests
The authors declare no conflict of interests
Acknowledgments
This study was supported by the 2015 Yeungnam UniversityResearch Grant
References
[1] X Nie H Qian Q Ge H Xu and R Jin ldquoCO oxidationcatalyzed by oxide-supported Au
25(SR)18
nanoclusters and
10 Journal of Chemistry
identification of perimeter sites as active centersrdquo ACS Nanovol 6 no 7 pp 6014ndash6022 2012
[2] H-F Li N Zhang P Chen M-F Luo and J-Q Lu ldquoHigh sur-face area AuCeO
2catalysts for low temperature formaldehyde
oxidationrdquoApplied Catalysis B Environmental vol 110 pp 279ndash285 2011
[3] K Y Ho and K L Yeung ldquoEffects of ozone pretreatment on theperformance of AuTiO
2catalyst for CO oxidation reactionrdquo
Journal of Catalysis vol 242 no 1 pp 131ndash141 2006[4] K Y Ho and K L Yeung ldquoProperties of TiO
2support and the
performance of AuTiO2catalyst for CO oxidation reactionrdquo
Gold Bulletin vol 40 no 1 pp 15ndash30 2007[5] J Qi J Chen G Li S Li Y Gao and Z Tang ldquoFacile
synthesis of core-shell AuCeO2nanocomposites with remark-
ably enhanced catalytic activity for CO oxidationrdquo Energy andEnvironmental Science vol 5 no 10 pp 8937ndash8941 2012
[6] D Jiang W Wang L Zhang Y Zheng and Z Wang ldquoInsightsinto the surface-defect dependence of photoreactivity overCeO2nanocrystals with well-defined crystal facetsrdquo ACS Catal-
ysis vol 5 no 8 pp 4851ndash4858 2015[7] W Lei T Zhang L Gu et al ldquoSurface-structure sensitivity
of CeO2nanocrystals in photocatalysis and enhancing the
reactivity with nanogoldrdquo ACS Catalysis vol 5 no 7 pp 4385ndash4393 2015
[8] B Li T Gu T Ming J Wang P Wang and J C Yu ldquoGoldcore)(ceria shell) nanostructures for plasmon-enhanced cat-alytic reactions under visible lightrdquo ACS Nano vol 8 no 8 pp8152ndash8162 2014
[9] P Lu B Qiao N Lu et al ldquoPhotochemical deposition of highlydispersed Pt nanoparticles on porous CeO
2nanofibers for the
water-gas shift reactionrdquoAdvanced FunctionalMaterials vol 25no 26 pp 4153ndash4162 2015
[10] L Meng A-P Jia J-Q Lu L-F Luo W-X Huang and M-FLuo ldquoSynergetic effects of PdO species on CO oxidation overPdO-CeO
2catalystsrdquo Journal of Physical Chemistry C vol 115
no 40 pp 19789ndash19796 2011[11] Y Park S K Kim D Pradhan and Y Sohn ldquoThermal H
2-
treatment effects on COCO2conversion over Pd-doped CeO
2
comparison with Au and Ag-doped CeO2rdquo Reaction Kinetics
Mechanisms and Catalysis vol 113 no 1 pp 85ndash100 2014[12] Y Park S K Kim D Pradhan and Y Sohn ldquoSurface treatment
effects on CO oxidation reactions over Co Cu and Ni-dopedand codopedCeO
2catalystsrdquoChemical Engineering Journal vol
250 pp 25ndash34 2014[13] B Xu Q Zhang S YuanM Zhang and T Ohno ldquoMorphology
control and photocatalytic characterization of yttrium-dopedhedgehog-like CeO
2rdquo Applied Catalysis B Environmental vol
164 pp 120ndash127 2015[14] W Huang and Y Gao ldquoMorphology-dependent surface chem-
istry and catalysis of CeO2nanocrystalsrdquo Catalysis Science and
Technology vol 4 no 11 pp 3772ndash3784 2014[15] Y Gao W Wang S Chang and W Huang ldquoMorphology
effect of CeO2support in the preparation metal-support
interaction and catalytic performance of PtCeO2catalystsrdquo
ChemCatChem vol 5 no 12 pp 3610ndash3620 2013[16] Y Zhang N Zhang Z-R Tang and Y-J Xu ldquoA unique
silk mat-like structured PdCeO2as an efficient visible light
photocatalyst for green organic transformation in waterrdquo ACSSustainable Chemistry amp Engineering vol 1 no 10 pp 1258ndash1266 2013
[17] W G Shin H J Jung H G Sung H S Hyun and YSohn ldquoSynergic CO oxidation activities of boron-CeO
2hybrid
materials prepared by dry and wet milling methodsrdquo CeramicsInternational vol 40 no 8 pp 11511ndash11517 2014
[18] H Wu P Wang H He and Y Jin ldquoControlled synthesisof porous AgAu bimetallic hollow nanoshells with tunableplasmonic and catalytic propertiesrdquo Nano Research vol 5 no2 pp 135ndash144 2012
[19] N Sasirekha P Sangeetha and Y-W Chen ldquoBimetallic AundashAgCeO
2catalysts for preferential oxidation ofCO inhydrogen-
rich stream effect of calcination temperaturerdquo The Journal ofPhysical Chemistry C vol 118 no 28 pp 15226ndash15233 2014
[20] S Chen L Luo Z Jiang and W Huang ldquoSize-dependent reac-tion pathways of low-temperature CO oxidation on AuCeO
2
catalystsrdquo ACS Catalysis vol 5 no 3 pp 1653ndash1662 2015[21] D LiuW Li X Feng andY Zhang ldquoGalvanic replacement syn-
thesis of Ag119909Au1minus119909
CeO2(0 le x le 1) coreshell nanospheres
with greatly enhanced catalytic performancerdquoChemical Sciencevol 6 pp 7015ndash7019 2015
[22] Y Kang M Sun and A Li ldquoStudies of the catalytic oxidationof CO over AgCeO
2catalystrdquo Catalysis Letters vol 142 no 12
pp 1498ndash1504 2012[23] S Chang M Li Q Hua et al ldquoShape-dependent inter-
play between oxygen vacancies and AgndashCeO2interaction in
AgCeO2catalysts and their influence on the catalytic activityrdquo
Journal of Catalysis vol 293 pp 195ndash204 2012[24] R Fiorenza C Crisafulli G G Condorelli F Lupo and S Scire
ldquoAu-AgCeO2and Au-CuCeO
2Catalysts for volatile organic
compounds oxidation and CO preferential oxidationrdquo CatalysisLetters vol 145 no 9 pp 1691ndash1702 2015
[25] J Zhang L Li X Huang and G Li ldquoFabrication of AgndashCeO2
core-shell nanospheres with enhanced catalytic performancedue to strengthening of the interfacial interactionsrdquo Journal ofMaterials Chemistry vol 22 no 21 pp 10480ndash10487 2012
[26] A Leyva-Perez D Combita-Merchan J R Cabrero-AntoninoS I Al-Resayes and A Corma ldquoOxyhalogenation of activatedarenes with nanocrystalline ceriardquo ACS Catalysis vol 3 no 2pp 250ndash258 2013
[27] Y Liu H Li J Yu DMao andG Lu ldquoElectronic storage capac-ity of ceria role of peroxide inAux supported onCeO
2(111) facet
and CO adsorptionrdquo Physical Chemistry Chemical Physics vol17 no 41 pp 27758ndash27768 2015
[28] D Jiang WWang S Sun L Zhang and Y Zheng ldquoEquilibrat-ing the plasmonic and catalytic roles of metallic nanostructuresin photocatalytic oxidation over Au-modified CeO
2rdquo ACS
Catalysis vol 5 no 2 pp 613ndash621 2015[29] M M Khan S A Ansari M O Ansari B K Min J Lee and
M H Cho ldquoBiogenic fabrication of AuCeO2nanocomposite
with enhanced visible light activityrdquo Journal of Physical Chem-istry C vol 118 no 18 pp 9477ndash9484 2014
[30] A Tanaka K Hashimoto and H Kominami ldquoPreparation ofAuCeO
2exhibiting strong surface plasmon resonance effective
for selective or chemoselective oxidation of alcohols to alde-hydes or ketones in aqueous suspensions under irradiation bygreen lightrdquo Journal of the American Chemical Society vol 134no 35 pp 14526ndash14533 2012
[31] H Y Kim H M Lee and G Henkelman ldquoCO oxidationmechanism on CeO
2-supported Au nanoparticlesrdquo Journal of
the American Chemical Society vol 134 no 3 pp 1560ndash15702012
[32] A Maldotti A Molinari R Juarez and H Garcia ldquoPhotoin-duced reactivity of AundashH intermediates in alcohol oxidation by
Journal of Chemistry 11
gold nanoparticles supported on ceriardquoChemical Science vol 2no 9 pp 1831ndash1834 2011
[33] L Vivier andDDuprez ldquoCeria-based solid catalysts for organicchemistryrdquo ChemSusChem vol 3 no 6 pp 654ndash678 2010
[34] N Zhang S Liu X Fu and Y-J Xu ldquoA simple strategy forfabrication of ldquoplum-puddingrdquo type PdCeO
2semiconductor
nanocomposite as a visible-light-driven photocatalyst for selec-tive oxidationrdquo Journal of Physical Chemistry C vol 115 no 46pp 22901ndash22909 2011
[35] Y Sohn ldquoSiO2nanospheres modified by Ag nanoparticles sur-
face charging and CO oxidation activityrdquo Journal of MolecularCatalysis A Chemical vol 379 pp 59ndash67 2013
[36] W J Kim D Pradhan and Y Sohn ldquoFundamental natureand CO oxidation activities of indium oxide nanostructures1D-wires 2D-plates and 3D-cubes and donutsrdquo Journal ofMaterials Chemistry A vol 1 no 35 pp 10193ndash10202 2013
[37] R-R Zhang L-H Ren A-H Lu and W-C Li ldquoInfluence ofpretreatment atmospheres on the activity of AuCeO
2catalyst
for low-temperature CO oxidationrdquo Catalysis Communicationsvol 13 no 1 pp 18ndash21 2011
[38] Y Li Y Cai X Xing N Chen D Deng and YWang ldquoCatalyticactivity for CO oxidation of CundashCeO
2composite nanoparticles
synthesized by a hydrothermal methodrdquo Analytical Methodsvol 7 no 7 pp 3238ndash3245 2015
[39] R Shang Y Duan X Zhong W Xie Y Luo and L HuangldquoFormic acid modified Co
3O4-CeO
2catalysts for CO oxida-
tionrdquo Catalysts vol 6 no 3 p 48 2016[40] A Abad P Concepcion A Corma and H Garcıa ldquoA collab-
orative effect between gold and a support induces the selectiveoxidation of alcoholsrdquo Angewandte ChemiemdashInternational Edi-tion vol 44 no 26 pp 4066ndash4069 2005
Submit your manuscripts athttpwwwhindawicom
Hindawi Publishing Corporationhttpwwwhindawicom Volume 2014
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CatalystsJournal of
4 Journal of Chemistry
Abso
rban
ce (a
rb u
nit)
CeO2Ag = 5mol
Au = 5mol
Wavelength (nm)800600400200
1mol 4mol25 mol 25 mol
4mol 1mol
Doped Ag Au
Figure 3 UV-visible diffuse reflectance spectra (expressed in termsof KubelkandashMunk absorbance arbitrary unit) of undoped CeO
2and
Au and Ag doped and codoped (50 05 41 2525 and 14mol)CeO2catalysts Optical microscopy images (inset) show the colors
of the corresponding samples
observed at 2120579 = 381∘ 443∘ and 646∘ corresponding tothe (111) (002) and (022) planes of cubic phase metallic Au[5] The new peaks were the most intense for the AgAu(14mol) doped sample which was attributed to the highercrystallinity No Ag peaks were observed indicating well-dispersed small amorphous states
TheUV-Vis diffuse reflectance characteristics of themetaldoped samples were examined to determine the metal-doping states as shown in Figure 3 For undoped CeO
2
no significant visible light absorption was observed and theabsorption edge was positioned at sim29 eV Upon metal-doping the absorption in the visible region was increasedsignificantly For Ag (5mol) doped CeO
2 the color of the
powder sample became yellow The color became reddish asthe amount of Au was increased and the UV-Vis absorp-tion in the visible region also increased For Au (5mol)doped CeO
2 a broad absorption peak was observed at
approximately 530 nm which was attributed to the surfaceplasmon resonance absorption of Au nanoparticles [30] Forthe AgAu (41 2525 and 14mol) doped samples theabsorption in the longer wavelength region was attributed tothe formation of larger particles
Figure 4 presents the FT-IR spectra of undopedCeO2and
Au and Ag doped and codoped (50 05 41 2525 and 14mol) CeO
2nanoparticles A broad peak was commonly
observed at 3400 cmminus1 which was attributed to the adsorbedsurface OH andor H
2O species The maximum of the broad
peak was shifted to a shorter wavenumber with increasing theamount of Au The complicated vibrational peaks observed
Tran
smitt
ance
(arb
uni
t)
CeO2
Ag = 5mol
Au = 5mol
Wavenumber (cmminus1)1000200030004000
Doped Ag Au
1mol 4mol
25 mol 25 mol
4mol 1mol
Figure 4 FT-IR spectra of undoped CeO2and Au and Ag doped
and codoped (50 05 41 2525 and 14mol) CeO2
H2
cons
umpt
ion
(arb
uni
t)
CeO2
Au = 5mol
H2-TPR
100800600400200
Temperature (∘C)
1mol 4mol
25 mol 25 mol
4mol 1mol
Doped Ag Au
Ag = 5mol
Figure 5 TPR profiles of undoped CeO2and Au and Ag doped and
codoped (50 05 41 2525 and 14mol) CeO2catalysts
between 1300 and 1800 cmminus1 were assigned to C=O C=C andCOO- functional groups [5] which were dependent on thesample states
Figure 5 shows the temperature programmed hydrogenreduction (TPR) profiles of the bare and metal doped CeO
2
catalysts For bare CeO2 two broad peaks were observed at
around 550 and 900∘C The higher temperature peak wasattributed to the reduction of bulk oxygen of CeO
2 The
lower temperature peak was assigned to the reduction ofsurface oxygen The reduction peak for bulk oxygen is
Journal of Chemistry 5
commonly observed for metal doped CeO2 but at a lower
temperature (by sim50∘C) In addition the strong peaks newlyappeared below 400∘C for the metal doped CeO
2 The peak
intensityposition and broadness were dependent on theinteractions between the dopedmetal and the lattice of CeO
2
Because doped Ag and Au are present as the metallic statethe doped metallic nanoparticles could cause the spillover oflattice oxygen by forming AundashOndashCe state to result in easyreduction [19 24] Ce3+ can be formed from Ce4+ by formingAundashO bond and charge transfer from Au to Ce [27] For Au(5mol) doped CeO
2 the lower TPR peak was observed at
approximately 300∘C For AgAu (14 and 2525mol)doped CeO
2 the peak was observed at a somewhat
higher temperature with different intensities For AgAu(41 and 50mol) doped CeO
2 the peak was observed
at lower temperatures indicating stronger interactions withCeO2
Figure 6 presents the 1st and 2nd run CO oxidationconversion profiles for undoped CeO
2and Au and Ag
doped and codoped (50 05 41 2525 and 14mol)CeO2catalysts The CO conversion () was calculated using
([CO]inndash[CO]out)[CO]in times 100 [35 36] T10 is definedas the temperature corresponding to CO conversion of 10As seen in the spectra the CO oxidation onset position wasdramatically different in all samples For the 1st and 2nd runsof bare CeO
2 T10 was observed at 405∘C Upon metal-
dopingT10 was lowered dramatically In the 1st runT
10 ofthe 5mol Au and Ag doped samples was observed at240∘C and 352∘C respectively Compared to that of bareCeO2 T10 was lowered by 165∘C and 53∘C respectively
(bottom left of Figure 6) As the amount of Au was increasedT10 was observed at a lower temperature The order of
catalytic activity was found to be bare CeO2lt AgAu
(50mol) lt AgAu (41mol) lt AgAu (2525mol)lt AgAu (14mol) lt AgAu (05mol) In the 2nd runT10 was drastically changed for the metal doped samples
T10 of the 5mol Au and Ag doped samples was observed
at 295∘C and 262∘C respectively The Au doped sampleshowed a 55∘C increase in T
10 while Ag doped sampleshowed a 90∘C decrease in T
10 The order of the catalyticactivity was bare CeO
2lt AgAu (2525mol) lt AgAu
(05mol) asymp AgAu (41mol) lt AgAu (50mol) ltAgAu (14mol)The AgAu (14mol) showed the high-est activity Compared to T
10 in the 1st run the AgAu(50mol) and AgAu (14mol) samples showed a lowerT10 while other samples showed a higher T
10 in the 2ndrun as shown in the bottom right of Figure 6 In the 2nd runboth the sintering of Au nanoparticles and alloying of twodifferent metals were expected to play a role in determiningthe activity because the sample had already experienced ahigh temperature up to 700∘C The colors of the sampleswere significantly changed after the CO oxidation reactionsParticularly the colors of the AgAu (41mol) AgAu(2525mol) andAgAu (05mol) became dark grey (orblack) after the CO oxidation unlike other three samplesThe corresponding catalysts showed catalyst deactivation inthe 2nd run compared with the 1st run (Figure 6(d)) Thisindicates that change in oxidation state carbon residues
after reaction and sinteringalloying of loaded metals areimportant factors for the determination of catalytic activitySasirekha et al examined CO oxidation under hydrogen-rich conditions for Au and Ag doped and codoped CeO
2
catalysts and reported that the Ag-Ag (5 5) doped sampleshowed the highest CO conversion and selectivity [19] Theenhancement was attributed to bimetallic alloy formation[19 24] On the other hand in the present study the AgAu(2525mol) sample showed the poorest activity amongthe metal doped samples in the 2nd run This suggests thatother factors (eg size and relative distributions) are alsoimportant for determining the activity CO oxidation hascommonly been understood by CO(ad) + [O]lowast rarr CO
2(g)
where [O]lowast is the active surface oxygen The surface oxygenis replenished by molecular oxygen present in air AdsorbedCO is plausibly present at the interface of doped metal andCeO2 on top of metal andor defect sites [31]The crystalline
size (reflecting the surface area) of the samples was estimatedusing the full width at half maximum of the (111) peak andScherrerrsquos equation [12] The order of the size was found tobe AgAu (2525mol) 80 nm lt AgAu (05mol)86 nm lt AgAu (14mol) 100 nm lt AgAu (41mol)124 nm lt bare CeO
2 130 nm lt AgAu (50mol) and
140 nm Based on this the size was not linearly related withthe catalytic activity For this reason the metal-loading isimportant and themetal-support interactions play significantroles in the catalytic activity [37] In the present study T
50for all the samples was observed to be gt300∘C Zhang et alreported significantly lower T
50 for AuCeO2prepared by a
deposition-precipitation method [37] They reported T50 of
63 35 and 17∘C for untreatedH2 andH
2-O2treated samples
respectively They concluded that the surface interactionbetween Au and CeO
2was the most important factor for
the catalytic activity Li et al reported T50 of lt150∘C for
crystalline Cu-CeO2(5ndash8 nm) nanopowders synthesized by a
hydrothermal method [38] The formic acid-treated Co3O4-
CeO2catalysts were reported to show T
50 at 695∘C for COoxidation [39]The CO oxidation catalytic activities for otherCeO2-based catalysts were summarized elsewhere [11]
Ethanol oxidation reaction performances were fullyexamined for all M doped (M=Ag Au Pd andNi) andMM1015840codoped CeO
2NPs by UV-visible absorption spectroscopy
Figure 7 shows the UV-Vis absorption spectra of the ethanolsolutions reacted at 80∘C for 5 days with and without cat-alysts and with different metal-doping concentration statesTwo broad absorption peaks were commonly observed ataround 220 and 280 nm which were tentatively attributedto ethyl acetate (CH
3COOCH
2CH3 EA) and acetaldehyde
(CH3CHO AcA) respectively for the oxidation products
of ethanol Further details were discussed below The EApeak became stronger and increased more sharply than theAcA peak with reaction time The AcA absorption peakintensity increased slightly gradually reaching a certain lowconcentration levelThe presence of EA as amajor andAcA asaminor productwas further confirmedbymass spectrometry(or UV-visible absorption) as discussed in detail belowTo examine the temperature effect we conducted ethanoloxidation experiments at 40∘C and 80∘C As expected theabsorbance of the two peaks was dramatically enhanced upon
6 Journal of Chemistry
1st run
CeO2
Ag = 5molAu = 5mol
Temperature (∘C)700600500400300200100
00
20
40
60
80
100CO
conv
ersio
n (
)
1 mol 4 mol25 mol 25 mol
4 mol 1molDoped Ag Au
(a)
2nd run
Temperature (∘C)700600500400300200100
00
20
40
60
80
100
CO co
nver
sion
()
CeO2
Ag = 5molAu = 5mol1 mol 4 mol25 mol 25 mol
4 mol 1molDoped Ag Au
(b)
1st run2nd run
Au=
5mol
14m
ol
25
25m
ol
41m
ol
Ag
=5m
ol
0
minus50
minus100
minus150
T10
(MC
eO2)
minusT
10(b
are)
(c)
Au = 5 mol
14 mol
2525 mol
41 mol
Ag = 5mol
T10
(2nd
)minusT
10
minus100
minus50
0
50
100
(1st)
(d)
Au = 5 mol14 mol2525 mol41 molAg = 5molCeO2
bf C
O o
xaf
CO
ox
(e)
Figure 6 1st (a) and 2nd (b) run temperature programmed CO oxidation conversion () profiles (a b) of undoped CeO2and Au and Ag
doped and codoped (50 05 41 2525 and 14mol) CeO2catalysts The difference (c) in T
10 between the metal doped and bare CeO2
for the 1st and 2nd runs The difference (d) in T10 between the 1st and 2nd runs for the metal doped CeO
2catalysts Optical microscope
images showed the color of the powder samples before and after CO oxidation reactions
Journal of Chemistry 7
Rxn in 5 daysat 80∘C
Wavelength (nm)350300250
Wavelength (nm)
350300250Wavelength (nm)
350300250
Doped Ag AuAb
sorb
ance
(arb
uni
t)
10
05
00
15
00
01
02
03
04
Abso
rban
ce (a
rb u
nit)
0
1
2
3
4
5
Abso
rban
ce (a
rb u
nit)
With reaction timeat 80
∘C5 days4 days3 days2 days1 day (24h)8 h4hAu-(5mol) CeO2
Au = 5molNo catalyst
Ag = 5 molCeO21 mol 4 mol
25 mol 25 mol
4 mol 1 mol
O
O
O
(a)
O
O
O
Au = 5mol
Rxn in 5 daysat 80∘C
at 80∘C
0
1
2
3
4
5
Abso
rban
ce (a
rb u
nit)
Wavelength (nm)350300250
Wavelength (nm)
350300250
Doped Ni Au
Rxn in 24 hrs
Abso
rban
ce (a
rb u
nit)
10
05
00
15
1 mol 4 mol25 mol 25 mol
Ni = 5 mol4 mol 1 mol
(b)
O
O
O
Au = 5mol
Rxn in 5 daysat 80∘C
at 80∘C
0
1
2
3
4
5
Abso
rban
ce (a
rb u
nit)
Wavelength (nm)350300250
Wavelength (nm)
350300250
Doped Pd Au
Rxn in 24 hrs
Abso
rban
ce (a
rb u
nit)
10
05
00
15
1 mol 4 mol25 mol 25 mol
Pd = 5 mol4 mol 1 mol
(c)
O
O
O
Au = 5mol
Rxn in 5 daysat 80∘C
at 80∘C
Wavelength (nm)350300250
Wavelength (nm)
350300250
Doped Ni Pd
Rxn in 24 hrs
Abso
rban
ce (a
rb u
nit)
10
05
00
15
0
1
2
3
4
5
Abso
rban
ce (a
rb u
nit)
1 mol 4 mol25 mol 25 mol
Pd = 5 molNi = 5 mol
4 mol 1 mol
(d)
Figure 7 UV-visible absorption spectra of the ethanol oxidation with no catalyst undoped CeO2 M doped (M = Ag Au Pd and Ni) and
MM1015840 codoped (AgAu (a) NiAu (b) PdAu (c) and NiPd (d)) CeO2catalysts at 80∘C for 5 days The left inset in (a) shows the magnified
spectra of the grey shadowed region The right inset in (a) shows the UV-Vis absorption spectra of ethanol oxidation with the 5mol Audoped CeO
2catalyst at 80∘C according to the reaction time
increasing reaction temperatureWithout catalysts no signif-icant ethanol oxidation occurred even at high temperatureFor further ethanol oxidation experiments we selected areaction temperature of 80∘C and a total metal-doping levelof 5mol
For Ag and Au doped and codoped samples (Figure 7(a))a strong absorption peak (below 250 nm) was observed forthe Au (5mol) and AuAg (14mol) doped CeO
2cata-
lysts Without a catalyst no significant absorption peak was
observed even after 5 days The absorption peak (shown inthe right inset of Figure 7(a)) increased with increasingreaction time This was attributed to an increase in reactionproducts that contain C=C andor C=O functional groupsFor the other metal doped samples the absorption peakswere much weaker In addition to the strong absorptionpeak a weaker peak at 280 nm was also observed (in theleft inset of Figure 7) The results suggest that at least tworeaction products (EA and AcA as mentioned above) were
8 Journal of Chemistry
present in the ethanol solution The catalytic activity wasobserved to be in the order of bare CeO
2asymp 2525 lt 41 lt
50 ≪ 14 lt 05 (AgAumol) When the concentration ofAu was the same as or lower than that of Ag the activitydeteriorated drastically For Au and Ni doped and codopedsamples (Figure 7(b)) the catalytic activity was decreasedupon adding Ni as a cocatalyst The activity was found to bein the order of 50 lt 41≪ 2525 lt 14 lt 05 (NiAumol)For Au and Pd doped and codoped samples (Figure 7(c))the oxidation performance was more greatly decreased uponadding Pd as a cocatalyst and found to be in the order of 41 le2525asymp 14asymp 50≪ 05 (PdAumol) ForNi and Pd dopedand codoped samples (Figure 7(d)) the catalytic activity wasobserved to be in the order of 50 lt 05≪ 41 asymp 14 le 2525(NiPdmol) The catalytic activity of the NiPd codopedsamples showed much higher catalytic activity than those ofthe single M- (Ni and Pd) doped samples For comparisonof the catalytic activities of single M doped CeO
2NPs the
ethanol oxidation performance showed an order of undopedasympNi ltAg lt Pd≪Au Interestingly the Ni-doping showed noincrease in catalytic activity for ethanol oxidation
For ethanol oxidation on a metal doped CeO2power
sample since the reaction mechanism was much more com-plicated than expected on a single crystal surface we proposethe following simplified mechanisms which are discussed ingreater detail below [32]
Acetaldehyde hemiacetal and ethyl acetate formationfrom ethanol is as follows
CH3CH2OndashH 997888rarr CH
3CH2O (ad) +H (ad) (1)
CH3CH2O (ad) +O species
997888rarr CH3CHO (ad) +OH (ad)
(2)
CH3CH2O (ad) ndashM
997888rarr CH3CHO (minor) +MH hydride shift
(3)
CH3CHO +O (ad) 997888rarr CH
3COO (ad) +H (ad)
997888rarr CH3COOH
(4)
CH3COOH (ad) + CH3CH2OH (ad)
997888rarr CH3COOCH
2CH3+H2O
(5)
2CH3CHO (ad) 997888rarr CH
3COOCH
2CH3 (6)
CH3CHO (ad) + CH3CH2OH (ad)
997888rarr CH3CH (OH)OC
2H5 (hemiacetal)
997888rarr CH3COOCH
2CH3(major) +H
2
(7)
The rate constant for each step is controlled by the surfacearea and metal-support interaction (or surface activity) Inreaction (1) the OndashH bond of ethanol dissociates to formCH3CH2O which may be mainly adsorbed onto the doped
metal siteThis then turns into adsorbedCH3CHOvia nearby
active oxygen species in (2) or the adsorbed CH3CH2O on
metal desorbs as CH3CHO (acetaldehyde) in response to a
hydride shift reaction in (3) [32 40] Although we have nodirect evidence of the hydride shift reaction the reactionprocess is highly plausible The acetaldehyde in (4) furtherprecedes oxidation reactions to form CH
3COOH (acetic
acid) if active oxygen species are available nearby Otherwisethe CH
3COOH with ethanol in (5) and 2CH
3CHO in (6)
react to form CH3COOCH
2CH3(ethyl acetate) In reaction
(7) CH3CHO and ethanol formCH
3CH(OH)OC
2H5(hemi-
acetal) which is converted to ethyl acetate Consequentlyethyl acetate (CH
3COOCH
2CH3) is formed as a final oxi-
dation product which was confirmed by mass spectrometryIn the present UV-Vis spectra two products of ethyl acetate(major) and acetaldehyde (minor) were observed For alcoholoxidation on the Au-CeO
2catalyst Maldotti et al reported
that the Au-H species is an important intermediate [32] Thisindicates that the hydride shift reaction is facilitated by activedopedmetalsThe present study showed that the Au-rich cat-alyst produced much higher oxidation products and the Auspecies is more active than other metal species (Ag Ni andPd)The reference UV-Vis spectra (Figure 8(a)) were checkedfor four plausible ethanol oxidation products acetaldehydeethyl acetate acetone and acetic acid and the stronger andweaker peak positions near 220 and 280 nm were assignedto the UV-Vis absorptions of ethyl acetate and acetaldehyderespectively Figure 8(b) displays the mass spectrum of thesolution sample after reaction relative to those of the referencesolvents (ethyl acetate and ethanol) As shown in the massspectrum the oxidation product in ethanol matched thatof the reference ethyl acetate well In addition the smell ofthe two samples was very similar As a result we concludedthat the final major product was ethyl acetate For someother extra mass fragmentation signals (59 73 and 75 amu)although no reference data were available the fragmentationsappeared to form from the hemiacetal as shown in reaction(7) Abad et al extensively studied oxidation of alcoholscatalyzed by AuCeO
2[40] and proposed a reaction of (7)
mentioned above in which hemiacetal was detected by H-NMR We have excluded diethyl ether as a major producteven though it could be formed by 2C
2H5OHrarrC
2H5OC2H5
+ H2O because the UV-visible absorption intensity (even
measuredwith 50 solution) was extremely low (Figure 8(a))when compared with that of the sample We also detected nofragmentation signals of diethyl ether by mass spectrometryThe acetone formation reaction 2CH
3CHOrarr CH
3COCH
3
(acetone) + CO2+ H2 was excluded due to absence of the
mass signal Acetic acid as a major product was also excludedbecause the solution is not acidic the mass signal is absentand it did not smell like acetic acid Table 1 summarizes thesizes of the metal-loaded CeO
2estimated using Scherrerrsquos
equation As for the CO oxidation the ethanol oxidationactivity was also found to be more loaded metal (and therelative concentrations) dependent than the size-dependent
4 Conclusion
To increase the catalytic activity of bare CeO2 the CeO
2
matrix was doped and codoped with Ag Au Pd and Ni bya hydrothermal method The novelty of the present study
Journal of Chemistry 9
Table 1 Particles sizes of the metal-loaded CeO2estimated using Scherrerrsquos equation
Loaded MM1015840 50mol (nm) 41mol (nm) 2525mol (nm) 14mol (nm) 05mol (nm)Ag Au 140 124 80 100 86Ni Au 152 123 106 82 86Pd Au 151 127 121 90 86Ni Pd 152 111 147 121 151
Catalysts without stirring
Tightly capped
OOH
O
O
O
lowast
lowast
O
OH
OHO
OO
Abso
rban
ce
10
05
00
Diethyl ether 50
Different smellAcetaldehyde sim1
Acetone sim1
Different smellAcetic acid 01
Ethyl acetate 01
Wavelength (nm)400350300250
(a)
Ethyl acetate(reference)
O
O
Mass (amu)1009080706050M
ass s
igna
l (au
)
OH Before reaction(ETOH)
50 60
Mass (amu)70 80 90 100M
ass s
igna
l (au
)
Afterreaction
01234
UV-VisO
O
Mass (amu)1009080706050M
ass s
igna
l (au
)
Abso
rban
ce
250 300Wavelength (nm)
(b)
Figure 8 UV-Vis absorption spectra (a) of standard samples of acetaldehyde (1) acetone (1) acetic acid (01) and ethyl acetate (01)Mass spectra (b) of reference samples (ethyl acetate and ethanol) and the solution sample after reactionThe inset shows theUV-Vis absorptionspectrum of the corresponding sample solution Blue and red lowast indicate the peak positions for acetaldehyde and ethyl acetate respectively
was that the catalytic efficiency of doped and codoped CeO2
was tested for both gas-phase CO and liquid-phase ethanoloxidation reactions For the 1st and 2nd runs of bare CeO
2
T10 was observed at 405∘C T
10 of bare CeO2for CO oxi-
dation was lowered significantly by 165∘C uponmetal (AgAu= 14mol) doping There were some synergic effects uponcodoping for the CO oxidation The CO oxidation activityvaries with the relative concentrations of two differentmetalsSintering and alloying of two different metals were found toplay important roles in the CO oxidation activity
For liquid-phase ethanol oxidation two liquid productsof ethyl acetate (major 120582max = 220 nm) and acetaldehyde(minor 120582max = 280 nm) were observed by UV-Vis absorptionspectroscopyThe concentration of acetaldehyde (CH
3CHO)
reached a saturation point while that of ethyl acetate(CH3COOCH
2CH3) dramatically increased with reaction
time These findings indicate that acetaldehyde speciespromptly undergo further reaction to form a major productethyl acetate whichwas confirmed bymass spectrometry andUV-visible absorption Undoped CeO
2produces negligible
acetaldehyde which is direct evidence that a hydride shiftreaction CH
3CH2O(ad)-MrarrCH
2CHO+MH is an impor-
tant step for acetaldehyde production for metal-loaded CeO2
catalysts For M- (single) doped CeO2NPs the ethanol
oxidation performance showed an order of Ni lt Ag lt Pd ≪Au For MM1015840 codoped CeO
2NPs the activity of Au doped
CeO2deteriorated drastically upon adding another metals
(Ag Ni and Pd) as cocatalyst The Au-rich CeO2catalyst
showed higher catalytic activity On the other hand the NiPd codoped sample showed much higher catalytic activitycompared with the single M- (Ni and Pd) doped samplesThis study provides further insights into the development ofcatalysts applicable to a range of oxidation reactions
Competing Interests
The authors declare no conflict of interests
Acknowledgments
This study was supported by the 2015 Yeungnam UniversityResearch Grant
References
[1] X Nie H Qian Q Ge H Xu and R Jin ldquoCO oxidationcatalyzed by oxide-supported Au
25(SR)18
nanoclusters and
10 Journal of Chemistry
identification of perimeter sites as active centersrdquo ACS Nanovol 6 no 7 pp 6014ndash6022 2012
[2] H-F Li N Zhang P Chen M-F Luo and J-Q Lu ldquoHigh sur-face area AuCeO
2catalysts for low temperature formaldehyde
oxidationrdquoApplied Catalysis B Environmental vol 110 pp 279ndash285 2011
[3] K Y Ho and K L Yeung ldquoEffects of ozone pretreatment on theperformance of AuTiO
2catalyst for CO oxidation reactionrdquo
Journal of Catalysis vol 242 no 1 pp 131ndash141 2006[4] K Y Ho and K L Yeung ldquoProperties of TiO
2support and the
performance of AuTiO2catalyst for CO oxidation reactionrdquo
Gold Bulletin vol 40 no 1 pp 15ndash30 2007[5] J Qi J Chen G Li S Li Y Gao and Z Tang ldquoFacile
synthesis of core-shell AuCeO2nanocomposites with remark-
ably enhanced catalytic activity for CO oxidationrdquo Energy andEnvironmental Science vol 5 no 10 pp 8937ndash8941 2012
[6] D Jiang W Wang L Zhang Y Zheng and Z Wang ldquoInsightsinto the surface-defect dependence of photoreactivity overCeO2nanocrystals with well-defined crystal facetsrdquo ACS Catal-
ysis vol 5 no 8 pp 4851ndash4858 2015[7] W Lei T Zhang L Gu et al ldquoSurface-structure sensitivity
of CeO2nanocrystals in photocatalysis and enhancing the
reactivity with nanogoldrdquo ACS Catalysis vol 5 no 7 pp 4385ndash4393 2015
[8] B Li T Gu T Ming J Wang P Wang and J C Yu ldquoGoldcore)(ceria shell) nanostructures for plasmon-enhanced cat-alytic reactions under visible lightrdquo ACS Nano vol 8 no 8 pp8152ndash8162 2014
[9] P Lu B Qiao N Lu et al ldquoPhotochemical deposition of highlydispersed Pt nanoparticles on porous CeO
2nanofibers for the
water-gas shift reactionrdquoAdvanced FunctionalMaterials vol 25no 26 pp 4153ndash4162 2015
[10] L Meng A-P Jia J-Q Lu L-F Luo W-X Huang and M-FLuo ldquoSynergetic effects of PdO species on CO oxidation overPdO-CeO
2catalystsrdquo Journal of Physical Chemistry C vol 115
no 40 pp 19789ndash19796 2011[11] Y Park S K Kim D Pradhan and Y Sohn ldquoThermal H
2-
treatment effects on COCO2conversion over Pd-doped CeO
2
comparison with Au and Ag-doped CeO2rdquo Reaction Kinetics
Mechanisms and Catalysis vol 113 no 1 pp 85ndash100 2014[12] Y Park S K Kim D Pradhan and Y Sohn ldquoSurface treatment
effects on CO oxidation reactions over Co Cu and Ni-dopedand codopedCeO
2catalystsrdquoChemical Engineering Journal vol
250 pp 25ndash34 2014[13] B Xu Q Zhang S YuanM Zhang and T Ohno ldquoMorphology
control and photocatalytic characterization of yttrium-dopedhedgehog-like CeO
2rdquo Applied Catalysis B Environmental vol
164 pp 120ndash127 2015[14] W Huang and Y Gao ldquoMorphology-dependent surface chem-
istry and catalysis of CeO2nanocrystalsrdquo Catalysis Science and
Technology vol 4 no 11 pp 3772ndash3784 2014[15] Y Gao W Wang S Chang and W Huang ldquoMorphology
effect of CeO2support in the preparation metal-support
interaction and catalytic performance of PtCeO2catalystsrdquo
ChemCatChem vol 5 no 12 pp 3610ndash3620 2013[16] Y Zhang N Zhang Z-R Tang and Y-J Xu ldquoA unique
silk mat-like structured PdCeO2as an efficient visible light
photocatalyst for green organic transformation in waterrdquo ACSSustainable Chemistry amp Engineering vol 1 no 10 pp 1258ndash1266 2013
[17] W G Shin H J Jung H G Sung H S Hyun and YSohn ldquoSynergic CO oxidation activities of boron-CeO
2hybrid
materials prepared by dry and wet milling methodsrdquo CeramicsInternational vol 40 no 8 pp 11511ndash11517 2014
[18] H Wu P Wang H He and Y Jin ldquoControlled synthesisof porous AgAu bimetallic hollow nanoshells with tunableplasmonic and catalytic propertiesrdquo Nano Research vol 5 no2 pp 135ndash144 2012
[19] N Sasirekha P Sangeetha and Y-W Chen ldquoBimetallic AundashAgCeO
2catalysts for preferential oxidation ofCO inhydrogen-
rich stream effect of calcination temperaturerdquo The Journal ofPhysical Chemistry C vol 118 no 28 pp 15226ndash15233 2014
[20] S Chen L Luo Z Jiang and W Huang ldquoSize-dependent reac-tion pathways of low-temperature CO oxidation on AuCeO
2
catalystsrdquo ACS Catalysis vol 5 no 3 pp 1653ndash1662 2015[21] D LiuW Li X Feng andY Zhang ldquoGalvanic replacement syn-
thesis of Ag119909Au1minus119909
CeO2(0 le x le 1) coreshell nanospheres
with greatly enhanced catalytic performancerdquoChemical Sciencevol 6 pp 7015ndash7019 2015
[22] Y Kang M Sun and A Li ldquoStudies of the catalytic oxidationof CO over AgCeO
2catalystrdquo Catalysis Letters vol 142 no 12
pp 1498ndash1504 2012[23] S Chang M Li Q Hua et al ldquoShape-dependent inter-
play between oxygen vacancies and AgndashCeO2interaction in
AgCeO2catalysts and their influence on the catalytic activityrdquo
Journal of Catalysis vol 293 pp 195ndash204 2012[24] R Fiorenza C Crisafulli G G Condorelli F Lupo and S Scire
ldquoAu-AgCeO2and Au-CuCeO
2Catalysts for volatile organic
compounds oxidation and CO preferential oxidationrdquo CatalysisLetters vol 145 no 9 pp 1691ndash1702 2015
[25] J Zhang L Li X Huang and G Li ldquoFabrication of AgndashCeO2
core-shell nanospheres with enhanced catalytic performancedue to strengthening of the interfacial interactionsrdquo Journal ofMaterials Chemistry vol 22 no 21 pp 10480ndash10487 2012
[26] A Leyva-Perez D Combita-Merchan J R Cabrero-AntoninoS I Al-Resayes and A Corma ldquoOxyhalogenation of activatedarenes with nanocrystalline ceriardquo ACS Catalysis vol 3 no 2pp 250ndash258 2013
[27] Y Liu H Li J Yu DMao andG Lu ldquoElectronic storage capac-ity of ceria role of peroxide inAux supported onCeO
2(111) facet
and CO adsorptionrdquo Physical Chemistry Chemical Physics vol17 no 41 pp 27758ndash27768 2015
[28] D Jiang WWang S Sun L Zhang and Y Zheng ldquoEquilibrat-ing the plasmonic and catalytic roles of metallic nanostructuresin photocatalytic oxidation over Au-modified CeO
2rdquo ACS
Catalysis vol 5 no 2 pp 613ndash621 2015[29] M M Khan S A Ansari M O Ansari B K Min J Lee and
M H Cho ldquoBiogenic fabrication of AuCeO2nanocomposite
with enhanced visible light activityrdquo Journal of Physical Chem-istry C vol 118 no 18 pp 9477ndash9484 2014
[30] A Tanaka K Hashimoto and H Kominami ldquoPreparation ofAuCeO
2exhibiting strong surface plasmon resonance effective
for selective or chemoselective oxidation of alcohols to alde-hydes or ketones in aqueous suspensions under irradiation bygreen lightrdquo Journal of the American Chemical Society vol 134no 35 pp 14526ndash14533 2012
[31] H Y Kim H M Lee and G Henkelman ldquoCO oxidationmechanism on CeO
2-supported Au nanoparticlesrdquo Journal of
the American Chemical Society vol 134 no 3 pp 1560ndash15702012
[32] A Maldotti A Molinari R Juarez and H Garcia ldquoPhotoin-duced reactivity of AundashH intermediates in alcohol oxidation by
Journal of Chemistry 11
gold nanoparticles supported on ceriardquoChemical Science vol 2no 9 pp 1831ndash1834 2011
[33] L Vivier andDDuprez ldquoCeria-based solid catalysts for organicchemistryrdquo ChemSusChem vol 3 no 6 pp 654ndash678 2010
[34] N Zhang S Liu X Fu and Y-J Xu ldquoA simple strategy forfabrication of ldquoplum-puddingrdquo type PdCeO
2semiconductor
nanocomposite as a visible-light-driven photocatalyst for selec-tive oxidationrdquo Journal of Physical Chemistry C vol 115 no 46pp 22901ndash22909 2011
[35] Y Sohn ldquoSiO2nanospheres modified by Ag nanoparticles sur-
face charging and CO oxidation activityrdquo Journal of MolecularCatalysis A Chemical vol 379 pp 59ndash67 2013
[36] W J Kim D Pradhan and Y Sohn ldquoFundamental natureand CO oxidation activities of indium oxide nanostructures1D-wires 2D-plates and 3D-cubes and donutsrdquo Journal ofMaterials Chemistry A vol 1 no 35 pp 10193ndash10202 2013
[37] R-R Zhang L-H Ren A-H Lu and W-C Li ldquoInfluence ofpretreatment atmospheres on the activity of AuCeO
2catalyst
for low-temperature CO oxidationrdquo Catalysis Communicationsvol 13 no 1 pp 18ndash21 2011
[38] Y Li Y Cai X Xing N Chen D Deng and YWang ldquoCatalyticactivity for CO oxidation of CundashCeO
2composite nanoparticles
synthesized by a hydrothermal methodrdquo Analytical Methodsvol 7 no 7 pp 3238ndash3245 2015
[39] R Shang Y Duan X Zhong W Xie Y Luo and L HuangldquoFormic acid modified Co
3O4-CeO
2catalysts for CO oxida-
tionrdquo Catalysts vol 6 no 3 p 48 2016[40] A Abad P Concepcion A Corma and H Garcıa ldquoA collab-
orative effect between gold and a support induces the selectiveoxidation of alcoholsrdquo Angewandte ChemiemdashInternational Edi-tion vol 44 no 26 pp 4066ndash4069 2005
Submit your manuscripts athttpwwwhindawicom
Hindawi Publishing Corporationhttpwwwhindawicom Volume 2014
Inorganic ChemistryInternational Journal of
Hindawi Publishing Corporation httpwwwhindawicom Volume 2014
International Journal ofPhotoenergy
Hindawi Publishing Corporationhttpwwwhindawicom Volume 2014
Carbohydrate Chemistry
International Journal of
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Journal of
Chemistry
Hindawi Publishing Corporationhttpwwwhindawicom Volume 2014
Advances in
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Analytical Methods in Chemistry
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Bioinorganic Chemistry and ApplicationsHindawi Publishing Corporationhttpwwwhindawicom Volume 2014
SpectroscopyInternational Journal of
Hindawi Publishing Corporationhttpwwwhindawicom Volume 2014
The Scientific World JournalHindawi Publishing Corporation httpwwwhindawicom Volume 2014
Medicinal ChemistryInternational Journal of
Hindawi Publishing Corporationhttpwwwhindawicom Volume 2014
Chromatography Research International
Hindawi Publishing Corporationhttpwwwhindawicom Volume 2014
Applied ChemistryJournal of
Hindawi Publishing Corporationhttpwwwhindawicom Volume 2014
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Analytical ChemistryInternational Journal of
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Quantum Chemistry
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ElectrochemistryInternational Journal of
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CatalystsJournal of
Journal of Chemistry 5
commonly observed for metal doped CeO2 but at a lower
temperature (by sim50∘C) In addition the strong peaks newlyappeared below 400∘C for the metal doped CeO
2 The peak
intensityposition and broadness were dependent on theinteractions between the dopedmetal and the lattice of CeO
2
Because doped Ag and Au are present as the metallic statethe doped metallic nanoparticles could cause the spillover oflattice oxygen by forming AundashOndashCe state to result in easyreduction [19 24] Ce3+ can be formed from Ce4+ by formingAundashO bond and charge transfer from Au to Ce [27] For Au(5mol) doped CeO
2 the lower TPR peak was observed at
approximately 300∘C For AgAu (14 and 2525mol)doped CeO
2 the peak was observed at a somewhat
higher temperature with different intensities For AgAu(41 and 50mol) doped CeO
2 the peak was observed
at lower temperatures indicating stronger interactions withCeO2
Figure 6 presents the 1st and 2nd run CO oxidationconversion profiles for undoped CeO
2and Au and Ag
doped and codoped (50 05 41 2525 and 14mol)CeO2catalysts The CO conversion () was calculated using
([CO]inndash[CO]out)[CO]in times 100 [35 36] T10 is definedas the temperature corresponding to CO conversion of 10As seen in the spectra the CO oxidation onset position wasdramatically different in all samples For the 1st and 2nd runsof bare CeO
2 T10 was observed at 405∘C Upon metal-
dopingT10 was lowered dramatically In the 1st runT
10 ofthe 5mol Au and Ag doped samples was observed at240∘C and 352∘C respectively Compared to that of bareCeO2 T10 was lowered by 165∘C and 53∘C respectively
(bottom left of Figure 6) As the amount of Au was increasedT10 was observed at a lower temperature The order of
catalytic activity was found to be bare CeO2lt AgAu
(50mol) lt AgAu (41mol) lt AgAu (2525mol)lt AgAu (14mol) lt AgAu (05mol) In the 2nd runT10 was drastically changed for the metal doped samples
T10 of the 5mol Au and Ag doped samples was observed
at 295∘C and 262∘C respectively The Au doped sampleshowed a 55∘C increase in T
10 while Ag doped sampleshowed a 90∘C decrease in T
10 The order of the catalyticactivity was bare CeO
2lt AgAu (2525mol) lt AgAu
(05mol) asymp AgAu (41mol) lt AgAu (50mol) ltAgAu (14mol)The AgAu (14mol) showed the high-est activity Compared to T
10 in the 1st run the AgAu(50mol) and AgAu (14mol) samples showed a lowerT10 while other samples showed a higher T
10 in the 2ndrun as shown in the bottom right of Figure 6 In the 2nd runboth the sintering of Au nanoparticles and alloying of twodifferent metals were expected to play a role in determiningthe activity because the sample had already experienced ahigh temperature up to 700∘C The colors of the sampleswere significantly changed after the CO oxidation reactionsParticularly the colors of the AgAu (41mol) AgAu(2525mol) andAgAu (05mol) became dark grey (orblack) after the CO oxidation unlike other three samplesThe corresponding catalysts showed catalyst deactivation inthe 2nd run compared with the 1st run (Figure 6(d)) Thisindicates that change in oxidation state carbon residues
after reaction and sinteringalloying of loaded metals areimportant factors for the determination of catalytic activitySasirekha et al examined CO oxidation under hydrogen-rich conditions for Au and Ag doped and codoped CeO
2
catalysts and reported that the Ag-Ag (5 5) doped sampleshowed the highest CO conversion and selectivity [19] Theenhancement was attributed to bimetallic alloy formation[19 24] On the other hand in the present study the AgAu(2525mol) sample showed the poorest activity amongthe metal doped samples in the 2nd run This suggests thatother factors (eg size and relative distributions) are alsoimportant for determining the activity CO oxidation hascommonly been understood by CO(ad) + [O]lowast rarr CO
2(g)
where [O]lowast is the active surface oxygen The surface oxygenis replenished by molecular oxygen present in air AdsorbedCO is plausibly present at the interface of doped metal andCeO2 on top of metal andor defect sites [31]The crystalline
size (reflecting the surface area) of the samples was estimatedusing the full width at half maximum of the (111) peak andScherrerrsquos equation [12] The order of the size was found tobe AgAu (2525mol) 80 nm lt AgAu (05mol)86 nm lt AgAu (14mol) 100 nm lt AgAu (41mol)124 nm lt bare CeO
2 130 nm lt AgAu (50mol) and
140 nm Based on this the size was not linearly related withthe catalytic activity For this reason the metal-loading isimportant and themetal-support interactions play significantroles in the catalytic activity [37] In the present study T
50for all the samples was observed to be gt300∘C Zhang et alreported significantly lower T
50 for AuCeO2prepared by a
deposition-precipitation method [37] They reported T50 of
63 35 and 17∘C for untreatedH2 andH
2-O2treated samples
respectively They concluded that the surface interactionbetween Au and CeO
2was the most important factor for
the catalytic activity Li et al reported T50 of lt150∘C for
crystalline Cu-CeO2(5ndash8 nm) nanopowders synthesized by a
hydrothermal method [38] The formic acid-treated Co3O4-
CeO2catalysts were reported to show T
50 at 695∘C for COoxidation [39]The CO oxidation catalytic activities for otherCeO2-based catalysts were summarized elsewhere [11]
Ethanol oxidation reaction performances were fullyexamined for all M doped (M=Ag Au Pd andNi) andMM1015840codoped CeO
2NPs by UV-visible absorption spectroscopy
Figure 7 shows the UV-Vis absorption spectra of the ethanolsolutions reacted at 80∘C for 5 days with and without cat-alysts and with different metal-doping concentration statesTwo broad absorption peaks were commonly observed ataround 220 and 280 nm which were tentatively attributedto ethyl acetate (CH
3COOCH
2CH3 EA) and acetaldehyde
(CH3CHO AcA) respectively for the oxidation products
of ethanol Further details were discussed below The EApeak became stronger and increased more sharply than theAcA peak with reaction time The AcA absorption peakintensity increased slightly gradually reaching a certain lowconcentration levelThe presence of EA as amajor andAcA asaminor productwas further confirmedbymass spectrometry(or UV-visible absorption) as discussed in detail belowTo examine the temperature effect we conducted ethanoloxidation experiments at 40∘C and 80∘C As expected theabsorbance of the two peaks was dramatically enhanced upon
6 Journal of Chemistry
1st run
CeO2
Ag = 5molAu = 5mol
Temperature (∘C)700600500400300200100
00
20
40
60
80
100CO
conv
ersio
n (
)
1 mol 4 mol25 mol 25 mol
4 mol 1molDoped Ag Au
(a)
2nd run
Temperature (∘C)700600500400300200100
00
20
40
60
80
100
CO co
nver
sion
()
CeO2
Ag = 5molAu = 5mol1 mol 4 mol25 mol 25 mol
4 mol 1molDoped Ag Au
(b)
1st run2nd run
Au=
5mol
14m
ol
25
25m
ol
41m
ol
Ag
=5m
ol
0
minus50
minus100
minus150
T10
(MC
eO2)
minusT
10(b
are)
(c)
Au = 5 mol
14 mol
2525 mol
41 mol
Ag = 5mol
T10
(2nd
)minusT
10
minus100
minus50
0
50
100
(1st)
(d)
Au = 5 mol14 mol2525 mol41 molAg = 5molCeO2
bf C
O o
xaf
CO
ox
(e)
Figure 6 1st (a) and 2nd (b) run temperature programmed CO oxidation conversion () profiles (a b) of undoped CeO2and Au and Ag
doped and codoped (50 05 41 2525 and 14mol) CeO2catalysts The difference (c) in T
10 between the metal doped and bare CeO2
for the 1st and 2nd runs The difference (d) in T10 between the 1st and 2nd runs for the metal doped CeO
2catalysts Optical microscope
images showed the color of the powder samples before and after CO oxidation reactions
Journal of Chemistry 7
Rxn in 5 daysat 80∘C
Wavelength (nm)350300250
Wavelength (nm)
350300250Wavelength (nm)
350300250
Doped Ag AuAb
sorb
ance
(arb
uni
t)
10
05
00
15
00
01
02
03
04
Abso
rban
ce (a
rb u
nit)
0
1
2
3
4
5
Abso
rban
ce (a
rb u
nit)
With reaction timeat 80
∘C5 days4 days3 days2 days1 day (24h)8 h4hAu-(5mol) CeO2
Au = 5molNo catalyst
Ag = 5 molCeO21 mol 4 mol
25 mol 25 mol
4 mol 1 mol
O
O
O
(a)
O
O
O
Au = 5mol
Rxn in 5 daysat 80∘C
at 80∘C
0
1
2
3
4
5
Abso
rban
ce (a
rb u
nit)
Wavelength (nm)350300250
Wavelength (nm)
350300250
Doped Ni Au
Rxn in 24 hrs
Abso
rban
ce (a
rb u
nit)
10
05
00
15
1 mol 4 mol25 mol 25 mol
Ni = 5 mol4 mol 1 mol
(b)
O
O
O
Au = 5mol
Rxn in 5 daysat 80∘C
at 80∘C
0
1
2
3
4
5
Abso
rban
ce (a
rb u
nit)
Wavelength (nm)350300250
Wavelength (nm)
350300250
Doped Pd Au
Rxn in 24 hrs
Abso
rban
ce (a
rb u
nit)
10
05
00
15
1 mol 4 mol25 mol 25 mol
Pd = 5 mol4 mol 1 mol
(c)
O
O
O
Au = 5mol
Rxn in 5 daysat 80∘C
at 80∘C
Wavelength (nm)350300250
Wavelength (nm)
350300250
Doped Ni Pd
Rxn in 24 hrs
Abso
rban
ce (a
rb u
nit)
10
05
00
15
0
1
2
3
4
5
Abso
rban
ce (a
rb u
nit)
1 mol 4 mol25 mol 25 mol
Pd = 5 molNi = 5 mol
4 mol 1 mol
(d)
Figure 7 UV-visible absorption spectra of the ethanol oxidation with no catalyst undoped CeO2 M doped (M = Ag Au Pd and Ni) and
MM1015840 codoped (AgAu (a) NiAu (b) PdAu (c) and NiPd (d)) CeO2catalysts at 80∘C for 5 days The left inset in (a) shows the magnified
spectra of the grey shadowed region The right inset in (a) shows the UV-Vis absorption spectra of ethanol oxidation with the 5mol Audoped CeO
2catalyst at 80∘C according to the reaction time
increasing reaction temperatureWithout catalysts no signif-icant ethanol oxidation occurred even at high temperatureFor further ethanol oxidation experiments we selected areaction temperature of 80∘C and a total metal-doping levelof 5mol
For Ag and Au doped and codoped samples (Figure 7(a))a strong absorption peak (below 250 nm) was observed forthe Au (5mol) and AuAg (14mol) doped CeO
2cata-
lysts Without a catalyst no significant absorption peak was
observed even after 5 days The absorption peak (shown inthe right inset of Figure 7(a)) increased with increasingreaction time This was attributed to an increase in reactionproducts that contain C=C andor C=O functional groupsFor the other metal doped samples the absorption peakswere much weaker In addition to the strong absorptionpeak a weaker peak at 280 nm was also observed (in theleft inset of Figure 7) The results suggest that at least tworeaction products (EA and AcA as mentioned above) were
8 Journal of Chemistry
present in the ethanol solution The catalytic activity wasobserved to be in the order of bare CeO
2asymp 2525 lt 41 lt
50 ≪ 14 lt 05 (AgAumol) When the concentration ofAu was the same as or lower than that of Ag the activitydeteriorated drastically For Au and Ni doped and codopedsamples (Figure 7(b)) the catalytic activity was decreasedupon adding Ni as a cocatalyst The activity was found to bein the order of 50 lt 41≪ 2525 lt 14 lt 05 (NiAumol)For Au and Pd doped and codoped samples (Figure 7(c))the oxidation performance was more greatly decreased uponadding Pd as a cocatalyst and found to be in the order of 41 le2525asymp 14asymp 50≪ 05 (PdAumol) ForNi and Pd dopedand codoped samples (Figure 7(d)) the catalytic activity wasobserved to be in the order of 50 lt 05≪ 41 asymp 14 le 2525(NiPdmol) The catalytic activity of the NiPd codopedsamples showed much higher catalytic activity than those ofthe single M- (Ni and Pd) doped samples For comparisonof the catalytic activities of single M doped CeO
2NPs the
ethanol oxidation performance showed an order of undopedasympNi ltAg lt Pd≪Au Interestingly the Ni-doping showed noincrease in catalytic activity for ethanol oxidation
For ethanol oxidation on a metal doped CeO2power
sample since the reaction mechanism was much more com-plicated than expected on a single crystal surface we proposethe following simplified mechanisms which are discussed ingreater detail below [32]
Acetaldehyde hemiacetal and ethyl acetate formationfrom ethanol is as follows
CH3CH2OndashH 997888rarr CH
3CH2O (ad) +H (ad) (1)
CH3CH2O (ad) +O species
997888rarr CH3CHO (ad) +OH (ad)
(2)
CH3CH2O (ad) ndashM
997888rarr CH3CHO (minor) +MH hydride shift
(3)
CH3CHO +O (ad) 997888rarr CH
3COO (ad) +H (ad)
997888rarr CH3COOH
(4)
CH3COOH (ad) + CH3CH2OH (ad)
997888rarr CH3COOCH
2CH3+H2O
(5)
2CH3CHO (ad) 997888rarr CH
3COOCH
2CH3 (6)
CH3CHO (ad) + CH3CH2OH (ad)
997888rarr CH3CH (OH)OC
2H5 (hemiacetal)
997888rarr CH3COOCH
2CH3(major) +H
2
(7)
The rate constant for each step is controlled by the surfacearea and metal-support interaction (or surface activity) Inreaction (1) the OndashH bond of ethanol dissociates to formCH3CH2O which may be mainly adsorbed onto the doped
metal siteThis then turns into adsorbedCH3CHOvia nearby
active oxygen species in (2) or the adsorbed CH3CH2O on
metal desorbs as CH3CHO (acetaldehyde) in response to a
hydride shift reaction in (3) [32 40] Although we have nodirect evidence of the hydride shift reaction the reactionprocess is highly plausible The acetaldehyde in (4) furtherprecedes oxidation reactions to form CH
3COOH (acetic
acid) if active oxygen species are available nearby Otherwisethe CH
3COOH with ethanol in (5) and 2CH
3CHO in (6)
react to form CH3COOCH
2CH3(ethyl acetate) In reaction
(7) CH3CHO and ethanol formCH
3CH(OH)OC
2H5(hemi-
acetal) which is converted to ethyl acetate Consequentlyethyl acetate (CH
3COOCH
2CH3) is formed as a final oxi-
dation product which was confirmed by mass spectrometryIn the present UV-Vis spectra two products of ethyl acetate(major) and acetaldehyde (minor) were observed For alcoholoxidation on the Au-CeO
2catalyst Maldotti et al reported
that the Au-H species is an important intermediate [32] Thisindicates that the hydride shift reaction is facilitated by activedopedmetalsThe present study showed that the Au-rich cat-alyst produced much higher oxidation products and the Auspecies is more active than other metal species (Ag Ni andPd)The reference UV-Vis spectra (Figure 8(a)) were checkedfor four plausible ethanol oxidation products acetaldehydeethyl acetate acetone and acetic acid and the stronger andweaker peak positions near 220 and 280 nm were assignedto the UV-Vis absorptions of ethyl acetate and acetaldehyderespectively Figure 8(b) displays the mass spectrum of thesolution sample after reaction relative to those of the referencesolvents (ethyl acetate and ethanol) As shown in the massspectrum the oxidation product in ethanol matched thatof the reference ethyl acetate well In addition the smell ofthe two samples was very similar As a result we concludedthat the final major product was ethyl acetate For someother extra mass fragmentation signals (59 73 and 75 amu)although no reference data were available the fragmentationsappeared to form from the hemiacetal as shown in reaction(7) Abad et al extensively studied oxidation of alcoholscatalyzed by AuCeO
2[40] and proposed a reaction of (7)
mentioned above in which hemiacetal was detected by H-NMR We have excluded diethyl ether as a major producteven though it could be formed by 2C
2H5OHrarrC
2H5OC2H5
+ H2O because the UV-visible absorption intensity (even
measuredwith 50 solution) was extremely low (Figure 8(a))when compared with that of the sample We also detected nofragmentation signals of diethyl ether by mass spectrometryThe acetone formation reaction 2CH
3CHOrarr CH
3COCH
3
(acetone) + CO2+ H2 was excluded due to absence of the
mass signal Acetic acid as a major product was also excludedbecause the solution is not acidic the mass signal is absentand it did not smell like acetic acid Table 1 summarizes thesizes of the metal-loaded CeO
2estimated using Scherrerrsquos
equation As for the CO oxidation the ethanol oxidationactivity was also found to be more loaded metal (and therelative concentrations) dependent than the size-dependent
4 Conclusion
To increase the catalytic activity of bare CeO2 the CeO
2
matrix was doped and codoped with Ag Au Pd and Ni bya hydrothermal method The novelty of the present study
Journal of Chemistry 9
Table 1 Particles sizes of the metal-loaded CeO2estimated using Scherrerrsquos equation
Loaded MM1015840 50mol (nm) 41mol (nm) 2525mol (nm) 14mol (nm) 05mol (nm)Ag Au 140 124 80 100 86Ni Au 152 123 106 82 86Pd Au 151 127 121 90 86Ni Pd 152 111 147 121 151
Catalysts without stirring
Tightly capped
OOH
O
O
O
lowast
lowast
O
OH
OHO
OO
Abso
rban
ce
10
05
00
Diethyl ether 50
Different smellAcetaldehyde sim1
Acetone sim1
Different smellAcetic acid 01
Ethyl acetate 01
Wavelength (nm)400350300250
(a)
Ethyl acetate(reference)
O
O
Mass (amu)1009080706050M
ass s
igna
l (au
)
OH Before reaction(ETOH)
50 60
Mass (amu)70 80 90 100M
ass s
igna
l (au
)
Afterreaction
01234
UV-VisO
O
Mass (amu)1009080706050M
ass s
igna
l (au
)
Abso
rban
ce
250 300Wavelength (nm)
(b)
Figure 8 UV-Vis absorption spectra (a) of standard samples of acetaldehyde (1) acetone (1) acetic acid (01) and ethyl acetate (01)Mass spectra (b) of reference samples (ethyl acetate and ethanol) and the solution sample after reactionThe inset shows theUV-Vis absorptionspectrum of the corresponding sample solution Blue and red lowast indicate the peak positions for acetaldehyde and ethyl acetate respectively
was that the catalytic efficiency of doped and codoped CeO2
was tested for both gas-phase CO and liquid-phase ethanoloxidation reactions For the 1st and 2nd runs of bare CeO
2
T10 was observed at 405∘C T
10 of bare CeO2for CO oxi-
dation was lowered significantly by 165∘C uponmetal (AgAu= 14mol) doping There were some synergic effects uponcodoping for the CO oxidation The CO oxidation activityvaries with the relative concentrations of two differentmetalsSintering and alloying of two different metals were found toplay important roles in the CO oxidation activity
For liquid-phase ethanol oxidation two liquid productsof ethyl acetate (major 120582max = 220 nm) and acetaldehyde(minor 120582max = 280 nm) were observed by UV-Vis absorptionspectroscopyThe concentration of acetaldehyde (CH
3CHO)
reached a saturation point while that of ethyl acetate(CH3COOCH
2CH3) dramatically increased with reaction
time These findings indicate that acetaldehyde speciespromptly undergo further reaction to form a major productethyl acetate whichwas confirmed bymass spectrometry andUV-visible absorption Undoped CeO
2produces negligible
acetaldehyde which is direct evidence that a hydride shiftreaction CH
3CH2O(ad)-MrarrCH
2CHO+MH is an impor-
tant step for acetaldehyde production for metal-loaded CeO2
catalysts For M- (single) doped CeO2NPs the ethanol
oxidation performance showed an order of Ni lt Ag lt Pd ≪Au For MM1015840 codoped CeO
2NPs the activity of Au doped
CeO2deteriorated drastically upon adding another metals
(Ag Ni and Pd) as cocatalyst The Au-rich CeO2catalyst
showed higher catalytic activity On the other hand the NiPd codoped sample showed much higher catalytic activitycompared with the single M- (Ni and Pd) doped samplesThis study provides further insights into the development ofcatalysts applicable to a range of oxidation reactions
Competing Interests
The authors declare no conflict of interests
Acknowledgments
This study was supported by the 2015 Yeungnam UniversityResearch Grant
References
[1] X Nie H Qian Q Ge H Xu and R Jin ldquoCO oxidationcatalyzed by oxide-supported Au
25(SR)18
nanoclusters and
10 Journal of Chemistry
identification of perimeter sites as active centersrdquo ACS Nanovol 6 no 7 pp 6014ndash6022 2012
[2] H-F Li N Zhang P Chen M-F Luo and J-Q Lu ldquoHigh sur-face area AuCeO
2catalysts for low temperature formaldehyde
oxidationrdquoApplied Catalysis B Environmental vol 110 pp 279ndash285 2011
[3] K Y Ho and K L Yeung ldquoEffects of ozone pretreatment on theperformance of AuTiO
2catalyst for CO oxidation reactionrdquo
Journal of Catalysis vol 242 no 1 pp 131ndash141 2006[4] K Y Ho and K L Yeung ldquoProperties of TiO
2support and the
performance of AuTiO2catalyst for CO oxidation reactionrdquo
Gold Bulletin vol 40 no 1 pp 15ndash30 2007[5] J Qi J Chen G Li S Li Y Gao and Z Tang ldquoFacile
synthesis of core-shell AuCeO2nanocomposites with remark-
ably enhanced catalytic activity for CO oxidationrdquo Energy andEnvironmental Science vol 5 no 10 pp 8937ndash8941 2012
[6] D Jiang W Wang L Zhang Y Zheng and Z Wang ldquoInsightsinto the surface-defect dependence of photoreactivity overCeO2nanocrystals with well-defined crystal facetsrdquo ACS Catal-
ysis vol 5 no 8 pp 4851ndash4858 2015[7] W Lei T Zhang L Gu et al ldquoSurface-structure sensitivity
of CeO2nanocrystals in photocatalysis and enhancing the
reactivity with nanogoldrdquo ACS Catalysis vol 5 no 7 pp 4385ndash4393 2015
[8] B Li T Gu T Ming J Wang P Wang and J C Yu ldquoGoldcore)(ceria shell) nanostructures for plasmon-enhanced cat-alytic reactions under visible lightrdquo ACS Nano vol 8 no 8 pp8152ndash8162 2014
[9] P Lu B Qiao N Lu et al ldquoPhotochemical deposition of highlydispersed Pt nanoparticles on porous CeO
2nanofibers for the
water-gas shift reactionrdquoAdvanced FunctionalMaterials vol 25no 26 pp 4153ndash4162 2015
[10] L Meng A-P Jia J-Q Lu L-F Luo W-X Huang and M-FLuo ldquoSynergetic effects of PdO species on CO oxidation overPdO-CeO
2catalystsrdquo Journal of Physical Chemistry C vol 115
no 40 pp 19789ndash19796 2011[11] Y Park S K Kim D Pradhan and Y Sohn ldquoThermal H
2-
treatment effects on COCO2conversion over Pd-doped CeO
2
comparison with Au and Ag-doped CeO2rdquo Reaction Kinetics
Mechanisms and Catalysis vol 113 no 1 pp 85ndash100 2014[12] Y Park S K Kim D Pradhan and Y Sohn ldquoSurface treatment
effects on CO oxidation reactions over Co Cu and Ni-dopedand codopedCeO
2catalystsrdquoChemical Engineering Journal vol
250 pp 25ndash34 2014[13] B Xu Q Zhang S YuanM Zhang and T Ohno ldquoMorphology
control and photocatalytic characterization of yttrium-dopedhedgehog-like CeO
2rdquo Applied Catalysis B Environmental vol
164 pp 120ndash127 2015[14] W Huang and Y Gao ldquoMorphology-dependent surface chem-
istry and catalysis of CeO2nanocrystalsrdquo Catalysis Science and
Technology vol 4 no 11 pp 3772ndash3784 2014[15] Y Gao W Wang S Chang and W Huang ldquoMorphology
effect of CeO2support in the preparation metal-support
interaction and catalytic performance of PtCeO2catalystsrdquo
ChemCatChem vol 5 no 12 pp 3610ndash3620 2013[16] Y Zhang N Zhang Z-R Tang and Y-J Xu ldquoA unique
silk mat-like structured PdCeO2as an efficient visible light
photocatalyst for green organic transformation in waterrdquo ACSSustainable Chemistry amp Engineering vol 1 no 10 pp 1258ndash1266 2013
[17] W G Shin H J Jung H G Sung H S Hyun and YSohn ldquoSynergic CO oxidation activities of boron-CeO
2hybrid
materials prepared by dry and wet milling methodsrdquo CeramicsInternational vol 40 no 8 pp 11511ndash11517 2014
[18] H Wu P Wang H He and Y Jin ldquoControlled synthesisof porous AgAu bimetallic hollow nanoshells with tunableplasmonic and catalytic propertiesrdquo Nano Research vol 5 no2 pp 135ndash144 2012
[19] N Sasirekha P Sangeetha and Y-W Chen ldquoBimetallic AundashAgCeO
2catalysts for preferential oxidation ofCO inhydrogen-
rich stream effect of calcination temperaturerdquo The Journal ofPhysical Chemistry C vol 118 no 28 pp 15226ndash15233 2014
[20] S Chen L Luo Z Jiang and W Huang ldquoSize-dependent reac-tion pathways of low-temperature CO oxidation on AuCeO
2
catalystsrdquo ACS Catalysis vol 5 no 3 pp 1653ndash1662 2015[21] D LiuW Li X Feng andY Zhang ldquoGalvanic replacement syn-
thesis of Ag119909Au1minus119909
CeO2(0 le x le 1) coreshell nanospheres
with greatly enhanced catalytic performancerdquoChemical Sciencevol 6 pp 7015ndash7019 2015
[22] Y Kang M Sun and A Li ldquoStudies of the catalytic oxidationof CO over AgCeO
2catalystrdquo Catalysis Letters vol 142 no 12
pp 1498ndash1504 2012[23] S Chang M Li Q Hua et al ldquoShape-dependent inter-
play between oxygen vacancies and AgndashCeO2interaction in
AgCeO2catalysts and their influence on the catalytic activityrdquo
Journal of Catalysis vol 293 pp 195ndash204 2012[24] R Fiorenza C Crisafulli G G Condorelli F Lupo and S Scire
ldquoAu-AgCeO2and Au-CuCeO
2Catalysts for volatile organic
compounds oxidation and CO preferential oxidationrdquo CatalysisLetters vol 145 no 9 pp 1691ndash1702 2015
[25] J Zhang L Li X Huang and G Li ldquoFabrication of AgndashCeO2
core-shell nanospheres with enhanced catalytic performancedue to strengthening of the interfacial interactionsrdquo Journal ofMaterials Chemistry vol 22 no 21 pp 10480ndash10487 2012
[26] A Leyva-Perez D Combita-Merchan J R Cabrero-AntoninoS I Al-Resayes and A Corma ldquoOxyhalogenation of activatedarenes with nanocrystalline ceriardquo ACS Catalysis vol 3 no 2pp 250ndash258 2013
[27] Y Liu H Li J Yu DMao andG Lu ldquoElectronic storage capac-ity of ceria role of peroxide inAux supported onCeO
2(111) facet
and CO adsorptionrdquo Physical Chemistry Chemical Physics vol17 no 41 pp 27758ndash27768 2015
[28] D Jiang WWang S Sun L Zhang and Y Zheng ldquoEquilibrat-ing the plasmonic and catalytic roles of metallic nanostructuresin photocatalytic oxidation over Au-modified CeO
2rdquo ACS
Catalysis vol 5 no 2 pp 613ndash621 2015[29] M M Khan S A Ansari M O Ansari B K Min J Lee and
M H Cho ldquoBiogenic fabrication of AuCeO2nanocomposite
with enhanced visible light activityrdquo Journal of Physical Chem-istry C vol 118 no 18 pp 9477ndash9484 2014
[30] A Tanaka K Hashimoto and H Kominami ldquoPreparation ofAuCeO
2exhibiting strong surface plasmon resonance effective
for selective or chemoselective oxidation of alcohols to alde-hydes or ketones in aqueous suspensions under irradiation bygreen lightrdquo Journal of the American Chemical Society vol 134no 35 pp 14526ndash14533 2012
[31] H Y Kim H M Lee and G Henkelman ldquoCO oxidationmechanism on CeO
2-supported Au nanoparticlesrdquo Journal of
the American Chemical Society vol 134 no 3 pp 1560ndash15702012
[32] A Maldotti A Molinari R Juarez and H Garcia ldquoPhotoin-duced reactivity of AundashH intermediates in alcohol oxidation by
Journal of Chemistry 11
gold nanoparticles supported on ceriardquoChemical Science vol 2no 9 pp 1831ndash1834 2011
[33] L Vivier andDDuprez ldquoCeria-based solid catalysts for organicchemistryrdquo ChemSusChem vol 3 no 6 pp 654ndash678 2010
[34] N Zhang S Liu X Fu and Y-J Xu ldquoA simple strategy forfabrication of ldquoplum-puddingrdquo type PdCeO
2semiconductor
nanocomposite as a visible-light-driven photocatalyst for selec-tive oxidationrdquo Journal of Physical Chemistry C vol 115 no 46pp 22901ndash22909 2011
[35] Y Sohn ldquoSiO2nanospheres modified by Ag nanoparticles sur-
face charging and CO oxidation activityrdquo Journal of MolecularCatalysis A Chemical vol 379 pp 59ndash67 2013
[36] W J Kim D Pradhan and Y Sohn ldquoFundamental natureand CO oxidation activities of indium oxide nanostructures1D-wires 2D-plates and 3D-cubes and donutsrdquo Journal ofMaterials Chemistry A vol 1 no 35 pp 10193ndash10202 2013
[37] R-R Zhang L-H Ren A-H Lu and W-C Li ldquoInfluence ofpretreatment atmospheres on the activity of AuCeO
2catalyst
for low-temperature CO oxidationrdquo Catalysis Communicationsvol 13 no 1 pp 18ndash21 2011
[38] Y Li Y Cai X Xing N Chen D Deng and YWang ldquoCatalyticactivity for CO oxidation of CundashCeO
2composite nanoparticles
synthesized by a hydrothermal methodrdquo Analytical Methodsvol 7 no 7 pp 3238ndash3245 2015
[39] R Shang Y Duan X Zhong W Xie Y Luo and L HuangldquoFormic acid modified Co
3O4-CeO
2catalysts for CO oxida-
tionrdquo Catalysts vol 6 no 3 p 48 2016[40] A Abad P Concepcion A Corma and H Garcıa ldquoA collab-
orative effect between gold and a support induces the selectiveoxidation of alcoholsrdquo Angewandte ChemiemdashInternational Edi-tion vol 44 no 26 pp 4066ndash4069 2005
Submit your manuscripts athttpwwwhindawicom
Hindawi Publishing Corporationhttpwwwhindawicom Volume 2014
Inorganic ChemistryInternational Journal of
Hindawi Publishing Corporation httpwwwhindawicom Volume 2014
International Journal ofPhotoenergy
Hindawi Publishing Corporationhttpwwwhindawicom Volume 2014
Carbohydrate Chemistry
International Journal of
Hindawi Publishing Corporationhttpwwwhindawicom Volume 2014
Journal of
Chemistry
Hindawi Publishing Corporationhttpwwwhindawicom Volume 2014
Advances in
Physical Chemistry
Hindawi Publishing Corporationhttpwwwhindawicom
Analytical Methods in Chemistry
Journal of
Volume 2014
Bioinorganic Chemistry and ApplicationsHindawi Publishing Corporationhttpwwwhindawicom Volume 2014
SpectroscopyInternational Journal of
Hindawi Publishing Corporationhttpwwwhindawicom Volume 2014
The Scientific World JournalHindawi Publishing Corporation httpwwwhindawicom Volume 2014
Medicinal ChemistryInternational Journal of
Hindawi Publishing Corporationhttpwwwhindawicom Volume 2014
Chromatography Research International
Hindawi Publishing Corporationhttpwwwhindawicom Volume 2014
Applied ChemistryJournal of
Hindawi Publishing Corporationhttpwwwhindawicom Volume 2014
Hindawi Publishing Corporationhttpwwwhindawicom Volume 2014
Theoretical ChemistryJournal of
Hindawi Publishing Corporationhttpwwwhindawicom Volume 2014
Journal of
Spectroscopy
Analytical ChemistryInternational Journal of
Hindawi Publishing Corporationhttpwwwhindawicom Volume 2014
Journal of
Hindawi Publishing Corporationhttpwwwhindawicom Volume 2014
Quantum Chemistry
Hindawi Publishing Corporationhttpwwwhindawicom Volume 2014
Organic Chemistry International
ElectrochemistryInternational Journal of
Hindawi Publishing Corporation httpwwwhindawicom Volume 2014
Hindawi Publishing Corporationhttpwwwhindawicom Volume 2014
CatalystsJournal of
6 Journal of Chemistry
1st run
CeO2
Ag = 5molAu = 5mol
Temperature (∘C)700600500400300200100
00
20
40
60
80
100CO
conv
ersio
n (
)
1 mol 4 mol25 mol 25 mol
4 mol 1molDoped Ag Au
(a)
2nd run
Temperature (∘C)700600500400300200100
00
20
40
60
80
100
CO co
nver
sion
()
CeO2
Ag = 5molAu = 5mol1 mol 4 mol25 mol 25 mol
4 mol 1molDoped Ag Au
(b)
1st run2nd run
Au=
5mol
14m
ol
25
25m
ol
41m
ol
Ag
=5m
ol
0
minus50
minus100
minus150
T10
(MC
eO2)
minusT
10(b
are)
(c)
Au = 5 mol
14 mol
2525 mol
41 mol
Ag = 5mol
T10
(2nd
)minusT
10
minus100
minus50
0
50
100
(1st)
(d)
Au = 5 mol14 mol2525 mol41 molAg = 5molCeO2
bf C
O o
xaf
CO
ox
(e)
Figure 6 1st (a) and 2nd (b) run temperature programmed CO oxidation conversion () profiles (a b) of undoped CeO2and Au and Ag
doped and codoped (50 05 41 2525 and 14mol) CeO2catalysts The difference (c) in T
10 between the metal doped and bare CeO2
for the 1st and 2nd runs The difference (d) in T10 between the 1st and 2nd runs for the metal doped CeO
2catalysts Optical microscope
images showed the color of the powder samples before and after CO oxidation reactions
Journal of Chemistry 7
Rxn in 5 daysat 80∘C
Wavelength (nm)350300250
Wavelength (nm)
350300250Wavelength (nm)
350300250
Doped Ag AuAb
sorb
ance
(arb
uni
t)
10
05
00
15
00
01
02
03
04
Abso
rban
ce (a
rb u
nit)
0
1
2
3
4
5
Abso
rban
ce (a
rb u
nit)
With reaction timeat 80
∘C5 days4 days3 days2 days1 day (24h)8 h4hAu-(5mol) CeO2
Au = 5molNo catalyst
Ag = 5 molCeO21 mol 4 mol
25 mol 25 mol
4 mol 1 mol
O
O
O
(a)
O
O
O
Au = 5mol
Rxn in 5 daysat 80∘C
at 80∘C
0
1
2
3
4
5
Abso
rban
ce (a
rb u
nit)
Wavelength (nm)350300250
Wavelength (nm)
350300250
Doped Ni Au
Rxn in 24 hrs
Abso
rban
ce (a
rb u
nit)
10
05
00
15
1 mol 4 mol25 mol 25 mol
Ni = 5 mol4 mol 1 mol
(b)
O
O
O
Au = 5mol
Rxn in 5 daysat 80∘C
at 80∘C
0
1
2
3
4
5
Abso
rban
ce (a
rb u
nit)
Wavelength (nm)350300250
Wavelength (nm)
350300250
Doped Pd Au
Rxn in 24 hrs
Abso
rban
ce (a
rb u
nit)
10
05
00
15
1 mol 4 mol25 mol 25 mol
Pd = 5 mol4 mol 1 mol
(c)
O
O
O
Au = 5mol
Rxn in 5 daysat 80∘C
at 80∘C
Wavelength (nm)350300250
Wavelength (nm)
350300250
Doped Ni Pd
Rxn in 24 hrs
Abso
rban
ce (a
rb u
nit)
10
05
00
15
0
1
2
3
4
5
Abso
rban
ce (a
rb u
nit)
1 mol 4 mol25 mol 25 mol
Pd = 5 molNi = 5 mol
4 mol 1 mol
(d)
Figure 7 UV-visible absorption spectra of the ethanol oxidation with no catalyst undoped CeO2 M doped (M = Ag Au Pd and Ni) and
MM1015840 codoped (AgAu (a) NiAu (b) PdAu (c) and NiPd (d)) CeO2catalysts at 80∘C for 5 days The left inset in (a) shows the magnified
spectra of the grey shadowed region The right inset in (a) shows the UV-Vis absorption spectra of ethanol oxidation with the 5mol Audoped CeO
2catalyst at 80∘C according to the reaction time
increasing reaction temperatureWithout catalysts no signif-icant ethanol oxidation occurred even at high temperatureFor further ethanol oxidation experiments we selected areaction temperature of 80∘C and a total metal-doping levelof 5mol
For Ag and Au doped and codoped samples (Figure 7(a))a strong absorption peak (below 250 nm) was observed forthe Au (5mol) and AuAg (14mol) doped CeO
2cata-
lysts Without a catalyst no significant absorption peak was
observed even after 5 days The absorption peak (shown inthe right inset of Figure 7(a)) increased with increasingreaction time This was attributed to an increase in reactionproducts that contain C=C andor C=O functional groupsFor the other metal doped samples the absorption peakswere much weaker In addition to the strong absorptionpeak a weaker peak at 280 nm was also observed (in theleft inset of Figure 7) The results suggest that at least tworeaction products (EA and AcA as mentioned above) were
8 Journal of Chemistry
present in the ethanol solution The catalytic activity wasobserved to be in the order of bare CeO
2asymp 2525 lt 41 lt
50 ≪ 14 lt 05 (AgAumol) When the concentration ofAu was the same as or lower than that of Ag the activitydeteriorated drastically For Au and Ni doped and codopedsamples (Figure 7(b)) the catalytic activity was decreasedupon adding Ni as a cocatalyst The activity was found to bein the order of 50 lt 41≪ 2525 lt 14 lt 05 (NiAumol)For Au and Pd doped and codoped samples (Figure 7(c))the oxidation performance was more greatly decreased uponadding Pd as a cocatalyst and found to be in the order of 41 le2525asymp 14asymp 50≪ 05 (PdAumol) ForNi and Pd dopedand codoped samples (Figure 7(d)) the catalytic activity wasobserved to be in the order of 50 lt 05≪ 41 asymp 14 le 2525(NiPdmol) The catalytic activity of the NiPd codopedsamples showed much higher catalytic activity than those ofthe single M- (Ni and Pd) doped samples For comparisonof the catalytic activities of single M doped CeO
2NPs the
ethanol oxidation performance showed an order of undopedasympNi ltAg lt Pd≪Au Interestingly the Ni-doping showed noincrease in catalytic activity for ethanol oxidation
For ethanol oxidation on a metal doped CeO2power
sample since the reaction mechanism was much more com-plicated than expected on a single crystal surface we proposethe following simplified mechanisms which are discussed ingreater detail below [32]
Acetaldehyde hemiacetal and ethyl acetate formationfrom ethanol is as follows
CH3CH2OndashH 997888rarr CH
3CH2O (ad) +H (ad) (1)
CH3CH2O (ad) +O species
997888rarr CH3CHO (ad) +OH (ad)
(2)
CH3CH2O (ad) ndashM
997888rarr CH3CHO (minor) +MH hydride shift
(3)
CH3CHO +O (ad) 997888rarr CH
3COO (ad) +H (ad)
997888rarr CH3COOH
(4)
CH3COOH (ad) + CH3CH2OH (ad)
997888rarr CH3COOCH
2CH3+H2O
(5)
2CH3CHO (ad) 997888rarr CH
3COOCH
2CH3 (6)
CH3CHO (ad) + CH3CH2OH (ad)
997888rarr CH3CH (OH)OC
2H5 (hemiacetal)
997888rarr CH3COOCH
2CH3(major) +H
2
(7)
The rate constant for each step is controlled by the surfacearea and metal-support interaction (or surface activity) Inreaction (1) the OndashH bond of ethanol dissociates to formCH3CH2O which may be mainly adsorbed onto the doped
metal siteThis then turns into adsorbedCH3CHOvia nearby
active oxygen species in (2) or the adsorbed CH3CH2O on
metal desorbs as CH3CHO (acetaldehyde) in response to a
hydride shift reaction in (3) [32 40] Although we have nodirect evidence of the hydride shift reaction the reactionprocess is highly plausible The acetaldehyde in (4) furtherprecedes oxidation reactions to form CH
3COOH (acetic
acid) if active oxygen species are available nearby Otherwisethe CH
3COOH with ethanol in (5) and 2CH
3CHO in (6)
react to form CH3COOCH
2CH3(ethyl acetate) In reaction
(7) CH3CHO and ethanol formCH
3CH(OH)OC
2H5(hemi-
acetal) which is converted to ethyl acetate Consequentlyethyl acetate (CH
3COOCH
2CH3) is formed as a final oxi-
dation product which was confirmed by mass spectrometryIn the present UV-Vis spectra two products of ethyl acetate(major) and acetaldehyde (minor) were observed For alcoholoxidation on the Au-CeO
2catalyst Maldotti et al reported
that the Au-H species is an important intermediate [32] Thisindicates that the hydride shift reaction is facilitated by activedopedmetalsThe present study showed that the Au-rich cat-alyst produced much higher oxidation products and the Auspecies is more active than other metal species (Ag Ni andPd)The reference UV-Vis spectra (Figure 8(a)) were checkedfor four plausible ethanol oxidation products acetaldehydeethyl acetate acetone and acetic acid and the stronger andweaker peak positions near 220 and 280 nm were assignedto the UV-Vis absorptions of ethyl acetate and acetaldehyderespectively Figure 8(b) displays the mass spectrum of thesolution sample after reaction relative to those of the referencesolvents (ethyl acetate and ethanol) As shown in the massspectrum the oxidation product in ethanol matched thatof the reference ethyl acetate well In addition the smell ofthe two samples was very similar As a result we concludedthat the final major product was ethyl acetate For someother extra mass fragmentation signals (59 73 and 75 amu)although no reference data were available the fragmentationsappeared to form from the hemiacetal as shown in reaction(7) Abad et al extensively studied oxidation of alcoholscatalyzed by AuCeO
2[40] and proposed a reaction of (7)
mentioned above in which hemiacetal was detected by H-NMR We have excluded diethyl ether as a major producteven though it could be formed by 2C
2H5OHrarrC
2H5OC2H5
+ H2O because the UV-visible absorption intensity (even
measuredwith 50 solution) was extremely low (Figure 8(a))when compared with that of the sample We also detected nofragmentation signals of diethyl ether by mass spectrometryThe acetone formation reaction 2CH
3CHOrarr CH
3COCH
3
(acetone) + CO2+ H2 was excluded due to absence of the
mass signal Acetic acid as a major product was also excludedbecause the solution is not acidic the mass signal is absentand it did not smell like acetic acid Table 1 summarizes thesizes of the metal-loaded CeO
2estimated using Scherrerrsquos
equation As for the CO oxidation the ethanol oxidationactivity was also found to be more loaded metal (and therelative concentrations) dependent than the size-dependent
4 Conclusion
To increase the catalytic activity of bare CeO2 the CeO
2
matrix was doped and codoped with Ag Au Pd and Ni bya hydrothermal method The novelty of the present study
Journal of Chemistry 9
Table 1 Particles sizes of the metal-loaded CeO2estimated using Scherrerrsquos equation
Loaded MM1015840 50mol (nm) 41mol (nm) 2525mol (nm) 14mol (nm) 05mol (nm)Ag Au 140 124 80 100 86Ni Au 152 123 106 82 86Pd Au 151 127 121 90 86Ni Pd 152 111 147 121 151
Catalysts without stirring
Tightly capped
OOH
O
O
O
lowast
lowast
O
OH
OHO
OO
Abso
rban
ce
10
05
00
Diethyl ether 50
Different smellAcetaldehyde sim1
Acetone sim1
Different smellAcetic acid 01
Ethyl acetate 01
Wavelength (nm)400350300250
(a)
Ethyl acetate(reference)
O
O
Mass (amu)1009080706050M
ass s
igna
l (au
)
OH Before reaction(ETOH)
50 60
Mass (amu)70 80 90 100M
ass s
igna
l (au
)
Afterreaction
01234
UV-VisO
O
Mass (amu)1009080706050M
ass s
igna
l (au
)
Abso
rban
ce
250 300Wavelength (nm)
(b)
Figure 8 UV-Vis absorption spectra (a) of standard samples of acetaldehyde (1) acetone (1) acetic acid (01) and ethyl acetate (01)Mass spectra (b) of reference samples (ethyl acetate and ethanol) and the solution sample after reactionThe inset shows theUV-Vis absorptionspectrum of the corresponding sample solution Blue and red lowast indicate the peak positions for acetaldehyde and ethyl acetate respectively
was that the catalytic efficiency of doped and codoped CeO2
was tested for both gas-phase CO and liquid-phase ethanoloxidation reactions For the 1st and 2nd runs of bare CeO
2
T10 was observed at 405∘C T
10 of bare CeO2for CO oxi-
dation was lowered significantly by 165∘C uponmetal (AgAu= 14mol) doping There were some synergic effects uponcodoping for the CO oxidation The CO oxidation activityvaries with the relative concentrations of two differentmetalsSintering and alloying of two different metals were found toplay important roles in the CO oxidation activity
For liquid-phase ethanol oxidation two liquid productsof ethyl acetate (major 120582max = 220 nm) and acetaldehyde(minor 120582max = 280 nm) were observed by UV-Vis absorptionspectroscopyThe concentration of acetaldehyde (CH
3CHO)
reached a saturation point while that of ethyl acetate(CH3COOCH
2CH3) dramatically increased with reaction
time These findings indicate that acetaldehyde speciespromptly undergo further reaction to form a major productethyl acetate whichwas confirmed bymass spectrometry andUV-visible absorption Undoped CeO
2produces negligible
acetaldehyde which is direct evidence that a hydride shiftreaction CH
3CH2O(ad)-MrarrCH
2CHO+MH is an impor-
tant step for acetaldehyde production for metal-loaded CeO2
catalysts For M- (single) doped CeO2NPs the ethanol
oxidation performance showed an order of Ni lt Ag lt Pd ≪Au For MM1015840 codoped CeO
2NPs the activity of Au doped
CeO2deteriorated drastically upon adding another metals
(Ag Ni and Pd) as cocatalyst The Au-rich CeO2catalyst
showed higher catalytic activity On the other hand the NiPd codoped sample showed much higher catalytic activitycompared with the single M- (Ni and Pd) doped samplesThis study provides further insights into the development ofcatalysts applicable to a range of oxidation reactions
Competing Interests
The authors declare no conflict of interests
Acknowledgments
This study was supported by the 2015 Yeungnam UniversityResearch Grant
References
[1] X Nie H Qian Q Ge H Xu and R Jin ldquoCO oxidationcatalyzed by oxide-supported Au
25(SR)18
nanoclusters and
10 Journal of Chemistry
identification of perimeter sites as active centersrdquo ACS Nanovol 6 no 7 pp 6014ndash6022 2012
[2] H-F Li N Zhang P Chen M-F Luo and J-Q Lu ldquoHigh sur-face area AuCeO
2catalysts for low temperature formaldehyde
oxidationrdquoApplied Catalysis B Environmental vol 110 pp 279ndash285 2011
[3] K Y Ho and K L Yeung ldquoEffects of ozone pretreatment on theperformance of AuTiO
2catalyst for CO oxidation reactionrdquo
Journal of Catalysis vol 242 no 1 pp 131ndash141 2006[4] K Y Ho and K L Yeung ldquoProperties of TiO
2support and the
performance of AuTiO2catalyst for CO oxidation reactionrdquo
Gold Bulletin vol 40 no 1 pp 15ndash30 2007[5] J Qi J Chen G Li S Li Y Gao and Z Tang ldquoFacile
synthesis of core-shell AuCeO2nanocomposites with remark-
ably enhanced catalytic activity for CO oxidationrdquo Energy andEnvironmental Science vol 5 no 10 pp 8937ndash8941 2012
[6] D Jiang W Wang L Zhang Y Zheng and Z Wang ldquoInsightsinto the surface-defect dependence of photoreactivity overCeO2nanocrystals with well-defined crystal facetsrdquo ACS Catal-
ysis vol 5 no 8 pp 4851ndash4858 2015[7] W Lei T Zhang L Gu et al ldquoSurface-structure sensitivity
of CeO2nanocrystals in photocatalysis and enhancing the
reactivity with nanogoldrdquo ACS Catalysis vol 5 no 7 pp 4385ndash4393 2015
[8] B Li T Gu T Ming J Wang P Wang and J C Yu ldquoGoldcore)(ceria shell) nanostructures for plasmon-enhanced cat-alytic reactions under visible lightrdquo ACS Nano vol 8 no 8 pp8152ndash8162 2014
[9] P Lu B Qiao N Lu et al ldquoPhotochemical deposition of highlydispersed Pt nanoparticles on porous CeO
2nanofibers for the
water-gas shift reactionrdquoAdvanced FunctionalMaterials vol 25no 26 pp 4153ndash4162 2015
[10] L Meng A-P Jia J-Q Lu L-F Luo W-X Huang and M-FLuo ldquoSynergetic effects of PdO species on CO oxidation overPdO-CeO
2catalystsrdquo Journal of Physical Chemistry C vol 115
no 40 pp 19789ndash19796 2011[11] Y Park S K Kim D Pradhan and Y Sohn ldquoThermal H
2-
treatment effects on COCO2conversion over Pd-doped CeO
2
comparison with Au and Ag-doped CeO2rdquo Reaction Kinetics
Mechanisms and Catalysis vol 113 no 1 pp 85ndash100 2014[12] Y Park S K Kim D Pradhan and Y Sohn ldquoSurface treatment
effects on CO oxidation reactions over Co Cu and Ni-dopedand codopedCeO
2catalystsrdquoChemical Engineering Journal vol
250 pp 25ndash34 2014[13] B Xu Q Zhang S YuanM Zhang and T Ohno ldquoMorphology
control and photocatalytic characterization of yttrium-dopedhedgehog-like CeO
2rdquo Applied Catalysis B Environmental vol
164 pp 120ndash127 2015[14] W Huang and Y Gao ldquoMorphology-dependent surface chem-
istry and catalysis of CeO2nanocrystalsrdquo Catalysis Science and
Technology vol 4 no 11 pp 3772ndash3784 2014[15] Y Gao W Wang S Chang and W Huang ldquoMorphology
effect of CeO2support in the preparation metal-support
interaction and catalytic performance of PtCeO2catalystsrdquo
ChemCatChem vol 5 no 12 pp 3610ndash3620 2013[16] Y Zhang N Zhang Z-R Tang and Y-J Xu ldquoA unique
silk mat-like structured PdCeO2as an efficient visible light
photocatalyst for green organic transformation in waterrdquo ACSSustainable Chemistry amp Engineering vol 1 no 10 pp 1258ndash1266 2013
[17] W G Shin H J Jung H G Sung H S Hyun and YSohn ldquoSynergic CO oxidation activities of boron-CeO
2hybrid
materials prepared by dry and wet milling methodsrdquo CeramicsInternational vol 40 no 8 pp 11511ndash11517 2014
[18] H Wu P Wang H He and Y Jin ldquoControlled synthesisof porous AgAu bimetallic hollow nanoshells with tunableplasmonic and catalytic propertiesrdquo Nano Research vol 5 no2 pp 135ndash144 2012
[19] N Sasirekha P Sangeetha and Y-W Chen ldquoBimetallic AundashAgCeO
2catalysts for preferential oxidation ofCO inhydrogen-
rich stream effect of calcination temperaturerdquo The Journal ofPhysical Chemistry C vol 118 no 28 pp 15226ndash15233 2014
[20] S Chen L Luo Z Jiang and W Huang ldquoSize-dependent reac-tion pathways of low-temperature CO oxidation on AuCeO
2
catalystsrdquo ACS Catalysis vol 5 no 3 pp 1653ndash1662 2015[21] D LiuW Li X Feng andY Zhang ldquoGalvanic replacement syn-
thesis of Ag119909Au1minus119909
CeO2(0 le x le 1) coreshell nanospheres
with greatly enhanced catalytic performancerdquoChemical Sciencevol 6 pp 7015ndash7019 2015
[22] Y Kang M Sun and A Li ldquoStudies of the catalytic oxidationof CO over AgCeO
2catalystrdquo Catalysis Letters vol 142 no 12
pp 1498ndash1504 2012[23] S Chang M Li Q Hua et al ldquoShape-dependent inter-
play between oxygen vacancies and AgndashCeO2interaction in
AgCeO2catalysts and their influence on the catalytic activityrdquo
Journal of Catalysis vol 293 pp 195ndash204 2012[24] R Fiorenza C Crisafulli G G Condorelli F Lupo and S Scire
ldquoAu-AgCeO2and Au-CuCeO
2Catalysts for volatile organic
compounds oxidation and CO preferential oxidationrdquo CatalysisLetters vol 145 no 9 pp 1691ndash1702 2015
[25] J Zhang L Li X Huang and G Li ldquoFabrication of AgndashCeO2
core-shell nanospheres with enhanced catalytic performancedue to strengthening of the interfacial interactionsrdquo Journal ofMaterials Chemistry vol 22 no 21 pp 10480ndash10487 2012
[26] A Leyva-Perez D Combita-Merchan J R Cabrero-AntoninoS I Al-Resayes and A Corma ldquoOxyhalogenation of activatedarenes with nanocrystalline ceriardquo ACS Catalysis vol 3 no 2pp 250ndash258 2013
[27] Y Liu H Li J Yu DMao andG Lu ldquoElectronic storage capac-ity of ceria role of peroxide inAux supported onCeO
2(111) facet
and CO adsorptionrdquo Physical Chemistry Chemical Physics vol17 no 41 pp 27758ndash27768 2015
[28] D Jiang WWang S Sun L Zhang and Y Zheng ldquoEquilibrat-ing the plasmonic and catalytic roles of metallic nanostructuresin photocatalytic oxidation over Au-modified CeO
2rdquo ACS
Catalysis vol 5 no 2 pp 613ndash621 2015[29] M M Khan S A Ansari M O Ansari B K Min J Lee and
M H Cho ldquoBiogenic fabrication of AuCeO2nanocomposite
with enhanced visible light activityrdquo Journal of Physical Chem-istry C vol 118 no 18 pp 9477ndash9484 2014
[30] A Tanaka K Hashimoto and H Kominami ldquoPreparation ofAuCeO
2exhibiting strong surface plasmon resonance effective
for selective or chemoselective oxidation of alcohols to alde-hydes or ketones in aqueous suspensions under irradiation bygreen lightrdquo Journal of the American Chemical Society vol 134no 35 pp 14526ndash14533 2012
[31] H Y Kim H M Lee and G Henkelman ldquoCO oxidationmechanism on CeO
2-supported Au nanoparticlesrdquo Journal of
the American Chemical Society vol 134 no 3 pp 1560ndash15702012
[32] A Maldotti A Molinari R Juarez and H Garcia ldquoPhotoin-duced reactivity of AundashH intermediates in alcohol oxidation by
Journal of Chemistry 11
gold nanoparticles supported on ceriardquoChemical Science vol 2no 9 pp 1831ndash1834 2011
[33] L Vivier andDDuprez ldquoCeria-based solid catalysts for organicchemistryrdquo ChemSusChem vol 3 no 6 pp 654ndash678 2010
[34] N Zhang S Liu X Fu and Y-J Xu ldquoA simple strategy forfabrication of ldquoplum-puddingrdquo type PdCeO
2semiconductor
nanocomposite as a visible-light-driven photocatalyst for selec-tive oxidationrdquo Journal of Physical Chemistry C vol 115 no 46pp 22901ndash22909 2011
[35] Y Sohn ldquoSiO2nanospheres modified by Ag nanoparticles sur-
face charging and CO oxidation activityrdquo Journal of MolecularCatalysis A Chemical vol 379 pp 59ndash67 2013
[36] W J Kim D Pradhan and Y Sohn ldquoFundamental natureand CO oxidation activities of indium oxide nanostructures1D-wires 2D-plates and 3D-cubes and donutsrdquo Journal ofMaterials Chemistry A vol 1 no 35 pp 10193ndash10202 2013
[37] R-R Zhang L-H Ren A-H Lu and W-C Li ldquoInfluence ofpretreatment atmospheres on the activity of AuCeO
2catalyst
for low-temperature CO oxidationrdquo Catalysis Communicationsvol 13 no 1 pp 18ndash21 2011
[38] Y Li Y Cai X Xing N Chen D Deng and YWang ldquoCatalyticactivity for CO oxidation of CundashCeO
2composite nanoparticles
synthesized by a hydrothermal methodrdquo Analytical Methodsvol 7 no 7 pp 3238ndash3245 2015
[39] R Shang Y Duan X Zhong W Xie Y Luo and L HuangldquoFormic acid modified Co
3O4-CeO
2catalysts for CO oxida-
tionrdquo Catalysts vol 6 no 3 p 48 2016[40] A Abad P Concepcion A Corma and H Garcıa ldquoA collab-
orative effect between gold and a support induces the selectiveoxidation of alcoholsrdquo Angewandte ChemiemdashInternational Edi-tion vol 44 no 26 pp 4066ndash4069 2005
Submit your manuscripts athttpwwwhindawicom
Hindawi Publishing Corporationhttpwwwhindawicom Volume 2014
Inorganic ChemistryInternational Journal of
Hindawi Publishing Corporation httpwwwhindawicom Volume 2014
International Journal ofPhotoenergy
Hindawi Publishing Corporationhttpwwwhindawicom Volume 2014
Carbohydrate Chemistry
International Journal of
Hindawi Publishing Corporationhttpwwwhindawicom Volume 2014
Journal of
Chemistry
Hindawi Publishing Corporationhttpwwwhindawicom Volume 2014
Advances in
Physical Chemistry
Hindawi Publishing Corporationhttpwwwhindawicom
Analytical Methods in Chemistry
Journal of
Volume 2014
Bioinorganic Chemistry and ApplicationsHindawi Publishing Corporationhttpwwwhindawicom Volume 2014
SpectroscopyInternational Journal of
Hindawi Publishing Corporationhttpwwwhindawicom Volume 2014
The Scientific World JournalHindawi Publishing Corporation httpwwwhindawicom Volume 2014
Medicinal ChemistryInternational Journal of
Hindawi Publishing Corporationhttpwwwhindawicom Volume 2014
Chromatography Research International
Hindawi Publishing Corporationhttpwwwhindawicom Volume 2014
Applied ChemistryJournal of
Hindawi Publishing Corporationhttpwwwhindawicom Volume 2014
Hindawi Publishing Corporationhttpwwwhindawicom Volume 2014
Theoretical ChemistryJournal of
Hindawi Publishing Corporationhttpwwwhindawicom Volume 2014
Journal of
Spectroscopy
Analytical ChemistryInternational Journal of
Hindawi Publishing Corporationhttpwwwhindawicom Volume 2014
Journal of
Hindawi Publishing Corporationhttpwwwhindawicom Volume 2014
Quantum Chemistry
Hindawi Publishing Corporationhttpwwwhindawicom Volume 2014
Organic Chemistry International
ElectrochemistryInternational Journal of
Hindawi Publishing Corporation httpwwwhindawicom Volume 2014
Hindawi Publishing Corporationhttpwwwhindawicom Volume 2014
CatalystsJournal of
Journal of Chemistry 7
Rxn in 5 daysat 80∘C
Wavelength (nm)350300250
Wavelength (nm)
350300250Wavelength (nm)
350300250
Doped Ag AuAb
sorb
ance
(arb
uni
t)
10
05
00
15
00
01
02
03
04
Abso
rban
ce (a
rb u
nit)
0
1
2
3
4
5
Abso
rban
ce (a
rb u
nit)
With reaction timeat 80
∘C5 days4 days3 days2 days1 day (24h)8 h4hAu-(5mol) CeO2
Au = 5molNo catalyst
Ag = 5 molCeO21 mol 4 mol
25 mol 25 mol
4 mol 1 mol
O
O
O
(a)
O
O
O
Au = 5mol
Rxn in 5 daysat 80∘C
at 80∘C
0
1
2
3
4
5
Abso
rban
ce (a
rb u
nit)
Wavelength (nm)350300250
Wavelength (nm)
350300250
Doped Ni Au
Rxn in 24 hrs
Abso
rban
ce (a
rb u
nit)
10
05
00
15
1 mol 4 mol25 mol 25 mol
Ni = 5 mol4 mol 1 mol
(b)
O
O
O
Au = 5mol
Rxn in 5 daysat 80∘C
at 80∘C
0
1
2
3
4
5
Abso
rban
ce (a
rb u
nit)
Wavelength (nm)350300250
Wavelength (nm)
350300250
Doped Pd Au
Rxn in 24 hrs
Abso
rban
ce (a
rb u
nit)
10
05
00
15
1 mol 4 mol25 mol 25 mol
Pd = 5 mol4 mol 1 mol
(c)
O
O
O
Au = 5mol
Rxn in 5 daysat 80∘C
at 80∘C
Wavelength (nm)350300250
Wavelength (nm)
350300250
Doped Ni Pd
Rxn in 24 hrs
Abso
rban
ce (a
rb u
nit)
10
05
00
15
0
1
2
3
4
5
Abso
rban
ce (a
rb u
nit)
1 mol 4 mol25 mol 25 mol
Pd = 5 molNi = 5 mol
4 mol 1 mol
(d)
Figure 7 UV-visible absorption spectra of the ethanol oxidation with no catalyst undoped CeO2 M doped (M = Ag Au Pd and Ni) and
MM1015840 codoped (AgAu (a) NiAu (b) PdAu (c) and NiPd (d)) CeO2catalysts at 80∘C for 5 days The left inset in (a) shows the magnified
spectra of the grey shadowed region The right inset in (a) shows the UV-Vis absorption spectra of ethanol oxidation with the 5mol Audoped CeO
2catalyst at 80∘C according to the reaction time
increasing reaction temperatureWithout catalysts no signif-icant ethanol oxidation occurred even at high temperatureFor further ethanol oxidation experiments we selected areaction temperature of 80∘C and a total metal-doping levelof 5mol
For Ag and Au doped and codoped samples (Figure 7(a))a strong absorption peak (below 250 nm) was observed forthe Au (5mol) and AuAg (14mol) doped CeO
2cata-
lysts Without a catalyst no significant absorption peak was
observed even after 5 days The absorption peak (shown inthe right inset of Figure 7(a)) increased with increasingreaction time This was attributed to an increase in reactionproducts that contain C=C andor C=O functional groupsFor the other metal doped samples the absorption peakswere much weaker In addition to the strong absorptionpeak a weaker peak at 280 nm was also observed (in theleft inset of Figure 7) The results suggest that at least tworeaction products (EA and AcA as mentioned above) were
8 Journal of Chemistry
present in the ethanol solution The catalytic activity wasobserved to be in the order of bare CeO
2asymp 2525 lt 41 lt
50 ≪ 14 lt 05 (AgAumol) When the concentration ofAu was the same as or lower than that of Ag the activitydeteriorated drastically For Au and Ni doped and codopedsamples (Figure 7(b)) the catalytic activity was decreasedupon adding Ni as a cocatalyst The activity was found to bein the order of 50 lt 41≪ 2525 lt 14 lt 05 (NiAumol)For Au and Pd doped and codoped samples (Figure 7(c))the oxidation performance was more greatly decreased uponadding Pd as a cocatalyst and found to be in the order of 41 le2525asymp 14asymp 50≪ 05 (PdAumol) ForNi and Pd dopedand codoped samples (Figure 7(d)) the catalytic activity wasobserved to be in the order of 50 lt 05≪ 41 asymp 14 le 2525(NiPdmol) The catalytic activity of the NiPd codopedsamples showed much higher catalytic activity than those ofthe single M- (Ni and Pd) doped samples For comparisonof the catalytic activities of single M doped CeO
2NPs the
ethanol oxidation performance showed an order of undopedasympNi ltAg lt Pd≪Au Interestingly the Ni-doping showed noincrease in catalytic activity for ethanol oxidation
For ethanol oxidation on a metal doped CeO2power
sample since the reaction mechanism was much more com-plicated than expected on a single crystal surface we proposethe following simplified mechanisms which are discussed ingreater detail below [32]
Acetaldehyde hemiacetal and ethyl acetate formationfrom ethanol is as follows
CH3CH2OndashH 997888rarr CH
3CH2O (ad) +H (ad) (1)
CH3CH2O (ad) +O species
997888rarr CH3CHO (ad) +OH (ad)
(2)
CH3CH2O (ad) ndashM
997888rarr CH3CHO (minor) +MH hydride shift
(3)
CH3CHO +O (ad) 997888rarr CH
3COO (ad) +H (ad)
997888rarr CH3COOH
(4)
CH3COOH (ad) + CH3CH2OH (ad)
997888rarr CH3COOCH
2CH3+H2O
(5)
2CH3CHO (ad) 997888rarr CH
3COOCH
2CH3 (6)
CH3CHO (ad) + CH3CH2OH (ad)
997888rarr CH3CH (OH)OC
2H5 (hemiacetal)
997888rarr CH3COOCH
2CH3(major) +H
2
(7)
The rate constant for each step is controlled by the surfacearea and metal-support interaction (or surface activity) Inreaction (1) the OndashH bond of ethanol dissociates to formCH3CH2O which may be mainly adsorbed onto the doped
metal siteThis then turns into adsorbedCH3CHOvia nearby
active oxygen species in (2) or the adsorbed CH3CH2O on
metal desorbs as CH3CHO (acetaldehyde) in response to a
hydride shift reaction in (3) [32 40] Although we have nodirect evidence of the hydride shift reaction the reactionprocess is highly plausible The acetaldehyde in (4) furtherprecedes oxidation reactions to form CH
3COOH (acetic
acid) if active oxygen species are available nearby Otherwisethe CH
3COOH with ethanol in (5) and 2CH
3CHO in (6)
react to form CH3COOCH
2CH3(ethyl acetate) In reaction
(7) CH3CHO and ethanol formCH
3CH(OH)OC
2H5(hemi-
acetal) which is converted to ethyl acetate Consequentlyethyl acetate (CH
3COOCH
2CH3) is formed as a final oxi-
dation product which was confirmed by mass spectrometryIn the present UV-Vis spectra two products of ethyl acetate(major) and acetaldehyde (minor) were observed For alcoholoxidation on the Au-CeO
2catalyst Maldotti et al reported
that the Au-H species is an important intermediate [32] Thisindicates that the hydride shift reaction is facilitated by activedopedmetalsThe present study showed that the Au-rich cat-alyst produced much higher oxidation products and the Auspecies is more active than other metal species (Ag Ni andPd)The reference UV-Vis spectra (Figure 8(a)) were checkedfor four plausible ethanol oxidation products acetaldehydeethyl acetate acetone and acetic acid and the stronger andweaker peak positions near 220 and 280 nm were assignedto the UV-Vis absorptions of ethyl acetate and acetaldehyderespectively Figure 8(b) displays the mass spectrum of thesolution sample after reaction relative to those of the referencesolvents (ethyl acetate and ethanol) As shown in the massspectrum the oxidation product in ethanol matched thatof the reference ethyl acetate well In addition the smell ofthe two samples was very similar As a result we concludedthat the final major product was ethyl acetate For someother extra mass fragmentation signals (59 73 and 75 amu)although no reference data were available the fragmentationsappeared to form from the hemiacetal as shown in reaction(7) Abad et al extensively studied oxidation of alcoholscatalyzed by AuCeO
2[40] and proposed a reaction of (7)
mentioned above in which hemiacetal was detected by H-NMR We have excluded diethyl ether as a major producteven though it could be formed by 2C
2H5OHrarrC
2H5OC2H5
+ H2O because the UV-visible absorption intensity (even
measuredwith 50 solution) was extremely low (Figure 8(a))when compared with that of the sample We also detected nofragmentation signals of diethyl ether by mass spectrometryThe acetone formation reaction 2CH
3CHOrarr CH
3COCH
3
(acetone) + CO2+ H2 was excluded due to absence of the
mass signal Acetic acid as a major product was also excludedbecause the solution is not acidic the mass signal is absentand it did not smell like acetic acid Table 1 summarizes thesizes of the metal-loaded CeO
2estimated using Scherrerrsquos
equation As for the CO oxidation the ethanol oxidationactivity was also found to be more loaded metal (and therelative concentrations) dependent than the size-dependent
4 Conclusion
To increase the catalytic activity of bare CeO2 the CeO
2
matrix was doped and codoped with Ag Au Pd and Ni bya hydrothermal method The novelty of the present study
Journal of Chemistry 9
Table 1 Particles sizes of the metal-loaded CeO2estimated using Scherrerrsquos equation
Loaded MM1015840 50mol (nm) 41mol (nm) 2525mol (nm) 14mol (nm) 05mol (nm)Ag Au 140 124 80 100 86Ni Au 152 123 106 82 86Pd Au 151 127 121 90 86Ni Pd 152 111 147 121 151
Catalysts without stirring
Tightly capped
OOH
O
O
O
lowast
lowast
O
OH
OHO
OO
Abso
rban
ce
10
05
00
Diethyl ether 50
Different smellAcetaldehyde sim1
Acetone sim1
Different smellAcetic acid 01
Ethyl acetate 01
Wavelength (nm)400350300250
(a)
Ethyl acetate(reference)
O
O
Mass (amu)1009080706050M
ass s
igna
l (au
)
OH Before reaction(ETOH)
50 60
Mass (amu)70 80 90 100M
ass s
igna
l (au
)
Afterreaction
01234
UV-VisO
O
Mass (amu)1009080706050M
ass s
igna
l (au
)
Abso
rban
ce
250 300Wavelength (nm)
(b)
Figure 8 UV-Vis absorption spectra (a) of standard samples of acetaldehyde (1) acetone (1) acetic acid (01) and ethyl acetate (01)Mass spectra (b) of reference samples (ethyl acetate and ethanol) and the solution sample after reactionThe inset shows theUV-Vis absorptionspectrum of the corresponding sample solution Blue and red lowast indicate the peak positions for acetaldehyde and ethyl acetate respectively
was that the catalytic efficiency of doped and codoped CeO2
was tested for both gas-phase CO and liquid-phase ethanoloxidation reactions For the 1st and 2nd runs of bare CeO
2
T10 was observed at 405∘C T
10 of bare CeO2for CO oxi-
dation was lowered significantly by 165∘C uponmetal (AgAu= 14mol) doping There were some synergic effects uponcodoping for the CO oxidation The CO oxidation activityvaries with the relative concentrations of two differentmetalsSintering and alloying of two different metals were found toplay important roles in the CO oxidation activity
For liquid-phase ethanol oxidation two liquid productsof ethyl acetate (major 120582max = 220 nm) and acetaldehyde(minor 120582max = 280 nm) were observed by UV-Vis absorptionspectroscopyThe concentration of acetaldehyde (CH
3CHO)
reached a saturation point while that of ethyl acetate(CH3COOCH
2CH3) dramatically increased with reaction
time These findings indicate that acetaldehyde speciespromptly undergo further reaction to form a major productethyl acetate whichwas confirmed bymass spectrometry andUV-visible absorption Undoped CeO
2produces negligible
acetaldehyde which is direct evidence that a hydride shiftreaction CH
3CH2O(ad)-MrarrCH
2CHO+MH is an impor-
tant step for acetaldehyde production for metal-loaded CeO2
catalysts For M- (single) doped CeO2NPs the ethanol
oxidation performance showed an order of Ni lt Ag lt Pd ≪Au For MM1015840 codoped CeO
2NPs the activity of Au doped
CeO2deteriorated drastically upon adding another metals
(Ag Ni and Pd) as cocatalyst The Au-rich CeO2catalyst
showed higher catalytic activity On the other hand the NiPd codoped sample showed much higher catalytic activitycompared with the single M- (Ni and Pd) doped samplesThis study provides further insights into the development ofcatalysts applicable to a range of oxidation reactions
Competing Interests
The authors declare no conflict of interests
Acknowledgments
This study was supported by the 2015 Yeungnam UniversityResearch Grant
References
[1] X Nie H Qian Q Ge H Xu and R Jin ldquoCO oxidationcatalyzed by oxide-supported Au
25(SR)18
nanoclusters and
10 Journal of Chemistry
identification of perimeter sites as active centersrdquo ACS Nanovol 6 no 7 pp 6014ndash6022 2012
[2] H-F Li N Zhang P Chen M-F Luo and J-Q Lu ldquoHigh sur-face area AuCeO
2catalysts for low temperature formaldehyde
oxidationrdquoApplied Catalysis B Environmental vol 110 pp 279ndash285 2011
[3] K Y Ho and K L Yeung ldquoEffects of ozone pretreatment on theperformance of AuTiO
2catalyst for CO oxidation reactionrdquo
Journal of Catalysis vol 242 no 1 pp 131ndash141 2006[4] K Y Ho and K L Yeung ldquoProperties of TiO
2support and the
performance of AuTiO2catalyst for CO oxidation reactionrdquo
Gold Bulletin vol 40 no 1 pp 15ndash30 2007[5] J Qi J Chen G Li S Li Y Gao and Z Tang ldquoFacile
synthesis of core-shell AuCeO2nanocomposites with remark-
ably enhanced catalytic activity for CO oxidationrdquo Energy andEnvironmental Science vol 5 no 10 pp 8937ndash8941 2012
[6] D Jiang W Wang L Zhang Y Zheng and Z Wang ldquoInsightsinto the surface-defect dependence of photoreactivity overCeO2nanocrystals with well-defined crystal facetsrdquo ACS Catal-
ysis vol 5 no 8 pp 4851ndash4858 2015[7] W Lei T Zhang L Gu et al ldquoSurface-structure sensitivity
of CeO2nanocrystals in photocatalysis and enhancing the
reactivity with nanogoldrdquo ACS Catalysis vol 5 no 7 pp 4385ndash4393 2015
[8] B Li T Gu T Ming J Wang P Wang and J C Yu ldquoGoldcore)(ceria shell) nanostructures for plasmon-enhanced cat-alytic reactions under visible lightrdquo ACS Nano vol 8 no 8 pp8152ndash8162 2014
[9] P Lu B Qiao N Lu et al ldquoPhotochemical deposition of highlydispersed Pt nanoparticles on porous CeO
2nanofibers for the
water-gas shift reactionrdquoAdvanced FunctionalMaterials vol 25no 26 pp 4153ndash4162 2015
[10] L Meng A-P Jia J-Q Lu L-F Luo W-X Huang and M-FLuo ldquoSynergetic effects of PdO species on CO oxidation overPdO-CeO
2catalystsrdquo Journal of Physical Chemistry C vol 115
no 40 pp 19789ndash19796 2011[11] Y Park S K Kim D Pradhan and Y Sohn ldquoThermal H
2-
treatment effects on COCO2conversion over Pd-doped CeO
2
comparison with Au and Ag-doped CeO2rdquo Reaction Kinetics
Mechanisms and Catalysis vol 113 no 1 pp 85ndash100 2014[12] Y Park S K Kim D Pradhan and Y Sohn ldquoSurface treatment
effects on CO oxidation reactions over Co Cu and Ni-dopedand codopedCeO
2catalystsrdquoChemical Engineering Journal vol
250 pp 25ndash34 2014[13] B Xu Q Zhang S YuanM Zhang and T Ohno ldquoMorphology
control and photocatalytic characterization of yttrium-dopedhedgehog-like CeO
2rdquo Applied Catalysis B Environmental vol
164 pp 120ndash127 2015[14] W Huang and Y Gao ldquoMorphology-dependent surface chem-
istry and catalysis of CeO2nanocrystalsrdquo Catalysis Science and
Technology vol 4 no 11 pp 3772ndash3784 2014[15] Y Gao W Wang S Chang and W Huang ldquoMorphology
effect of CeO2support in the preparation metal-support
interaction and catalytic performance of PtCeO2catalystsrdquo
ChemCatChem vol 5 no 12 pp 3610ndash3620 2013[16] Y Zhang N Zhang Z-R Tang and Y-J Xu ldquoA unique
silk mat-like structured PdCeO2as an efficient visible light
photocatalyst for green organic transformation in waterrdquo ACSSustainable Chemistry amp Engineering vol 1 no 10 pp 1258ndash1266 2013
[17] W G Shin H J Jung H G Sung H S Hyun and YSohn ldquoSynergic CO oxidation activities of boron-CeO
2hybrid
materials prepared by dry and wet milling methodsrdquo CeramicsInternational vol 40 no 8 pp 11511ndash11517 2014
[18] H Wu P Wang H He and Y Jin ldquoControlled synthesisof porous AgAu bimetallic hollow nanoshells with tunableplasmonic and catalytic propertiesrdquo Nano Research vol 5 no2 pp 135ndash144 2012
[19] N Sasirekha P Sangeetha and Y-W Chen ldquoBimetallic AundashAgCeO
2catalysts for preferential oxidation ofCO inhydrogen-
rich stream effect of calcination temperaturerdquo The Journal ofPhysical Chemistry C vol 118 no 28 pp 15226ndash15233 2014
[20] S Chen L Luo Z Jiang and W Huang ldquoSize-dependent reac-tion pathways of low-temperature CO oxidation on AuCeO
2
catalystsrdquo ACS Catalysis vol 5 no 3 pp 1653ndash1662 2015[21] D LiuW Li X Feng andY Zhang ldquoGalvanic replacement syn-
thesis of Ag119909Au1minus119909
CeO2(0 le x le 1) coreshell nanospheres
with greatly enhanced catalytic performancerdquoChemical Sciencevol 6 pp 7015ndash7019 2015
[22] Y Kang M Sun and A Li ldquoStudies of the catalytic oxidationof CO over AgCeO
2catalystrdquo Catalysis Letters vol 142 no 12
pp 1498ndash1504 2012[23] S Chang M Li Q Hua et al ldquoShape-dependent inter-
play between oxygen vacancies and AgndashCeO2interaction in
AgCeO2catalysts and their influence on the catalytic activityrdquo
Journal of Catalysis vol 293 pp 195ndash204 2012[24] R Fiorenza C Crisafulli G G Condorelli F Lupo and S Scire
ldquoAu-AgCeO2and Au-CuCeO
2Catalysts for volatile organic
compounds oxidation and CO preferential oxidationrdquo CatalysisLetters vol 145 no 9 pp 1691ndash1702 2015
[25] J Zhang L Li X Huang and G Li ldquoFabrication of AgndashCeO2
core-shell nanospheres with enhanced catalytic performancedue to strengthening of the interfacial interactionsrdquo Journal ofMaterials Chemistry vol 22 no 21 pp 10480ndash10487 2012
[26] A Leyva-Perez D Combita-Merchan J R Cabrero-AntoninoS I Al-Resayes and A Corma ldquoOxyhalogenation of activatedarenes with nanocrystalline ceriardquo ACS Catalysis vol 3 no 2pp 250ndash258 2013
[27] Y Liu H Li J Yu DMao andG Lu ldquoElectronic storage capac-ity of ceria role of peroxide inAux supported onCeO
2(111) facet
and CO adsorptionrdquo Physical Chemistry Chemical Physics vol17 no 41 pp 27758ndash27768 2015
[28] D Jiang WWang S Sun L Zhang and Y Zheng ldquoEquilibrat-ing the plasmonic and catalytic roles of metallic nanostructuresin photocatalytic oxidation over Au-modified CeO
2rdquo ACS
Catalysis vol 5 no 2 pp 613ndash621 2015[29] M M Khan S A Ansari M O Ansari B K Min J Lee and
M H Cho ldquoBiogenic fabrication of AuCeO2nanocomposite
with enhanced visible light activityrdquo Journal of Physical Chem-istry C vol 118 no 18 pp 9477ndash9484 2014
[30] A Tanaka K Hashimoto and H Kominami ldquoPreparation ofAuCeO
2exhibiting strong surface plasmon resonance effective
for selective or chemoselective oxidation of alcohols to alde-hydes or ketones in aqueous suspensions under irradiation bygreen lightrdquo Journal of the American Chemical Society vol 134no 35 pp 14526ndash14533 2012
[31] H Y Kim H M Lee and G Henkelman ldquoCO oxidationmechanism on CeO
2-supported Au nanoparticlesrdquo Journal of
the American Chemical Society vol 134 no 3 pp 1560ndash15702012
[32] A Maldotti A Molinari R Juarez and H Garcia ldquoPhotoin-duced reactivity of AundashH intermediates in alcohol oxidation by
Journal of Chemistry 11
gold nanoparticles supported on ceriardquoChemical Science vol 2no 9 pp 1831ndash1834 2011
[33] L Vivier andDDuprez ldquoCeria-based solid catalysts for organicchemistryrdquo ChemSusChem vol 3 no 6 pp 654ndash678 2010
[34] N Zhang S Liu X Fu and Y-J Xu ldquoA simple strategy forfabrication of ldquoplum-puddingrdquo type PdCeO
2semiconductor
nanocomposite as a visible-light-driven photocatalyst for selec-tive oxidationrdquo Journal of Physical Chemistry C vol 115 no 46pp 22901ndash22909 2011
[35] Y Sohn ldquoSiO2nanospheres modified by Ag nanoparticles sur-
face charging and CO oxidation activityrdquo Journal of MolecularCatalysis A Chemical vol 379 pp 59ndash67 2013
[36] W J Kim D Pradhan and Y Sohn ldquoFundamental natureand CO oxidation activities of indium oxide nanostructures1D-wires 2D-plates and 3D-cubes and donutsrdquo Journal ofMaterials Chemistry A vol 1 no 35 pp 10193ndash10202 2013
[37] R-R Zhang L-H Ren A-H Lu and W-C Li ldquoInfluence ofpretreatment atmospheres on the activity of AuCeO
2catalyst
for low-temperature CO oxidationrdquo Catalysis Communicationsvol 13 no 1 pp 18ndash21 2011
[38] Y Li Y Cai X Xing N Chen D Deng and YWang ldquoCatalyticactivity for CO oxidation of CundashCeO
2composite nanoparticles
synthesized by a hydrothermal methodrdquo Analytical Methodsvol 7 no 7 pp 3238ndash3245 2015
[39] R Shang Y Duan X Zhong W Xie Y Luo and L HuangldquoFormic acid modified Co
3O4-CeO
2catalysts for CO oxida-
tionrdquo Catalysts vol 6 no 3 p 48 2016[40] A Abad P Concepcion A Corma and H Garcıa ldquoA collab-
orative effect between gold and a support induces the selectiveoxidation of alcoholsrdquo Angewandte ChemiemdashInternational Edi-tion vol 44 no 26 pp 4066ndash4069 2005
Submit your manuscripts athttpwwwhindawicom
Hindawi Publishing Corporationhttpwwwhindawicom Volume 2014
Inorganic ChemistryInternational Journal of
Hindawi Publishing Corporation httpwwwhindawicom Volume 2014
International Journal ofPhotoenergy
Hindawi Publishing Corporationhttpwwwhindawicom Volume 2014
Carbohydrate Chemistry
International Journal of
Hindawi Publishing Corporationhttpwwwhindawicom Volume 2014
Journal of
Chemistry
Hindawi Publishing Corporationhttpwwwhindawicom Volume 2014
Advances in
Physical Chemistry
Hindawi Publishing Corporationhttpwwwhindawicom
Analytical Methods in Chemistry
Journal of
Volume 2014
Bioinorganic Chemistry and ApplicationsHindawi Publishing Corporationhttpwwwhindawicom Volume 2014
SpectroscopyInternational Journal of
Hindawi Publishing Corporationhttpwwwhindawicom Volume 2014
The Scientific World JournalHindawi Publishing Corporation httpwwwhindawicom Volume 2014
Medicinal ChemistryInternational Journal of
Hindawi Publishing Corporationhttpwwwhindawicom Volume 2014
Chromatography Research International
Hindawi Publishing Corporationhttpwwwhindawicom Volume 2014
Applied ChemistryJournal of
Hindawi Publishing Corporationhttpwwwhindawicom Volume 2014
Hindawi Publishing Corporationhttpwwwhindawicom Volume 2014
Theoretical ChemistryJournal of
Hindawi Publishing Corporationhttpwwwhindawicom Volume 2014
Journal of
Spectroscopy
Analytical ChemistryInternational Journal of
Hindawi Publishing Corporationhttpwwwhindawicom Volume 2014
Journal of
Hindawi Publishing Corporationhttpwwwhindawicom Volume 2014
Quantum Chemistry
Hindawi Publishing Corporationhttpwwwhindawicom Volume 2014
Organic Chemistry International
ElectrochemistryInternational Journal of
Hindawi Publishing Corporation httpwwwhindawicom Volume 2014
Hindawi Publishing Corporationhttpwwwhindawicom Volume 2014
CatalystsJournal of
8 Journal of Chemistry
present in the ethanol solution The catalytic activity wasobserved to be in the order of bare CeO
2asymp 2525 lt 41 lt
50 ≪ 14 lt 05 (AgAumol) When the concentration ofAu was the same as or lower than that of Ag the activitydeteriorated drastically For Au and Ni doped and codopedsamples (Figure 7(b)) the catalytic activity was decreasedupon adding Ni as a cocatalyst The activity was found to bein the order of 50 lt 41≪ 2525 lt 14 lt 05 (NiAumol)For Au and Pd doped and codoped samples (Figure 7(c))the oxidation performance was more greatly decreased uponadding Pd as a cocatalyst and found to be in the order of 41 le2525asymp 14asymp 50≪ 05 (PdAumol) ForNi and Pd dopedand codoped samples (Figure 7(d)) the catalytic activity wasobserved to be in the order of 50 lt 05≪ 41 asymp 14 le 2525(NiPdmol) The catalytic activity of the NiPd codopedsamples showed much higher catalytic activity than those ofthe single M- (Ni and Pd) doped samples For comparisonof the catalytic activities of single M doped CeO
2NPs the
ethanol oxidation performance showed an order of undopedasympNi ltAg lt Pd≪Au Interestingly the Ni-doping showed noincrease in catalytic activity for ethanol oxidation
For ethanol oxidation on a metal doped CeO2power
sample since the reaction mechanism was much more com-plicated than expected on a single crystal surface we proposethe following simplified mechanisms which are discussed ingreater detail below [32]
Acetaldehyde hemiacetal and ethyl acetate formationfrom ethanol is as follows
CH3CH2OndashH 997888rarr CH
3CH2O (ad) +H (ad) (1)
CH3CH2O (ad) +O species
997888rarr CH3CHO (ad) +OH (ad)
(2)
CH3CH2O (ad) ndashM
997888rarr CH3CHO (minor) +MH hydride shift
(3)
CH3CHO +O (ad) 997888rarr CH
3COO (ad) +H (ad)
997888rarr CH3COOH
(4)
CH3COOH (ad) + CH3CH2OH (ad)
997888rarr CH3COOCH
2CH3+H2O
(5)
2CH3CHO (ad) 997888rarr CH
3COOCH
2CH3 (6)
CH3CHO (ad) + CH3CH2OH (ad)
997888rarr CH3CH (OH)OC
2H5 (hemiacetal)
997888rarr CH3COOCH
2CH3(major) +H
2
(7)
The rate constant for each step is controlled by the surfacearea and metal-support interaction (or surface activity) Inreaction (1) the OndashH bond of ethanol dissociates to formCH3CH2O which may be mainly adsorbed onto the doped
metal siteThis then turns into adsorbedCH3CHOvia nearby
active oxygen species in (2) or the adsorbed CH3CH2O on
metal desorbs as CH3CHO (acetaldehyde) in response to a
hydride shift reaction in (3) [32 40] Although we have nodirect evidence of the hydride shift reaction the reactionprocess is highly plausible The acetaldehyde in (4) furtherprecedes oxidation reactions to form CH
3COOH (acetic
acid) if active oxygen species are available nearby Otherwisethe CH
3COOH with ethanol in (5) and 2CH
3CHO in (6)
react to form CH3COOCH
2CH3(ethyl acetate) In reaction
(7) CH3CHO and ethanol formCH
3CH(OH)OC
2H5(hemi-
acetal) which is converted to ethyl acetate Consequentlyethyl acetate (CH
3COOCH
2CH3) is formed as a final oxi-
dation product which was confirmed by mass spectrometryIn the present UV-Vis spectra two products of ethyl acetate(major) and acetaldehyde (minor) were observed For alcoholoxidation on the Au-CeO
2catalyst Maldotti et al reported
that the Au-H species is an important intermediate [32] Thisindicates that the hydride shift reaction is facilitated by activedopedmetalsThe present study showed that the Au-rich cat-alyst produced much higher oxidation products and the Auspecies is more active than other metal species (Ag Ni andPd)The reference UV-Vis spectra (Figure 8(a)) were checkedfor four plausible ethanol oxidation products acetaldehydeethyl acetate acetone and acetic acid and the stronger andweaker peak positions near 220 and 280 nm were assignedto the UV-Vis absorptions of ethyl acetate and acetaldehyderespectively Figure 8(b) displays the mass spectrum of thesolution sample after reaction relative to those of the referencesolvents (ethyl acetate and ethanol) As shown in the massspectrum the oxidation product in ethanol matched thatof the reference ethyl acetate well In addition the smell ofthe two samples was very similar As a result we concludedthat the final major product was ethyl acetate For someother extra mass fragmentation signals (59 73 and 75 amu)although no reference data were available the fragmentationsappeared to form from the hemiacetal as shown in reaction(7) Abad et al extensively studied oxidation of alcoholscatalyzed by AuCeO
2[40] and proposed a reaction of (7)
mentioned above in which hemiacetal was detected by H-NMR We have excluded diethyl ether as a major producteven though it could be formed by 2C
2H5OHrarrC
2H5OC2H5
+ H2O because the UV-visible absorption intensity (even
measuredwith 50 solution) was extremely low (Figure 8(a))when compared with that of the sample We also detected nofragmentation signals of diethyl ether by mass spectrometryThe acetone formation reaction 2CH
3CHOrarr CH
3COCH
3
(acetone) + CO2+ H2 was excluded due to absence of the
mass signal Acetic acid as a major product was also excludedbecause the solution is not acidic the mass signal is absentand it did not smell like acetic acid Table 1 summarizes thesizes of the metal-loaded CeO
2estimated using Scherrerrsquos
equation As for the CO oxidation the ethanol oxidationactivity was also found to be more loaded metal (and therelative concentrations) dependent than the size-dependent
4 Conclusion
To increase the catalytic activity of bare CeO2 the CeO
2
matrix was doped and codoped with Ag Au Pd and Ni bya hydrothermal method The novelty of the present study
Journal of Chemistry 9
Table 1 Particles sizes of the metal-loaded CeO2estimated using Scherrerrsquos equation
Loaded MM1015840 50mol (nm) 41mol (nm) 2525mol (nm) 14mol (nm) 05mol (nm)Ag Au 140 124 80 100 86Ni Au 152 123 106 82 86Pd Au 151 127 121 90 86Ni Pd 152 111 147 121 151
Catalysts without stirring
Tightly capped
OOH
O
O
O
lowast
lowast
O
OH
OHO
OO
Abso
rban
ce
10
05
00
Diethyl ether 50
Different smellAcetaldehyde sim1
Acetone sim1
Different smellAcetic acid 01
Ethyl acetate 01
Wavelength (nm)400350300250
(a)
Ethyl acetate(reference)
O
O
Mass (amu)1009080706050M
ass s
igna
l (au
)
OH Before reaction(ETOH)
50 60
Mass (amu)70 80 90 100M
ass s
igna
l (au
)
Afterreaction
01234
UV-VisO
O
Mass (amu)1009080706050M
ass s
igna
l (au
)
Abso
rban
ce
250 300Wavelength (nm)
(b)
Figure 8 UV-Vis absorption spectra (a) of standard samples of acetaldehyde (1) acetone (1) acetic acid (01) and ethyl acetate (01)Mass spectra (b) of reference samples (ethyl acetate and ethanol) and the solution sample after reactionThe inset shows theUV-Vis absorptionspectrum of the corresponding sample solution Blue and red lowast indicate the peak positions for acetaldehyde and ethyl acetate respectively
was that the catalytic efficiency of doped and codoped CeO2
was tested for both gas-phase CO and liquid-phase ethanoloxidation reactions For the 1st and 2nd runs of bare CeO
2
T10 was observed at 405∘C T
10 of bare CeO2for CO oxi-
dation was lowered significantly by 165∘C uponmetal (AgAu= 14mol) doping There were some synergic effects uponcodoping for the CO oxidation The CO oxidation activityvaries with the relative concentrations of two differentmetalsSintering and alloying of two different metals were found toplay important roles in the CO oxidation activity
For liquid-phase ethanol oxidation two liquid productsof ethyl acetate (major 120582max = 220 nm) and acetaldehyde(minor 120582max = 280 nm) were observed by UV-Vis absorptionspectroscopyThe concentration of acetaldehyde (CH
3CHO)
reached a saturation point while that of ethyl acetate(CH3COOCH
2CH3) dramatically increased with reaction
time These findings indicate that acetaldehyde speciespromptly undergo further reaction to form a major productethyl acetate whichwas confirmed bymass spectrometry andUV-visible absorption Undoped CeO
2produces negligible
acetaldehyde which is direct evidence that a hydride shiftreaction CH
3CH2O(ad)-MrarrCH
2CHO+MH is an impor-
tant step for acetaldehyde production for metal-loaded CeO2
catalysts For M- (single) doped CeO2NPs the ethanol
oxidation performance showed an order of Ni lt Ag lt Pd ≪Au For MM1015840 codoped CeO
2NPs the activity of Au doped
CeO2deteriorated drastically upon adding another metals
(Ag Ni and Pd) as cocatalyst The Au-rich CeO2catalyst
showed higher catalytic activity On the other hand the NiPd codoped sample showed much higher catalytic activitycompared with the single M- (Ni and Pd) doped samplesThis study provides further insights into the development ofcatalysts applicable to a range of oxidation reactions
Competing Interests
The authors declare no conflict of interests
Acknowledgments
This study was supported by the 2015 Yeungnam UniversityResearch Grant
References
[1] X Nie H Qian Q Ge H Xu and R Jin ldquoCO oxidationcatalyzed by oxide-supported Au
25(SR)18
nanoclusters and
10 Journal of Chemistry
identification of perimeter sites as active centersrdquo ACS Nanovol 6 no 7 pp 6014ndash6022 2012
[2] H-F Li N Zhang P Chen M-F Luo and J-Q Lu ldquoHigh sur-face area AuCeO
2catalysts for low temperature formaldehyde
oxidationrdquoApplied Catalysis B Environmental vol 110 pp 279ndash285 2011
[3] K Y Ho and K L Yeung ldquoEffects of ozone pretreatment on theperformance of AuTiO
2catalyst for CO oxidation reactionrdquo
Journal of Catalysis vol 242 no 1 pp 131ndash141 2006[4] K Y Ho and K L Yeung ldquoProperties of TiO
2support and the
performance of AuTiO2catalyst for CO oxidation reactionrdquo
Gold Bulletin vol 40 no 1 pp 15ndash30 2007[5] J Qi J Chen G Li S Li Y Gao and Z Tang ldquoFacile
synthesis of core-shell AuCeO2nanocomposites with remark-
ably enhanced catalytic activity for CO oxidationrdquo Energy andEnvironmental Science vol 5 no 10 pp 8937ndash8941 2012
[6] D Jiang W Wang L Zhang Y Zheng and Z Wang ldquoInsightsinto the surface-defect dependence of photoreactivity overCeO2nanocrystals with well-defined crystal facetsrdquo ACS Catal-
ysis vol 5 no 8 pp 4851ndash4858 2015[7] W Lei T Zhang L Gu et al ldquoSurface-structure sensitivity
of CeO2nanocrystals in photocatalysis and enhancing the
reactivity with nanogoldrdquo ACS Catalysis vol 5 no 7 pp 4385ndash4393 2015
[8] B Li T Gu T Ming J Wang P Wang and J C Yu ldquoGoldcore)(ceria shell) nanostructures for plasmon-enhanced cat-alytic reactions under visible lightrdquo ACS Nano vol 8 no 8 pp8152ndash8162 2014
[9] P Lu B Qiao N Lu et al ldquoPhotochemical deposition of highlydispersed Pt nanoparticles on porous CeO
2nanofibers for the
water-gas shift reactionrdquoAdvanced FunctionalMaterials vol 25no 26 pp 4153ndash4162 2015
[10] L Meng A-P Jia J-Q Lu L-F Luo W-X Huang and M-FLuo ldquoSynergetic effects of PdO species on CO oxidation overPdO-CeO
2catalystsrdquo Journal of Physical Chemistry C vol 115
no 40 pp 19789ndash19796 2011[11] Y Park S K Kim D Pradhan and Y Sohn ldquoThermal H
2-
treatment effects on COCO2conversion over Pd-doped CeO
2
comparison with Au and Ag-doped CeO2rdquo Reaction Kinetics
Mechanisms and Catalysis vol 113 no 1 pp 85ndash100 2014[12] Y Park S K Kim D Pradhan and Y Sohn ldquoSurface treatment
effects on CO oxidation reactions over Co Cu and Ni-dopedand codopedCeO
2catalystsrdquoChemical Engineering Journal vol
250 pp 25ndash34 2014[13] B Xu Q Zhang S YuanM Zhang and T Ohno ldquoMorphology
control and photocatalytic characterization of yttrium-dopedhedgehog-like CeO
2rdquo Applied Catalysis B Environmental vol
164 pp 120ndash127 2015[14] W Huang and Y Gao ldquoMorphology-dependent surface chem-
istry and catalysis of CeO2nanocrystalsrdquo Catalysis Science and
Technology vol 4 no 11 pp 3772ndash3784 2014[15] Y Gao W Wang S Chang and W Huang ldquoMorphology
effect of CeO2support in the preparation metal-support
interaction and catalytic performance of PtCeO2catalystsrdquo
ChemCatChem vol 5 no 12 pp 3610ndash3620 2013[16] Y Zhang N Zhang Z-R Tang and Y-J Xu ldquoA unique
silk mat-like structured PdCeO2as an efficient visible light
photocatalyst for green organic transformation in waterrdquo ACSSustainable Chemistry amp Engineering vol 1 no 10 pp 1258ndash1266 2013
[17] W G Shin H J Jung H G Sung H S Hyun and YSohn ldquoSynergic CO oxidation activities of boron-CeO
2hybrid
materials prepared by dry and wet milling methodsrdquo CeramicsInternational vol 40 no 8 pp 11511ndash11517 2014
[18] H Wu P Wang H He and Y Jin ldquoControlled synthesisof porous AgAu bimetallic hollow nanoshells with tunableplasmonic and catalytic propertiesrdquo Nano Research vol 5 no2 pp 135ndash144 2012
[19] N Sasirekha P Sangeetha and Y-W Chen ldquoBimetallic AundashAgCeO
2catalysts for preferential oxidation ofCO inhydrogen-
rich stream effect of calcination temperaturerdquo The Journal ofPhysical Chemistry C vol 118 no 28 pp 15226ndash15233 2014
[20] S Chen L Luo Z Jiang and W Huang ldquoSize-dependent reac-tion pathways of low-temperature CO oxidation on AuCeO
2
catalystsrdquo ACS Catalysis vol 5 no 3 pp 1653ndash1662 2015[21] D LiuW Li X Feng andY Zhang ldquoGalvanic replacement syn-
thesis of Ag119909Au1minus119909
CeO2(0 le x le 1) coreshell nanospheres
with greatly enhanced catalytic performancerdquoChemical Sciencevol 6 pp 7015ndash7019 2015
[22] Y Kang M Sun and A Li ldquoStudies of the catalytic oxidationof CO over AgCeO
2catalystrdquo Catalysis Letters vol 142 no 12
pp 1498ndash1504 2012[23] S Chang M Li Q Hua et al ldquoShape-dependent inter-
play between oxygen vacancies and AgndashCeO2interaction in
AgCeO2catalysts and their influence on the catalytic activityrdquo
Journal of Catalysis vol 293 pp 195ndash204 2012[24] R Fiorenza C Crisafulli G G Condorelli F Lupo and S Scire
ldquoAu-AgCeO2and Au-CuCeO
2Catalysts for volatile organic
compounds oxidation and CO preferential oxidationrdquo CatalysisLetters vol 145 no 9 pp 1691ndash1702 2015
[25] J Zhang L Li X Huang and G Li ldquoFabrication of AgndashCeO2
core-shell nanospheres with enhanced catalytic performancedue to strengthening of the interfacial interactionsrdquo Journal ofMaterials Chemistry vol 22 no 21 pp 10480ndash10487 2012
[26] A Leyva-Perez D Combita-Merchan J R Cabrero-AntoninoS I Al-Resayes and A Corma ldquoOxyhalogenation of activatedarenes with nanocrystalline ceriardquo ACS Catalysis vol 3 no 2pp 250ndash258 2013
[27] Y Liu H Li J Yu DMao andG Lu ldquoElectronic storage capac-ity of ceria role of peroxide inAux supported onCeO
2(111) facet
and CO adsorptionrdquo Physical Chemistry Chemical Physics vol17 no 41 pp 27758ndash27768 2015
[28] D Jiang WWang S Sun L Zhang and Y Zheng ldquoEquilibrat-ing the plasmonic and catalytic roles of metallic nanostructuresin photocatalytic oxidation over Au-modified CeO
2rdquo ACS
Catalysis vol 5 no 2 pp 613ndash621 2015[29] M M Khan S A Ansari M O Ansari B K Min J Lee and
M H Cho ldquoBiogenic fabrication of AuCeO2nanocomposite
with enhanced visible light activityrdquo Journal of Physical Chem-istry C vol 118 no 18 pp 9477ndash9484 2014
[30] A Tanaka K Hashimoto and H Kominami ldquoPreparation ofAuCeO
2exhibiting strong surface plasmon resonance effective
for selective or chemoselective oxidation of alcohols to alde-hydes or ketones in aqueous suspensions under irradiation bygreen lightrdquo Journal of the American Chemical Society vol 134no 35 pp 14526ndash14533 2012
[31] H Y Kim H M Lee and G Henkelman ldquoCO oxidationmechanism on CeO
2-supported Au nanoparticlesrdquo Journal of
the American Chemical Society vol 134 no 3 pp 1560ndash15702012
[32] A Maldotti A Molinari R Juarez and H Garcia ldquoPhotoin-duced reactivity of AundashH intermediates in alcohol oxidation by
Journal of Chemistry 11
gold nanoparticles supported on ceriardquoChemical Science vol 2no 9 pp 1831ndash1834 2011
[33] L Vivier andDDuprez ldquoCeria-based solid catalysts for organicchemistryrdquo ChemSusChem vol 3 no 6 pp 654ndash678 2010
[34] N Zhang S Liu X Fu and Y-J Xu ldquoA simple strategy forfabrication of ldquoplum-puddingrdquo type PdCeO
2semiconductor
nanocomposite as a visible-light-driven photocatalyst for selec-tive oxidationrdquo Journal of Physical Chemistry C vol 115 no 46pp 22901ndash22909 2011
[35] Y Sohn ldquoSiO2nanospheres modified by Ag nanoparticles sur-
face charging and CO oxidation activityrdquo Journal of MolecularCatalysis A Chemical vol 379 pp 59ndash67 2013
[36] W J Kim D Pradhan and Y Sohn ldquoFundamental natureand CO oxidation activities of indium oxide nanostructures1D-wires 2D-plates and 3D-cubes and donutsrdquo Journal ofMaterials Chemistry A vol 1 no 35 pp 10193ndash10202 2013
[37] R-R Zhang L-H Ren A-H Lu and W-C Li ldquoInfluence ofpretreatment atmospheres on the activity of AuCeO
2catalyst
for low-temperature CO oxidationrdquo Catalysis Communicationsvol 13 no 1 pp 18ndash21 2011
[38] Y Li Y Cai X Xing N Chen D Deng and YWang ldquoCatalyticactivity for CO oxidation of CundashCeO
2composite nanoparticles
synthesized by a hydrothermal methodrdquo Analytical Methodsvol 7 no 7 pp 3238ndash3245 2015
[39] R Shang Y Duan X Zhong W Xie Y Luo and L HuangldquoFormic acid modified Co
3O4-CeO
2catalysts for CO oxida-
tionrdquo Catalysts vol 6 no 3 p 48 2016[40] A Abad P Concepcion A Corma and H Garcıa ldquoA collab-
orative effect between gold and a support induces the selectiveoxidation of alcoholsrdquo Angewandte ChemiemdashInternational Edi-tion vol 44 no 26 pp 4066ndash4069 2005
Submit your manuscripts athttpwwwhindawicom
Hindawi Publishing Corporationhttpwwwhindawicom Volume 2014
Inorganic ChemistryInternational Journal of
Hindawi Publishing Corporation httpwwwhindawicom Volume 2014
International Journal ofPhotoenergy
Hindawi Publishing Corporationhttpwwwhindawicom Volume 2014
Carbohydrate Chemistry
International Journal of
Hindawi Publishing Corporationhttpwwwhindawicom Volume 2014
Journal of
Chemistry
Hindawi Publishing Corporationhttpwwwhindawicom Volume 2014
Advances in
Physical Chemistry
Hindawi Publishing Corporationhttpwwwhindawicom
Analytical Methods in Chemistry
Journal of
Volume 2014
Bioinorganic Chemistry and ApplicationsHindawi Publishing Corporationhttpwwwhindawicom Volume 2014
SpectroscopyInternational Journal of
Hindawi Publishing Corporationhttpwwwhindawicom Volume 2014
The Scientific World JournalHindawi Publishing Corporation httpwwwhindawicom Volume 2014
Medicinal ChemistryInternational Journal of
Hindawi Publishing Corporationhttpwwwhindawicom Volume 2014
Chromatography Research International
Hindawi Publishing Corporationhttpwwwhindawicom Volume 2014
Applied ChemistryJournal of
Hindawi Publishing Corporationhttpwwwhindawicom Volume 2014
Hindawi Publishing Corporationhttpwwwhindawicom Volume 2014
Theoretical ChemistryJournal of
Hindawi Publishing Corporationhttpwwwhindawicom Volume 2014
Journal of
Spectroscopy
Analytical ChemistryInternational Journal of
Hindawi Publishing Corporationhttpwwwhindawicom Volume 2014
Journal of
Hindawi Publishing Corporationhttpwwwhindawicom Volume 2014
Quantum Chemistry
Hindawi Publishing Corporationhttpwwwhindawicom Volume 2014
Organic Chemistry International
ElectrochemistryInternational Journal of
Hindawi Publishing Corporation httpwwwhindawicom Volume 2014
Hindawi Publishing Corporationhttpwwwhindawicom Volume 2014
CatalystsJournal of
Journal of Chemistry 9
Table 1 Particles sizes of the metal-loaded CeO2estimated using Scherrerrsquos equation
Loaded MM1015840 50mol (nm) 41mol (nm) 2525mol (nm) 14mol (nm) 05mol (nm)Ag Au 140 124 80 100 86Ni Au 152 123 106 82 86Pd Au 151 127 121 90 86Ni Pd 152 111 147 121 151
Catalysts without stirring
Tightly capped
OOH
O
O
O
lowast
lowast
O
OH
OHO
OO
Abso
rban
ce
10
05
00
Diethyl ether 50
Different smellAcetaldehyde sim1
Acetone sim1
Different smellAcetic acid 01
Ethyl acetate 01
Wavelength (nm)400350300250
(a)
Ethyl acetate(reference)
O
O
Mass (amu)1009080706050M
ass s
igna
l (au
)
OH Before reaction(ETOH)
50 60
Mass (amu)70 80 90 100M
ass s
igna
l (au
)
Afterreaction
01234
UV-VisO
O
Mass (amu)1009080706050M
ass s
igna
l (au
)
Abso
rban
ce
250 300Wavelength (nm)
(b)
Figure 8 UV-Vis absorption spectra (a) of standard samples of acetaldehyde (1) acetone (1) acetic acid (01) and ethyl acetate (01)Mass spectra (b) of reference samples (ethyl acetate and ethanol) and the solution sample after reactionThe inset shows theUV-Vis absorptionspectrum of the corresponding sample solution Blue and red lowast indicate the peak positions for acetaldehyde and ethyl acetate respectively
was that the catalytic efficiency of doped and codoped CeO2
was tested for both gas-phase CO and liquid-phase ethanoloxidation reactions For the 1st and 2nd runs of bare CeO
2
T10 was observed at 405∘C T
10 of bare CeO2for CO oxi-
dation was lowered significantly by 165∘C uponmetal (AgAu= 14mol) doping There were some synergic effects uponcodoping for the CO oxidation The CO oxidation activityvaries with the relative concentrations of two differentmetalsSintering and alloying of two different metals were found toplay important roles in the CO oxidation activity
For liquid-phase ethanol oxidation two liquid productsof ethyl acetate (major 120582max = 220 nm) and acetaldehyde(minor 120582max = 280 nm) were observed by UV-Vis absorptionspectroscopyThe concentration of acetaldehyde (CH
3CHO)
reached a saturation point while that of ethyl acetate(CH3COOCH
2CH3) dramatically increased with reaction
time These findings indicate that acetaldehyde speciespromptly undergo further reaction to form a major productethyl acetate whichwas confirmed bymass spectrometry andUV-visible absorption Undoped CeO
2produces negligible
acetaldehyde which is direct evidence that a hydride shiftreaction CH
3CH2O(ad)-MrarrCH
2CHO+MH is an impor-
tant step for acetaldehyde production for metal-loaded CeO2
catalysts For M- (single) doped CeO2NPs the ethanol
oxidation performance showed an order of Ni lt Ag lt Pd ≪Au For MM1015840 codoped CeO
2NPs the activity of Au doped
CeO2deteriorated drastically upon adding another metals
(Ag Ni and Pd) as cocatalyst The Au-rich CeO2catalyst
showed higher catalytic activity On the other hand the NiPd codoped sample showed much higher catalytic activitycompared with the single M- (Ni and Pd) doped samplesThis study provides further insights into the development ofcatalysts applicable to a range of oxidation reactions
Competing Interests
The authors declare no conflict of interests
Acknowledgments
This study was supported by the 2015 Yeungnam UniversityResearch Grant
References
[1] X Nie H Qian Q Ge H Xu and R Jin ldquoCO oxidationcatalyzed by oxide-supported Au
25(SR)18
nanoclusters and
10 Journal of Chemistry
identification of perimeter sites as active centersrdquo ACS Nanovol 6 no 7 pp 6014ndash6022 2012
[2] H-F Li N Zhang P Chen M-F Luo and J-Q Lu ldquoHigh sur-face area AuCeO
2catalysts for low temperature formaldehyde
oxidationrdquoApplied Catalysis B Environmental vol 110 pp 279ndash285 2011
[3] K Y Ho and K L Yeung ldquoEffects of ozone pretreatment on theperformance of AuTiO
2catalyst for CO oxidation reactionrdquo
Journal of Catalysis vol 242 no 1 pp 131ndash141 2006[4] K Y Ho and K L Yeung ldquoProperties of TiO
2support and the
performance of AuTiO2catalyst for CO oxidation reactionrdquo
Gold Bulletin vol 40 no 1 pp 15ndash30 2007[5] J Qi J Chen G Li S Li Y Gao and Z Tang ldquoFacile
synthesis of core-shell AuCeO2nanocomposites with remark-
ably enhanced catalytic activity for CO oxidationrdquo Energy andEnvironmental Science vol 5 no 10 pp 8937ndash8941 2012
[6] D Jiang W Wang L Zhang Y Zheng and Z Wang ldquoInsightsinto the surface-defect dependence of photoreactivity overCeO2nanocrystals with well-defined crystal facetsrdquo ACS Catal-
ysis vol 5 no 8 pp 4851ndash4858 2015[7] W Lei T Zhang L Gu et al ldquoSurface-structure sensitivity
of CeO2nanocrystals in photocatalysis and enhancing the
reactivity with nanogoldrdquo ACS Catalysis vol 5 no 7 pp 4385ndash4393 2015
[8] B Li T Gu T Ming J Wang P Wang and J C Yu ldquoGoldcore)(ceria shell) nanostructures for plasmon-enhanced cat-alytic reactions under visible lightrdquo ACS Nano vol 8 no 8 pp8152ndash8162 2014
[9] P Lu B Qiao N Lu et al ldquoPhotochemical deposition of highlydispersed Pt nanoparticles on porous CeO
2nanofibers for the
water-gas shift reactionrdquoAdvanced FunctionalMaterials vol 25no 26 pp 4153ndash4162 2015
[10] L Meng A-P Jia J-Q Lu L-F Luo W-X Huang and M-FLuo ldquoSynergetic effects of PdO species on CO oxidation overPdO-CeO
2catalystsrdquo Journal of Physical Chemistry C vol 115
no 40 pp 19789ndash19796 2011[11] Y Park S K Kim D Pradhan and Y Sohn ldquoThermal H
2-
treatment effects on COCO2conversion over Pd-doped CeO
2
comparison with Au and Ag-doped CeO2rdquo Reaction Kinetics
Mechanisms and Catalysis vol 113 no 1 pp 85ndash100 2014[12] Y Park S K Kim D Pradhan and Y Sohn ldquoSurface treatment
effects on CO oxidation reactions over Co Cu and Ni-dopedand codopedCeO
2catalystsrdquoChemical Engineering Journal vol
250 pp 25ndash34 2014[13] B Xu Q Zhang S YuanM Zhang and T Ohno ldquoMorphology
control and photocatalytic characterization of yttrium-dopedhedgehog-like CeO
2rdquo Applied Catalysis B Environmental vol
164 pp 120ndash127 2015[14] W Huang and Y Gao ldquoMorphology-dependent surface chem-
istry and catalysis of CeO2nanocrystalsrdquo Catalysis Science and
Technology vol 4 no 11 pp 3772ndash3784 2014[15] Y Gao W Wang S Chang and W Huang ldquoMorphology
effect of CeO2support in the preparation metal-support
interaction and catalytic performance of PtCeO2catalystsrdquo
ChemCatChem vol 5 no 12 pp 3610ndash3620 2013[16] Y Zhang N Zhang Z-R Tang and Y-J Xu ldquoA unique
silk mat-like structured PdCeO2as an efficient visible light
photocatalyst for green organic transformation in waterrdquo ACSSustainable Chemistry amp Engineering vol 1 no 10 pp 1258ndash1266 2013
[17] W G Shin H J Jung H G Sung H S Hyun and YSohn ldquoSynergic CO oxidation activities of boron-CeO
2hybrid
materials prepared by dry and wet milling methodsrdquo CeramicsInternational vol 40 no 8 pp 11511ndash11517 2014
[18] H Wu P Wang H He and Y Jin ldquoControlled synthesisof porous AgAu bimetallic hollow nanoshells with tunableplasmonic and catalytic propertiesrdquo Nano Research vol 5 no2 pp 135ndash144 2012
[19] N Sasirekha P Sangeetha and Y-W Chen ldquoBimetallic AundashAgCeO
2catalysts for preferential oxidation ofCO inhydrogen-
rich stream effect of calcination temperaturerdquo The Journal ofPhysical Chemistry C vol 118 no 28 pp 15226ndash15233 2014
[20] S Chen L Luo Z Jiang and W Huang ldquoSize-dependent reac-tion pathways of low-temperature CO oxidation on AuCeO
2
catalystsrdquo ACS Catalysis vol 5 no 3 pp 1653ndash1662 2015[21] D LiuW Li X Feng andY Zhang ldquoGalvanic replacement syn-
thesis of Ag119909Au1minus119909
CeO2(0 le x le 1) coreshell nanospheres
with greatly enhanced catalytic performancerdquoChemical Sciencevol 6 pp 7015ndash7019 2015
[22] Y Kang M Sun and A Li ldquoStudies of the catalytic oxidationof CO over AgCeO
2catalystrdquo Catalysis Letters vol 142 no 12
pp 1498ndash1504 2012[23] S Chang M Li Q Hua et al ldquoShape-dependent inter-
play between oxygen vacancies and AgndashCeO2interaction in
AgCeO2catalysts and their influence on the catalytic activityrdquo
Journal of Catalysis vol 293 pp 195ndash204 2012[24] R Fiorenza C Crisafulli G G Condorelli F Lupo and S Scire
ldquoAu-AgCeO2and Au-CuCeO
2Catalysts for volatile organic
compounds oxidation and CO preferential oxidationrdquo CatalysisLetters vol 145 no 9 pp 1691ndash1702 2015
[25] J Zhang L Li X Huang and G Li ldquoFabrication of AgndashCeO2
core-shell nanospheres with enhanced catalytic performancedue to strengthening of the interfacial interactionsrdquo Journal ofMaterials Chemistry vol 22 no 21 pp 10480ndash10487 2012
[26] A Leyva-Perez D Combita-Merchan J R Cabrero-AntoninoS I Al-Resayes and A Corma ldquoOxyhalogenation of activatedarenes with nanocrystalline ceriardquo ACS Catalysis vol 3 no 2pp 250ndash258 2013
[27] Y Liu H Li J Yu DMao andG Lu ldquoElectronic storage capac-ity of ceria role of peroxide inAux supported onCeO
2(111) facet
and CO adsorptionrdquo Physical Chemistry Chemical Physics vol17 no 41 pp 27758ndash27768 2015
[28] D Jiang WWang S Sun L Zhang and Y Zheng ldquoEquilibrat-ing the plasmonic and catalytic roles of metallic nanostructuresin photocatalytic oxidation over Au-modified CeO
2rdquo ACS
Catalysis vol 5 no 2 pp 613ndash621 2015[29] M M Khan S A Ansari M O Ansari B K Min J Lee and
M H Cho ldquoBiogenic fabrication of AuCeO2nanocomposite
with enhanced visible light activityrdquo Journal of Physical Chem-istry C vol 118 no 18 pp 9477ndash9484 2014
[30] A Tanaka K Hashimoto and H Kominami ldquoPreparation ofAuCeO
2exhibiting strong surface plasmon resonance effective
for selective or chemoselective oxidation of alcohols to alde-hydes or ketones in aqueous suspensions under irradiation bygreen lightrdquo Journal of the American Chemical Society vol 134no 35 pp 14526ndash14533 2012
[31] H Y Kim H M Lee and G Henkelman ldquoCO oxidationmechanism on CeO
2-supported Au nanoparticlesrdquo Journal of
the American Chemical Society vol 134 no 3 pp 1560ndash15702012
[32] A Maldotti A Molinari R Juarez and H Garcia ldquoPhotoin-duced reactivity of AundashH intermediates in alcohol oxidation by
Journal of Chemistry 11
gold nanoparticles supported on ceriardquoChemical Science vol 2no 9 pp 1831ndash1834 2011
[33] L Vivier andDDuprez ldquoCeria-based solid catalysts for organicchemistryrdquo ChemSusChem vol 3 no 6 pp 654ndash678 2010
[34] N Zhang S Liu X Fu and Y-J Xu ldquoA simple strategy forfabrication of ldquoplum-puddingrdquo type PdCeO
2semiconductor
nanocomposite as a visible-light-driven photocatalyst for selec-tive oxidationrdquo Journal of Physical Chemistry C vol 115 no 46pp 22901ndash22909 2011
[35] Y Sohn ldquoSiO2nanospheres modified by Ag nanoparticles sur-
face charging and CO oxidation activityrdquo Journal of MolecularCatalysis A Chemical vol 379 pp 59ndash67 2013
[36] W J Kim D Pradhan and Y Sohn ldquoFundamental natureand CO oxidation activities of indium oxide nanostructures1D-wires 2D-plates and 3D-cubes and donutsrdquo Journal ofMaterials Chemistry A vol 1 no 35 pp 10193ndash10202 2013
[37] R-R Zhang L-H Ren A-H Lu and W-C Li ldquoInfluence ofpretreatment atmospheres on the activity of AuCeO
2catalyst
for low-temperature CO oxidationrdquo Catalysis Communicationsvol 13 no 1 pp 18ndash21 2011
[38] Y Li Y Cai X Xing N Chen D Deng and YWang ldquoCatalyticactivity for CO oxidation of CundashCeO
2composite nanoparticles
synthesized by a hydrothermal methodrdquo Analytical Methodsvol 7 no 7 pp 3238ndash3245 2015
[39] R Shang Y Duan X Zhong W Xie Y Luo and L HuangldquoFormic acid modified Co
3O4-CeO
2catalysts for CO oxida-
tionrdquo Catalysts vol 6 no 3 p 48 2016[40] A Abad P Concepcion A Corma and H Garcıa ldquoA collab-
orative effect between gold and a support induces the selectiveoxidation of alcoholsrdquo Angewandte ChemiemdashInternational Edi-tion vol 44 no 26 pp 4066ndash4069 2005
Submit your manuscripts athttpwwwhindawicom
Hindawi Publishing Corporationhttpwwwhindawicom Volume 2014
Inorganic ChemistryInternational Journal of
Hindawi Publishing Corporation httpwwwhindawicom Volume 2014
International Journal ofPhotoenergy
Hindawi Publishing Corporationhttpwwwhindawicom Volume 2014
Carbohydrate Chemistry
International Journal of
Hindawi Publishing Corporationhttpwwwhindawicom Volume 2014
Journal of
Chemistry
Hindawi Publishing Corporationhttpwwwhindawicom Volume 2014
Advances in
Physical Chemistry
Hindawi Publishing Corporationhttpwwwhindawicom
Analytical Methods in Chemistry
Journal of
Volume 2014
Bioinorganic Chemistry and ApplicationsHindawi Publishing Corporationhttpwwwhindawicom Volume 2014
SpectroscopyInternational Journal of
Hindawi Publishing Corporationhttpwwwhindawicom Volume 2014
The Scientific World JournalHindawi Publishing Corporation httpwwwhindawicom Volume 2014
Medicinal ChemistryInternational Journal of
Hindawi Publishing Corporationhttpwwwhindawicom Volume 2014
Chromatography Research International
Hindawi Publishing Corporationhttpwwwhindawicom Volume 2014
Applied ChemistryJournal of
Hindawi Publishing Corporationhttpwwwhindawicom Volume 2014
Hindawi Publishing Corporationhttpwwwhindawicom Volume 2014
Theoretical ChemistryJournal of
Hindawi Publishing Corporationhttpwwwhindawicom Volume 2014
Journal of
Spectroscopy
Analytical ChemistryInternational Journal of
Hindawi Publishing Corporationhttpwwwhindawicom Volume 2014
Journal of
Hindawi Publishing Corporationhttpwwwhindawicom Volume 2014
Quantum Chemistry
Hindawi Publishing Corporationhttpwwwhindawicom Volume 2014
Organic Chemistry International
ElectrochemistryInternational Journal of
Hindawi Publishing Corporation httpwwwhindawicom Volume 2014
Hindawi Publishing Corporationhttpwwwhindawicom Volume 2014
CatalystsJournal of
10 Journal of Chemistry
identification of perimeter sites as active centersrdquo ACS Nanovol 6 no 7 pp 6014ndash6022 2012
[2] H-F Li N Zhang P Chen M-F Luo and J-Q Lu ldquoHigh sur-face area AuCeO
2catalysts for low temperature formaldehyde
oxidationrdquoApplied Catalysis B Environmental vol 110 pp 279ndash285 2011
[3] K Y Ho and K L Yeung ldquoEffects of ozone pretreatment on theperformance of AuTiO
2catalyst for CO oxidation reactionrdquo
Journal of Catalysis vol 242 no 1 pp 131ndash141 2006[4] K Y Ho and K L Yeung ldquoProperties of TiO
2support and the
performance of AuTiO2catalyst for CO oxidation reactionrdquo
Gold Bulletin vol 40 no 1 pp 15ndash30 2007[5] J Qi J Chen G Li S Li Y Gao and Z Tang ldquoFacile
synthesis of core-shell AuCeO2nanocomposites with remark-
ably enhanced catalytic activity for CO oxidationrdquo Energy andEnvironmental Science vol 5 no 10 pp 8937ndash8941 2012
[6] D Jiang W Wang L Zhang Y Zheng and Z Wang ldquoInsightsinto the surface-defect dependence of photoreactivity overCeO2nanocrystals with well-defined crystal facetsrdquo ACS Catal-
ysis vol 5 no 8 pp 4851ndash4858 2015[7] W Lei T Zhang L Gu et al ldquoSurface-structure sensitivity
of CeO2nanocrystals in photocatalysis and enhancing the
reactivity with nanogoldrdquo ACS Catalysis vol 5 no 7 pp 4385ndash4393 2015
[8] B Li T Gu T Ming J Wang P Wang and J C Yu ldquoGoldcore)(ceria shell) nanostructures for plasmon-enhanced cat-alytic reactions under visible lightrdquo ACS Nano vol 8 no 8 pp8152ndash8162 2014
[9] P Lu B Qiao N Lu et al ldquoPhotochemical deposition of highlydispersed Pt nanoparticles on porous CeO
2nanofibers for the
water-gas shift reactionrdquoAdvanced FunctionalMaterials vol 25no 26 pp 4153ndash4162 2015
[10] L Meng A-P Jia J-Q Lu L-F Luo W-X Huang and M-FLuo ldquoSynergetic effects of PdO species on CO oxidation overPdO-CeO
2catalystsrdquo Journal of Physical Chemistry C vol 115
no 40 pp 19789ndash19796 2011[11] Y Park S K Kim D Pradhan and Y Sohn ldquoThermal H
2-
treatment effects on COCO2conversion over Pd-doped CeO
2
comparison with Au and Ag-doped CeO2rdquo Reaction Kinetics
Mechanisms and Catalysis vol 113 no 1 pp 85ndash100 2014[12] Y Park S K Kim D Pradhan and Y Sohn ldquoSurface treatment
effects on CO oxidation reactions over Co Cu and Ni-dopedand codopedCeO
2catalystsrdquoChemical Engineering Journal vol
250 pp 25ndash34 2014[13] B Xu Q Zhang S YuanM Zhang and T Ohno ldquoMorphology
control and photocatalytic characterization of yttrium-dopedhedgehog-like CeO
2rdquo Applied Catalysis B Environmental vol
164 pp 120ndash127 2015[14] W Huang and Y Gao ldquoMorphology-dependent surface chem-
istry and catalysis of CeO2nanocrystalsrdquo Catalysis Science and
Technology vol 4 no 11 pp 3772ndash3784 2014[15] Y Gao W Wang S Chang and W Huang ldquoMorphology
effect of CeO2support in the preparation metal-support
interaction and catalytic performance of PtCeO2catalystsrdquo
ChemCatChem vol 5 no 12 pp 3610ndash3620 2013[16] Y Zhang N Zhang Z-R Tang and Y-J Xu ldquoA unique
silk mat-like structured PdCeO2as an efficient visible light
photocatalyst for green organic transformation in waterrdquo ACSSustainable Chemistry amp Engineering vol 1 no 10 pp 1258ndash1266 2013
[17] W G Shin H J Jung H G Sung H S Hyun and YSohn ldquoSynergic CO oxidation activities of boron-CeO
2hybrid
materials prepared by dry and wet milling methodsrdquo CeramicsInternational vol 40 no 8 pp 11511ndash11517 2014
[18] H Wu P Wang H He and Y Jin ldquoControlled synthesisof porous AgAu bimetallic hollow nanoshells with tunableplasmonic and catalytic propertiesrdquo Nano Research vol 5 no2 pp 135ndash144 2012
[19] N Sasirekha P Sangeetha and Y-W Chen ldquoBimetallic AundashAgCeO
2catalysts for preferential oxidation ofCO inhydrogen-
rich stream effect of calcination temperaturerdquo The Journal ofPhysical Chemistry C vol 118 no 28 pp 15226ndash15233 2014
[20] S Chen L Luo Z Jiang and W Huang ldquoSize-dependent reac-tion pathways of low-temperature CO oxidation on AuCeO
2
catalystsrdquo ACS Catalysis vol 5 no 3 pp 1653ndash1662 2015[21] D LiuW Li X Feng andY Zhang ldquoGalvanic replacement syn-
thesis of Ag119909Au1minus119909
CeO2(0 le x le 1) coreshell nanospheres
with greatly enhanced catalytic performancerdquoChemical Sciencevol 6 pp 7015ndash7019 2015
[22] Y Kang M Sun and A Li ldquoStudies of the catalytic oxidationof CO over AgCeO
2catalystrdquo Catalysis Letters vol 142 no 12
pp 1498ndash1504 2012[23] S Chang M Li Q Hua et al ldquoShape-dependent inter-
play between oxygen vacancies and AgndashCeO2interaction in
AgCeO2catalysts and their influence on the catalytic activityrdquo
Journal of Catalysis vol 293 pp 195ndash204 2012[24] R Fiorenza C Crisafulli G G Condorelli F Lupo and S Scire
ldquoAu-AgCeO2and Au-CuCeO
2Catalysts for volatile organic
compounds oxidation and CO preferential oxidationrdquo CatalysisLetters vol 145 no 9 pp 1691ndash1702 2015
[25] J Zhang L Li X Huang and G Li ldquoFabrication of AgndashCeO2
core-shell nanospheres with enhanced catalytic performancedue to strengthening of the interfacial interactionsrdquo Journal ofMaterials Chemistry vol 22 no 21 pp 10480ndash10487 2012
[26] A Leyva-Perez D Combita-Merchan J R Cabrero-AntoninoS I Al-Resayes and A Corma ldquoOxyhalogenation of activatedarenes with nanocrystalline ceriardquo ACS Catalysis vol 3 no 2pp 250ndash258 2013
[27] Y Liu H Li J Yu DMao andG Lu ldquoElectronic storage capac-ity of ceria role of peroxide inAux supported onCeO
2(111) facet
and CO adsorptionrdquo Physical Chemistry Chemical Physics vol17 no 41 pp 27758ndash27768 2015
[28] D Jiang WWang S Sun L Zhang and Y Zheng ldquoEquilibrat-ing the plasmonic and catalytic roles of metallic nanostructuresin photocatalytic oxidation over Au-modified CeO
2rdquo ACS
Catalysis vol 5 no 2 pp 613ndash621 2015[29] M M Khan S A Ansari M O Ansari B K Min J Lee and
M H Cho ldquoBiogenic fabrication of AuCeO2nanocomposite
with enhanced visible light activityrdquo Journal of Physical Chem-istry C vol 118 no 18 pp 9477ndash9484 2014
[30] A Tanaka K Hashimoto and H Kominami ldquoPreparation ofAuCeO
2exhibiting strong surface plasmon resonance effective
for selective or chemoselective oxidation of alcohols to alde-hydes or ketones in aqueous suspensions under irradiation bygreen lightrdquo Journal of the American Chemical Society vol 134no 35 pp 14526ndash14533 2012
[31] H Y Kim H M Lee and G Henkelman ldquoCO oxidationmechanism on CeO
2-supported Au nanoparticlesrdquo Journal of
the American Chemical Society vol 134 no 3 pp 1560ndash15702012
[32] A Maldotti A Molinari R Juarez and H Garcia ldquoPhotoin-duced reactivity of AundashH intermediates in alcohol oxidation by
Journal of Chemistry 11
gold nanoparticles supported on ceriardquoChemical Science vol 2no 9 pp 1831ndash1834 2011
[33] L Vivier andDDuprez ldquoCeria-based solid catalysts for organicchemistryrdquo ChemSusChem vol 3 no 6 pp 654ndash678 2010
[34] N Zhang S Liu X Fu and Y-J Xu ldquoA simple strategy forfabrication of ldquoplum-puddingrdquo type PdCeO
2semiconductor
nanocomposite as a visible-light-driven photocatalyst for selec-tive oxidationrdquo Journal of Physical Chemistry C vol 115 no 46pp 22901ndash22909 2011
[35] Y Sohn ldquoSiO2nanospheres modified by Ag nanoparticles sur-
face charging and CO oxidation activityrdquo Journal of MolecularCatalysis A Chemical vol 379 pp 59ndash67 2013
[36] W J Kim D Pradhan and Y Sohn ldquoFundamental natureand CO oxidation activities of indium oxide nanostructures1D-wires 2D-plates and 3D-cubes and donutsrdquo Journal ofMaterials Chemistry A vol 1 no 35 pp 10193ndash10202 2013
[37] R-R Zhang L-H Ren A-H Lu and W-C Li ldquoInfluence ofpretreatment atmospheres on the activity of AuCeO
2catalyst
for low-temperature CO oxidationrdquo Catalysis Communicationsvol 13 no 1 pp 18ndash21 2011
[38] Y Li Y Cai X Xing N Chen D Deng and YWang ldquoCatalyticactivity for CO oxidation of CundashCeO
2composite nanoparticles
synthesized by a hydrothermal methodrdquo Analytical Methodsvol 7 no 7 pp 3238ndash3245 2015
[39] R Shang Y Duan X Zhong W Xie Y Luo and L HuangldquoFormic acid modified Co
3O4-CeO
2catalysts for CO oxida-
tionrdquo Catalysts vol 6 no 3 p 48 2016[40] A Abad P Concepcion A Corma and H Garcıa ldquoA collab-
orative effect between gold and a support induces the selectiveoxidation of alcoholsrdquo Angewandte ChemiemdashInternational Edi-tion vol 44 no 26 pp 4066ndash4069 2005
Submit your manuscripts athttpwwwhindawicom
Hindawi Publishing Corporationhttpwwwhindawicom Volume 2014
Inorganic ChemistryInternational Journal of
Hindawi Publishing Corporation httpwwwhindawicom Volume 2014
International Journal ofPhotoenergy
Hindawi Publishing Corporationhttpwwwhindawicom Volume 2014
Carbohydrate Chemistry
International Journal of
Hindawi Publishing Corporationhttpwwwhindawicom Volume 2014
Journal of
Chemistry
Hindawi Publishing Corporationhttpwwwhindawicom Volume 2014
Advances in
Physical Chemistry
Hindawi Publishing Corporationhttpwwwhindawicom
Analytical Methods in Chemistry
Journal of
Volume 2014
Bioinorganic Chemistry and ApplicationsHindawi Publishing Corporationhttpwwwhindawicom Volume 2014
SpectroscopyInternational Journal of
Hindawi Publishing Corporationhttpwwwhindawicom Volume 2014
The Scientific World JournalHindawi Publishing Corporation httpwwwhindawicom Volume 2014
Medicinal ChemistryInternational Journal of
Hindawi Publishing Corporationhttpwwwhindawicom Volume 2014
Chromatography Research International
Hindawi Publishing Corporationhttpwwwhindawicom Volume 2014
Applied ChemistryJournal of
Hindawi Publishing Corporationhttpwwwhindawicom Volume 2014
Hindawi Publishing Corporationhttpwwwhindawicom Volume 2014
Theoretical ChemistryJournal of
Hindawi Publishing Corporationhttpwwwhindawicom Volume 2014
Journal of
Spectroscopy
Analytical ChemistryInternational Journal of
Hindawi Publishing Corporationhttpwwwhindawicom Volume 2014
Journal of
Hindawi Publishing Corporationhttpwwwhindawicom Volume 2014
Quantum Chemistry
Hindawi Publishing Corporationhttpwwwhindawicom Volume 2014
Organic Chemistry International
ElectrochemistryInternational Journal of
Hindawi Publishing Corporation httpwwwhindawicom Volume 2014
Hindawi Publishing Corporationhttpwwwhindawicom Volume 2014
CatalystsJournal of
Journal of Chemistry 11
gold nanoparticles supported on ceriardquoChemical Science vol 2no 9 pp 1831ndash1834 2011
[33] L Vivier andDDuprez ldquoCeria-based solid catalysts for organicchemistryrdquo ChemSusChem vol 3 no 6 pp 654ndash678 2010
[34] N Zhang S Liu X Fu and Y-J Xu ldquoA simple strategy forfabrication of ldquoplum-puddingrdquo type PdCeO
2semiconductor
nanocomposite as a visible-light-driven photocatalyst for selec-tive oxidationrdquo Journal of Physical Chemistry C vol 115 no 46pp 22901ndash22909 2011
[35] Y Sohn ldquoSiO2nanospheres modified by Ag nanoparticles sur-
face charging and CO oxidation activityrdquo Journal of MolecularCatalysis A Chemical vol 379 pp 59ndash67 2013
[36] W J Kim D Pradhan and Y Sohn ldquoFundamental natureand CO oxidation activities of indium oxide nanostructures1D-wires 2D-plates and 3D-cubes and donutsrdquo Journal ofMaterials Chemistry A vol 1 no 35 pp 10193ndash10202 2013
[37] R-R Zhang L-H Ren A-H Lu and W-C Li ldquoInfluence ofpretreatment atmospheres on the activity of AuCeO
2catalyst
for low-temperature CO oxidationrdquo Catalysis Communicationsvol 13 no 1 pp 18ndash21 2011
[38] Y Li Y Cai X Xing N Chen D Deng and YWang ldquoCatalyticactivity for CO oxidation of CundashCeO
2composite nanoparticles
synthesized by a hydrothermal methodrdquo Analytical Methodsvol 7 no 7 pp 3238ndash3245 2015
[39] R Shang Y Duan X Zhong W Xie Y Luo and L HuangldquoFormic acid modified Co
3O4-CeO
2catalysts for CO oxida-
tionrdquo Catalysts vol 6 no 3 p 48 2016[40] A Abad P Concepcion A Corma and H Garcıa ldquoA collab-
orative effect between gold and a support induces the selectiveoxidation of alcoholsrdquo Angewandte ChemiemdashInternational Edi-tion vol 44 no 26 pp 4066ndash4069 2005
Submit your manuscripts athttpwwwhindawicom
Hindawi Publishing Corporationhttpwwwhindawicom Volume 2014
Inorganic ChemistryInternational Journal of
Hindawi Publishing Corporation httpwwwhindawicom Volume 2014
International Journal ofPhotoenergy
Hindawi Publishing Corporationhttpwwwhindawicom Volume 2014
Carbohydrate Chemistry
International Journal of
Hindawi Publishing Corporationhttpwwwhindawicom Volume 2014
Journal of
Chemistry
Hindawi Publishing Corporationhttpwwwhindawicom Volume 2014
Advances in
Physical Chemistry
Hindawi Publishing Corporationhttpwwwhindawicom
Analytical Methods in Chemistry
Journal of
Volume 2014
Bioinorganic Chemistry and ApplicationsHindawi Publishing Corporationhttpwwwhindawicom Volume 2014
SpectroscopyInternational Journal of
Hindawi Publishing Corporationhttpwwwhindawicom Volume 2014
The Scientific World JournalHindawi Publishing Corporation httpwwwhindawicom Volume 2014
Medicinal ChemistryInternational Journal of
Hindawi Publishing Corporationhttpwwwhindawicom Volume 2014
Chromatography Research International
Hindawi Publishing Corporationhttpwwwhindawicom Volume 2014
Applied ChemistryJournal of
Hindawi Publishing Corporationhttpwwwhindawicom Volume 2014
Hindawi Publishing Corporationhttpwwwhindawicom Volume 2014
Theoretical ChemistryJournal of
Hindawi Publishing Corporationhttpwwwhindawicom Volume 2014
Journal of
Spectroscopy
Analytical ChemistryInternational Journal of
Hindawi Publishing Corporationhttpwwwhindawicom Volume 2014
Journal of
Hindawi Publishing Corporationhttpwwwhindawicom Volume 2014
Quantum Chemistry
Hindawi Publishing Corporationhttpwwwhindawicom Volume 2014
Organic Chemistry International
ElectrochemistryInternational Journal of
Hindawi Publishing Corporation httpwwwhindawicom Volume 2014
Hindawi Publishing Corporationhttpwwwhindawicom Volume 2014
CatalystsJournal of
Submit your manuscripts athttpwwwhindawicom
Hindawi Publishing Corporationhttpwwwhindawicom Volume 2014
Inorganic ChemistryInternational Journal of
Hindawi Publishing Corporation httpwwwhindawicom Volume 2014
International Journal ofPhotoenergy
Hindawi Publishing Corporationhttpwwwhindawicom Volume 2014
Carbohydrate Chemistry
International Journal of
Hindawi Publishing Corporationhttpwwwhindawicom Volume 2014
Journal of
Chemistry
Hindawi Publishing Corporationhttpwwwhindawicom Volume 2014
Advances in
Physical Chemistry
Hindawi Publishing Corporationhttpwwwhindawicom
Analytical Methods in Chemistry
Journal of
Volume 2014
Bioinorganic Chemistry and ApplicationsHindawi Publishing Corporationhttpwwwhindawicom Volume 2014
SpectroscopyInternational Journal of
Hindawi Publishing Corporationhttpwwwhindawicom Volume 2014
The Scientific World JournalHindawi Publishing Corporation httpwwwhindawicom Volume 2014
Medicinal ChemistryInternational Journal of
Hindawi Publishing Corporationhttpwwwhindawicom Volume 2014
Chromatography Research International
Hindawi Publishing Corporationhttpwwwhindawicom Volume 2014
Applied ChemistryJournal of
Hindawi Publishing Corporationhttpwwwhindawicom Volume 2014
Hindawi Publishing Corporationhttpwwwhindawicom Volume 2014
Theoretical ChemistryJournal of
Hindawi Publishing Corporationhttpwwwhindawicom Volume 2014
Journal of
Spectroscopy
Analytical ChemistryInternational Journal of
Hindawi Publishing Corporationhttpwwwhindawicom Volume 2014
Journal of
Hindawi Publishing Corporationhttpwwwhindawicom Volume 2014
Quantum Chemistry
Hindawi Publishing Corporationhttpwwwhindawicom Volume 2014
Organic Chemistry International
ElectrochemistryInternational Journal of
Hindawi Publishing Corporation httpwwwhindawicom Volume 2014
Hindawi Publishing Corporationhttpwwwhindawicom Volume 2014
CatalystsJournal of