Investigation of thermal oxidation of Al2O3-coated SiC powder
Transcript of Investigation of thermal oxidation of Al2O3-coated SiC powder
Accepted Manuscript
Title: Investigation of Thermal Oxidation of Al2O3-CoatedSiC Powder
Author: Atanu Dey Nijhuma Kayal Atiar Rahaman MollaOmprakash Chakrabarti
PII: S0040-6031(14)00094-XDOI: http://dx.doi.org/doi:10.1016/j.tca.2014.03.011Reference: TCA 76800
To appear in: Thermochimica Acta
Received date: 19-12-2013Revised date: 14-3-2014Accepted date: 16-3-2014
Please cite this article as: A. Dey, N. Kayal, A.R. Molla, O. Chakrabarti, Investigationof Thermal Oxidation of Al2O3-Coated SiC Powder, Thermochimica Acta (2014),http://dx.doi.org/10.1016/j.tca.2014.03.011
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Investigation of Thermal Oxidation of Al2O3-Coated SiC
Powder
Atanu Dey, Nijhuma Kayal, Atiar Rahaman Molla and Omprakash Chakrabarti*
CSIR-Central Glass and Ceramic Research Institute, 196 Raja S.C.Mullick Road,
Jadavpur, Kolkata-700 032, India
Abstract
SiC powder (-form) of sub-micrometer size (d50 of 0.65 m) was coated with a thin
layer (~12 nm) of boehmite by sol-gel technique. The final powder having ~ 24 wt%
boehmite was characterized by particle size and surface area determination, chemical
analysis, surface potential measurement and Fourier transform infrared (FTIR)
spectroscopic analysis. The thermal oxidation behaviour of the coated powder was
examined using the simultaneous TG/DTA technique in dry air. The results indicated
crystallization of mullite phase and the activation energy of crystallization was
determined to be 368.9±15.1 kJ mol-1. Synthesis of porous SiC ceramics of fine pore
structure (with average porosity and pore size ranging from 47-54% and 170-260 nm,
respectively) using thermal oxidation of coated powder was also demonstrated.
Key words: Oxidation kinetics, Sub-micron SiC powder, Thermal analysis, Al2O3
coating, Porous SiC
_______________
*Corresponding author. Tel.: +91-33-24733469/76/77
E-mail address: [email protected]
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1. Introduction
SiC ceramics have low bulk density, excellent mechanical and chemical
stability, high thermal conductivity and thermal shock resistance, and they can also
withstand high temperatures and hostile atmospheres. Processing routes are found to
retain or create porosity without sacrificing these special properties. One of the
important methods of producing porous SiC ceramics of pore size in micrometer scale
involves heating of a porous compact of SiC powders in air when oxidation derived
silica bridges the gap between the SiC particles at the contacting regions forming a
porous body.1-3 Al2O3 is added as a secondary phase in the starting mixture to produce
mullite for improvement of mechanical properties, corrosion and thermal shock
resistance of the porous ceramics.4-6 Porous SiC ceramics produced by the oxidation
bonding technique are promising filter materials and they can be used for removal of
dust and fine particles in the off-gas cleaning systems of many important industrial
processes (coal combustion and gasification processes for power generation, thermal
remediation of contaminated soils, incineration of hospital and industrial wastes, metal
smelting, manufacturing of cements, carbon blacks and glasses, etc.7-10). Efforts are
also made to bring the emissions of ultrafine particles ~ particles finer than 0.1 m ~
from industrial processes under the stringent regulatory control.11 Porous media
composed of agglomerates or granules of ceramic nanoparticles are successfully used
for filtration of submicron solid or liquid aerosol particles.12 In this respect
development of oxidation bonded porous SiC ceramics of very fine pore structure
using SiC-Al2O3 powders of sub-micrometer sizes assumes importance. For this
purpose complete understanding of oxidation behaviour of ultrafine SiC+Al2O3
powder systems becomes necessary. Al2O3 coating on SiC particles may serve as a
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way to distribute the secondary phase more uniformly in the system of SiC-Al2O3
powder of submicron sizes and makes possible the use of coated powder in oxidation
bonding of porous SiC of fine pore sizes. In this paper we present the results of an
investigation on Al2O3 coating of SiC powder of sub-micron size and the kinetic study
of oxidation of the coated powder.
2. Experimental Procedure
-SiC powder (Grade 059N/200; Lot # 050710C10; SiC: Min. 98 % w/w, Free
C: Max. 2.0% w/w, Oxygen: Max.1.1% w/w, Nitrogen: Max. 0.25% w/w, Metallic Si:
Max.0.03 % w/w; Superior Graphite, Chicago, IL, USA) with an average particle size
(d50) of 0.65 m and surface area of 11-16 m2 g-1 was used. Boehmite coating of SiC
powder was carried out following the method described by Yang and Shih.13 Aluminum
tri-sec-butoxide (Product No. 201073; Mol. Formula: C12H27AlO3; Purity: 97%; Sigma
Aldrich Co., MO, USA) was used as the precursor for boehmite. As-received SiC
powder was dispersed in de-ionized water with ultrasonication (Sonaprob PR-1000MP,
Oscar Ultrasonic Sakinaka, Mumbai, India) to disintegrate the agglomerates. The
suspension was heated to 90°C under constant magnetic stirring. 97% aluminum-tri-sec-
butoxide was then added and the molar ratio of alkoxide to water was kept at 1:150 in
order to ensure complete hydrolysis. After the alkoxide addition, HCl was continually
added to maintain the suspension pH at 3. After stirring for about half an hour the
suspension was centrifuged (REMI-PR-24, Remi Electronics Ltd., Vasai, India) and the
coated powder was obtained by repeatedly rinsing with water followed by drying and
grinding. In the present work the final powder with ~ 24% boehmite coating was
prepared using 12 g of aluminum tri-sec-butoxide and 8.8 g of SiC powder. The coated
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powder was characterized by measuring particle size (ZEN 3690, Malvern Instrument
Ltd., Worcestershire, U.K.) and, BET surface area (NOVA 4000e, Quantachrome
Instrument, FL, USA). Zeta potential measurement (ZEN 3690, Malvern Instrument
Ltd., Worcestershire, U.K.) of the coated and uncoated SiC powders was done and their
Fourier transform infrared transmission spectra (Nicolet 5700, Thermo Scientific, MA,
USA; wave number range of 400 to 4000 cm-1) were also recorded. The amount of
coating in the final powder was determined by wet chemical analysis method
(complexometric determination of aluminium). The oxidation experiment was carried
out using a simultaneous thermal analyzer (STA 449 F3 Jupiter, NETZSCH Geratbau
GmbH, Selb, Germany). DTA tests under non-isothermal conditions were performed
keeping a constant flow of dry air (XL Grade, BOC India Ltd., Kolkata, India; flow rate
of 60 ml min-1 under atmospheric pressure) at different linear heating rate (20 K min-1;
25 K min-1; 30 K min-1 and 40 K min-1).
3. Results and discussion
(1) Preparation of Boehmite Coated SiC Powder
The coating material was produced from the aluminium secondary butoxide
solution following the same process but without the presence of SiC. The particles so
produced were boehmite as was evident from the XRD pattern of the precipitate from
the aluminium secondary butoxide solution after drying at 100°C (Fig. 1). Formation
of boehmite was also reported in the experimental conditions similar to those of
present study.13 The average particle size of SiC powder before and after coating was
measure to be 400 and 479 nm, respectively, based on the number average and 517 and
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689 nm, respectively, based on the volume average (Fig. 2). The results of particle size
measurement tests indicated presence of very few free boehmite particles in the
suspension of coated particles. The mean particle size of boehmite was reported to be
around 80 nm.13 In the present study an average particle size of ~ 90 nm has been
obtained (Fig.2). None of the peaks centred on this average particle size was found in
case of coated powder. The average particle size of SiC increased after the coating
process. The individual boehmite particles possibly aggregated on SiC particles
increasing the average particle size after coating. Figure 3 shows the zeta potential
versus pH plots for the uncoated and coated SiC particles. The SiC particles exhibited
the isoelectric potential (IEP) at pH 4.6. With boehmite coating the IEP shifted to a
higher value at pH 9.4. The boehmite powders were reported to have an IEP at pH
9.8.14 The surface of boehmite has neutral surface sites and can react with either H+ or
OH- ions in acidic or basic solutions to produce dominant positive or negative surface
sites below or above the IEP, respectively. After coating SiC particles with boehmite
the surface was terminated with neutral surface sites and the behaviour of the coated
SiC suspension became similar to that of boehmite suspension. The zeta potential
measurement test further confirmed that the coating was successful as the surface
potential of SiC changed to that of boehmite after coating. The FTIR transmission
spectrum of the uncoated powder had the characteristic peak of SiC at 866 cm-1 (Fig.
4). For coated powder peaks appeared at 487, 534, 649, 717 and 877 cm-1. The band
position at 717 cm-1 indicated formation of the Al-O-Si linkage.15 The peaks at 487,
534 and 649 cm-1 were for boehmite.16 The peak at 877 cm-1 was similar to the
characteristic peak of SiC; Lee and Kim examined simultaneous hydrolysis and coating
of Al(OH)3 on SiC particles in water/aluminum isopropoxide solution containing SiC
and -Al2O3 (seeding material) particles and observed no peak of SiC in the FTIR
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spectrum of hydrolysed powder, inferring that the SiC particles were completely
embedded in SiC matrix.16 Hareesh observed that the characteristic peak of SiC
remained unchanged in the FTIR spectra of SiC powders coated with alumina
following hydrolysis of aluminum nitrate solution.17 Saraswati also observed that the
characteristic peak of SiC remained unchanged in the FTIR spectrum of boehmite
coated SiC whisker reinforced alumina composite after sintering at 1800°C.18 In
boehmite the aluminum ions can occupy two sub-lattices ~ tetrahedral sites and
octahedral sites and the band positions measured on coated powder in the range of 400
to 800 cm-1 are likely due to the stretching and bending of octahedrally coordinated
aluminum (AlO6 atomic group) while the band position at around 880 cm-1 wave
number is due to the stretching of tetrahedrally coordinated aluminum (AlO4 atom
group) of shorter Al-O bond length.19 The AlO4 band has probably been overlapped
with the characteristic peak of SiC in the coated powder.17 The SiC powder has surface
active silanol (Si-OH) groups and the coating takes place via the reaction of hydroxyl
group of silanol and the alkoxy group of Al-alkoxide. Initially an initial surface layer is
formed by chemical adsorption and the amount of reacted alkoxide is then increased by
starting the hydrolysis reaction. Hydrolysis reaction upon addition of water links the
alkoxide molecules by a polymerization type sol-gel reaction.20 FTIR analysis of the
boehmite coated SiC powder showed the nature of the coating phase. The experimental
results confirmed that the boehmite coating was in reality a thin and low density layer
of finely particulate crystallite material and it adhered fairly strongly to the underlying
SiC surface. The coating had a high specific surface area (a value of 64.18 m2 g-1 was
obtained by the BET surface area measurement) which showed the porous structure of
the coating. This open structure would facilitate ingress of other species of ionic
dimension to the underlying SiC surface. Though the coating was porous in nature, the
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overall electrical nature of the SiC particles was dominated by the adsorbed species
forming the coating making the surface electrical potential of the particles nearly equal
to that of the coating materials. Chemical analysis showed that the final powder had
22.54 wt% of boehmite. The thickness (d) of the coating layer was calculated using the
following equation:21
vs
a
Sm
md (1)
where, ma and ms represent the respective weight (in g) of the coating material (of
density g cm-3) and the coated particle (of specific surface area Sv m2 g-1). The
thickness of the boehmite coating was estimated to be 1.2 nm. The actual coating
thickness was larger than the estimated value as the actual coating was porous and
fully dense boehmite was assumed in the theoretical estimate. A similar discrepancy
was reported by other researchers in boehmite coating of ceramic powders who
obtained around ten times increase of actual coating thickness than the theoretically
estimated value.13,22 Taking this point into consideration the actual coating thickness in
the present work is expected to be around 12 nm.
(2) Oxidation of Boehmite Coated SiC Powder
The typical TG plot showing the change in weight during heating of the coated
SiC at a rate of 40 K min-1 in air is presented in Fig. 5. A gradual weight loss was
recorded on heating to 700°C. Above this temperature weight loss reached a maximum
value and a weight gain was observed at higher temperatures because of onset of
oxidation of SiC. The plateau value at maximum weight loss can be considered as a
reference when silica first forms as an oxidation product on the surface of SiC
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particles. The thermogram obtained in the DTA experiment shows an endothermic
peak ending at ~300°C. This is followed by a small endothermic peak at ~500°C, an
exothermic peak at ~800°C and another exothermic peak at 1297°C. The endothermic
peaks and the first exothermic peak fall in the weight loss region of the TG curve. The
second exothermic peak occurs in the weight gain region. Comparison of the
experimental results with the published literature data of thermal analysis of boehmite
helps to infer that the first endothermic peak is related to weight loss due to desorption
of physically bound water and the small endothermic peak results from release of
chemically bound water (the hydroxyl group) converting boehmite to -Al2O3.23
Published results of experiments conducted to monitor thermal desorption of gases
from SiC powder in oxygen atmosphere mentioned evolution of CO and CO2 at around
650°C.24 The first exothermic peak is thus possibly related to evolution of carbon oxide
from carbon impurities. Figure 6 shows the XRD patterns of coated SiC heat treated at
different temperatures in air. Although SiC might begin to oxidize at >800°C it became
noticeable only at 1100°C.In the sample heat-treated at 1100°C, a small diffusive
peak of -cristobalite (SiO2) could be detected. The mullite phase was first detected at
T=1250°C, indicating that the exothermic peak at 1297°C corresponds to mullite
crystallization reaction. The oxidation reaction of coated powder at T>1200°C is
therefore expected to be suppressed due to formation of mullite. Figure 7 shows the
DTA peak corresponding to mullite crystallization reaction at different heating rates. A
clear shifting of the peak to higher temperatures is visible with increase of heating
rates. Intervals of the initial peak temperature, Tin, maximum peak temperature, Tmax
and ending peak temperature, Ten, corresponding to different experimental heating rates
and calculated enthalpies are presented in Table 1. From the results of DTA
experiments done at different heating rates, the kinetic parameters of mullite
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crystallization reaction were determined. The areas under the exothermic peaks were
integrated using the trapezodial rule of numerical method. The ratio of the area under
the peak up to a certain value of abscissa, and the total area of the peak, represents the
crystallized fraction (x) of mullite corresponding to the instant (t) under consideration.
The relationship between crystallized fraction of mullite, x, and time under different
heating rates is shown in Fig. 8(a); the crystallization rate against time for different
heating rates is represented in Fig. 8(b). The rate of the crystallization reaction
increased with heating rate. The process of mullite crystallization can be compared
with several processes of phase transformation including the process of crystallization
of glass. The well-known Johnson-Mehl-Avrami theory describes an isothermal
crystallization process:26,27
])(exp[1 nktx (2)
where n is the Avrami exponent, k is the rate constant (k has the Arrhenius type of
temperature dependence: ]exp[ RTEkk o
), E is the activation energy and ko is the
frequency factor. Differentiation of Eq. (2) and further rearrangement give the rate of
crystallization of mullite:
)(xkfdt
dx (3)
where n
n
xxnxf
1
)]1ln()[1()(
(4)
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These equations are described for an isothermal crystallization process. But many
authors show that they can be applied to a non-isothermal process with satisfactory
results under certain boundary conditions.27 Taking logarithm of Eq.(3) and
rearrangement give:
)](ln[ln xfkRT
E
dt
dxo (5)
In a first approximation linearity between rate of crystallization and temperature
inverse was assumed for values of x in which the values of ln[kof(x)] remained
constant. The experimental values were adjusted to a straight line whose slope gave the
first value of activation energy (apparent activation energy). The value of ln[kof(x)]
corresponding to each value of x was calculated by this apparent activation energy
through Eq.(5). From the plots of ln[kof(x)] against x the intervals of x for which the
value of ln[kof(x)] was nearly constant were selected. Figure 9 shows the typical plot of
ln[kof(x)] versus x corresponding to the heating rate of 20 K min-1. With the
experimental data limited to this new interval, linear adjustment was carried out thus
obtaining a second value of the activation energy which was more accurate as the
condition of constancy for ln[kof(x)] was maintained to a greater extent. The repetition
of the procedure gave the more correct value of E. Figure 10 shows the plot of dt
dxln
against temperature inverse for different heating rates and all linear adjustment
correlation coefficients were close to 0.99. For each heating rate activation energy was
calculated and on an average it was equal to 368.9±15.1 kJ mol-1. In the new interval it
was verified that ln[kof(x)] was constant. Then rearrangement of Eq.(4) gives:
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Cxn
nxnko
)]1ln(ln[
1)1ln(lnln (6)
where C is a constant. Equation (6) is valid for any value of x contained in the new
interval. By writing Eq. (6) for two given values of crystallized fractions, x1 and x2 and
subtraction of expression obtained in each case gives:
)1ln(
)1ln(ln
1
1
1ln
2
1
2
1
x
x
n
n
x
x
(7)
Equation (7) on further rearrangement gives the expression for Avrami exponent:
1
11
22
1
2 }])1ln()1(
)1ln()1(][ln{
)1ln(
)1ln(ln[
xx
xx
x
xn (8)
The frequency factor, ko, can be determined from Eq.(6) by substituting the value of n
and the constant C by the value taken by function ln[kof(x)] in the constancy interval
for each heating rate. The kinetic parameters of mullite crystallization reaction
occurring during oxidation of coated powder were determined by these equations and
are listed in Table 1.
The temperature of mullite crystallization depends on the degree of mixing of
aluminium and silicon in the precursors. Natural precursors like aluminosilicate
minerals are advantageous for mullite production because of mixing of Al2O3 and SiO2
on a molecular scale. Li and Thomson studied the formation of mullite in a single-
phase aluminosilicate gel (monophasic precursor) in which Al2O3 and SiO2 were mixed
to achieve three dimensional molecular homogeneity.28 The crystallization of mullite
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occurred at temperatures as low as 940°C by a nucleation controlled process with
activation energy of 293-362 kJ mol-1 29 For similar reasons mullite forms in kaolinite
clays at low temperatures (980-1100°C) in which molecular mixing of Al2O3 and SiO2
is found in only one dimension.30-32 The wide range of mullite crystallization
temperature in kaolin is stated to be due to different kaolin samples having different
impurities or particle size distribution of starting materials. The activation energy of
mullite crystallization in kaolin is 1182 kJ mol-1 with an associated growth morphology
parameter (n) of 2, indicating a nucleation and two-dimension diffusion-controlled
growth process of mullite crystalls.32 When scale of homogeneity is in nanometer
range, i.e. from 1 to 100 nm in diphasic aluminosilicate gels, mullite formation can be
delayed to temperatures as high as 1350°C and mullite forms in this case by a
nucleation and growth process in the silica rich matrix (that fits Avrami model) with an
apparent activation energy of 1070±200 kJ mol-1.29,33 The mullite crystallization
temperatures above 1200°C are likely to be related to processing related alumina-silica
segregation and corresponding increase in diffusion path length. In case of a
monophasic precursor three dimensional molecular homogeneity minimizes the
diffusion path length and makes mullite formation no longer be a diffusion controlled
process. When mullite is produced through reaction of powder samples Al2O3 and
SiO2 (micron-sized powders) at temperatures above 1650°C, nucleation and growth of
mullite as an interfacial product can occur and the growth is controlled by
interdiffusion of aluminum and silicon ions through mullite layer.34,35 Because of low
diffusivities the Al2O3 and SiO2 mixed on a micrometer scale require high
temperatures for mullite formation. In the present work average activation energy of
368.9±15.1 kJ mol-1 was obtained and it can be attributed to some kind of molecular
structure with Al-O-Si bonding similar to that of mullite in the alumina-silica
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precursor. Li and Thomson observed that when the single phase aluminosilicate gels
were heat-treated at 900°C, the absorption peak at 850 cm-1, corresponding to Al-O-Al
stretching vibrations in tetrahedral Al, shifted to a higher frequency with increasing
temperature because of coupling of AlO4 tetrahedra with SiO4 tetrahedra.28 Moenke
also found a similar shift to a higher wavenumber in the absorption bands of SiO4
tetrahedra at 1100 cm-1 with formation of Al-O-Si bonds.36 For examination of
favourable molecular structure formation before mullite formation, the boehmite
coated SiC powder was heat-treated to 1000°C and characterized by FTIR
spectroscopic analysis. It was observed that the peak at around 880 cm-1,
corresponding to tetrahedrally coordinated aluminum (AlO4 atom group), shifted to a
higher frequency of 1106 cm-1 after the heat treatment, likely because of coupling of
the AlO4 tetrahedra with SiO4 tetrahedra (Fig.4). The mullite crystallization reaction in
a single-phase gel and boehmite coated SiC (of present study), therefore, has a low
activation energy due to formation of the favourable molecular structure before
mullitization. The low activation energy of mullite crystallization indicates possibility
of oxidation bonding of porous SiC at low temperature using the coated powder. To
realize the possibility compacts of coated powder at were heat treated at 1250 and
1350°C for 4 h in air and the oxidation bonded samples were characterized by
measuring porosity and pore size and examining the microstructure. The recorded
porosity of the SiC ceramics oxidation bonded at 1250 and 1300°C were 54% and
48%, respectively; microstructure examination revealed formation of interconnected
pores in the SiC ceramics. The image analysis results showed that the samples
prepared at 1250 and 1300°C had average pore sizes of 174 and 263 nm, respectively.
The typical microstructure of the porous ceramic sample prepared at 1250°C is shown
in Fig. 11. The experimental results demonstrated that SiC ceramics of high porosity
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(around 50%) and fine pore sizes (170-260 nm) could be synthesized using the
boehmite coated SiC powder of sub-micron size following a low temperature oxidation
bonding method.
4. Conclusions
The effect of boehmite coating on the thermal oxidation of boehmite coated
SiC powder was examined. With ~24 wt.% boehmite, a coating thickness of ~ 12 nm
was achieved and thermal oxidation of the coated powder was found to involve mullite
crystallization at a low temperature of around 1250°C because of atomic scale
arrangement of –Al-O-Si- groupings similar to that of mullite (before mullite
formation). The experimental rate data were fitted with the Johnson-Mehl-Avrami
transformation equations which suggested a low activation energy equal to 368.9±15.1
kJ mol-1 ~ similar in values obtained for mullite formation in monophasic
aluminosilicate precursor gels ~ likely because of mixing of Al2O3 and SiO2 on a
molecular scale. Porous SiC ceramics (of porosity and pore size of around 50% and
170-260 nm) were possible to be synthesized using the oxidation of coated powder at
low temperatures (1250-1300°C).
Acknowledgment
The authors are grateful for the financial support provided by CSIR-CGCRI
under the 12th Five Year Plan Project entitled “Advanced ceramic materials and
components for energy and structural application, CERMESA, ESC0104, (WP 1.2)”.
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One of the authors (AD) expresses grateful appreciation to CSIR-CGCRI for its
support to him under the CSIR Project.
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Figure Caption:
Fig.1. XRD pattern of the precipitate from the aluminium secondary butoxide solution
after drying at 100°C.
Fig.2. Particle size distribution of different particles: ● boehmite coating material; ▲
SiC powder; ■ SiC powder coated with ~24wt.% boehmite.
Fig.3. Zeta potential versus pH: ▲ SiC powder; ■ SiC powder coated with ~24wt.%
boehmite.
Fig.4. FTIR spectrum of the boehmite coated SiC powder within 400-3200 cm-1 after
heat treatment at 1000°C (top); also presented are the spectra of SiC powder (bottom)
and boehmite coated SiC powder (middle) without heat treatment.
Fig.5. TG/DTA curves of boehmite coated SiC at a heating rate of 40 K min-1.
Fig.6. X-ray diffraction patterns of boehmite coated SiC after heat treatment at
different temperatures; also plotted is the XRD pattern of SiC without heat treatment
(bottom). s = SiC (JCPDS Code: 01-075-0254), cr = SiO2 (JCPDS Code: 00-076-
0936), m = mullite (JCPDS Code: 00-015-0776).
Fig.7. DTA curves of SiC powder coated with ~24 wt.% boehmite at different heating
rates in a stream of air.
Fig.8. Plots showing (a) relationship between mullite crystallized fraction ‘x’ with time
‘t’ and (b) rate of mullite crystallization reaction versus time under different
experimental heating rates.
Fig.9. Plot of ln [kof(x)] versus x for the heating rate of 20 K min-1.
Fig.10. Plot of ln(dx/dt) versus absolute temperature inverse; open circle represents the
experimental data and dotted lines show the fitting curves.
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Fig.11. Microstructure of porous SiC ceramics sintered at 1250°C using boehmite
coated SiC powder; microstructure viewed under higher magnification is shown in the
inset.
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Highlights
Oxidation of Al2O3 coated 0.6 m SiC powder was studied by thermal analysis
method
Oxidation of coated powder involves crystallization of mullite at ~1300°C
Process of mullite crystallization has an activation energy of 369 kJ mole-1
Oxidation bonding of porous SiC is possible using coated powder at low
temperature
Oxidation bonded SiC ceramics have interconnected porosity and fine pore structure
Highlights (for review)
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Table 1: The kinetic parameters obtained for mullite crystallization reaction by
analyzing the exothermic peaks corresponding to different experimental heating
rates
Heating
rate
(K min-1
)
Temperatures relating to
the mullite crystallization
exotherm
Enthalpy
(mcal mg-1
)
Interval of
crystallized size
fraction for
constant
ln[k0f(x)]
Correlat
ion co-
efficient
(R2)
Activation
energy
(kJ mole-1
)
Abhrami
Exponent
(n)
Frequency
factor
(k0)
Tin Tmax Tend
20 1183.1 1294.4 1334.2 1.13 0.37-0.64 0.99 385.27 1.05±0.30 9.2×1017
25 1187.4 1305.9 1355.2 1.57 0.15-0.46 0.99 367.20 1.22±0.71 5.1×1018
30 1196.5 1317.9 1376.7 1.41 0.19-0.44 0.99 349.32 1.19±1.62 4.0×1016
40 1203.5 1323.7 1386.1 1.11 0.13-0.59 0.99 374.15 1.23±1.04 5.4×1019
Table(s)
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Figure(s)