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Hydrogen transport in 2.5 m Pd-Agmembranes: experimental and
modeling results
Marco Giacinti Baschetti, Giulio Cesare Sarti
Dipartimento di Ingegneria Chimica, Mineraria e delleTecnologie Ambientali
Alma Mater Studiorum - Università di Bologna
Motivation
† B.C.R. Ewan and R.W.K. Allen, International Journal of Hydrogen Energy, 30 (2005), Pages 809-819.
Conventional Hydrocarbon steam reforming
Membrane Units• Same theoretical efficiency as PSA• more compact and less energy demanding
Alma Mater Studiorun – Università di Bologna
AIM• Study membrane behavior with different feed compositions• Study membrane units• Model and design membrane units
Experimental and Materials
Pd0.8-Ag0.2 membrane. Selective layer ~2.5 m
An extensive study has beenconducted on Pd-Ag membranesproduced by NGK Inc. (Japan)
Membrane featuresDeposition Technique Electroless Deposition
Membrane length 90 mm
Membrane O.D. 10 mm
Support Asymmetric -Al2O3
Layer thickness 2.5 m
Pd-Ag composition 80%w Pd - 20%w Ag
Alma Mater Studiorun – Università di Bologna
Experimental and Materials
An experimental module has been set up, able to measure permeation of purehydrogen as well as hydrogen mixtures in Pd-Ag membranes at temperatures up to700°C and pressure up to 15 bar.
Operative conditions in the test
Gases H2, N2, CH4, CO,H2O
Temperaturerange 200 - 500 °C
Max pressure 7 bar
Feed flow-rate 1-3 Nl/min
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Experimental Results: Pure Hydrogen
723 K
673 K
773 K
The Hydrogen flux:
closely follows the Sieverts’ law;Is not affected by feed-flow rate
Membranes are defect-free
2 2
2 2
u dH H
H H
p p
N
I II
III
I. Dissociativeadsorption
II. Surface-to-Bulktransition
III. Atomic diffusion
Step I and II at equilibrium Sieverts’ Law
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Feed flowrate
Feed flowrate
88% H2
50% H2
The Hydrogen flux:
Is lower than for pure H2 at
same driving force;
Is affected by feed-flow rate:Increases by increasing
feed flow-rates
Depends on H2 feed content:Increases with H2 content
in the feed.
Concentration Polarization isimportant in the membrane
module
Experimental Results: H2-N2 Mixtures
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Similar behavior in comparisonwith H2-N2 mixtures:
The difference between pureHydrogen data and mixtures one is
not in the chemistry (i.e.competitive adsorption) but in the
transport.
Methane and Nitrogen have to beconsidered as inert gases, andconcentration polarization isconfirmed in the membrane
module
1 NL min-1
2 NL min-1
The mixtures have:
Experimental Results: H2-N2-CH4
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2 2 2 2H H H Hint retp p N K
boundarylayer
2
s h e l lHP
2
,s h e l l IHP
2
l u m e nHP
feed permeate
Permeate flux
Bulk flow
nH
Gas phase resistanceHp. high mass transfer rate
Membrane resistance
2
2
2
2 2
2
H ,H ,
H ,
H , H ,
H
1ln
1int
int Gret
ret intG
ML
xk
x
p pk
p p
N
2
shellNP
2
,shell INP
The hydrogen depletion (and theaccumulation of non permeating gases) inthe boundary layer is modeled using the
two resistance in series.
Metal membrane
Modeling inert mixtures behavior
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Modeling inert mixtures behavior
Regression results: lines are obtained through model calculations
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300°C 250°C
400°C450°C
Water interacts with themetallic membrane and
actively hinders hydrogenpermeation through Pd-
based membranes.
Experimental Results: H2-H2O Mixtures
The inhibition effect iscompletely reversible and
the membrane recoverthe initial permeability
value as soon as the watervapor is removed from
the feed.
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H2-CO experiments showed a flux depletion also at 2% of CO. The membrane experienced anon reversible poisoning upon CO exposure; the original permeance of pure H2 could be
restored only by applying a cleaning process
Experimental Results: H2-CO Mixtures
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The effects on the hydrogenflux depletion in ternarymixtures experimentscontaining two competitivegases seems to be nonadditive.
Experimental Results: H2-H2O-CO
No substantial changes inhydrogen permeation flux areobserved by substitutingcarbon monoxide to nitrogenin a H2-H2O-N2 mixture.
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Kinetic stage Flux equation
(I) Surfaceadsorption/desorption
processes(upstream surface)
(II) Surface to bulktransition
(upstream side)
( III) Solid-state atomicdiffusion
(IV) Bulk to surface(downstream side)
(V) Surfacedesorption/adsorption
processes(downstream surface)
† T. L. Ward and T. Dao, Journal of Membrane Science, 153 (1999), Pages 211-231
H2 transport in Pd membranes can be described by the well known approach proposed by wardand Dao† , that is based on a 5 step process:
2 2
2
0.522
H H , 0 H,1H
2 2,0 H,1
1 12
2 exp
i S
Dd S
p S nkTm
Ek nRT
N
2H 0 H,1 ,1
,1 H,1 0
1 exp 12
1 1 exp2
S BS b s
B SS b s
En n xRT
En n xRT
N
2H 0 ,1 ,2
1 exp /2
diffb s s
En x x
RT
N D
2H ,2 H,2 0
0 H,2 ,2
1 1 exp2
1 exp 12
B SS b s
S BS b s
En n xRT
En n xRT
N
2
2
2
2 2H ,0 H,2
0.522
H ,2 0 H,2H
2exp
1 12
Dd S
S
Ek nRT
p S nkTm
N
Modeling permeability: pure hydrogen
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Effects of CO on H2 permeability
Carbon monoxide is known to adsorb on Pd through a rather complex process thatinvolves different type of configurations characterized by different adsorption energies †.
† O. Dulaurent et Al., Journal of Catalysis, Volume 188 (1999), Pages 237-251
Bridge bonded
LinearECO=92-54 kJ/mol
The adsoprtion energy of each species of adsorbedCO has changes with surface coverages.
Relative fraction of the different species adsorbedchanges with temperature and is dependent on thesurface history.
ECO=168-92 kJ/mol
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A model has been evelopedconsidering competitiveadsorption of CO and H2.The adsorption energy ECOis linear with CO surfacecoverage and is the onlyfitting parameter.
The model is able todescribe a broad variety ofbehaviors
data from J. Chabot, J. Lecomte, C. Grumet and J. Sannier, Fusion Technology,14 (1988), Pages 614–618
CO COE a b
a = -30 kJ mol-1
b = 140 kJ mol-1
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Effects of CO on H2 permeability
data from H. Nguyen, S. Mori, M. Suzuki, Chemical Engineering Journal, 155 (2009), Pages 55-61
Comparison with literature data
When a linear decrease ofECO with CO surface
coverage is consideredexperimental data fromdifferent sources can bedescribed very well usingthis quantity as fittingparameter.At least until the value of
CO does not become toohigh.
CO COE a b
a = -30 kJ mol-1
b = 120 kJ mol-1
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In order to model thepermeation of hydrogen inpresence of water vapor bothconcentration polarization andcompetitive adsorption needto be considered.
A local approach has beenconsidered by dividing themembrane in an arbitrarynumber of small segments.
x
Model steps
Transport in the gas phase
Surface adsorption/desorption processes(upstream surface)
Surface to bulk transition(upstream side)
Solid-state atomic diffusion
Bulk to surface(downstream side)
Surface desorption/adsorption processes(downstream surface)
Application to current exp. data
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Experimental data ofhydrogen flux in presence ofwater vapor are welldescribed in the rangebetween 450-350°C with asingle fitting parameters thatis:
EH2O = 125 kJ/mol
*J. Catalano et.al., Int J. Hydrogen Energy, 36 (2011) pages 8658-8673
Application to current exp. data
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Permeation tests of pure hydrogen and several mixtures were performed on aPd-Ag membranes endowed with a high permeable dense and defect free Pd-Aglayer
Experimental work on several binary mixtures showed decrease in hydrogenflux with respect to pure hydrogen experiments. However the data suggest that:
• Nitrogen can be considered as an inert and H2 flux depletion is due toconcentration polarization phenomena .• Steam and carbon monoxide seems to hinder hydrogen permeation and
possible competitive adsorption on the metal surface has to be considered.A simple model for to account for concentration polarization allowed to
describe the hydrogen flow in the presence of N2
A physically consistent approach was developed to account for the influence onhydrogen flux of non-inert gases.
• Coupling this model allowed to describe also the effect of water vapor onthe hydrogen permeate flux in the membrane
Final Conclusion
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Acknowledegements
Dr. K. I. Noda and NGK Insulator Ltd (Japan) for the membranes
Italian Ministry of Research (MIUR) for funding
David Alique, Ryan Worth, Franscesco Fusi, Marco Castellani, Matthew Purcell forthe help in the experimental work
Alma Mater Studiorun – Università di Bologna