35nd acs national meeting april 6-10, 2008 new orleans, louisiana organizers : umit s. ozkan...
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35nd ACS National Meeting April 6-10, 2008 New Orleans, Louisiana
Organizers : Umit S. Ozkan Jingguang G Chen
Presiding: Thursday April 10, 2008, 11:45 am. -12:15 PM. Morial Convention Center, Room: Rm. 208
N.Galea, D.Knapp, E.Kadantsev, M.Shiskin, T.Ziegler Department of Chemistry University of Calgary,Alberta, Canada T2N 1N4
New Orleans National Meeting
Studying SOFC anode activity with DFT: Suggestions for cokereduction and the effects of hydrogen sulfide adsorption
Symposium on Roles of Catalysis in Fuel Cells
Division for Petrochemistry
Solid Oxide Fuel Cell – CH4
2O2-
O2 + 4 e-
O2 -
H2O + 2e-
H2 + O2-
*Most commonSOFC material
*Ni-YSZTemp.800 –
1000 oC
V +-
Anode CathodeElectrolyte
*YSZ
CH4 + 4O2- 2H2O + CO2 + 8e- (Direct Oxidation,coaking) CH4 + H2O CO + 3H2 (Steam Reforming Reaction) H2/CO + O2- H2O/CO2 + 2e- (Oxidation Reaction)
Molecular hydrogen or methane gas is typical anode fuel.CH4 adsorbs on Ni anode surface and decomposes, blocking adsorption sites with graphene, most stable form of carbon.
The problem of cokingThe problem of coking
Activation on Ni
H2 --> 2H*
CH4 --> xH*+CH4-x
Triple Phase Boundary (TPB) Reactions
Anode Electrolyte Cathode
2O2- 2O2-
2O2-
Nickel/YSZ YSZ
Nickel
YSZ
O2(g)
Oxygen rich YSZ
4e-
Pre-activation on Ni
Burning on oxygen rich YSZ
2H+ O2 ----> H2O +2e-
CH4-x + +(8-x)/2 O2- ---> CO2+(4-x)/2H2O+(8-x)e-
+C(Coke)
Surface Calculations – CH4
Two classes of active adsorption sites. Stepped surfaces more reactive than planar surfaces. Supercell; 3 layers, 2x2(planar) or 2x3(stepped) surface.
Planar (111) - *CStepped (211) - *C
Steps and TerracesSteps and Terraces
Calculations – CH4
Vienna Ab Initio Package (VASP). ADF BAND Projector augmented wave (PAW) method. Frozen core (BAND) Generalized gradient approximation (GGA) functional PBE96. Planar (111) Surfaces: 2x2 unit cell, with 3 layers. Stepped (211) Surfaces: 3x3 unit cell, with 3 layers. Theoretical equilibrium bulk lattice constants, aO(Ni) is 3.52Ǻ and aO(Cu) is 3.61Ǻ. 10Ǻ vacuum region between slabs. Cu(111): 5 x 5 x 1 Monkhorst-Pack k-point mesh. Other Surfaces: 4 x 4 x 1 Monkhorst-Pack k-point mesh. Kinetic energy (wave function) cutoff energy is 25Ry = 340eV. Charge density (augmentation) cutoff energy is 50Ry = 680eV. Energies converged to 10-3eV. TS and reaction barriers calculated using the nudged-elastic band (NEB) method.
MatLab mathematical software package.
Computational DetailsComputational Details
N.Galea,D.Knapp,T.Ziegler Journal of Catalysis 247 (2007) 20-33
Ni(111) and Ni(211) Surfaces :Adsorption and Decomposition of CH4
Theoretical literature – Nørskov. Planar surface implies that coking should not occur. Stepped surface energies illustrating final exothermic
dissociation reaction is driving force of coke formation.
-25
-20
-15
-10
-5
0
5
10
Relative Energy (kcal/mol)
Surface
Ni(211)
CH4(g)
(b)
(a)
Ni(111)
*CH3, *H *CH2, 2*H *CH, 3*H *C, 4*H
(a) (b)
Decomposition of CH4 on steps and terraces of NiDecomposition of CH4 on steps and terraces of Ni
Graphene
Ni(111) & Ni(211)
25
1317
24
11
41
24
31
2320
1011
23
4
-5
22
-15
-10
-5
0
5
10
15
20
25
30
35
40
45
Relative Energy (kCalmol
-1)
Ni(111) : Planar SurfaceNi(211) : Stepped Surface
Graphene
CH4(g)+ Surface
*CH3,*H *CH2,2*H
*CH,3*H
*C,4*H
Bengaard et al. J. Catal. 2002, 209 , 365-384.
Ni
NiNi
NiNi
C
NiNi
Ni
Ni
NiNi
NiNi C
Ni
H
H
Ni
Ni
Ni
NiNi
H
Ni
HC
Ni
Ni
H
Ni
Ni
Ni
NiNi
NiNi
C
Ni
H
Ni
Ni
Ni
Ni
Ni
H
Ni
H
Ni
C
H
H
Ni
Ni
Ni
Ni
NiNi
NiNi
Ni
H
Ni
Ni
Ni
Ni
H
C
Ni
H
H
1-fold@edge
2-fold@edge
5 coordinate site
3-fold
Decomposition of CH4 on steps and terraces of NiDecomposition of CH4 on steps and terraces of Ni
N.Galea,D.Knapp,T.Ziegler Journal of Catalysis 247 (2007) 20-33
Graphene
Carbon is adsorbed at step base, resulting in formation of graphene (coke) layer on (111) terrace. Ni and hexagonally structured carbon atoms lie parallel to one another.
Graphene island of finite size
is required for stability.
Blocking all step sites is
NOT needed to prevent formation.
Sparse covering of promoter atoms (e.g. gold, sulfur, alkali) or replacing Ni with Cu can hinder coke formation.
NiNiNi
NiNiNiNi
Ni
Ni
Ni
Ni
Ni
Ni
NiNi
NiNi
Ni
Ni
Ni
Ni
NiNi
NiNiNi
(Pictorialrepresentation
of surface)
Graphen formationGraphen formation
Cu(111) and Cu(211) Surfaces :Adsorption and Decomposition of CH4
Activity of copper in the dissociation of methane will be poor. Carbon cokes will not form on copper surfaces. Consistent with experimental SOFC observations.
0
10
20
30
40
50
60
70
80
90
100
110
Relative Energy (kcal/mol)
Surface
Cu(211)
CH4(g)
Cu(111)
*CH3, *H *CH2, 2*H *CH, 3*H *C, 4*HTS TS TS TS
Galea et al. Journal of Catalysis 247 (2007) 20-33
Decomposition of CH4 on steps and terraces of CuDecomposition of CH4 on steps and terraces of Cu
N.Galea,D.Knapp,T.Ziegler Journal of Catalysis 247 (2007) 20-33
Cu(111) and Cu(211) Surfaces :Adsorption and Decomposition of CH4
Activity of copper in the dissociation of methane will be poor. Carbon cokes will not form on copper surfaces. Consistent with experimental SOFC observations.
0
10
20
30
40
50
60
70
80
90
100
110
Relative Energy (kcal/mol)
Surface
Cu(211)
CH4(g)
Cu(111)
*CH3, *H *CH2, 2*H *CH, 3*H *C, 4*HTS TS TS TS
Galea et al. Journal of Catalysis 247 (2007) 20-33
Decomposition of CH4 on steps and terraces of CuDecomposition of CH4 on steps and terraces of Cu
N.Galea,D.Knapp,T.Ziegler Journal of Catalysis 247 (2007) 20-33
Cu(111) and Cu(211) Surfaces :Adsorption and Decomposition of CH4
Activity of copper in the dissociation of methane will be poor. Carbon cokes will not form on copper surfaces. Consistent with experimental SOFC observations.
0
10
20
30
40
50
60
70
80
90
100
110
Relative Energy (kcal/mol)
Surface
Cu(211)
CH4(g)
Cu(111)
*CH3, *H *CH2, 2*H *CH, 3*H *C, 4*HTS TS TS TS
Galea et al. Journal of Catalysis 247 (2007) 20-33
Decomposition of CH4 on steps and terraces of CuDecomposition of CH4 on steps and terraces of Cu
N.Galea,D.Knapp,T.Ziegler Journal of Catalysis 247 (2007) 20-33
Cu(111) and Cu(211) Surfaces :Adsorption and Decomposition of CH4
Activity of copper in the dissociation of methane will be poor. Carbon cokes will not form on copper surfaces. Consistent with experimental SOFC observations.
Galea et al. Journal of Catalysis 247 (2007) 20-33
0
10
20
30
40
50
60
70
80
90
100
110
Relative Energy (kcal/mol)
Surface
Cu(211)
CH4(g)
Cu(111)
*CH3, *H *CH2, 2*H *CH, 3*H *C, 4*HTS TS TS TS
Decomposition of CH4 on steps and terraces of CuDecomposition of CH4 on steps and terraces of Cu
N.Galea,D.Knapp,T.Ziegler Journal of Catalysis 247 (2007) 20-33
Cu(111) and Cu(211) Surfaces :Adsorption and Decomposition of CH4
Activity of copper in the dissociation of methane will be poor. Carbon cokes will not form on copper surfaces. Consistent with experimental SOFC observations.
Galea et al. Journal of Catalysis 247 (2007) 20-33
0
10
20
30
40
50
60
70
80
90
100
110
Relative Energy (kcal/mol)
Surface
Cu(211)
CH4(g)
Cu(111)
*CH3, *H *CH2, 2*H *CH, 3*H *C, 4*HTS TS TS TS
Decomposition of CH4 on steps and terraces of CuDecomposition of CH4 on steps and terraces of Cu
N.Galea,D.Knapp,T.Ziegler Journal of Catalysis 247 (2007) 20-33
Cu(111) & Cu(211)
86.79
105.35
56.09
70.50
44.70
23.33
70.69
44.54
27.11
40.10
7.75
33.24 30.49
48.19
72.03 72.30
0
10
20
30
40
50
60
70
80
90
100
110
Relative Energy (kCal/mol)
Cu(111)Cu(211)
CH4(g) + Surface *CH3 + *H *CH2 + 2*H *CH + 3*H *C + 4*H
*CH3 = 2-fold@Edge
*CH2 = 3-fold@edge2f
*CH = 5-coordination site
*C = 5-coordination site*H = 3-fold@edge2f
CH4(g) = 2-fold@Edge
Cu(111) & Cu(211)Supercell surface unit cells = (2x2) & (3x3).
Layers = 3 & 9.Lattice Constant, a = 3.615 Angstroms.
Lattice Vectors (Angstroms) :-x = 4.316 & 6.261.y = 4.984 & 7.668.
z = 14.069 & 16.588.GGA = PBE, utilizing PAW Method.
Cutoff Energies (Ry) :-Wavefunction = 37 & 25.
Charge Density = 74 & 50.k-points : Monkhorst-pack = 3x2x1 & 4x4x1.
Adsorption Energy(eV)
*CH3 : 1.30 & 1.78*CH2 : 3.91 & 3.33*CH : 4.69 & 5.47*C : 4.50 & 5.81*H : 2.42 & 2.58
Cu
Cu
Cu
Cu
Cu
HH
H
C
Cu
Cu
Cu
H
Cu
Cu
Cu
Cu
Cu
H
C
H
Cu
Cu
Cu
H
Cu
CuCu
H
Cu
C
Cu
H
Cu
CuCu
Cu
C
Cu H
CuCu
H
Cu
H
Cu
Galea et al. Journal of Catalysis 247 (2007) 20-33
Decomposition of CH4 on steps and terraces of CuDecomposition of CH4 on steps and terraces of Cu
N.Galea,D.Knapp,T.Ziegler Journal of Catalysis 247 (2007) 20-33
Step Edge - Cu-Ni(211) : Adsorption and Decomposition of CH4
Cu surface segregation occurs as Cu has a lower surface energy than Ni.
Likely that Ni steps that nucleate *C formation are blocked by Cu atoms, exposed terrace Ni sites contribute to activity.
Endothermic *C production on alloy, with reasonable activity.
(a)
-30
-20
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0
10
20
30
40
50
Relative Energy (kcal/mol)
Surface
Ni(211)
CH4(g)
Cu(211)
*CH3, *H *CH2, 2*H *CH, 3*H *C, 4*H
Cu-Ni(211)
(a)
Copper
Galea et al. Journal of Catalysis 247 (2007) 20-33
Decomposition of CH4 on Cu-steps and Ni-terraces Decomposition of CH4 on Cu-steps and Ni-terraces
S-Ni(211)
4.05
17.78
38.85
22.52
10.05
28.81
14.35
25.66
0
5
10
15
20
25
30
35
40
Relative Energy (kCal/mol)
CH4(g) + Surface *CH3 + *H *CH2 + 2*H *CH + 3*H *C + 4*H
NiS(211)Supercell surface unit cells = (2x3).
Layers = 9.Lattice Constant, a = 3.615
Angstroms.Lattice Vectors (Angstroms) :-
x = 6.1005, y = 4.9796, z = 16.000.GGA = PBE, utilizing PAW Method.
Cutoff Energies (Ry) :-Wavefunction = 25.
Charge Density = 50.k-points : Monkhorst-pack = 4x4x1.
*CH = 3-fold@edge2f
*C = 3-fold@edge2f
*H = 3-fold@edge2f
*CH3 = 3-fold@edge2f
*CH2 = 3-fold@edge2f
*Ni(111) = 24*Ni(211) = 20
*Ni(111) = 18*Ni(211) = 12
*Ni(111) = 7*Ni(211) = 12
*Ni(111) = 30*Ni(211) = 19
(26)
(19) (8)
(35)
*Bengaard et al. J. Catal. 2002, 209 , 365-384.
Ni
H
NiNi
S
NiNi
H
H
C
Ni
S
Ni
H
Ni
Ni
H
NiNi
S
NiNi
H
C
H
Ni
S
NiNi
Ni
H
NiNi
S
C
Ni
H
Ni
Ni
S
NiNi
Ni
Ni
H
Ni
S
Ni
C
Ni
H
Ni
S
NiNi
Galea et al. Journal of Catalysis 247 (2007) 20-33
Decomposition of CH4 on S-steps and Ni-terraces Decomposition of CH4 on S-steps and Ni-terraces
N.Galea,D.Knapp,T.Ziegler Journal of Catalysis 247 (2007) 20-33
100% Step – Au/S-Ni(211) : Adsorption and Decomposition of CH4
Small amounts of sulfur / gold can discourage the adsorption of carbon at the step by blocking edge sites, mimicking the nature of the planar nickel surface.
(a)-30
-20
-10
0
10
20
30
Relative Energy (kcal/mol)
Surface
Ni(211)
CH4(g)
*CH3, *H *CH2, 2*H *CH, 3*H *C, 4*H
S100%-Ni(211)
*C", 4*H
(a)Ni(111)
Au100%-Ni(211)Sulfur or Gold
Galea et al. Journal of Catalysis 247 (2007) 20-33
Decomposition of CH4 on (S,Au,S) steps and Ni-terraces Decomposition of CH4 on (S,Au,S) steps and Ni-terraces
N.Galea,D.Knapp,T.Ziegler Journal of Catalysis 247 (2007) 20-33
A. Conclusions – CH4
Our research theoretically studies methods used experimentally to block step sites and reduce graphitic carbon formation.
Propensity to coking of Ni surface explained by strong adsorption of *C atoms at step edge, followed by graphene growth over terrace sites.
Thermodynamic energies and kinetic barriers of methane ads.n and dis.n on Cu surfaces are high, explaining poor activity and lack of coke.
Cu-Ni alloys, where Cu blocks step sites, the catalyst retains activity due to Ni, while *C formation remains endothermic due to Cu.
S-Ni stepped surface (and Au) demonstrates that step blocking renders step sites inactive to methane dis.n and forces ads.n onto terrace sites.
Galea, N.M.; Knapp, D.; Ziegler, T. J. Catal. 2007, 247, 20.
Activation on Ni
H2 --> 2H*
CH4 --> xH*+CH4-x
Triple Phase Boundary (TPB) Reactions
Anode Electrolyte Cathode
2O2- 2O2-
2O2-
Nickel/YSZ YSZ
Nickel
YSZ
O2(g)
Oxygen rich YSZ
4e-
Pre-activation on Ni
Burning on oxygen rich YSZ
2H+ O2 ----> H2O +2e-
CH4-x + +(8-x)/2 O2- ---> CO2+(4-x)/2H2O+(8-x)e-
M.Shishkin N.Galea,D.Knapp,T.Ziegler, work in progress
Triple Phase Boundary (TPB) Reactions
Anode Electrolyte Cathode
2O2- 2O2-
2O2-
Nickel/YSZ YSZ
Nickel
YSZ
O2(g)
Oxygen rich YSZ
4e-
Activation on YSZ
Activation and burning on oxygen rich YSZ
H2+O2- ----> H2O +2e-
CH4 +4 O2- ---> CO2+2H2O+8e-
M.Shishkin N.Galea,D.Knapp,T.Ziegler, work in progress
Triple Phase Boundary (TPB) Reactions
Anode Electrolyte Cathode
2O2- 2O2-
2O2-
Nickel/YSZ YSZ
Nickel
YSZ
O2(g)
Oxygen rich YSZ
4e-
Activation on YSZ
9%-YSZ
Zr
O
Y
M.Shishkin N.Galea,D.Knapp,T.Ziegler, work in progress
Molecular Hydrogen Adsorption onOxygen Rich YSZ
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Relative Energy (kcal/mol)
O"-Surface 2*OH *OH2 O'-Surface
H2(g)
H2O(g)
Initial adsorption of H2(g) on 9%-YSZ is energetically more favourable than on nickel.
TS energy barriers all < +5 kcal/mol.
M.Shishkin N.Galea,D.Knapp,T.Ziegler, work in progress
Methane adsorption on Oxygen rich YSZ: initial stage.
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↑CH4
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*CH4
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↑CH3OH + V
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*CH3 + *H-100
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E (kcal/mol)
M.Shishkin N.Galea,D.Knapp,T.Ziegler, work in progress
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↑CH2O+↑ H2 + V
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*CH3 + *H
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*CH + *H+↑ H2
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E (kcal/mol)
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*CH2+↑ H2
Methane adsorption on Oxygen rich YSZ: Second stage.
Third stage: formaldehyde decomposition on oxygen enriched YSZ surface.
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↑CH2O
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*CH2O
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*CHO + *H
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Energy (kcal/mol)
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*CHO+↑ H2
Methane adsorption on oxygen deficient YSZ surface.
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E (kcal/mol)
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↑CH4
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*CH4
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↑CH3OH + V
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*CH3 + *H
B. Conclusions – CH4
It might be possible to construct anodes of inactive conductors and electrolytes that can oxydize fuels
.
M.Shishkin N.Galea,D.Knapp,T.Ziegler, work in progress
Activation on Ni
H2 --> 2H*
CH4 --> xH*+CH4-x
Solid Oxide Fuel Cell – H2S
Anode Electrolyte Cathode
2O2- 2O2-
2O2-
Nickel/YSZ YSZ
Nickel
YSZ
O2(g)
Oxygen rich YSZ
4e-
Pre-activation on Ni with sulfur deposition
Burning on oxygen rich YSZ
2H+ O2 ----> H2O +2e-
CH4-x + +(8-x)/2 O2- ---> CO2+(4-x)/2H2O+(8-x)e- H2S --> S*+H2(g)
Calculations – H2S
Vienna Ab Initio Package (VASP). Projector augmented wave (PAW) method. Generalized gradient approximation (GGA) functional PBE96. Orthorhombic 2x2 unit cell, with 3 layers. Theoretical equilibrium bulk lattice constant, aO, is 3.52Ǻ. 10Ǻ vacuum region between slabs. 5 x 5 x 1 Monkhorst-Pack k-point mesh. Kinetic energy (wave function) cutoff energy is 400eV. Charge density (augmentation) cutoff energy is 800eV. Energies converged to 10-3eV. TS and reaction barriers calculated using the nudged-elastic band (NEB) method.
MatLab mathematical software package.
Galea, N.M.; Kadantsev, E.S.; Ziegler, T. J. Phys. Chem. C 2007, 111, 14457.Galea, N.M.; Kadantsev, E.S.; Ziegler, T. J. Phys. Chem. C 2007, 111, 14457.
Surface Calculations – H2S
Hydrogen (pairs) Surface Coverage, 2H , is ratio between number of adsorbed hydrogen atom pairs and number of Ni surface atoms.
i.e. 2H:Ni = 1:4, 2H = 0.25ML.
Repeated supercell; 3 layers, 2x2 surface.
Sulfur Surface Coverage, S , is ratio between number of adsorbed sulfur atoms and number of Ni surface atoms.
i.e. S:Ni = 1:4, S = 0.25ML.
Steps and TerracesSteps and Terraces
-60
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0
20
40
60
Relative Energy (kcal/mol)
"S",
S = 0.25ML
"CleanSurface",
S = 0ML
"S__S",
S = 0.50ML
"S_S_S",
S = 0.75ML
"S_S_S_S",
S =1ML
H2S(g)
H2(g)
H2S(g)
H2(g)
H2S(g)
H2(g)
H2S(g)
H2(g)
Maximum Adsorption of H2S(g)
On the basis of thermodynamic energy, the most stable sulfur surface coverage is S = 0.50ML.
Concurs with experimental coverage of 0.50-0.60 ML. Natural S ads.n cutoff point explains decreased exp. activity.
Surface + 4H2S(g) 4*S-Surface + 4H2(g)
“S”
“S__S” “S_S_S”
“S_S_S_S”
Surface+4H2S(g) <--> 4S*-surface+ 4H2S(g)Surface+4H2S(g) <--> 4S*-surface+ 4H2S(g)
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0
10
20
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Relative Energy (kcal/mol)
n*S-Surfacen*S-*SH2
n*S-*S-*H-*H
S = 0.25 - 0.50 ML, n = 1]
S = 0 - 0.25 ML, n = 0]
n*S-*Sn*S-
*SH-*Hn*S-
*SH-*H'n*S-
*S-*H*Hn*S-
*S-*H*H' *S--*S
TSTSTSTSTSTSTS
H2S(g)H2(g)
(b)
(a)
(c)
(d)
Hydrogen Sulfide Adsorption
S = 0-0.25 ML : H2S adsorption is an exothermic reaction. S = 0.25-0.50 ML : H2S adsorption is endothermic. Overall difference in energy is due to steric interactions on the
surface.
n*S-Surface + H2S(g) (n+1)*S-Surface + H2(g)
(c)
(a)
(d)
(b)
nS*-Surface+H2S(g) <--> (n+1)S*-surface+ H2(g)nS*-Surface+H2S(g) <--> (n+1)S*-surface+ H2(g)
Galea, N.M.; Kadantsev, E.S.; Ziegler, T. J. Phys. Chem. C 2007, 111, 14457.Galea, N.M.; Kadantsev, E.S.; Ziegler, T. J. Phys. Chem. C 2007, 111, 14457.
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0
10
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Relative Energy (kcal/mol)
n*S-Surfacen*S-*SH2
n*S-*S-*H-*H
S = 0.25 - 0.50 ML, n = 1]
S = 0 - 0.25 ML, n = 0]
n*S-*Sn*S-
*SH-*Hn*S-
*SH-*H'n*S-
*S-*H*Hn*S-
*S-*H*H' *S--*S
TSTSTSTSTSTSTS
H2S(g)H2(g)
(b)
(a)
(c)
(d)
Hydrogen Sulfide Adsorption
S = 0-0.25 ML : H2S adsorption is an exothermic reaction. S = 0.25-0.50 ML : H2S adsorption is endothermic. Overall difference in energy is due to steric interactions on the
surface.
n*S-Surface + H2S(g) (n+1)*S-Surface + H2(g)
(c)
(a)
(d)
(b)
nS*-Surface+H2S(g) <--> (n+1)S*-surface+ H2(g)nS*-Surface+H2S(g) <--> (n+1)S*-surface+ H2(g)
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0
10
20
30
Relative Energy (kcal/mol)
n*S-Surfacen*S-*SH2
n*S-*S-*H-*H
S = 0.25 - 0.50 ML, n = 1]
S = 0 - 0.25 ML, n = 0]
n*S-*Sn*S-
*SH-*Hn*S-
*SH-*H'n*S-
*S-*H*Hn*S-
*S-*H*H' *S--*S
TSTSTSTSTSTSTS
H2S(g)H2(g)
(b)
(a)
(c)
(d)
Hydrogen Sulfide Adsorption
S = 0-0.25 ML : H2S adsorption is an exothermic reaction. S = 0.25-0.50 ML : H2S adsorption is endothermic. Overall difference in energy is due to steric interactions on the
surface.
n*S-Surface + H2S(g) (n+1)*S-Surface + H2(g)
(c)
(a)
(d)
(b)
nS*-Surface+H2S(g) <--> (n+1)S*-surface+ H2(g)nS*-Surface+H2S(g) <--> (n+1)S*-surface+ H2(g)
-50
-40
-30
-20
-10
0
10
20
30
Relative Energy (kcal/mol)
n*S-Surfacen*S-*SH2
n*S-*S-*H-*H
S = 0.25 - 0.50 ML, n = 1]
S = 0 - 0.25 ML, n = 0]
n*S-*Sn*S-
*SH-*Hn*S-
*SH-*H'n*S-
*S-*H*Hn*S-
*S-*H*H' *S--*S
TSTSTSTSTSTSTS
H2S(g)H2(g)
(b)
(a)
(c)
(d)
Hydrogen Sulfide Adsorption
S = 0-0.25 ML : H2S adsorption is an exothermic reaction. S = 0.25-0.50 ML : H2S adsorption is endothermic. Overall difference in energy is due to steric interactions on the
surface.
n*S-Surface + H2S(g) (n+1)*S-Surface + H2(g)
(c)
(a)
(d)
(b)
nS*-Surface+H2S(g) <--> (n+1)S*-surface+ H2(g)nS*-Surface+H2S(g) <--> (n+1)S*-surface+ H2(g)
-50
-40
-30
-20
-10
0
10
20
30
Relative Energy (kcal/mol)
n*S-Surfacen*S-*SH2
n*S-*S-*H-*H
S = 0.25 - 0.50 ML, n = 1]
S = 0 - 0.25 ML, n = 0]
n*S-*Sn*S-
*SH-*Hn*S-
*SH-*H'n*S-
*S-*H*Hn*S-
*S-*H*H' *S--*S
TSTSTSTSTSTSTS
H2S(g)H2(g)
(b)
(a)
(c)
(d)
Hydrogen Sulfide Adsorption
S = 0-0.25 ML : H2S adsorption is an exothermic reaction. S = 0.25-0.50 ML : H2S adsorption is endothermic. Overall difference in energy is due to steric interactions on the
surface.
n*S-Surface + H2S(g) (n+1)*S-Surface + H2(g)
(c)
(a)
(d)
(b)
nS*-Surface+H2S(g) <--> (n+1)S*-surface+ H2(g)nS*-Surface+H2S(g) <--> (n+1)S*-surface+ H2(g)
Adsorption Energies
Adsorbed *S-Surface, Adsorption Ni-S Bond
Species Final S. Energy, EAds. Distance (Ǻ)
*SH2 10 2.18
*SH 0.25ML 77 2.18(x2)
*S 116 2.15(x3)
(*H) (64)
*SH2 7 2.30
*SH 0.50ML 53 2.24(x2)
*S 90 2.22, 2.19(x2)
(*H) (61) -
EAds (kcal/mol) = ESurface + EGas - EAdsorbedSpecies
Galea, N.M.; Kadantsev, E.S.; Ziegler, T. J. Phys. Chem. C 2007, 111, 14457.Galea, N.M.; Kadantsev, E.S.; Ziegler, T. J. Phys. Chem. C 2007, 111, 14457.
-50
-40
-30
-20
-10
0
10
20
30
Relative Energy (kcal/mol)
n*S-*H*H'
n*S-*H*H
n*S-*H-*H *H --*Hn*S-Surface*S --*S
S = 0.25ML, n = 1]
S = 0.50ML, n = 2]
2H = 0 - 0.25 ML)
TS TS TS TS TS TS
*H -*H
TS*H -*H-*H*H 4*H
2H = 0.25- 0.50 ML)
S = 0ML, n = 0]
H2(g)
H2(g)
Molecular Hydrogen Adsorption
0S : S = 0.00ML, max. 2H = 0.50ML : Ads.n strongly exothermic. 1S : S = 0.25ML, max. 2H = 0.25ML : Adsorption exothermic. 2S : S = 0.50ML, max. 2H = 0.25ML : Adsorption endothermic. Presence of surface sulfur reduces hydrogen adsorption by half.
n*S-Surface + xH2(g) 2x*H-n*S-SurfacenS*-Surface+xH2(g) <--> 2xH*-nS*-SurfacenS*-Surface+xH2(g) <--> 2xH*-nS*-Surface
-50
-40
-30
-20
-10
0
10
20
30
Relative Energy (kcal/mol)
n*S-*H*H'
n*S-*H*H
n*S-*H-*H *H --*Hn*S-Surface*S --*S
S = 0.25ML, n = 1]
S = 0.50ML, n = 2]
2H = 0 - 0.25 ML)
TS TS TS TS TS TS
*H -*H
TS*H -*H-*H*H 4*H
2H = 0.25- 0.50 ML)
S = 0ML, n = 0]
H2(g)
H2(g)
Molecular Hydrogen Adsorption
0S : S = 0.00ML, max. 2H = 0.50ML : Ads.n strongly exothermic. 1S : S = 0.25ML, max. 2H = 0.25ML : Adsorption exothermic. 2S : S = 0.50ML, max. 2H = 0.25ML : Adsorption endothermic. Presence of surface sulfur reduces hydrogen adsorption by half.
n*S-Surface + xH2(g) 2x*H-n*S-SurfacenS*-Surface+xH2(g) <--> 2xH*-nS*-SurfacenS*-Surface+xH2(g) <--> 2xH*-nS*-Surface
-50
-40
-30
-20
-10
0
10
20
30
Relative Energy (kcal/mol)
n*S-*H*H'
n*S-*H*H
n*S-*H-*H *H --*Hn*S-Surface*S --*S
S = 0.25ML, n = 1]
S = 0.50ML, n = 2]
2H = 0 - 0.25 ML)
TS TS TS TS TS TS
*H -*H
TS*H -*H-*H*H 4*H
2H = 0.25- 0.50 ML)
S = 0ML, n = 0]
H2(g)
H2(g)
Molecular Hydrogen Adsorption
0S : S = 0.00ML, max. 2H = 0.50ML : Ads.n strongly exothermic. 1S : S = 0.25ML, max. 2H = 0.25ML : Adsorption exothermic. 2S : S = 0.50ML, max. 2H = 0.25ML : Adsorption endothermic. Presence of surface sulfur reduces hydrogen adsorption by half.
n*S-Surface + xH2(g) 2x*H-n*S-SurfacenS*-Surface+xH2(g) <--> 2xH*-nS*-SurfacenS*-Surface+xH2(g) <--> 2xH*-nS*-Surface
-70
-50
-30
-10
10
30
50
70
Relative Energy (kcal/mol)
"CleanSurface" "S__S"
"S" "S_S"
S = 0.25ML] S = 0.50ML]H2S(g)
H2S(g)
H2(g)
H2(g)
"S_H_H"
"S_S_H_H"
Multiple H2S(g) Adsorptions at 800oC
Surface + 2H2S(g) 2*S-Surface + 2H2(g)
Point A : Despite large TS barriers, exothermic/exergonic nature of overall reaction produces a S = 0.50ML surface.
Point B : Removal of H2S from the anode fuel feed allows the partial removal of surface sulfur, due to small difference in energy between species “S__S” and “S”.
Surface+2H2S(g) <--> 2S*-Surface+ 2H2(g) Surface+2H2S(g) <--> 2S*-Surface+ 2H2(g)
CSTR Kinetic Model
Continually Stirred Tank Reactor (CSTR) model. Reactor described by a ‘box’ (mimicking the anode), with a specific
volume and maintained at a particular temperature. The ‘surface’ within the box (mimicking the anode surface) has a specific
reactive surface and vacant adsorption site concentration. Gaseous fuel continually flows into CSTR (anode fuel feed) and gaseous
products or unused fuel continually flow out with a specific flowrate. Gaseous species can adsorb/desorb on the surface, and adsorbed species can
react with each other. Sulfur surface coverage and surface steric interactions are considered by
dissecting the surface into equally sized sections (2x2) and considering each section as a vacant site.
Determining Rate of Reactions : TS = T.S(translational/rotational).
H2S(g)/800oC, TS = 53 kcal/mol,
H2(g)/800oC, TS = 34 kcal/mol.
€
G = Δ H − TΔ S
k =kBT
hexp −
ΔG
RT
⎛
⎝ ⎜
⎞
⎠ ⎟
Galea, N.M.; Kadantsev, E.S.; Ziegler, T. J. Phys. Chem. C 2007, 111, 14457.Galea, N.M.; Kadantsev, E.S.; Ziegler, T. J. Phys. Chem. C 2007, 111, 14457.
Rate of Formation of Individual Species
Individual rate constants, k, used to determine time-dependant rate of formation of each species in reaction scheme.
Example reaction mechanism :
Integration over time :
€
A + Bk−1
k1↔ C
k−2
k2↔ D
€
d
dtC[ ] = k1 A[ ] B[ ] − k−1 C[ ] − k2 C[ ] + k−2 D[ ]
d
dtD[ ] = k2 C[ ] − k−2 D[ ]
€
d
dtA[ ] = −k1 A[ ] B[ ] + k−1 C[ ]
d
dtB[ ] = −k1 A[ ] B[ ] + k−1 C[ ]
Galea, N.M.; Kadantsev, E.S.; Ziegler, T. J. Phys. Chem. C 2007, 111, 14457.Galea, N.M.; Kadantsev, E.S.; Ziegler, T. J. Phys. Chem. C 2007, 111, 14457.
Point A – Surface Sulfur Formation : Initial Adsorption on S = 0ML Surface
A S=0.25ML surface (a 100% CSTR surface coverage of *S) is initially formed via H2S(g) adsorption and H2(g) desorption.
Anode Fuel at 800oC
pH2 = ~1atm,
pH2S = 1x10-5atm = 10ppm.
Initial Surface, S = 0.00ML.
Surface + H2S(g) *S-*H-*H
*S-*H-*H *S + H2(g)
*S + H2S(g) *S-*S-*H-*H
*S-*S-*H-*H *S--*S + H2(g)
Surface + 2H2(g) 4*H
Further H2S(g)/H2(g) adsorption/desorption results in a 100% CSTR surface coverage of 2*S, a S=0.50ML surface .
Point B - Surface Sulfur Removal :Initial Adsorption on S = 0.50ML Surface
Equilibrium is reached upon the production of a S=0.25ML surface (a 100% CSTR surface coverage of *S).
Anode Fuel at 800oC
pH2 = 1atm,
(No H2S(g) in fuel).
Initial Surface, S = 0.50ML.
*S--*S + H2(g) *S-*S-*H-*H
*S-*S-*H-*H *S + H2S(g)
*S + H2(g) *S-*H-*H
*S-*H-*H Surface + H2S(g)
Surface + 2H2(g) 4*H Model mimics experimental attempts to purge sulfur
from surface by eliminating H2S from anode fuel feed.
A. Conclusions – H2S
Our research studies the affects of consecutive adsorption and dissociation of H2S and subsequent desorption of H2 on Ni surfaces.
Failure of S-based pollutants in anode fuel to cause completely inoperable conditions within SOFC anode is due to inability of planar Ni to favourably adsorb H2S at a S coverage greater than 50%. The endergonic nature of H2S ads.n at S >0.50ML causes cutoff point.
Complete irreversibility of H2S ads.n caused by large endothermic/ endergonic energy difference between S = 0 and 0.25 (*S) ML.
A 2H = 0.50ML is achieved without the presence of surface sulfur. At S = 0.25 and 0.50 ML, only a 2H = 0.25ML coverage is formed.
Galea, N.M.; Kadantsev, E.S.; Ziegler, T. J. Phys. Chem. C
2007, 111, 14457.
Removal of Remaining Sulfur by O2 Treatment
1S*-Surface+O2(g) --> “Clean surface +SO2(g)1S*-Surface+O2(g) --> “Clean surface +SO2(g)
Galea, N.M.; Kadantsev, E.S.; Ziegler, T. J. Phys. Chem. C , accepted.Galea, N.M.; Kadantsev, E.S.; Ziegler, T. J. Phys. Chem. C , accepted.
Removal of Sulfur by O2 Treatment
1S*-Surface+O2(g) --> “Clean surface +SO2(g)1S*-Surface+O2(g) --> “Clean surface +SO2(g)
Galea, N.M.; Kadantsev, E.S.; Ziegler, T. J. Phys. Chem. C , accepted.Galea, N.M.; Kadantsev, E.S.; Ziegler, T. J. Phys. Chem. C , accepted.
Removal of Sulfur by O2 Treatment
1S*-Surface+O2(g) --> “Clean surface +SO2(g)1S*-Surface+O2(g) --> “Clean surface +SO2(g)
Galea, N.M.; Kadantsev, E.S.; Ziegler, T. J. Phys. Chem. C , accepted.Galea, N.M.; Kadantsev, E.S.; Ziegler, T. J. Phys. Chem. C , accepted.
Removal of Sulfur by O2 Treatment
1S*-Surface+O2(g) --> “Clean surface +SO2(g)1S*-Surface+O2(g) --> “Clean surface +SO2(g)
Galea, N.M.; Kadantsev, E.S.; Ziegler, T. J. Phys. Chem. C , accepted.Galea, N.M.; Kadantsev, E.S.; Ziegler, T. J. Phys. Chem. C , accepted.
Removal of Sulfur by O2 Treatment
1S*-Surface+O2(g) --> “Clean surface +SO2(g)1S*-Surface+O2(g) --> “Clean surface +SO2(g)
Galea, N.M.; Kadantsev, E.S.; Ziegler, T. J. Phys. Chem. C , accepted.Galea, N.M.; Kadantsev, E.S.; Ziegler, T. J. Phys. Chem. C , accepted.
Removal of Sulfur by O2 Treatment
1S*-Surface+O2(g) --> “Clean surface +SO2(g)1S*-Surface+O2(g) --> “Clean surface +SO2(g)
Galea, N.M.; Kadantsev, E.S.; Ziegler, T. J. Phys. Chem. C , accepted.Galea, N.M.; Kadantsev, E.S.; Ziegler, T. J. Phys. Chem. C , accepted.
Removal of Sulfur by O2 Treatment
1S*-Surface+O2(g) --> “Clean surface +SO2(g)1S*-Surface+O2(g) --> “Clean surface +SO2(g)
Galea, N.M.; Kadantsev, E.S.; Ziegler, T. J. Phys. Chem. C , accepted.Galea, N.M.; Kadantsev, E.S.; Ziegler, T. J. Phys. Chem. C , accepted.
Removal of Sulfur by O2 Treatment
1S*-Surface+O2(g) --> “Clean surface +SO2(g)1S*-Surface+O2(g) --> “Clean surface +SO2(g)
Galea, N.M.; Kadantsev, E.S.; Ziegler, T. J. Phys. Chem. C , accepted.Galea, N.M.; Kadantsev, E.S.; Ziegler, T. J. Phys. Chem. C , accepted.
Removal of Sulfur by O2 Treatment
2S*-Surface+O2(g) --> “1S* surface +SO2(g)2S*-Surface+O2(g) --> “1S* surface +SO2(g)
Galea, N.M.; Kadantsev, E.S.; Ziegler, T. J. Phys. Chem. C , accepted.Galea, N.M.; Kadantsev, E.S.; Ziegler, T. J. Phys. Chem. C , accepted.
Removal of Sulfur by O2 Treatment
2S*-Surface+O2(g) --> “1S* surface +SO2(g)2S*-Surface+O2(g) --> “1S* surface +SO2(g)
Galea, N.M.; Kadantsev, E.S.; Ziegler, T. J. Phys. Chem. C , accepted.Galea, N.M.; Kadantsev, E.S.; Ziegler, T. J. Phys. Chem. C , accepted.
Removal of Sulfur by O2 Treatment
2S*-Surface+O2(g) --> “1S* surface +SO2(g)2S*-Surface+O2(g) --> “1S* surface +SO2(g)
Galea, N.M.; Kadantsev, E.S.; Ziegler, T. J. Phys. Chem. C , accepted.Galea, N.M.; Kadantsev, E.S.; Ziegler, T. J. Phys. Chem. C , accepted.
Removal of Sulfur by O2 Treatment
2S*-Surface+O2(g) --> “1S* surface +SO2(g)2S*-Surface+O2(g) --> “1S* surface +SO2(g)
Galea, N.M.; Kadantsev, E.S.; Ziegler, T. J. Phys. Chem. C , accepted.Galea, N.M.; Kadantsev, E.S.; Ziegler, T. J. Phys. Chem. C , accepted.
Removal of Sulfur by O2 Treatment
Surface coverage of selected species determined by kineticCSTR model at 8000 C of O2 exposure to S = 0.50ML surface.
Galea, N.M.; Kadantsev, E.S.; Ziegler, T. J. Phys. Chem. C , accepted.Galea, N.M.; Kadantsev, E.S.; Ziegler, T. J. Phys. Chem. C , accepted.
B Conclusions – H2S
Sulfur with coverage S = 0.25 ML can be removed by O2
Galea, N.M.; Kadantsev, E.S.; Ziegler, T. J. Phys. Chem. C
accepted.
Acknowledgements Thank You!
Financial support was provided by the Alberta Energy Research Institute and the Western Economic Diversification Department.
Calculations were carried out on WestGrid computing resources, funded in part by the Canadian Foundation for Innovation, Alberta Innovation and Science, BC Advanced Education, and the participating research institutions.