CAMD, DTU, Denmarkfolk.uio.no/ravi/CMS-ET2009/Jan_lecture_1.pdf• Bulk electrochemical oxidation...
Transcript of CAMD, DTU, Denmarkfolk.uio.no/ravi/CMS-ET2009/Jan_lecture_1.pdf• Bulk electrochemical oxidation...
Electro-catalysis
J. Rossmeisl
CAMD, DTU, Denmark
jr1
Slide 1
jr1 two talks about electro catalysisfirst issues, aproximations and fundementals Jan Rossmeisl; 26.04.2009
Andreas Züttel, Switzerland, 4/27/20092
Sustainable hydrogen
O2
O2
H2
H2
H2O
Dissociation
of water
Transport
Storage
Combustion
H2 O2
Sun
Photovoltaics
Wind
Hydropower ENERGY
ENERGY
A. Züttel, U. Friboug
e- e-
e- e-
HO
O2 is reducedH2 is oxidized
2H2 + O2 → 2H2OChemical energy → Heat
Electrochemistry
2H2 + O2 → 2H2O
Anode CathodeH2 → 2H++2e- 4H++4e-+O2 →2H2O
Uθ=0 Uθ=1.23V
Separate oxidation and reduction
The PEM Fuel cell
Cathode:
½O2+2H++2e- ���� H2O
½O2+H2 ���� H2O+electricity
Anode:
H2 ���� 2H++2e-
Electrochemical cell
e- e-
O2 + 2H+ + 2e-↔↔↔↔ H2OH2↔↔↔↔ 2H+ + 2e-
Electrolyte +
+
+
+
+
-
-
---
Electrochemistry
2H2 + O2 → 2H2OChemical energy → Heat
H2 → 2H++2e- 4H++4e-+O2 →2H2OChemical energy → Electrical energy
AnodeCathode
+
-
-
Electrolyte+
+
+
+-
-
-
φφφφcathode
φφφφelectrolyte
φφφφanode
Real electrochemical cell:
-
+
Challenges
• Chemical potential of H+ and e-
• Liquid solid interface
• Field effects
• Phase diagrams
• Charge transfer reactions
Ogasawara, Brena, Nordlund, Nyberg, Pelmenschikov, Petterson and Nilsson.PRL, 89, 2002, 276102
Henderson, Surf. Science Rep 46 (2002)
H2O-OH phases on Pt(111) (K. Bedürftiget al., J. Chem. Phys. 111 (1999), 11147).
STM image of layer on Pt(111), formed by adsorption of 2 L H2O on a (2x2)-O layer at 123 K and short annealing at 170 K. Tunneling parameters were -0.55 V, 0.17 nA, 220 x 220 Å2. Inset: Detail of a boundary between translational domains of the (3x3)/(r3xr3)R30°structure; -0.01 V, 27 nA, 22 x 25 Å2.
Details of areas with (a) the Pt(111) (r3xr3)R30° and (b) the Pt(111)-(3x3) structure from the measurement shown in left figure. -0.5 V, 0.17 nA, 34x25 Å2.
(a) (b)
Similar to Clay, Haq and Hodgon.PRL, 92, 2004, 46102
OH+H2O
∆∆∆∆Gw = -.33eV
In electrochemistry?
Water molecules are highly oriented in a ice like structure on Pt electrode. From a H-O stretching peak of 3200 cm-1 compared to 3400 cm-1 in liquid water.
Noguchi,Okada, Uosaki Faraday 140 (2008)
Including the water by-layer
Water by-layer
Ogasawara, Brena, Nordlund, Nyberg, Pelmenschikov, Petterson and Nilsson.PRL, 89, 2002, 276102
Similar to Clay, Haq and Hodgon.PRL, 92, 2004, 46102
OH+H2O
∆∆∆∆Gw = -.60eVOOH+H2O
∆∆∆∆Gw = -.22 eV
O+H2O
∆∆∆∆Gw = .0 eV
Challenges
• Chemical potential of H+ and e-
• Liquid solid interface
• Field effects
• Phase diagrams
• Charge transfer reactions
Field effect on binding energies
G.S. Karlberg, J. Rossmeisl, J.K. Nørskov, PCCP, 9 (2007) 5158-5161
Field effects
Rossmeisl, Nørskov, Taylor, Janik, Neurock. J. Phys. Chem. B 110, (2006), 21833-21839
Effect of water and field!!
G.S. Karlberg, T. Jaramillo, E.Skulason, J. Rossmeisl, T. Bligaard, J.K. Nørskov. PRL, 99, (2007), 126101
Challenges
• Chemical potential of H+ and e-
• Liquid solid interface
• Field effects
• Phase diagrams
• Charge transfer reactions
Theoretical Standard Hydrogen Electrode
Relating gas phase with electrochemistry
H2O� OH*+½H21. Get ∆∆∆∆E with DFT
2. Water surroundings: ∆∆∆∆Ew
3. Effects of local fields :∆∆∆∆Ew(U)
4. Zero point energy and entropy:
∆∆∆∆G0 =∆∆∆∆Ew+∆∆∆∆Ezpe-T∆∆∆∆S0
H2O � OH*+H++e-
1/2H2 ↔H++e-
1. SHE Convention:
∆∆∆∆G(U=0,cH+=1M ) = 0
2. Potential and pH:
∆∆∆∆G(U,cH+) = -eU-kTln(cH+)
Challenges
• Chemical potential of H+ and e-
• Liquid solid interface
• Field effects
• Phase diagrams
• Charge transfer reactions
U vs. SHE
H++e-+*↔ H*
How does the surface depends on potential?
µµµµ(H++e-) = -eU-kTln(aH+)
Hydrogen and potential
U=0
U=0.5V
H2(g)
H*
H+(aq)+e-
U=-0.5V
Water and potential
U=0
U=0.5V
H2O(l)
HO*+H++e-
O*+2(H++e-)
U=-0.5V
Phase-diagrams
Phase diagram 1
eU+Field effectOnly eU
Phase-diagram 2
Rossmeisl, Nørskov, Taylor, Janik, Neurock. J. Phys. Chem. B 101, (2006), 21833-21839
Only eU term
Charged surface
U vs. SHE
H++e-+*↔ H*
How does the surface depends on potential?
µµµµ(H++e-) = -eU-kTln(aH+)
Pourbaix Diagram• Bulk phase diagram with
potential and pH variables.
• In electro-catalysis the solid-liquid interface is of particular interest.
• The state of the surfacedepends on pH and potential.
• Limited experimental data on surface phase diagrams.
• Bulk electrochemical oxidation and reduction may be kinetically hindered.
M. Pourbaix, Atlas of Electrochemical Equilibria in Aqueous Solutions, Pergamon Press, 1966
pH
U
Surface Pourbaix diagram
Assuming ideal gas activity. (Clearly wrong at extreme pressures).
Essentially obtaining the U-pO2 relation fromH2O (l) ↔ ½ O2 (g) + 2 e- + 2 H+
H.A. Hansen, J. Rossmeisl, J.K. Nørskov. PCCP. (2008) DOI: 10.1039/b803956a
U
pH
Ag
Cyclic voltammetry
t
i
Reversible but saturating surface reaction
i
t
Irreversible and saturating surface reaction
U
t
For instance, sweep rate 50 mV/s
Constant capacitancei = C dU/dt
i
t
CV for Pt(111) in different electrolytes [1]
OH related
[1] Markovic, N. M., Gasteiger, H. A., and Ross, P. N., J. Electrochem. Soc., 144, 1591–1597 (1997)
H2SO4related
H2 evolution
Cyclic voltammetry
Capacitance
Theoretical results
∆E versus coverage
Theoretical results
Low coverage free energy of adsorption
H-H
interaction
Markovic et al J. Phys. Chem. 101, 5405 (1997)
G.S. Karlberg, T. Jaramillo, E.Skulason, J. Rossmeisl, T. Bligaard, J.K. Nørskov. PRL, 99, (2007), 126101
Challenges
• Chemical potential of H+ and e-
• Liquid solid interface
• Field effects
• Phase diagrams
• Charge transfer reactions
Hydrogen Evolution Reaction
H+H2
VolmerH+ + e- -> Had
Tafel2Had -> H2
e-
V
H2H+
HeyrovskyHad + H
+ + e- -> H2
Pte-
HadHad
Overall reaction: 2(H+ + e-) -> H2
or
AnodeCathode
+
-
-
Electrolyte+
+
+
+-
-
-
φφφφcathode
φφφφelectrolyte
φφφφanode
Real electrochemical cell:
-
+
Adding hydrogen to the water
WF gives a relative U scale
Challenges
• Absolute scale of the potential – linking the vacuum level with the standard hydrogen electrode
• Keeping the potential constant during charge transfer reaction
U=0 vs. SHE
WF
Potential
?
Vacuum
Challenge 1: Vacuum vs. SHE
1/2H2(g)↔H+(aq)+e-
SHE Convention:
∆∆∆∆G(U=0) = 0
4.4 to 4.8eV
Hydrogen Evolution Reaction
H+H2
VolmerH+ + e- -> Had
Tafel2Had -> H2
e-
V
H2H+
HeyrovskyHad + H
+ + e- -> H2
Pte-
HadHad
Overall reaction: 2(H+ + e-) -> H2
or
Challenge 2: Constant potential
The potential is not the same in initial and final state
n=1
N=3
Θ=n/N=1/3
n=0
N=3
Θ=n/N=0
+ + +
- - -
n=3
N=9
Θ=n/N=3/9=1/3
n=2
N=9
Θ=n/N=2/9
- - -
+ + +
++
--
Challenges
• Absolute scale of the potential – linking the vacuum level with the standard hydrogen electrode
• Keeping the potential constant during charge transfer reaction
n=3
N=9
Θ=n/N=3/9=1/3
n=0
N=9
Θ=n/N=0
---
+ + +
The energy stored
Gint=(G(N,n)-G(N,0)-nµµµµH2/2)/N
=½C (U-Upzc)2
=½e2θθθθ2/C
(U-Upzc)=eθθθθ/C
µµµµH2/2*n/N ∝∝∝∝ θ ∝∝∝∝ U
Liniar in U :means
defines the minimum
C=26µµµµF/cm2
C=20µµµµF/cm2
T. Pajkossy, D.M. Kolb Electrochimica Acta 46 (2001) 3063
UPZC
WF
Vacuum
Vacuum vs. SHE
U=0 vs. SHE
Potential
Challenges
• Absolute scale of the potential – linking the vacuum level with the standard hydrogen electrode
• Keeping the potential constant during charge transfer reaction
n=1
N=9
Θ=n/N=1/9
n=0
N=9
∆∆∆∆Θ=1/9=1/N ∝∝∝∝ ∆∆∆∆U
+
-
Reacting one proton
Reacting one Proton∆∆∆∆Gcapacitor = N( Gint(N,n-1)- Gint(N,n))
=½e2N/C((θθθθ-1/N)2 - θθθθ2)
=-eU – ½e∆∆∆∆U
Potential energy diagram
Summary
• Electrochemical DFT is starting
• Linking electrochemistry and surfacescience
• Could play a part in electrocatalyst design-tomorrow!