State-Space Modeling of Electrochemical Processes · ETH - Ceramics State-Space Modeling of...
Transcript of State-Space Modeling of Electrochemical Processes · ETH - Ceramics State-Space Modeling of...
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State-Space Modeling of Electrochemical Processes
„Who uses up my battery power ?“
Michel Prestat
ETH-ZürichInstitute for Nonmetallic Materials
Head: Prof. L.J. Gauckler
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Outline
Electrochemistry
Electrochemical Impedance Spectroscopy and State-Space Modeling
Oxygen reduction at solid oxide fuel cell cathodes
Comparison modeling – experiments
Summary
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Electrochemistrycorrosion
electropolishing
coloration of titanium
batteries, fuel cells
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Solid Oxide Fuel Cell (SOFC)
cathode
O2-
e-
e-
H2OH2
O2 O2
anode
electrolyte
O2 reduction
O2
O2-
½O2 + 2e- O2-
mechanism?rate-limiting steps?
fuel oxidation
O2-
H2 + O2- H2O + 2e-
mechanism?rate-limiting steps?
H2OH2
single cell
Sulzer Hexis SOFCmicrostructure
½O2 + 2e- O2-
H2 + O2- H2O + 2e-
overall: H2 + ½O2 → H2O
800-1000°C
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Electrochemistry and Materials
cathode
O2-
O2 O2
electrolyte
O2 reduction
O2
O2-
O2 + 4e- 2O2-
mechanism?rate-limiting steps?
Overpotential η = E - Eeq
~ electrokinetic losses
Potential (V)
Current (A)
Eeq
La0.85Sr0.15MnO3 (LSM)
Au
ideal electrode:no kinetic losses
ηηLSM < ηAu
real electrode
η strongly dependant on the material
Aim:find the appropriate material to gethigh current and low overpotential(reduction of electrokinetic losses)
What limits the performanceof my system ?
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Electrochemical Impedance Spectroscopy (EIS)
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EIS principle
Potential (V)
Current (A)
E~
I~
steady-stateoperating point
Small amplitude (5-10 mV) input signal→ Linearization
I =Z(jω)
1E~~
Admittance Transfer Function
Z = impedance
complex ( j2 = -1)
frequency dependant ( ω = 2π f )
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EIS spectra and equivalent circuits
Re (Z)
Im (Z)
R-6
-4
-2
00 2 4 6 8 10 12
Re (Z) / Ω
Im (Z
) /Ω
110
102103
104
f (Hz)
experimental EIS spectra
Re (Z)
Im (Z)
R
Cf = 12π RC
R
Re (Z)
Im (Z)
R2
C2
R1
How to interpretthe experimental equivalent circuit ??
Re (Z)
Im (Z)
R2
C2
R1 R3
C3
R1 R2+R3
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Alternative approch: modeling the impedance
Re (Z)
Im (Z)
Re (Z)
Im (Z)
experimental impedance
reaction modelnew model
O2 Oads O2-O2 O2,ads O2-
state-space modeling
faradaic impedance
validation of the modelassessment of kinetics
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State-Space Modeling (SSM)
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State-Space Model
electrode potential
E (input)
faradaic current
IF (output)O2(g) Oads O2-
electrochemical system
Kb
KfKdes
Kads
K = model parameters (Kads, Kdes, Kf , Kb …)
θ = state variable (Oads concentration)
= f (θ , E, K) → state equation
IF = g (θ , E, K) → output equation
dθdtState-Space Model
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State-Space Modeling
time domain frequency domain
I
E
θ = Aθ +B E
IF = Cθ +D E
.
linearization
θ = 0.
steady-state analysis
ZF(jω)
Laplace transform varying ω
Re(ZF)*
* * * ** **
**
*Im(Z
F)θ = Kads(1- θ)2 +...
IF = -Kf θ e-fE + …
.
state-space model*
Simulink®: easy implementation of the model.
Matlab®: state-space calculations and computing
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Oxygen Reduction
at
Solid Oxide Fuel Cell Cathodes
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Reaction Models
Oads Oads (tpb)Surface diffusion:
Oads + 2e- O2-Charge transfer at the tpb:
O2(g) + 2s 2OadsDissociative adsorption:
s = adsorption site
electrolytexO2- ( Oo )
electrode
Oads
O2
Oads
O2
pO2 , [Oo] and [Vo] are constantx ..
Electrolyte = O2- conductor (Vo and Oo).. x
Typically YSZ (Y2O3 - ZrO2)
triple phase boundary (tpb)
Model 1: surface diffusion negligible
Model 2: with surface diffusion
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Model 1 (without surf. diffusion)Dissociative adsorption:
O2(g) + 2s 2Oads
Kads
Kdes
O2- ( Oo )x
Oads
O2
electrolyte
electrode
θads
Charge transfer:
Oads + 2e- O2-
Kf(E)
Kb(E)
→ consecutive reaction steps
→ state variable θads = scalar
Kads pO2(1-θads) 2 – Kdesθads2 – Kf(E) θads + Kb(E) (1-θads)
IF = Ki [– Kf(E) θads + Kb(E) (1-θads)]
dθads
dt =→ state-space model
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Model Implementation in Simulink®
Kads pO2(1-θads) 2 – Kdesθads2 – Kf(E) θads + Kb(E) (1-θads)
IF = Ki [– Kf(E) θads + Kb(E) (1-θads)]
dθads
dt =
+-
1
-++
Kads pO2
u2Kdes
x
x
-+
integrator
Einput
Ki IFoutput
kf exp(-2 β f E)
kb exp (2 (1-β) f E)
function Kf (E)
function Kb (E)
1-θadsθads
θads
u2
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Model 2 (with surf. diffusion)
O2(g) + 2s 2Oads
Kads
Kdes
tpb
Oads reservoirθeq
electrolyte
diffusionlayer
θ1
θ2
θ3
O2- ( Oo )x
OadsO2
OadsO2
OadsO2
OadsO2
Oads Oads
Kdif
Oads + 2e- O2-
Kf(E)
Kb(E)
2
2θ θt
∂ ∂=
∂ ∂zDiffusion processes
2nd Fick‘s law:
→ Finite difference approach toestimate time and space derivatives
→ state variable θ (θ1, θ2, θ3) = vectorθ1 ≤ θ2 ≤ θ3
→ Parallel reaction pathways
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Model Implementation in Simulink®Subsystems: as many as compartments
i( ) ( ) 2
i-12 2 dif i 1iads O i des i 2i-2
Kθ 2K 1 θ K θ θ ( + chg transfer kinetics)
t 3 32θθ +∂
= − − + − +∂
p
Einput
IFoutput
θ1
θ1
θ3
θ2θ2
θ2 θ3
tpb (1)
(2)(3)
in-port out-port
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Model Implementation in Simulink®
Compartment n°2
( ) ( )2
2 2 dif 32 1ads O 2 des 2 2
K θθ 2θK 1 θ K θ θt 4 3 3
∂= − − + − +
∂p
+-
1
u2
-++
Kads pO2
u2Kdes
1s
Integrator (θ2)
θ2out-port to
compartment (1) and (3)
Kdif/4
-
+
+
1/3
2/3θ1
θ3
in-ports
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Modeling results
Oads
Oads
O2
O2
O2-
electrode
electrolyte
ads. – diff. - charge transfer(model 2)
-0.6
-0.4
-0.2
02 2.5 3 3.5
Re(ZF) / Ω
Im(Z
F ) /
Ω
Oads
Oads
O2
O2
O2-
electrode
electrolyte
diffusion - charge transfer(model 2)
-0.6
-0.4
-0.2
02 2.5 3 3.5
Re(ZF) / Ω
Im(Z
F ) /
Ω
45°
Oads
Oads
O2
O2
O2-
electrode
electrolyte
adsorption - charge transfer(model 1 = diffusion slow)
-0.6
-0.4
-0.2
02 2.5 3 3.5
Re(ZF) / Ω
Im(Z
F ) /
Ω
R2
C2
R1
Oads
Oads
O2
O2
O2-
electrode
electrolyte
charge transfer(model 1 = diffusion slow)
-0.6
-0.4
-0.2
02 2.5 3 3.5
Re(ZF) / Ω
Im(Z
F ) /
ΩR1
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Comparison Modeling - Experiments
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Electrode / electrolyte interfaces
porous
industrial application~10-30 µm
dense
~100 nm -1 µm
control of theelectrode dimensions
microstructured ~20 µm -100 µm
top view
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Experimental
E+E~
I+I~
potentiostat(DC)
workingelectrode
frequencyresponseanalyzer
(AC)counter
electrode
referenceelectrode
ZF
ZTOT =R2
CF
R1RΩ
CDL
0 2 3 4 5Re (ZTOT) / Ω
1
-1
-2
-3
0Im
(ZTO
T) / Ω
CDL high CDL moderate CDL=0(ZF)
CDL may mask ZF → Berthier‘s method in Corrosion 51 (1995) 105
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Comparison modeling - experiments
Kdif << Kads, Kf
slow surface diffusion = Model 1
-1.5
-1
-0.5
02 3 4 5
Re(ZEXP) / Ω
Im(Z
EXP)
/ Ω
La0.85Sr0.15MnO3 @ 800°Cη= -270mV, I =150 mA.cm-2
102
103
104
- (RΩ, CDL)
Oads
Oads
O2
O2
O2-
electrode
electrolyte
mixed controladsorption - charge transfer
-1.5
-1
-0.5
00 1 2 3
Re(ZF) / Ω
Im(Z
F) /
Ω
La0.85Sr0.15MnO3 @ 800°Cη= -270mV, 150 mA.cm-2
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Ongoing SOFC projects
Mixed ionic-electronic electrodes Modeling the whole SOFC
cathode
O2-
anode
electrolyte
½O2 + 2e- O2-
H2 + O2- H2O + 2e-
electrolyteO2-
Oads
Oads
O2
electrodeO2-
O2-
O2-
Additional reaction pathway throughthe electrode bulk.
Oxygen reduction, fuel oxidation, transport in the electrolyte.
Intermediate T° SOFC (600-800°C).
Typical material: LaxSr1-xCoyFe1-yO3(LSCF).
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Summary
• electrochemical reactions yield sophisticated impedance behavior⇒ necessity of a modeling approach (analytical or numerical).
• SSM (with modern computation tools) enables to simulate the faradaic impedance of such reactions.⇒ “fingerprint” of reaction models.
• SSM approach applicable to any other field of electrochemistry.
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Many thanks to ...
SOFC group Prof. L.J. Gauckler
References
M. Prestat and L.J. Gauckler, Solid State Ionics, submitted (2003)Faradaic impedance of oxygen reduction at solid oxide fuel cell cathodesPart I: adsorption and charge transfer limited reactions
M. Prestat and L.J. Gauckler, Solid State Ionics, submitted (2003)Faradaic impedance of oxygen reduction at solid oxide fuel cell cathodesPart Ii: surface diffusion limited reactions
A. Bieberle and L.J. Gauckler, Solid State Ionics, 146 (2002) 23State-Space Modeling of the anodic SOFC system Ni, H2-H2O|YSZ
A. Mitterdorfer and L.J. Gauckler, Solid State Ionics, 117 (1999) 187Identification of the reaction mechanism of the Pt, O2 (g)|Yttria-Stabilized Zirconia system,Part I: general framework, modelling and structural investigation
A. Mitterdorfer and L.J. Gauckler, Solid State Ionics, 117 (1999) 203Identification of the reaction mechanism of the Pt, O2 (g)|Yttria-Stabilized Zirconia system,Part II: model implementation, parameter estimation and model validation