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Institute of Physical Chemistry,
Physical Chemistry of Condensed Matter
1 Rolf Schuster
Electrochemical Microcalorimetry
Kai Etzel, Katrin Bickel and Rolf SchusterPhysical Chemistry, Karlsruhe Institute of Technology, Germany
-Thermodynamics and kinetics of electrochemical reactions
10 nm
research interests:
-Surfaces in vacuum and electrochemical environment structure, phase transition, ordering processes‚electronic structure‘, scanning tunneling spectroscopy
metal deposition, H-adsorption/evolution
-Electrochemical microstructuring
(electrochemical STM, XPS, …)
(electrochemical STM, microcalorimetry, surface plasmon resonance,…)
Tem
pera
ture
[mK
]
Time [s]
0
-0.30 0.1 0.2
Institute of Physical Chemistry,
Physical Chemistry of Condensed Matter
2 Rolf Schuster
Electrochemical Microcalorimetry
Kai Etzel, Katrin Bickel and Rolf SchusterPhysical Chemistry, Karlsruhe Institute of Technology, Germany
Historical: E. J. Mills, „On Electrostriction“, Proc. Roy. Soc. Lond. 26, 504 (1877)
E. Bouty, „Sur un phénomène analogue au phénomène de Peltier“,Comptes Rendus 89, 146 (1879)
Cu-deposition⇒ decreasing temperature
Cu-dissolution⇒ increasing temperature
Cu2+
SO42-
Cu-plated
„electrochemical Peltier heats“
Institute of Physical Chemistry,
Physical Chemistry of Condensed Matter
3 Rolf Schuster
What do we learn from electrochemical microcalorimetry?
In „conventional“ calorimetry:
;STHGq RRRm Δ−=Δ−Δ=⇒
;Hq Rm Δ= p,T = const.
In electrochemical calorimetry:electrical work: ( );, STHGFzw RRRmel Δ−Δ−=Δ−=⋅⋅= φ
from the ‚chemical reaction‘heat transfer from surrounding
We measure the reaction entropy, ΔRS, (if we are close to equilibrium).
Ostwald (1903)
-stoechiometry of the reaction, i.e. hints on elementary steps-entropies of hydration, i.e., involvement of solvent water -phase transitions and surface entropies
in addition: irreversible heat due to chemical reactions, i.e., complexation, crystallization,...
⇒
Institute of Physical Chemistry,
Physical Chemistry of Condensed Matter
4 Rolf Schuster
Can we achieve „monolayer sensitivity“?
Use thin electrode/sensor assembly with low heat capacity
Use pulsed electrochemical reactions:-fast enough to avoid heat loss into the electrolyte (and uptake of Joule heat
from the electrolyte)-slow enough to ensure thermal equilibration of the electrode/sensor assembly
potentiostat/galvanostat
+
-
charge amplifier
electrolyte
reference electrode
Au-foil
metalizedPVDF-foil
p 100 mbar≈
potentialpulse
temperaturesignalsocket
counter electrode
C. E. Borroni-Bird, and D. A. King, Rev. Sci. Instr. 62 (1991) 2177.J. T. Stuckless, N. A. Frei, and C. T. Campbell, Rev. Sci. Instr. 69 (1998) 2427.
Institute of Physical Chemistry,
Physical Chemistry of Condensed Matter
5 Rolf Schuster
20x10-3
100
E [V
]
100x10-3806040200t [s]
0.80.40.0I [
mA
]
0.120.080.040.00
ΔT [a
rb. u
nits
]
Cu dissolution from a Cu-layer (≈ 300 ML) on a 50 µm Au foil
(0.5 M CuSO4 / 5mM H2SO4)
potential
current
temperature
10 ms dissolution at η = 20 mV
current set to zero after 10 ms
2.5·10-6 C/cm2 ≅ 0.04 ML Cu
00 <Δ⇒>Δ ST entropy gain due to Cu-dissolution!?
No: entropy loss due to water bonding in the hydration shell
21 1
( )122 JK molabs
Cu aqs +
− −≈ −
Cu deposition/dissolution on Cu-bulk Ag deposition/dissolution on Ag-bulk20mM Cu(ClO4)2 / 1M HClO4 20mM AgClO4 / 1M HClO450 µm Au-foil +Cu 50 µm Au-foil + Ag
11)( molJK1222
−−−≈+abs
aqCus 11)( molJK51 −−+≈+
absaqAgs
-0.180-0.172E
[V]
0.300.250.200.150.100.050.00t [s]
-2.5
0.0
I [m
A]
1.00.80.60.40.20.0ΔT
[arb
. uni
ts]
-0.168-0.160
E [V
]
0.300.250.200.150.100.050.00t [s]
2.5
0.0I [m
A]
-1.0-0.8-0.6-0.4-0.20.0
ΔT [a
rb. u
nits
]
-0.600-0.592
E [V
]
0.300.250.200.150.100.050.00t [s]
-1.0
0.0I [
mA
]
-60x10-3-40-20
0
ΔT [a
rb. u
nits
]
-0.590-0.582
E [V
]
0.300.200.100.00t [s]
1.0
0.0I [m
A]
60x10-3
4020
0
ΔT
[arb
. uni
ts]
Cu dissolution: ΔRS < 0 Ag dissolution: ΔRS > 0
dominated by water bonding in the hydration shell
dominated by production of ions
Institute of Physical Chemistry,
Physical Chemistry of Condensed Matter
7 Rolf Schuster
Polycrystalline Au in 10 mM CuSO4 / 0.1 M H2SO4
-200
-100
0
100
j /(µ
A/c
m²)
0.50.40.30.20.10.0
E /V
Cu UPDCu bulk
Cu bulk deposition vs. Cu underpotential deposition (UPD)
0.40.30.2E
/V
-25
0
j /(m
A/c
m²)
-100
-50
0
ΔT
/a. u
.
-0.2
0.0
E /V
100806040200t /ms
-25
0
j /(m
A/c
m²)
80604020
0ΔT
/a. u
.
Same net reaction Cu2+ + 2e- → Cu !?
Institute of Physical Chemistry,
Physical Chemistry of Condensed Matter
8 Rolf Schuster
0.3Cu2+ + 0.3SO42- →
0.3Cu2+ad + 0.3 SO4
2-ad
Compatible with:Sabs(Cu2+) ≈ -128 J/KmolSabs(SO4
2-) ≈ 1 J/Kmol
Cu depositon on Cu bulk
Cu UPD formation
Microscopic processes
Cu2+ + 2e- → Cu
reve
rsib
lehe
at (µ
J/cm
2 )(c
orre
cted
for o
verp
oten
tial)
-25
-20
-15
-10
-5
0
-400 -300 -200 -100 0
conversion /(µC/cm²)
-0.7 -0.6 -0.5 -0.4 -0.3 -0.2 -0.1 0.0ML of Cu(111)
heat, due to
heat, due to anion coadsorption:
ΔRS helps in identifying reaction pathways and side reactions!
Institute of Physical Chemistry,
Physical Chemistry of Condensed Matter
9 Rolf Schuster
First test experiments on charging/discharging LiCoO2
in cooperation with Heino Sommer and Petr Novák, Paul Scherrer Institut
-15
-10
-5
0
5
10
15
curre
nt d
ensi
ty /
mA
cm
-2
2.01.51.00.50.0
Potential vs. Pt / V
scan rate: 5 mV/s
charging: LiCo(III)O2 → ‚Co(IV)O2‘ + Li+ + e-
discharging: ‚Co(IV)O2‘+ Li+ + e- → LiCo(III)O2
LiCoO2 in dimethyl-carbonate /ethylene-carbonate, LiPF6
1 2 3
Institute of Physical Chemistry,
Physical Chemistry of Condensed Matter
10 Rolf Schuster
0.300.280.26E
[V]
100x10-3806040200t [s]
-0.20-0.100.00
I [m
A]
-15-10-505
ΔT
[arb
. uni
ts]
0.340.32E
[V]
100x10-3806040200t [s]
0.15
0.00I [m
A]
302010
0
ΔT
[arb
. uni
ts]
Charging and discharging of slightly charged LiCoO2
We measure reversible heat effects, i.e., ΔRS
conversion ca. 2·1013 e-/cm2
(c.f., a Au(111) surface has 1.4·1015 atoms/cm2)
in cooperation with Heino Sommer and Petr Novák, Paul Scherrer Institut
Institute of Physical Chemistry,
Physical Chemistry of Condensed Matter
11 Rolf Schuster
40
30
20
10
0
-10heat
/ co
nver
sion
[kJ/
eq]
0.30.20.10.0-0.1-0.2
pulse amplitude [V]
COLD
COLD
WARM
WARM
Φ = 0.3V, slightly charged
Φ = 0.5V, moderately chargedΦ = 1V, strongly charged
in cooperation with Heino Sommer and Petr Novák, Paul Scherrer Institut
- We can measure heat effects and determine the reversible heat, i.e., ΔRS.- Charging, i.e., Li+ formation leads to warming, i.e., ΔRS < 0.- The heat per equivalent dependens on the state of charge of the electrode - ΔRS < 0 !? Explicable by:
stong solvation of Li+ in dimethyl-carbonate /ethylene-carbonate (?)or side reactions (decomposition of LiCoO2, coadsorption prosesses,…)
Institute of Physical Chemistry,
Physical Chemistry of Condensed Matter
12 Rolf Schuster
Future work on Li-ion batteries
- ΔRS for different states of charge of the electrode
- relyable calibration
- ΔRS for Li+ + e- → Li on Li-electrodes, dependence on the electrolyte
- effect of charging and discharging cycles on ΔRS
- ‚ideas‘ on elementary steps of the charging/discharging process
- ΔRS for Li+ + e- → Li upon intercalation of graphite / formation of the SEI