The document presents the Nernst equation, which describes the relationship between the electrode potential and concentrations of oxidized and reduced chemical species in electrochemical cells at equilibrium. It defines the terms in the Nernst equation and shows the step-by-step derivation and simplification of the equation. It then provides an example of applying the Nernst equation to a concentration cell with copper half-cells of different concentrations to calculate the potential.

1. Die Nernst – Gleichung
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2. Universelle Gaskonstante Temperatur in °K (Kelvin)
c(Oxidierte Form)
R⋅T ox
E= E 0+ ⋅ln c(reduzierte
z⋅F rd Form)
Standardpotential
Natürlicher Logarithmus
Anzahl der Elektronen
Faraday-Konstante
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3. R⋅T ox
E= E 0+ ⋅ln
z⋅F rd
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4. R⋅T ox
E= E 0+ ⋅ln
z⋅F rd
ln=2,3⋅lg
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5. R⋅T ox
E= E 0+ ⋅2,3⋅lg
z⋅F rd
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6. J
R=8,3144621⋅
mol⋅K
R⋅T ox
E= E 0+ ⋅2,3⋅lg
z⋅F rd
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7. J
8,3144621⋅ ⋅T
mol⋅K ox
E= E 0+ ⋅2,3⋅lg
z⋅F rd
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8. J =W⋅s
J
8,3144621⋅ ⋅T
mol⋅K ox
E= E 0+ ⋅2,3⋅lg
z⋅F rd
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9. W⋅s
8,3144621⋅ ⋅T
mol⋅K ox
E= E 0+ ⋅2,3⋅lg
z⋅F rd
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10. A⋅V
W⋅s
8,3144621⋅ ⋅T
mol⋅K ox
E= E 0+ ⋅2,3⋅lg
z⋅F rd
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11. A⋅V⋅s
8,3144621⋅ ⋅T
mol⋅K ox
E= E 0+ ⋅2,3⋅lg
z⋅F rd
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12. 298K
A⋅V⋅s
8,3144621⋅ ⋅T
mol⋅K ox
E= E 0+ ⋅2,3⋅lg
z⋅F rd
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13. A⋅V⋅s
8,3144621⋅ ⋅298K
mol⋅K ox
E= E 0+ ⋅2,3⋅lg
z⋅F rd
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14. A⋅V⋅s
8,3144621⋅ ⋅298K
mol⋅K ox
E= E 0+ ⋅2,3⋅lg
z⋅F rd
C
96485,3365⋅
mol
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15. A⋅V⋅s
8,3144621⋅ ⋅298K
mol⋅K ox
E= E 0+ ⋅2,3⋅lg
C rd
z⋅96485,3365⋅
mol
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16. A⋅V⋅s
8,3144621⋅ ⋅298K
mol⋅K ox
E= E 0+ ⋅2,3⋅lg
C rd
z⋅96485,3365⋅
mol
C= A⋅s
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17. A⋅V⋅s
8,3144621⋅ ⋅298K
mol⋅K ox
E= E 0+ ⋅2,3⋅lg
A⋅s rd
z⋅96485,3365⋅
mol
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18. A⋅V⋅s
8,3144621⋅ ⋅298 K
mol⋅K ox
E= E 0+ ⋅2,3⋅lg
A⋅s rd
z⋅96485,3365⋅
mol
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19. 8,3144621⋅V⋅298 ox
E= E 0+ ⋅2,3⋅lg
z⋅96485,3365 rd
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20. 0,059⋅V ox
E= E 0+ ⋅lg
z rd
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21. 0,059⋅V ox
E= E 0+ ⋅lg
z rd
Elementare Metalle kann man als Konstant (1)
sehen
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22. Vereinfachte Nernst-Gleichung
0,059⋅V
E= E 0+ ⋅lg c (ox)
z
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23. Beispiel einer Konzentrationszelle
Donator-Halbzelle Akzeptor-Halbzelle
2+ mol 2+ mol
Cu/ Cu (0,0001 ) Cu/Cu (0,1 )
l l
Standardpotential Kupfer Vereinfachte Nernst-Gleichung
0,059⋅V
E 0=+ 0,35 V E= E 0+ ⋅lg c (ox)
z
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24. Beispiel einer Konzentrationszelle
Nernst-Gleichung für Akzeptor-Halbzelle
0,059 V
E A=0,35V + ⋅lg 0,1
2
E A=0,3205V
Nernst-Gleichung für Donator-Halbzelle
0,059V
E D=0,35V + ⋅lg 0,0001
2
E D=0,232V
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25. Beispiel einer Konzentrationszelle
E A=0,3205V E D=0,232V
E= E A−E D
E=0,3205V −0,232 V
E=0,0885V
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