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Questions
Derive the relationship between standard cell potential and equilibrium constant of cell reaction.
Derive relation between rate of reaction (k) and cell potential `("E"_"cell"^0)`
Solution
The relation between standard Gibbs energy change of cell reaction and standard cell potential is given by
- ΔG° = - nF `"E"_"cell"^circ` .....(1)
The relation between standard Gibbs energy change of a chemical reaction and its equilibrium constant as given in thermodynamics is:
ΔG° = - RT ln K .....(2)
Combining equations (1) and (2), we have
- nF `"E"_"cell"^circ` = - RT ln K
∴ `"E"_"cell"^circ = "RT"/"nF"` ln K
`= (2.303 "RT")/"nF" log_10` K
`= 0.0592/"n" log_10` K at 25 °C
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