Reaction involved in present electrochemical cell,
At Anode: Zn → Zn^2+ + 2e^2-
At cathode: Zn^2+ + 2e^2- → Zn
Net Reaction: Zn + Zn^2+ ('x' m) → Zn^2+(0.1 m) + Zn
Number of electrons involved in present electrochemical cell = n = 2
According to Nernst equation for electrochemical cell,
Ecell = -2.303![\frac{RT}{nT} log \frac{[Zn^2+]R}{[Zn^2+]L}](https://tex.z-dn.net/?f=%20%5Cfrac%7BRT%7D%7BnT%7D%20log%20%20%5Cfrac%7B%5BZn%5E2%2B%5DR%7D%7B%5BZn%5E2%2B%5DL%7D%20%20)
= 0.014
Given: T =
, F = 96500 C, R = gas constant = 8.314J/K.mol, [Zn^2+]R = 0.1 m , Ecell = 0.014 v
∴ 0.014 = - 2.303
∴ log
= 
= -2.1117
∴ log x = log(0.1) + 2.1117
∴x = 13.09 m
At Anode: Zn → Zn^2+ + 2e^2-
At cathode: Zn^2+ + 2e^2- → Zn
Net Reaction: Zn + Zn^2+ ('x' m) → Zn^2+(0.1 m) + Zn
Number of electrons involved in present electrochemical cell = n = 2
According to Nernst equation for electrochemical cell,
Ecell = -2.303
Given: T =
∴ 0.014 = - 2.303
∴ log
∴ log x = log(0.1) + 2.1117
∴x = 13.09 m