Relation between Electrode cell potential and Gibb's Free Energy

Question

Q. For the cell reaction: 2Fe³⁺(aq) + 2I^-(aq) → 2Fe²⁺(aq) + I₂(aq) E° = 0.24 V at 298 K. The standard Gibbs energy (G°) of the cell reaction is: [Given that Faraday constant F = 96500 C mol^-1]

A) 23.16 kJ mol^-1
B) -46.32 kJ mol^-1
C) -23.16 kJ mol^-1
D) 46.32 kJ mol^-1

Answer 1

Correct option: B) -46.32 kJ mol^-1  

\(\Delta G^{\ominus} = -nF\,E^{\ominus}_{cell}\)

\(=-2\times96500\times0.24\,J\, mol^{-1}\)

= -46320 mol^-1

= -46.32 kJ mol^-1