For the cell reaction $2Fe^{3+} (aq) + 2I^- (aq) \rightarrow 2Fe^{2+} (aq) + I_2 (aq)$, $E^{\ominus}_{cell} =

Question

For the cell reaction $2Fe^{3+} (aq) + 2I^- (aq) ightarrow 2Fe^{2+} (aq) + I_2 (aq)$, $E^{\ominus}_{cell} = 0.24 	ext{ V}$ at 298 K. The standard Gibbs energy ($\Delta_r G^{\ominus}$) of the cell reaction is : [Given that Faraday constant $F = 96500 	ext{ C mol}^{-1}$]

Accepted Answer

$\Delta G^{\ominus} = -nF E^{\ominus}_{cell} = -2 	imes 96500 	imes 0.24 	ext{ J mol}^{-1} = -46320 	ext{ J mol}^{-1} = -46.32 	ext{ kJ mol}^{-1}$.

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