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For the cell reaction
\( 2 \mathrm{Fe}^{3+}(\mathrm{aq})+2 \mathrm{I}^{-}(\mathrm{aq}) \rightarrow 2 \mathrm{Fe}^{2+}(\mathrm{aq})+\mathrm{I}_{2}(\mathrm{aq}) \)
\( \mathrm{P} \)
\( \mathrm{E}_{\text {cell }}^{\circ}=0.24 \mathrm{~V} \) at \( 298 \mathrm{~K} \). The standard Gibbs energy
W
\( \left(\Delta_{\mathrm{r}} \mathrm{G}^{\circ}\right) \) of the cell reaction is :
[Given that Faraday constant \( \mathrm{F}=96500 \mathrm{C} \mathrm{mol}^{-1} \) ]
(1) \( -46.32 \mathrm{~kJ} \mathrm{~mol}^{-1} \)
(2) \( -23.16 \mathrm{~kJ} \mathrm{~mol}^{-1} \)
(3) \( 46.32 \mathrm{~kJ} \mathrm{~mol}^{-1} \)
(4) \( 23.16 \mathrm{~kJ} \mathrm{~mol}^{-1} \)
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