For the cell reaction:

$2{\mathrm{Fe}}_{\left(\mathrm{aq}\right)}^{3+}+2{\mathrm{I}}_{\left(\mathrm{aq}\right)}^{-}⟶2{\mathrm{Fe}}_{\left(\mathrm{aq}\right)}^{2+}+{\mathrm{I}}_{2\left(\mathrm{aq}\right)}$

${{\mathrm{E}}^{\mathrm{o}}}_{\text{cell }}=0.24 \mathrm{V}\text{ at }298 \mathrm{K}$. The standard Gibbs energy $\left({\mathrm{\Delta }}_{\mathrm{r}}\mathrm{G}°\right)$of the cell reaction is

$\text{ [Given that Faraday constant }\left.\mathrm{F}=96500{\mathrm{Cmol}}^{-1}\right]$