The Gibbs energy change (in J ) for the given reaction at $[\mathrm{Cu} 2+]=[\mathrm{Sn} 2+]=1 \mathrm{M}$ and 298 K is:
$\begin{aligned} & \mathrm{Cu}(\mathrm{s})+\mathrm{Sn}^{2+}(\text { aq. }) \rightarrow \mathrm{Cu}^{2+}(\text { aq. })+\mathrm{Sn}(\mathrm{s}) \\ & \left(\mathrm{E}_{\mathrm{Sn}^{2+} \mid \mathrm{Sn}}^0=-0.16 \mathrm{~V}, \mathrm{E}_{\mathrm{Cu}^{2+} \mid \mathrm{Cu}}^0=0.34 \mathrm{~V}\right.\end{aligned}$
Take $\left.\mathrm{F}=96500 \mathrm{C} \mathrm{mol}^{-1}\right)$