For the reaction taking place in the cell:
$$
\begin{aligned}
& \mathrm{Pt}(\mathrm{~s})\left|\mathrm{H}_2(\mathrm{~g})\right| \mathrm{H}^{+}(\mathrm{aq}) \| \mathrm{Ag}^{+}(\mathrm{aq}) \mid \mathrm{Ag}(\mathrm{~s}) \\
& \mathrm{E}_{\text {Cell }}^{\circ}=+0.5332 \mathrm{~V} .
\end{aligned}
$$
The value of $\Delta_{\mathrm{f}} \mathrm{G}^0$ is $\_\_\_\_$ $\mathrm{kJ} \mathrm{mol}^{-1}$. (if $\mathrm{n}=1$ ) (in nearest integer)
