For the reaction taking place in the cell \[ \begin{array}{l} \mathrm{Pt}\left|\mathrm{H}_{2}(\m...

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For the reaction taking place in the cell
\[
\begin{array}{l}
\mathrm{Pt}\left|\mathrm{H}_{2}(\mathrm{~g})\right| \mathrm{H}^{+}(\mathrm{aq}) \| \mathrm{Ag}^{+}(\mathrm{aq}) \mid \mathrm{Ag}(\mathrm{s}) \\
\mathrm{E}^{\mathrm{o}} \text { cell }=+0.5332 \mathrm{~V} .
\end{array}
\]
The value of \( \Delta_{\mathrm{f}} \mathrm{G}^{0} \) is \( \mathrm{kJ} \mathrm{mol}^{-1} \). (in nearest integer)
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