For the cell reaction, $3 \mathrm{Sn}^{4+}+2 \mathrm{Cr} \longrightarrow 3 \mathrm{Sn}^{2+}+2 \mathrm{Cr}^{3+}, E_{\text {cell }}^{\circ}$ is $0.89 \mathrm{~V}$. Then $\Delta G^{\circ}$ for the reaction is

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Aicharya · Accepted Answer

$\begin{aligned} \Delta G^{\circ} & =-n F E_{\text {cell }}^{\circ} \ & =-6 \times 96500 \times 0.89 \times 10^{-3} \mathrm{~kJ} \mathrm{~mol}^{-1} \ & =-515.31 \mathrm{~kJ} \mathrm{~mol}^{-1} \end{aligned}$

For the cell reaction, \(3 \mathrm{Sn}^{4+}+2 \mathrm{Cr} \longrightarrow 3 \mathrm{Sn}^{2+}+2…

Solution