Consider the following cell reaction :
$\mathrm{Cd}_{(\mathrm{s})}+\mathrm{Hg}_2 \mathrm{SO}_{4(\mathrm{~s})}+\frac{9}{5} \mathrm{H}_2 \mathrm{O}_{(\mathrm{i})} \rightleftharpoons \mathrm{CdSO}_4 \cdot \frac{9}{5} \mathrm{H}_2 \mathrm{O}_{(\mathrm{s})}+2 \mathrm{Hg}_{(\mathrm{i})}$
The value of $\mathrm{E}_{\text {cell }}^0$ is 4.315 V at $25^{\circ} \mathrm{C}$. If $\Delta \mathrm{H}^{\circ}=-825.2 \mathrm{~kJ} \mathrm{~mol}^{-1}$, the standard entropy change $\Delta \mathrm{S}^{\circ}$ in $\mathrm{J} \mathrm{K}^{-1}$ is $\_\_\_\_$ . (Nearest integer) [Given : Faraday constant = $96487 \mathrm{C} \mathrm{mol}^{-1}$ ]