Chemistry - Electrochemistry Question with Solution | TestHub

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