Consider the following cell reaction :

$C{d_{(s)}} + H{g_2}S{O_{4(s)}} + {9 \over 5}{H_2}{O_{(l)}}$ $\rightleftharpoons$ $CdS{O_4}.{9 \over 5}{H_2}{O_{(s)}} + 2H{g_{(l)}}$

The value of $E_{cell}^0$ is 4.315 V at 25$^\circ$C. If $\Delta$H$^\circ$ = $-$825.2 kJ mol^$-$1, the standard entropy change $\Delta$S$^\circ$ in J K^$-$1 is ___________. (Nearest integer) [Given : Faraday constant = 96487 C mol^$-$1]