Consider the following cell reaction: 

$C{d}_{\left(s\right)}+H{g}_{2}S{O}_{4\left(s\right)}+\frac{9}{5}{H}_2{O}_{\left(I\right)}+CdS{O}_4\cdot \frac{9}{5}{H}_2{O}_{\left(s\right)}+2H{g}_{\left(I\right)}$

The value of $E_{cell}^0$ is 4.315V at 25°C. If $\Delta H^o$ = -825.2 kJ mol^-1, the standard entropy change   $\Delta S°$  in JK^-1 is_________. (Nearest integer)

           [Given: Faraday constant = 96487 C mol^-1]