Cu(s) + Sn2+(0.001M) Cu2+ (0.01M) + Sn(s)

The Gibbs free energy change for the above reaction at 298 K is x * 101 KJmol1. The value of x is __________. (nearest integer)

[Given : ${}_{{}^{}}^{}$ 0.34V; ${}_{{}^{}}^{}$ = 0.14V; F = 96500 Cmol1]

cell reaction is ;

              $Cu\left(s\right)+S{n}_{\left(aq\right)}^{2+}\to C{u}_{\left(aq\right)}^{++}+S{n}_{\left(s\right)}$  

              $Q=\frac{\left[C{u}^{++}\right]}{\left[S{n}^{++}\right]}=\frac{0.01}{0.001}andn=2$  

              $E_{cell}=E_{cell}^o-\frac{0.059}{2}log\frac{0.01}{0.001}$  

              $=-0.48-\frac{0.059}{2}log10=-0.509$  

              $=983.33*10^{-1}KJ/mole$  

              Nearest integer = 983