$E _{\text {cell }} = E _{\text {cathode }}^{\circ}- E _{\text {anode }}^{\circ}$

$=-0.14-(0.34)$

$=-0.48 \,V$

$E _{\text {cell }} = E _{\text {cell }}^{\circ}-\frac{0.059}{2} \log \frac{\left[ Cu ^{2+}\right]}{\left[ Sn ^{2+}\right]}$

$=-0.48-\frac{0.059}{2} \log \frac{0.01}{0.001}$

$=-0.509$

$\Delta G =- nF E _{\text {cell }}$

$=-2 \times 96500 \times(-0.5095)$

$=98333.5\, J / mol$

$=98.335\, kJ / mol$

$=983.35 \times 10^{-1} \,kJ / mol$

$\text { Nearest Integer : } 983$