Calculate the $K_C$ and $\Delta G^o$ for the chemical reaction :
$Ni_{(s)} + 2Ag_{(aq)}^{+} \to Ni_{(aq)}^{2+} + 2Ag_{(s)}$ $ [E^o = 1.05 \, V] $

(N/A) The number of electrons transferred in the reaction is $n = 2$.
Using the formula $\Delta G^o = -nFE^o$:
$\Delta G^o = -2 \times 96487 \, C \, mol^{-1} \times 1.05 \, V = -202622.7 \, J \, mol^{-1} \approx -2.026 \times 10^{2} \, kJ \, mol^{-1}$.
Using the relation $\Delta G^o = -RT \ln K_C$ or $\log K_C = \frac{nE^o}{0.059}$ at $298 \, K$:
$\log K_C = \frac{2 \times 1.05}{0.059} = 35.593$.
$K_C = 10^{35.593} \approx 3.92 \times 10^{35}$.