Using the Gibbs energy change, $\Delta G^{\circ }=+63.3\text{kJ}$, for the reaction:
$${\text{Ag}}_2{\text{CO}}_3(s)\rightleftharpoons 2{\text{Ag}}^{+}(aq)+{\text{CO}}_3^{2-}(aq)$$
The $K_{sp}$ of ${\text{Ag}}_2{\text{CO}}_3(s)$ in water at $25^{\circ }\text{C}$ is: ($R=8.314{\text{J K}}^{-1}{\text{mol}}^{-1}$)

1. A
   $3.2\times 10^{-26}$
2. B
   $8.0\times 10^{-12}$
3. C
   $2.9\times 10^{-3}$
4. D
   $7.9\times 10^{-2}$