Using the Gibbs energy change, Δ G^o =+63.3 kJ, for the following reaction, Ag_2 CO_3( s ) ⇌ 2 Ag^+( aq )+ CO_3^2-( aq ) the K_sp of Ag_2 CO_3( s )…

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