The Equilibrium Constant for the Reaction AgBr(s) Ag⁺(aq)+ Br^{- $\times$}

Multiple Choice

The equilibrium constant for the reaction AgBr(s) Ag⁺(aq) + Br^- (aq) is the solubility product constant, K_sp = 7.7 $\times$ 10^-13 at 25°C. Calculate $\Delta$ G for the reaction when [Ag⁺] = 1.0 $\times$ 10^-2 M and [Br^-] = 1.0 $\times$ 10^-3 M. Is the reaction spontaneous or nonspontaneous at these concentrations?

A) ( $\Delta$ G = 69.1 kJ/mol, nonspontaneous)
B) ( $\Delta$ G = -69.1 kJ/mol, spontaneous)
C) ( $\Delta$ G = 97.5 kJ/mol, spontaneous)
D) ( $\Delta$ G = 40.6 kJ/mol, nonspontaneous)
E) ( $\Delta$ G = -97.5 kJ/mol, nonspontaneous)