The Equilibrium Constant for the Reaction AgBr(s) $\rarr$ Ag⁺(aq)+ Br^- (aq)is the Solubility Product Constant, K_sp = 7

The equilibrium constant for the reaction AgBr(s) $\rarr$ Ag⁺(aq) + Br^- (aq) is the solubility product constant, K_sp = 7.7* 10^-13 at 25°C. Calculate $\Delta$ G for the reaction when [Ag⁺] = 1.0 * 10^-2 M and [Br^-] = 1.0 * 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