The Equilibrium Constant for the Reaction AgBr(s) Ag⁺(aq)

The equilibrium constant for the reaction AgBr(s) Ag⁺(aq) + Br^- (aq) is the solubility product constant, K_sp = 7.7 × 10^-13 at 25°C. Calculate ΔG 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? (R = 8.314 J/K • mol)

A) ΔG = 69.1 kJ/mol, nonspontaneous
B) ΔG = -69.1 kJ/mol, spontaneous
C) ΔG = 97.5 kJ/mol, spontaneous
D) ΔG = 40.6 kJ/mol, nonspontaneous
E) ΔG = -97.5 kJ/mol, nonspontaneous