The equilibrium constant for the reaction AgBr(s) Ag (aq) Br– (aq) is the solubility product constant, Ksp = 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? Question 14 options: ΔG = 97.5 kJ/mol, spontaneous ΔG = 40.6 kJ/mol, nonspontaneous ΔG = 69.1 kJ/mol, nonspontaneous ΔG = –69.1 kJ/mol, spontaneous ΔG = –97.5 kJ/mol, nonspontaneous
