🤓 Based on our data, we think this question is relevant for Professor Cavagnero's class at UW-MADISON.
Solution: The equilibrium constant for the reaction: AgBr(s) ⇌ Ag+(aq) + Br-(aq)is the solubility product constant, Ksp= 7.7 x 10 -13 at 25°C. Calculate ΔG for the reaction when [Ag+] = 1.0 x 10-2 M and [Br-] = 1.0 x 10-3 M. Is the reaction spontaneous or nonspontaneous at these concentrations?A. ΔG = 69.1 kJ, nonspontaneousB. ΔG = -97.5 kJ, spontaneousC. ΔG = 40.6 kJ, nonspontaneousD. ΔG = -69.1 kJ, spontaneousE. ΔG = 97.5 kJ, nonspontaneous