Problem: 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

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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, nonspontaneous
B. ΔG = -97.5 kJ, spontaneous
C. ΔG = 40.6 kJ, nonspontaneous
D. ΔG = -69.1 kJ, spontaneous
E. ΔG = 97.5 kJ, nonspontaneous

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