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? (R = 8.314 J/K • mol) A. ΔG = –97.5 kJ/mol, nonspontaneous B. ΔG = 40.6 kJ/mol, nonspontaneous C. ΔG = 97.5 kJ/mol, spontaneous D. ΔG = 69.1 kJ/mol, nonspontaneous E. ΔG = –69.1 kJ/mol, spontaneous

Question

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? (R = 8.314 J/K • mol)

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

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