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The equilibrium constant for the reaction image 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)



ΔG = 69.1 kJ/mol, nonspontaneous



ΔG = –69.1 kJ/mol, spontaneous



ΔG = 97.5 kJ/mol, spontaneous



ΔG = 40.6 kJ/mol, nonspontaneous



ΔG = –97.5 kJ/mol, nonspontaneous

Textbook 
Chemistry: Atoms First

Chemistry: Atoms First


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