# 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 25oC. Calculate ΔG for the reaction when [Ag+] = 1.0 x 10–2 M and [Br–] = 1.0 x 10–3 M. Is the precipitation of AgBr spontaneous or nonspontaneous at these concentrations? a) ΔG = 69.1 kJ/mol, spontaneous b) ΔG = ‐69.1 kJ/mol, non‐spontaneous c) ΔG = 97.5 kJ/mol, non‐spontaneous d) ΔG = 40.6 kJ/mol, spontaneous e) ΔG = ‐97.5 kJ/mol, spontaneous

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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 25oC. Calculate ΔG for the reaction when [Ag+] = 1.0 x 10–2 M and [Br] = 1.0 x 10–3 M. Is the precipitation of AgBr spontaneous or nonspontaneous at these concentrations?

a) ΔG = 69.1 kJ/mol, spontaneous

b) ΔG = ‐69.1 kJ/mol, non‐spontaneous

c) ΔG = 97.5 kJ/mol, non‐spontaneous

d) ΔG = 40.6 kJ/mol, spontaneous

e) ΔG = ‐97.5 kJ/mol, spontaneous

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