The equilibrium constant for the reaction AgBr(s) Ag⁺(aq)+ Br^-(aq)is the solubility product constant, K_sp = 7.7 $\times$ 10^-13 at 25°C. Calculate $\Delta$G for the reaction when [Ag⁺] = 1.0 $\times$ 10^-2 M and [Br^-] = 1.0 $\times$ 10^-3 M. Is the reaction spontaneous or nonspontaneous at these concentrations? A)($\Delta$G = 69.1 kJ/mol, nonspontaneous) B)($\Delta$G = -69.1 kJ/mol, spontaneous) C)($\Delta$G = 97.5 kJ/mol, spontaneous) D)($\Delta$G = 40.6 kJ/mol, nonspontaneous) E)($\Delta$G = -97.5 kJ/mol, nonspontaneous)

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The Answer of The equilibrium constant for the reaction AgBr(s) Ag⁺(aq)+ Br^-(aq)is the solubility product constant, K_sp = 7.7 $\times$ 10^-13 at 25°C. Calculate $\Delta$G for the reaction when [Ag⁺] = 1.0 $\times$ 10^-2 M and [Br^-] = 1.0 $\times$ 10^-3 M. Is the reaction spontaneous or nonspontaneous at these concentrations? A)($\Delta$G = 69.1 kJ/mol, nonspontaneous) B)($\Delta$G = -69.1 kJ/mol, spontaneous) C)($\Delta$G = 97.5 kJ/mol, spontaneous) D)($\Delta$G = 40.6 kJ/mol, nonspontaneous) E)($\Delta$G = -97.5 kJ/mol, nonspontaneous)

The Equilibrium Constant for the Reaction AgBr(s) Ag+(aq)+ Br- ×\times×

The Equilibrium Constant for the Reaction AgBr(s) Ag⁺(aq)+ Br^{- $\times$}