The equilibrium constant for the reaction AgBr(s) $\leftrightharpoons$ Ag⁺(aq) + Br^- (aq) is the solubility product constant, K_sp = 7.7 *10^-13 at 25^$\circ$C. Calculate $\Delta$G 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 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

Question

Quizplus · Accepted Answer

The Answer of The equilibrium constant for the reaction AgBr(s) $\leftrightharpoons$ Ag⁺(aq) + Br^- (aq) is the solubility product constant, K_sp = 7.7 *10^-13 at 25^$\circ$C. Calculate $\Delta$G 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 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) ⇋\leftrightharpoons⇋ Ag+(aq) + Br- (Aq) Is the Solubility Product Constant, Ksp

The Equilibrium Constant for the Reaction AgBr(s) $\leftrightharpoons$ Ag⁺(aq) + Br^- (Aq) Is the Solubility Product Constant, K_sp