The equilibrium constant for the reaction AgBr(s) ![The equilibrium constant for the reaction AgBr(s) Ag<sup>+</sup>(aq) + Br<sup>-</sup> (aq) is the solubility product constant,K<sub>sp</sub> = 7.7 × 10<sup>-13</sup> at 25°C.Calculate ΔG for the reaction when [Ag<sup>+</sup>] = 1.0 × 10<sup>-2</sup> M and [Br<sup>-</sup>] = 1.0 × 10<sup>-3</sup> M.Is the reaction spontaneous or nonspontaneous at these concentrations? (R = 8.314 J/K • mol) A) ΔG = 69.1 kJ/mol,nonspontaneous B) ΔG = -69.1 kJ/mol,spontaneous C) ΔG = 97.5 kJ/mol,spontaneous D) ΔG = 40.6 kJ/mol,nonspontaneous E) ΔG = -97.5 kJ/mol,nonspontaneous](https://d2lvgg3v3hfg70.cloudfront.net/TB6485/11eab46b_9cab_16f9_a889_75a86584b61f_TB6485_11.jpg)
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 = 69.1 kJ/mol,nonspontaneous
B) ΔG = -69.1 kJ/mol,spontaneous
C) ΔG = 97.5 kJ/mol,spontaneous
D) ΔG = 40.6 kJ/mol,nonspontaneous
E) ΔG = -97.5 kJ/mol,nonspontaneous
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