ΔG° = 91.7 kJ/mol at 25°C for the following process. Which of the following statements is correct when [Ag+] = 1.1 × 10–9 M and [I–] = 1.5 × 10–9 M. (R = 8.314 J/K • mol) AgI(s) ⟷ Ag+(aq) + I–(aq) A) Under the current conditions, ΔG > 0. Hence, this reaction will go in the forward direction to reach equilibrium. B) This reaction favors the reactants because Δ G ∘> 0 C) K > 1, because ΔG < 0. D) K > 1, because ΔG° > 0. E) None of the choices is correct.

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