The equilibrium constant for the reaction below is 7.2 x 10^-4 at 298 K and 1 atm. HNO₂(aq) + H₂O(l) ⇌ NO₂^-(aq) + H₃O⁺(aq)
When [HNO₂(aq) ] = 1.0 M and [NO₂^-(aq) ] = [H₃O⁺(aq) ] = 1.0 x 10^-5 M, calculate ΔG.

Question

Quizplus · Accepted Answer

The reaction quotient, Q, is calculated as:Q = [NO2-] [H3O+] / [HNO2] = (1.0 x 10^-5) (1.0 x 10^-5) / 1.0 = 1.0 x 10^-10Since Q < K, the reaction will proceed in the forward direction to reach equilibrium. The change in free energy, ΔG, is calculated using the equation:ΔG = -RT ln(Q/K) = -(8.314 J/mol K) (298 K) ln(1.0 x 10^-10 / 7.2 x 10^-4) = -39.1 kJ/molTherefore, the correct answer is A) -39.1 kJ/mol.

The Equilibrium Constant for the Reaction Below Is 7