Question #44290

Consider the following halogen exchange equilibria at 298 K: Reaction I: $\ce{Cl(g) + F^{-}(g) \rightleftharpoons Cl^{-}(g) + F(g)}$ (Equilibrium constant $K_1$) Reaction II: $\ce{Cl(g) + F^{-}(aq) \rightleftharpoons Cl^{-}(aq) + F(g)}$ (Equilibrium constant $K_2$) Assume entropic contributions ($\Delta S^\ominus$) are negligible such that $\Delta G^\ominus \approx \Delta H^\ominus$. Given the standard thermodynamic data at 298 K: Electron gain enthalpy ($\Delta_{eg}H^\ominus$): $\ce{F} = -333 \text{ kJ/mol}$, $\ce{Cl} = -349 \text{ kJ/mol}$ Hydration enthalpy ($\Delta_{hyd}H^\ominus$): $\ce{F^{-}} = -515 \text{ kJ/mol}$, $\ce{Cl^{-}} = -381 \text{ kJ/mol}$ Which of the following correctly identifies the standard enthalpy changes ($\Delta H^\ominus$) for Reactions I and II, and the relationship between their equilibrium constants?