is this correct?

Question

Sr²⁺(aq) + F^-(aq) ⇄ SrF⁺(aq)

At 25°C, the equilibrium constant for the reaction represented above has a value of 1.3. At 50°C, the value of the equilibrium constant is less than 1.3. Based on this information, which of the following must be correct?

1. At 25°C, ∆H° for the reaction is negative.
2. At 25°C, ∆G° for the reaction is positive.
3. At 25°C, ∆, S, ° for the reaction is positive.
4. The reaction is thermodynamically favorable only at temperatures above 25°C.

is this correct?

Answer 1

Your response seems to be correct. Since an elevated temperature reduces the Keq, this suggests the reaction is exothermic and thus ∆H is negative @ 25ºC.