The value of K_eq nearly always changes with a change in temperature.

This can expressed alternatively by

When ΔH is negative, the log term is negative, so the log is a fraction, so K₂ is less than K₁. In other words, the equilibrium for exothermic reactions shifts to the reactant side with increased temeprature.

When ΔH is positive, the log term is positve, so the log is greater than one, so K₂ is greater than K₁. In other words, the equilibrium for endothermic reactions shifts to the product side with increased temperature.