What happens to the value of Kc if the forward reaction is favored due to an increase in temperature?

When considering the value of the equilibrium constant (Kc) in relation to temperature changes, it is essential to understand the nature of the reactions and how they respond to temperature. If the forward reaction is favored due to an increase in temperature, this typically indicates that the reaction is endothermic.

In endothermic reactions, heat is absorbed when the reaction proceeds in the forward direction. According to Le Chatelier’s principle, increasing temperature shifts the equilibrium position to favor the endothermic direction as the system attempts to counteract the added heat. As a result, more products are formed, which increases the concentrations of the products at equilibrium.

The equilibrium constant, Kc, is defined as the ratio of the concentrations of products raised to their stoichiometric coefficients divided by the concentrations of reactants raised to their stoichiometric coefficients. When the formation of products is favored with the increase in temperature, the concentration of products increases relative to that of reactants, leading to an increase in the value of Kc.

This principle is further supported by the Van't Hoff equation, which relates changes in temperature to changes in the equilibrium constant for a given reaction. Therefore, an increase in temperature, when the forward reaction is favored, results in an increase