What happens to the relative amount of products at equilibrium when the temperature is increased for an exothermic reaction?

In an exothermic reaction, heat is released as a product of the reaction. According to Le Chatelier's principle, when the temperature of a system at equilibrium is increased, the system will respond by attempting to counteract that increase in temperature. In the case of an exothermic reaction, this means that the equilibrium will shift in such a way as to favor the reactants, thereby reducing the amount of heat generated by the reaction.

As the equilibrium shifts towards the reactants, the relative amount of products in the reaction decreases. This adjustment helps restore balance to the system despite the added heat. Consequently, increasing the temperature of an exothermic reaction results in a decrease in the concentration of products relative to reactants as the system moves to reach a new equilibrium state.