How does increasing temperature affect an exothermic reaction at equilibrium?

In an exothermic reaction, heat is released as a product, meaning that when the reaction is at equilibrium, it can be represented in the form of a reaction where heat can be considered a product. According to Le Chatelier’s principle, when a system at equilibrium is subjected to a change in temperature, pressure, or concentration, the equilibrium will shift to counteract that change.

When the temperature is increased in an exothermic reaction, the system tries to reduce this increase by shifting the equilibrium toward the reactants. This shift means that the reaction favors the reverse process, which absorbs heat, thus mitigating the effect of the added heat. Therefore, raising the temperature results in a shift to the side of the reactants, demonstrating that the equilibrium is affected by temperature changes.

This understanding is crucial in predicting how temperature changes can affect chemical processes and reactions, particularly in industrial applications where controlling temperature can optimize the yield of desired products.