What is the effect of temperature on exothermic reactions?

In exothermic reactions, where heat is released as a product, an increase in temperature generally results in an increased reaction rate. This acceleration occurs because higher temperatures provide more kinetic energy to the reactant molecules, leading to more frequent and effective collisions among them.

Moreover, according to the principles of chemical kinetics, reactions typically exhibit higher rates at elevated temperatures due to increased molecular motion, which overcomes the activation energy barrier more efficiently. This means that the molecules are more likely to collide with enough energy and proper orientation to produce the products of the reaction.

It's important to note that while higher temperatures can increase the reaction rates for exothermic processes, they may also influence the equilibrium position in reversible reactions, but in the context of this question, the focus is specifically on the rate of the exothermic reactions themselves.