What is the relationship between temperature and reaction rates for most reactions?

The relationship between temperature and reaction rates for most reactions is that higher temperatures generally speed up reactions. This occurs because an increase in temperature provides reactant molecules with more kinetic energy. As the temperature rises, the molecules move faster, leading to a greater frequency of collisions among them.

Furthermore, not only do the molecules collide more often, but they also collide with greater energy. This increased energy means that a larger proportion of these collisions will have enough energy to overcome the activation energy barrier required for the reaction to proceed. As a result, the rate of formation of products increases at higher temperatures.

This principle is widely applicable in various chemical reactions, including both exothermic and endothermic reactions, making it a fundamental concept in chemical kinetics. Understanding this relationship helps explain why many chemical processes are run at elevated temperatures, especially in industrial settings, to enhance reaction rates and improve efficiency.