How does temperature generally affect the rate of a chemical reaction?

Increasing temperature generally increases the rate of a chemical reaction due to the fact that temperature is a measure of the average kinetic energy of the molecules involved in the reaction. As temperature rises, the molecules move faster, leading to an increase in the frequency of collisions between reactant molecules. Furthermore, a higher temperature provides reactant molecules with more energy, increasing the likelihood that collisions will have sufficient energy to overcome the activation energy barrier necessary for the reaction to occur. This results in a greater number of successful reactions and, consequently, a higher reaction rate.

In contrast, lower temperatures tend to slow down molecular movement, which can reduce both the frequency and energy of collisions, leading to a slower reaction rate. Therefore, while a few specific reactions might behave differently under unique conditions, the general principle holds true across a wide range of chemical reactions.