What does an increase in temperature generally do to the rate of a chemical reaction?

An increase in temperature generally increases the rate of a chemical reaction due to several factors related to molecular behavior. When temperature rises, the kinetic energy of the molecules involved in the reaction also increases. This boost in kinetic energy causes molecules to move faster, leading to more frequent collisions between the reactant molecules. Not only do collisions happen more often, but they are also more energetic.

For a chemical reaction to occur, the colliding molecules must have sufficient energy to overcome the activation energy barrier—the minimum energy required for the reaction to take place. As the temperature increases, a greater fraction of the molecules possess the energy needed to surpass this barrier, thereby facilitating a higher reaction rate.

This concepts underpins the principle that temperature is a critical factor in reaction kinetics, affecting both the frequency and energy of collisions between reactants. Additionally, the impact of temperature on reaction rates applies to various states of matter, not limited to gaseous reactions alone.