What will happen to reaction rates when the kinetic energy of molecules increases?

When the kinetic energy of molecules increases, the reaction rates will also increase. This relationship is fundamentally rooted in the principles of collision theory, which states that for a reaction to occur, reactant molecules must collide with sufficient energy to overcome the activation energy barrier—the minimum energy required for a reaction to happen.

As the temperature rises, the kinetic energy of the molecules increases, leading to more frequent and more forceful collisions. With more molecules colliding at greater energies, the likelihood that these collisions will be effective in producing a reaction also increases. Consequently, the overall rate of reaction tends to rise.

Additionally, an increase in kinetic energy often results in a greater proportion of molecules having enough energy to overcome the activation energy, further driving the reaction forward. Thus, an increase in molecular kinetic energy directly correlates with an increase in reaction rates.