How does temperature influence the rate of a reaction according to collision theory?

Higher temperatures increase the average kinetic energy of the particles involved in a reaction. According to collision theory, for a reaction to take place, reacting particles must collide with sufficient energy and the correct orientation. When the temperature rises, the kinetic energy of the particles also rises, causing them to move more quickly. This increased movement leads to more frequent collisions between the reactant particles.

Furthermore, as the particles have higher energy, a larger proportion of these collisions will have the necessary energy to overcome the activation energy barrier, allowing more reactions to occur. This is why an increase in temperature is directly related to an increase in the rate of reaction, as it enhances both the frequency and the effectiveness of the collisions between reactants.