Explain how increasing the temperature of a reaction mixture increases the rate of reaction.

Increasing the temperature raises the kinetic energy of the reacting particles.

Higher kinetic energy means that, on average, particles move faster and therefore collide more often – the collision frequency increases.

With more energy, a larger proportion of the particles possess energy equal to or greater than the activation energy of the reaction.

Consequently, a greater number of collisions are successful, leading to more reaction events per unit time.

Thus, both the increased collision frequency and the larger fraction of collisions that exceed the activation energy combine to raise the overall rate of reaction.