Note that the mean energy of the collisions changes when the temperature changes. When the temperature is increased, the mean energy of the particles also increases. The frequency of collisions increases, but so does the likelihood that the collision exceeds the activation energy. Both changes mean that the proportion of collisions that are successful increases.
Explain what is meant by a 'successful' collision.
A collision between reactant particles with enough energy (the activation energy or more than the activation energy) to produce a reaction.
The gradient of the line is equal to the rate of reaction. The faster reaction at the higher temperature:
Note that the amount of product does not change when the reaction rate changes. The same amount of product is formed, but in a shorter time. Therefore, both lines on the graph finish in the same value of mass or volume, but the reaction at the higher temperature reaches this mass or volume sooner.