If the temperature is increased , the number of collision per second increases.
Explanation
Temperature is proportional to the average kinetic energy of a sample of a gas according to the equation PV=n R T. An increased in temperature , increases the kinetic energy of the gas particles which in turn rises the velocity of the gas particles hitting the walls of the container. The more the number of particles the higher the collision rate and greater the pressure as long as the volume of container and the temperature are constant.
This increases the rate of rxn because the particles, because according to the Collision Theory, <span>the </span>rate of rxn <span>is proportional to number of effective collisions between the </span>reactant <span>molecules.</span>