For two molecules to react, they must collide at just the right angle and with enough energy to break the original bonds and form new ones. Based on these facts, why does the reaction tend to go more quickly at higher temperatures

Explanation:

An increase in temperature typically increases the rate of reaction. An increase in temperature will raise the average kinetic energy of the reactant molecules. Therefore, a greater proportion of molecules will have the minimum energy necessary for an effective collision.

Increasing the temperature increases reaction rates because of the disproportionately large increase in the number of high energy collisions. It is only these collisions (possessing at least the activation energy for the reaction) which result in a reaction.

When temperature increases, the amount of atomic or molecular collisions between molecules increases. But the change in reaction rate with temperature is not just a function of the temperature; instead, temperature increases actually affect the rate constants (written k) of reactions in a predictable way.

As a rule of thumb, a rise in temperature of 10 °C doubles the reaction rate.