Collision Theory?

Question

It has been observed that more gas station fires occur on hot days than cold days. Explain this phenomenon using knowledge of the collision theory. (Hint: it is not just the temperature factor that causes). I need help with this question, please explain well, I'm only 15 years old!

Answer 1

In order for a chemical reaction occur the two substances which are reaction must collide with each other and have sufficient energy to react.

Temperature is the measure of the average kinetic energy of a substance. The higher the temperature, the higher the average kinetic energy, thus the faster the particles of the substance are moving.

On hotter days the gasoline and air molecules have higher temperatures and are thus moving around much faster than on cold days. When molecules are moving around faster two things happen...firstly the molecules collide more often, and secondly, on average there is more energy present per collision.
So on hot days the gasoline and Oxygen molecules collide with more energy than they would on colder days...resulting in a higher probability of a reaction between the molecules. So it would make sense that more gasoline fires start on hot days rather than cold days using the collision theory of gasses.

Answer 2

Collision theory explains how chemical reactions occur and why rates of reaction differ. For a reaction to occur the reactant particles must collide. Only a certain fraction of the total collisions cause chemical change; these are called "successful collisions". The successful collisions have sufficient energy (activation energy) at the moment of impact to break the existing bonds and form new bonds, resulting in the products of the reaction