Can you please explain the effect of increasing temperature on the rate of reaction

For a given reaction, it is often seen that the rate of reaction doubles following a 10oC increase in temperature. But why is this?

(note: Here I would plot a graph of Rate vs Temperature, to show the non-linear relationship)

The rate of reaction is the speed at which a chemical reaction takes. To understand how a given factor alters the rate of reaction, we use ‘collision theory’. Collision theory is a scientific model which allows us to consider the rate of reaction, by understanding the interactions of molecules within a liquid or gas solution. Collision theory states that in order to have a successful reaction, molecules must collide with a given energy – this is known as the activation energy (EA).

At higher temperatures, the molecules in a reaction mixture move at a greater speed and so have a higher energy. Subsequently, following an increase in temperature, a greater number of particles have an energy that is greater than or equal to the EA, and so there is a greater proportion of successful collisions – meaning there is an increase in the rate of reaction.

(note: Here I would plot a graph of Energy vs reaction coordinate, to show the energy requirement for a successful reaction)