6.2.2-6.2.3

Definition of activation energy
Activation energy is defined as the minimum value of kinetic energy which particles must have before they are able to react.
Three factors that affect the rate of reaction
1 Collision frequency- The higher the frequency the more likely there will be a successive collision therefore the faster the reaction.

2 Energy of collision- For a reaction to take place, the particles must have a certain minimum value for their kinetic energy. This energy is needed to overcome the repulsion between molecules and often to break some bonds in the reactants before they can react (activation energy). Only particles which have a kinetic energy value greater than the Ea will be able to achieve a reaction- have successful collision. KINETIC > Ea

3 Geometry of collision- Since collisions are random, they are likely to occur with the particles in many different orientations. In some reactions, this can be crucial in determining whether or not the collisions will be successful and therefore what proportion of collisions will lead to a reaction.