Use the collision theory to explain how increasing the temperature of a reaction will affect the rate of the reaction.

Explanation:

Reaction rate is a measure of the speed of a chemical reaction. There are many theories that have been put forward to explain reaction rates. One of which is the collision theory.

The collision theory postulates that for a reaction to occur, there must be collisions between reacting particles. This implies that the number of successful or effective collision of particles determines the rate of a chemical reaction. For a collision to be successful, the particles must be properly oriented and equiped with adequate energy for the reaction.

One of the key component of the energy required for effective collision is temeperature. The  number of effective collision and consequently the rate of chemical reactions are directly proportional to the temperature at which the reaction occurs. With increasing temperature, the activation energy becomes activated and the number of collision increases.

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