How does the collision theory explain the rate of a chemical reaction?

Kingsley Thompson December 03, 2025

5(a) How does the collision theory explain the rate of a chemical reaction?

5(b) State how each of the following affects the rates of chemical reactions: 

(i) Surface area

(ii) Catalyst

Answers

5(a) The collision theory assumes that there must be collisions between reactant particles for a chemical to occur, i.e. the number of collision between the reactant molecules is directly proportional to the rate of reaction.

5(b)(i) The greater the surface area available for the reactant, the faster the rate of the reaction

5(b)(ii) A catalyst (positive) increases the rate of a spontaneous chemical reaction by lowering the energy barrier (activation energy) of the reactant.


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Kingsley Thompson

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