Activation energy is the minimum amount of energy that is needed by the reactant molecules to initiate a chemical reaction. It is represented as Ea and is typically measured in the units of joules/mole, kilojoules/mole, or kilocalories/mole. This term was coined by Svante Arrhenius in 1889.
In order to proceed with a chemical reaction, some temperature must be provided to the reacting molecules so that their translational energy becomes equal to or greater than the activation energy. The catalyst is those molecules which have an ability to lower the activation energy of a system and therefore, the rate of the reaction is increased.
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