<P> The term was introduced in 1889 by the Swedish scientist Svante Arrhenius . </P> <P> The Arrhenius equation gives the quantitative basis of the relationship between the activation energy and the rate at which a reaction proceeds . From the equation, the activation energy can be found through the relation </P> <Dl> <Dd> k = A e − E a / (R T) (\ displaystyle k = Ae ^ ((- E_ (\ textrm (a))) / ((RT)))) </Dd> </Dl> <Dd> k = A e − E a / (R T) (\ displaystyle k = Ae ^ ((- E_ (\ textrm (a))) / ((RT)))) </Dd>

Minimum amount of energy required to start a reaction