# Arrhenius equation - Proper Interpretation of Activation Energy term

Consider the normal form of Arrhenius Equation:$$k=Ae^{-\frac {E_a}{RT}}$$

The term, $$e^{-\frac {E_a}{RT}}$$, is interpreted as the fraction of molecules having energy greater than Activation Energy.

My question: Isn't the term threshold energy better than activation energy?

Please provide a suitable interpretation of the terms involved.

• In principle, the activation energy could have been called threshold energy. But nobody uses this word. It is a question of habit. – Maurice Aug 30 '20 at 16:43
• There is an answer here chemistry.stackexchange.com/questions/139196/… – porphyrin Aug 30 '20 at 16:51
• @Maurice Sir does that mean it is in actual sense Threshold Energy? – Tony Stark Aug 30 '20 at 17:24