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.

  • $\begingroup$ In principle, the activation energy could have been called threshold energy. But nobody uses this word. It is a question of habit. $\endgroup$
    – Maurice
    Commented Aug 30, 2020 at 16:43
  • 1
    $\begingroup$ There is an answer here chemistry.stackexchange.com/questions/139196/… $\endgroup$
    – porphyrin
    Commented Aug 30, 2020 at 16:51
  • $\begingroup$ @Maurice Sir does that mean it is in actual sense Threshold Energy? $\endgroup$
    – Tony Stark
    Commented Aug 30, 2020 at 17:24


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