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Why a reaction does not have a zero acti...

Why a reaction does not have a zero activation energy?

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According to Arrhenius equation,
`k= Ae^(- E_(a) // RT)`
If `E_(a) = 0, k = A`, i.e., rate constant equals to collision frequency which suggests that every collision results into a chemical reaction that cannot be true. Hence, `E_(a) ne 0`.
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