A: - A reaction can have zero activation energy
R: - The minimum extra amount of energy absorbed by reactant molecules so that their energy becomes equal to threshold value, is called activation energy

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Both A and R are true and the R is not the correct explanation of A

Both A and R are true and the R is the correct explanation of A

A is false but R is true

A is true but R is false

answer is D.

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Detailed Solution

If E_a= 0, then according to Arrhenius equation k=Ae^−Ea/RT = Ae⁰ =A . This implies that every collision results into a chemical reaction which cannot be true. So, a reaction cannot have zero activation energy.
The minimum extra amount of energy absorbed by the reactant molecules so that their energy becomes equal to threshold value is called activation energy. In other words, activation energy is the difference between the threshold energy and the average energy of the reactant molecules.

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