(A) : If the activation energy of a reaction is zero, temperature has no effect on the rate constant.
(R) : Lower the activation energy, faster is the reaction.

see full answer

Your Exam Success, Personally Taken Care Of

1:1 expert mentors customize learning to your strength and weaknesses – so you score higher in school , IIT JEE and NEET entrance exams.

An Intiative by Sri Chaitanya

Both (A) and (R) are correct but (R) is not the correct explanation of (A).

(A) is correct but (R) is wrong.

Both (A) and (R) are correct and (R) is the correct explanation of (A).

(A) and (R) both are wrong.

answer is B.

(Unlock A.I Detailed Solution for FREE)

Best Courses for You

JEE

NEET

Foundation JEE

Foundation NEET

CBSE

Detailed Solution

The Arrhenius expression is $k = {Ae}^{- EaRT}$ .
When the activation energy is zero, the term $e^{- EaRT}$ becomes equal to 1 . Hence, the rate constant becomes independent of the temperature.
When the value of the activation energy is low, the value of the rate constant is higher. Hence, the rate of the reaction is also high.

Therefore, the correct option is (B).

Watch 3-min video & get full concept clarity