Assertion :If the activation energy of reaction is zero, temperature will have no effect on the rate constant. Reason: Lower the activation energy faster is the reaction.

Both Assertion and Reason are correct and Reason is the correct explanation for Assertion

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Both Assertion and Reason are correct but Reason is not the correct explanation for Assertion

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Assertion is correct but Reason is incorrect

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Assertion is incorrect but Reason is correct

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Solution

The correct option is B Both Assertion and Reason are correct but Reason is not the correct explanation for Assertion
The Arrhenius expression is $k = A e^{- E a / R T} .$

When the activation energy is zero, the term $e^{- E a / R T}$ 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.

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Similar questions

Assertion (A) The enthalpy of reaction remains constant in the presence of a catalyst.

Reason (R) A catalyst participating in the reaction forms different activated complex and lowers down the activation energy but the difference in enrgy of reactant and product remains the same.

(a) Both assertion and reason are correct and the reason is correct explanation of assertion
(b) Both assertion and reason are correct, but reason does not explain assertion.
(c) Assertion is correct, but reason is incorrect
(d) Both assertion and reason are incorrect
(e) Assertion is incorrect but reason is correct.

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