Assertion :If the activation energy of a 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 are correct

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Solution

The correct option is C Assertion is correct but Reason is incorrect
According to the Arrhenius equation, $k = A e^{- E_{a} / R T}$
When $E_{a} = 0, k = A$
The temperature will have no effect on the rate constant when activation energy is zero.
Lower the activation energy, faster the reaction rate.
If the activation energy is less, the molecules will reach the transition stage early as they have to absorb less energy.

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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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