Assertion : If the activation energy of a rea | vedclass

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(B) According to the Arrhenius equation,$k = A e^{-E_a / RT}$.When the activation energy $E_a = 0$,the equation becomes $k = A e^0 = A$.Since $A$ (the

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If both Assertion and Reason are correct but Reason is not a correct explanation of the Assertion.

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(B) According to the Arrhenius equation,$k = A e^{-E_a / RT}$.When the activation energy $E_a = 0$,the equation becomes $k = A e^0 = A$.Since $A$ (the frequency factor) is a constant,the rate constant $k$ becomes independent of temperature,making the Assertion correct.The Reason states that lower activation energy leads to a faster reaction,which is a correct general statement in chemical kinetics.However,the Reason does not explain why the rate constant becomes independent of temperature when $E_a = 0$; it merely describes the effect of $E_a$ on the reaction rate. Thus,the Reason is not the correct explanation for the Assertion.

$Step$	$Rate\ Constant\ /\ Activation\ energy$
$Step\ 1$	$k_1, E_{a_1} = 180\ kJ/mol$
$Step\ 2$	$k_2, E_{a_2} = 80\ kJ/mol$
$Step\ 3$	$k_3, E_{a_3} = 50\ kJ/mol$

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.

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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.