(A) catalyst provides an alternate reaction pathway with a lower activation energy $(E_a)$.It speeds up both the forward and backward reactions to the

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(A) catalyst provides an alternate reaction pathway with a lower activation energy $(E_a)$.It speeds up both the forward and backward reactions to the same extent.Since the rate of both reactions increases equally,the equilibrium position remains unchanged,and the equilibrium constant $(K_{eq})$ is not altered.

Class 11 Chemistry 1 Equilibrium: Chemical Equilibrium Le-Chaterlier principle and It’s application

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Assertion : $A$ catalyst does not alter the equilibrium constant of a reaction.
Reason : The catalyst forms a complex with the reactants and provides an alternate path with lower energy of activation for the reaction; the forward and the backward reactions are affected to the same extent.

AIIMS 2010 All AIIMS

A
If both Assertion and Reason are correct and the Reason is a correct explanation of the Assertion.
B
If both Assertion and Reason are correct but Reason is not a correct explanation of the Assertion.
C
If the Assertion is correct but Reason is incorrect.
D
If both the Assertion and Reason are incorrect.

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1 Equilibrium: Chemical Equilibrium

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Le-Chaterlier principle and It’s application

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Assertion : $A$ catalyst does not alter the equilibrium constant of a reaction.Reason : The catalyst forms a complex with the reactants and provides an alternate path with lower energy of activation for the reaction; the forward and the backward reactions are affected to the same extent.

Similar Questions

For the equilibrium $2NO_{2(g)} \rightleftharpoons N_2O_{4(g)} + 21.9 \ kcal$,an increase in temperature will:

For the reaction $PCl_{3(g)} + Cl_{2(g)} \rightleftharpoons PCl_{5(g)}$,the position of equilibrium can be shifted to the right by

In which reaction will an increase in the volume of the container favour the formation of products?

Two systems $PCl_{5(g)} \rightleftharpoons PCl_{3(g)} + Cl_{2(g)}$ and $COCl_{2(g)} \rightleftharpoons CO_{(g)} + Cl_{2(g)}$ are in equilibrium simultaneously in a container of constant volume. If some $CO_{(g)}$ is added to the container at constant volume,then at the new equilibrium:

The reaction $CaCO_3 \rightleftharpoons CaO + CO_2$ goes to completion in a lime kiln because:

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Assertion : $A$ catalyst does not alter the equilibrium constant of a reaction.
Reason : The catalyst forms a complex with the reactants and provides an alternate path with lower energy of activation for the reaction; the forward and the backward reactions are affected to the same extent.