(A) According to Le Chatelier's principle,a change in volume affects the equilibrium position only if there is a change in the total number of moles o

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$N_{2(g)} + O_{2(g)} \rightleftharpoons 2NO_{(g)}$

(A) According to Le Chatelier's principle,a change in volume affects the equilibrium position only if there is a change in the total number of moles of gaseous species,i.e.,$\Delta n_g \neq 0$.For option $A$: $\Delta n_g = (2) - (1 + 1) = 0$.Since $\Delta n_g = 0$,a change in volume will not shift the equilibrium,and the number of moles of components will remain unchanged.For options $B$,$C$,and $D$,$\Delta n_g \neq 0$,so a change in volume will affect the equilibrium.

Class 11 Chemistry 6-1.Equilibrium (Chemical Equilibrium)Le-Chaterlier principle and It’s application

Easy

For which of the following reactions will a change in the volume of the system $NOT$ result in a change in the number of moles of the components?

A
$N_{2(g)} + O_{2(g)} \rightleftharpoons 2NO_{(g)}$
B
$PCl_{5(g)} \rightleftharpoons PCl_{3(g)} + Cl_{2(g)}$
C
$N_{2(g)} + 3H_{2(g)} \rightleftharpoons 2NH_{3(g)}$
D
$SO_2Cl_{2(g)} \rightleftharpoons SO_{2(g)} + Cl_{2(g)}$

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6-1.Equilibrium (Chemical Equilibrium)

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Le-Chaterlier principle and It’s application

Which among the following reactions is favoured in the forward direction by an increase in temperature?

Medium

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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.

MediumAIIMS 2010

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At $25 \ ^oC$,the reaction $SO_2Cl_2(g) \rightleftharpoons SO_2(g) + Cl_2(g)$ is in equilibrium in a closed vessel. If an inert gas,$He$,is added to this system at constant volume,which of the following statements is true?

Easy

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In the equilibrium $2A_{(g)} + 3B_{(g)} \rightleftharpoons 3C_{(g)} + 2D_{(g)}$,an increase in pressure will:

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What will be the effect of pressure on the equilibrium reaction $C_{(s)} + H_2O_{(g)} \rightleftharpoons H_{2_{(g)}} + CO_{(g)}$?

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For which of the following reactions will a change in the volume of the system $NOT$ result in a change in the number of moles of the components?

Similar Questions

Which among the following reactions is favoured in the forward direction by an increase in temperature?

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.

At $25 \ ^oC$,the reaction $SO_2Cl_2(g) \rightleftharpoons SO_2(g) + Cl_2(g)$ is in equilibrium in a closed vessel. If an inert gas,$He$,is added to this system at constant volume,which of the following statements is true?

In the equilibrium $2A_{(g)} + 3B_{(g)} \rightleftharpoons 3C_{(g)} + 2D_{(g)}$,an increase in pressure will:

What will be the effect of pressure on the equilibrium reaction $C_{(s)} + H_2O_{(g)} \rightleftharpoons H_{2_{(g)}} + CO_{(g)}$?

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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.