(D) catalyst increases the rate of both the forward and backward reactions to the same extent. It helps the system reach the state of equilibrium fast

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The forward reaction is favoured by the addition of a catalyst

(D) catalyst increases the rate of both the forward and backward reactions to the same extent. It helps the system reach the state of equilibrium faster but does not shift the position of the equilibrium or favor one direction over the other. Therefore,the statement that the forward reaction is favoured by the addition of a catalyst is incorrect.

Class 11 Chemistry 6-1.Equilibrium (Chemical Equilibrium)Mix Examples- 6-1.Equilibrium (Chemical Equilibrium)

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Which of the following statements regarding a chemical equilibrium is wrong?

A
An equilibrium can be shifted by altering the temperature or pressure
B
An equilibrium is dynamic
C
The same state of equilibrium is reached whether one starts with the reactants or the products
D
The forward reaction is favoured by the addition of a catalyst

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6-1.Equilibrium (Chemical Equilibrium)

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Mix Examples- 6-1.Equilibrium (Chemical Equilibrium)

Assign $A, B, C, D$ from the given type of reaction.
$PbCl_2 \downarrow + H_2SO_4 \rightleftharpoons PbSO_4 \downarrow + 2HCl$

Medium

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$28 \, g$ of $N_2$ and $6 \, g$ of $H_2$ were kept at $400 \, ^oC$ in a $1 \, L$ vessel. The equilibrium mixture contained $27.54 \, g$ of $NH_3$. The approximate value of $K_c$ for the reaction $N_2(g) + 3H_2(g) \rightleftharpoons 2NH_3(g)$ is (in $L^2 \, mol^{-2}$):

DifficultAIPMT 1990

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For which of the following reactions will $K_p < K_c$?

Medium

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For the reaction,$NO_2 + CO \rightleftharpoons NO + CO_2$,one mole of $NO_2$ and $2$ moles of $CO$ were kept in a vessel. Calculate the equilibrium constant $K_p$,if at equilibrium $25 \%$ of the initial amount of $CO$ is consumed.

MediumAP EAMCET 2020

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At a certain temperature,$2HI \rightleftharpoons H_2 + I_2$. If only $50\%$ of $HI$ is dissociated at equilibrium,the equilibrium constant $(K_c)$ is:

Medium

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Which of the following statements regarding a chemical equilibrium is wrong?

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Assign $A, B, C, D$ from the given type of reaction.$PbCl_2 \downarrow + H_2SO_4 \rightleftharpoons PbSO_4 \downarrow + 2HCl$

$28 \, g$ of $N_2$ and $6 \, g$ of $H_2$ were kept at $400 \, ^oC$ in a $1 \, L$ vessel. The equilibrium mixture contained $27.54 \, g$ of $NH_3$. The approximate value of $K_c$ for the reaction $N_2(g) + 3H_2(g) \rightleftharpoons 2NH_3(g)$ is (in $L^2 \, mol^{-2}$):

For which of the following reactions will $K_p < K_c$?

For the reaction,$NO_2 + CO \rightleftharpoons NO + CO_2$,one mole of $NO_2$ and $2$ moles of $CO$ were kept in a vessel. Calculate the equilibrium constant $K_p$,if at equilibrium $25 \%$ of the initial amount of $CO$ is consumed.

At a certain temperature,$2HI \rightleftharpoons H_2 + I_2$. If only $50\%$ of $HI$ is dissociated at equilibrium,the equilibrium constant $(K_c)$ is:

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Assign $A, B, C, D$ from the given type of reaction.
$PbCl_2 \downarrow + H_2SO_4 \rightleftharpoons PbSO_4 \downarrow + 2HCl$