(A) For a reversible reaction at equilibrium,the equilibrium constant $K_c$ is defined as the ratio of the rate constant of the forward reaction ($k_f

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(A) For a reversible reaction at equilibrium,the equilibrium constant $K_c$ is defined as the ratio of the rate constant of the forward reaction ($k_f$ or $k_1$) to the rate constant of the backward reaction ($k_b$ or $k_2$).Given:$k_f = 2.1 \times 10^{-3} \ s^{-1}$$k_b = 4.2 \times 10^{-4} \ s^{-1}$Using the formula:$K_c = \frac{k_f}{k_b}$Substituting the values:$K_c = \frac{2.1 \times 10^{-3}}{4.2 \times 10^{-4}}$$K_c = \frac{21 \times 10^{-4}}{4.2 \times 10^{-4}}$$K_c = \frac{21}{4.2} = 5.0$

Class 11 Chemistry 1 Equilibrium: Chemical Equilibrium Kp and Kc Relationship

Medium

For the reversible reaction in equilibrium
$N_{2(g)} + O_{2(g)} \underset{k_2}{\overset{k_1}{\longleftrightarrow}} 2NO_{(g)}$
If the rate constant for the forward reaction is $k_1 = 2.1 \times 10^{-3} \ s^{-1}$ and for the backward reaction is $k_2 = 4.2 \times 10^{-4} \ s^{-1}$,then the equilibrium constant $K_c$ for the above reaction is:

A
$5.0$
B
$2.0$
C
$0.5$
D
$2.5$

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Class 11

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1 Equilibrium: Chemical Equilibrium

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Kp and Kc Relationship

For the equilibrium $N_2O_{4(g)} \rightleftharpoons 2NO_{2(g)}$,$K_p$ is equal to $K_c$ when $T = ....... \ K$.

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The reaction for which $K_{c} = 2.3 \times 10^3 \ mol \ L^{-1}$ is $-$

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For the reaction $N_2O_{4(g)} \rightleftharpoons 2NO_{2(g)}$,the value of $\frac{K_c}{K_p}$ is:

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For the reaction $NH_4HS_{(s)} \rightleftharpoons NH_{3(g)} + H_2S_{(g)}$,if the total pressure in the reaction vessel at $105 \ ^\circ C$ is $1.12 \ atm$,then the $K_p$ for this equilibrium will be .........

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The equilibrium constant for the reaction $N_{2(g)} + O_{2(g)} \rightleftharpoons 2NO_{(g)}$ at temperature $T$ is $4 \times 10^{-4}$. The value of $K_c$ for the reaction $NO_{(g)} \rightleftharpoons \frac{1}{2}N_{2(g)} + \frac{1}{2}O_{2(g)}$ at the same temperature is

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For the equilibrium $N_2O_{4(g)} \rightleftharpoons 2NO_{2(g)}$,$K_p$ is equal to $K_c$ when $T = ....... \ K$.

The reaction for which $K_{c} = 2.3 \times 10^3 \ mol \ L^{-1}$ is $-$

For the reaction $N_2O_{4(g)} \rightleftharpoons 2NO_{2(g)}$,the value of $\frac{K_c}{K_p}$ is:

For the reaction $NH_4HS_{(s)} \rightleftharpoons NH_{3(g)} + H_2S_{(g)}$,if the total pressure in the reaction vessel at $105 \ ^\circ C$ is $1.12 \ atm$,then the $K_p$ for this equilibrium will be .........

The equilibrium constant for the reaction $N_{2(g)} + O_{2(g)} \rightleftharpoons 2NO_{(g)}$ at temperature $T$ is $4 \times 10^{-4}$. The value of $K_c$ for the reaction $NO_{(g)} \rightleftharpoons \frac{1}{2}N_{2(g)} + \frac{1}{2}O_{2(g)}$ at the same temperature is

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