(A) The rate constant for the forward reaction is $k_f = 2.1 \times 10^{-3} \ s^{-1}$.The rate constant for the backward reaction is $k_b = 4.2 \times

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(A) The rate constant for the forward reaction is $k_f = 2.1 \times 10^{-3} \ s^{-1}$.The rate constant for the backward reaction is $k_b = 4.2 \times 10^{-4} \ s^{-1}$.The equilibrium constant $K_c$ is defined as the ratio of the forward rate constant to the backward rate constant:$K_c = \frac{k_f}{k_b} = \frac{2.1 \times 10^{-3}}{4.2 \times 10^{-4}} = \frac{21 \times 10^{-4}}{4.2 \times 10^{-4}} = 5.0$.

Class 11 Chemistry 6-1.Equilibrium (Chemical Equilibrium)Kp and Kc Relationship

Difficult

For the reversible reaction in equilibrium:
$N_{2(g)} + O_{2(g)} \underset{k_2}{\overset{k_1}{\longleftrightarrow}} 2NO_{(g)}$
Given $C_0 = C e^{-2.1 \times 10^{-3}t}$ for the forward reaction and $C'_0 = C' e^{-4.2 \times 10^{-4}t}$ for the backward reaction,calculate the equilibrium constant $K_c$ for the above reaction.

A
$5.0$
B
$2.0$
C
$0.5$
D
$0.2$

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6-1.Equilibrium (Chemical Equilibrium)

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Kp and Kc Relationship

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

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Equilibrium constants $K_1$ and $K_2$ for the following equilibria:
$(a)$ $NO_{(g)} + \frac{1}{2}O_{2(g)} \rightleftharpoons NO_{2(g)}$
$(b)$ $2NO_{2(g)} \rightleftharpoons 2NO_{(g)} + O_{2(g)}$
are related as:

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For the reaction $2SO_{2(g)} + O_{2(g)} \rightleftharpoons 2SO_{3(g)}$ at $298 \ K$,the $K_c$ is $7 \times 10^{25}$. Calculate $K_c$ for the reaction $SO_{3(g)} \rightleftharpoons SO_{2(g)} + \frac{1}{2}O_{2(g)}$.

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What is the relationship between $K_{p}$ and $K_{c}$ when $\Delta n = 0$,$\Delta n > 0$,and $\Delta n < 0$?

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If ${K_c}$ is the equilibrium constant for the formation of $NH_3$,the dissociation constant of ammonia under the same temperature will be

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

Equilibrium constants $K_1$ and $K_2$ for the following equilibria: $(a)$ $NO_{(g)} + \frac{1}{2}O_{2(g)} \rightleftharpoons NO_{2(g)}$ $(b)$ $2NO_{2(g)} \rightleftharpoons 2NO_{(g)} + O_{2(g)}$ are related as:

For the reaction $2SO_{2(g)} + O_{2(g)} \rightleftharpoons 2SO_{3(g)}$ at $298 \ K$,the $K_c$ is $7 \times 10^{25}$. Calculate $K_c$ for the reaction $SO_{3(g)} \rightleftharpoons SO_{2(g)} + \frac{1}{2}O_{2(g)}$.

What is the relationship between $K_{p}$ and $K_{c}$ when $\Delta n = 0$,$\Delta n > 0$,and $\Delta n < 0$?

If ${K_c}$ is the equilibrium constant for the formation of $NH_3$,the dissociation constant of ammonia under the same temperature will be

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Equilibrium constants $K_1$ and $K_2$ for the following equilibria:
$(a)$ $NO_{(g)} + \frac{1}{2}O_{2(g)} \rightleftharpoons NO_{2(g)}$
$(b)$ $2NO_{2(g)} \rightleftharpoons 2NO_{(g)} + O_{2(g)}$
are related as: