(B) For the reaction $N_{2(g)} + O_{2(g)} \rightleftharpoons 2NO_{(g)}$,the equilibrium constant is $K_c = \frac{[NO]^2}{[N_2][O_2]} = 4 \times 10^{-4

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(B) For the reaction $N_{2(g)} + O_{2(g)} \rightleftharpoons 2NO_{(g)}$,the equilibrium constant is $K_c = \frac{[NO]^2}{[N_2][O_2]} = 4 \times 10^{-4}$.For the reaction $NO_{(g)} \rightleftharpoons \frac{1}{2}N_{2(g)} + \frac{1}{2}O_{2(g)}$,the equilibrium constant $K'_c$ is given by $K'_c = \frac{[N_2]^{1/2}[O_2]^{1/2}}{[NO]}$.Comparing the two expressions,we see that $K'_c = \frac{1}{\sqrt{K_c}}$.Substituting the value of $K_c$,we get $K'_c = \frac{1}{\sqrt{4 \times 10^{-4}}} = \frac{1}{2 \times 10^{-2}} = \frac{100}{2} = 50$.

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

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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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A
$4 \times 10^{-4}$
B
$50$
C
$2.5 \times 10^{2}$
D
$0.02$

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6-1.Equilibrium (Chemical Equilibrium)

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Kp and Kc Relationship

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What is the unit of $K_p$ for the reaction?
$CS_{2(g)} + 4H_{2(g)} \to CH_{4(g)} + 2H_2S_{(g)}$

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$1 \ mole$ of $HI$ is heated in a closed container of capacity $2 \ L$. At equilibrium,half a mole of $HI$ is dissociated. The equilibrium constant of the reaction is

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For the reaction $2NOCl_{(g)} \rightleftharpoons 2NO_{(g)} + Cl_{2(g)}$,the value of equilibrium constant $K_p$ is $0.033 \ bar$ at $1060 \ K$. Calculate the value of $K_c$.

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Find out the value of $K_{c}$ for each of the following equilibria from the value of $K_{p}$:
$(i)$ $2 NOCl_{(g)} \longleftrightarrow 2 NO_{(g)} + Cl_{2(g)}$; $K_{p} = 1.8 \times 10^{-2}$ at $500 \ K$
$(ii)$ $CaCO_{3(s)} \longleftrightarrow CaO_{(s)} + CO_{2(g)}$; $K_{p} = 167$ at $1073 \ K$

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Given the equilibria:
$I: A + 2B \rightleftharpoons C ; K_{eq} = K_1$
$II: C + D \rightleftharpoons 3A ; K_{eq} = K_2$
$III: 6B + D \rightleftharpoons 2C ; K_{eq} = K_3$
Which of the following relations is correct?

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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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What is the unit of $K_p$ for the reaction?$CS_{2(g)} + 4H_{2(g)} \to CH_{4(g)} + 2H_2S_{(g)}$

$1 \ mole$ of $HI$ is heated in a closed container of capacity $2 \ L$. At equilibrium,half a mole of $HI$ is dissociated. The equilibrium constant of the reaction is

For the reaction $2NOCl_{(g)} \rightleftharpoons 2NO_{(g)} + Cl_{2(g)}$,the value of equilibrium constant $K_p$ is $0.033 \ bar$ at $1060 \ K$. Calculate the value of $K_c$.

Find out the value of $K_{c}$ for each of the following equilibria from the value of $K_{p}$:$(i)$ $2 NOCl_{(g)} \longleftrightarrow 2 NO_{(g)} + Cl_{2(g)}$; $K_{p} = 1.8 \times 10^{-2}$ at $500 \ K$$(ii)$ $CaCO_{3(s)} \longleftrightarrow CaO_{(s)} + CO_{2(g)}$; $K_{p} = 167$ at $1073 \ K$

Given the equilibria:$I: A + 2B \rightleftharpoons C ; K_{eq} = K_1$$II: C + D \rightleftharpoons 3A ; K_{eq} = K_2$$III: 6B + D \rightleftharpoons 2C ; K_{eq} = K_3$Which of the following relations is correct?

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What is the unit of $K_p$ for the reaction?
$CS_{2(g)} + 4H_{2(g)} \to CH_{4(g)} + 2H_2S_{(g)}$

Find out the value of $K_{c}$ for each of the following equilibria from the value of $K_{p}$:
$(i)$ $2 NOCl_{(g)} \longleftrightarrow 2 NO_{(g)} + Cl_{2(g)}$; $K_{p} = 1.8 \times 10^{-2}$ at $500 \ K$
$(ii)$ $CaCO_{3(s)} \longleftrightarrow CaO_{(s)} + CO_{2(g)}$; $K_{p} = 167$ at $1073 \ K$

Given the equilibria:
$I: A + 2B \rightleftharpoons C ; K_{eq} = K_1$
$II: C + D \rightleftharpoons 3A ; K_{eq} = K_2$
$III: 6B + D \rightleftharpoons 2C ; K_{eq} = K_3$
Which of the following relations is correct?