(B) For the reaction,$CO_{2(g)} + C_{(s)} \rightleftharpoons 2 CO_{(g)}$$K_p = \frac{(p_{CO})^2}{p_{CO_2}} = \frac{(0.6)^2}{0.15} = \frac{0.36}{0.15}

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(B) For the reaction,$CO_{2(g)} + C_{(s)} \rightleftharpoons 2 CO_{(g)}$$K_p = \frac{(p_{CO})^2}{p_{CO_2}} = \frac{(0.6)^2}{0.15} = \frac{0.36}{0.15} = 2.4$Using the relation $K_p = K_c(RT)^{\Delta n}$,where $\Delta n = 2 - 1 = 1$ and $R = 0.08314 \ L \ bar \ K^{-1} \ mol^{-1}$.$K_c = \frac{K_p}{RT} = \frac{2.4}{0.08314 \times 1000} = \frac{2.4}{83.14} \approx 0.02887 \approx 2.89 \times 10^{-2}$.Thus,the correct option is $(B)$.

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

Difficult

At $1000 \ K$,the partial pressures of $CO_{2(g)}$ and $CO_{(g)}$ for the reaction $CO_{2(g)} + C_{(s)} \rightleftharpoons 2 CO_{(g)}$ in a closed vessel at equilibrium are $0.15 \ bar$ and $0.60 \ bar$ respectively. The $K_c$ for this reaction at the same temperature is approximately

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A
$2.0 \times 10^{-4}$
B
$2.89 \times 10^{-2}$
C
$2.89 \times 10^{-3}$
D
$5.78 \times 10^{-3}$

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6-1.Equilibrium (Chemical Equilibrium)

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Kp and Kc Relationship

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$CoO_{2(g)} + H_{2(g)} \rightleftharpoons CoO_{(s)} + H_2O_{(g)} \,;\, K_1 = 67$
$CoO_{2(g)} + CO_{(g)} \rightleftharpoons CoO_{(s)} + CO_{2(g)} \,;\, K_2 = 490$
Then the equilibrium constant for the following reaction is ....
$CO_{2(g)} + H_{2(g)} \rightleftharpoons CO_{(g)} + H_2O_{(g)}$

Medium

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For the reaction $N_2O_{4_{(g)}} \rightleftharpoons 2NO_{2_{(g)}}$ at $298 \ K$,the equilibrium constant $K_p$ is $0.14 \ atm$. Calculate the value of $K_c$. $(R = 0.082 \ L \ atm \ K^{-1} \ mol^{-1})$

Medium

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Which among the following denotes the correct relationship between $K_{p}$ and $K_{c}$ for the reaction $2A_{(g)} \rightleftharpoons B_{(g)} + C_{(g)}$?

MediumAP EAMCET 2021

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For the reaction $N_{2(g)} + O_{2(g)} \rightleftharpoons 2NO_{(g)}$,the value of $K_c$ at $800 \ ^oC$ is $0.1$. When the equilibrium concentrations of both the reactants are $0.5 \ M$,what is the value of $K_p$ at the same temperature?

Medium

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The plot of $log_{10} K$ vs $\frac{1}{T}$ gives a straight line. The intercept and slope respectively are (where $K$ is equilibrium constant).

DifficultJEE MAIN 2026

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At $1000 \ K$,the partial pressures of $CO_{2(g)}$ and $CO_{(g)}$ for the reaction $CO_{2(g)} + C_{(s)} \rightleftharpoons 2 CO_{(g)}$ in a closed vessel at equilibrium are $0.15 \ bar$ and $0.60 \ bar$ respectively. The $K_c$ for this reaction at the same temperature is approximately

Similar Questions

$CoO_{2(g)} + H_{2(g)} \rightleftharpoons CoO_{(s)} + H_2O_{(g)} \,;\, K_1 = 67$$CoO_{2(g)} + CO_{(g)} \rightleftharpoons CoO_{(s)} + CO_{2(g)} \,;\, K_2 = 490$Then the equilibrium constant for the following reaction is ....$CO_{2(g)} + H_{2(g)} \rightleftharpoons CO_{(g)} + H_2O_{(g)}$

For the reaction $N_2O_{4_{(g)}} \rightleftharpoons 2NO_{2_{(g)}}$ at $298 \ K$,the equilibrium constant $K_p$ is $0.14 \ atm$. Calculate the value of $K_c$. $(R = 0.082 \ L \ atm \ K^{-1} \ mol^{-1})$

Which among the following denotes the correct relationship between $K_{p}$ and $K_{c}$ for the reaction $2A_{(g)} \rightleftharpoons B_{(g)} + C_{(g)}$?

For the reaction $N_{2(g)} + O_{2(g)} \rightleftharpoons 2NO_{(g)}$,the value of $K_c$ at $800 \ ^oC$ is $0.1$. When the equilibrium concentrations of both the reactants are $0.5 \ M$,what is the value of $K_p$ at the same temperature?

The plot of $log_{10} K$ vs $\frac{1}{T}$ gives a straight line. The intercept and slope respectively are (where $K$ is equilibrium constant).

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$CoO_{2(g)} + H_{2(g)} \rightleftharpoons CoO_{(s)} + H_2O_{(g)} \,;\, K_1 = 67$
$CoO_{2(g)} + CO_{(g)} \rightleftharpoons CoO_{(s)} + CO_{2(g)} \,;\, K_2 = 490$
Then the equilibrium constant for the following reaction is ....
$CO_{2(g)} + H_{2(g)} \rightleftharpoons CO_{(g)} + H_2O_{(g)}$