(D) The given reaction is $CO(g) + 2H_2(g) \rightleftharpoons CH_3OH(g)$.For this reaction,$K_P = \frac{P_{CH_3OH}}{P_{CO} \times (P_{H_2})^2} = \frac

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(D) The given reaction is $CO(g) + 2H_2(g) \rightleftharpoons CH_3OH(g)$.For this reaction,$K_P = \frac{P_{CH_3OH}}{P_{CO} \times (P_{H_2})^2} = \frac{2.0}{1.0 \times (0.1)^2} = \frac{2.0}{0.01} = 200 \, atm^{-2}$.The question asks for the $K_P$ of the decomposition of $CH_3OH$,which is the reverse reaction: $CH_3OH(g) \rightleftharpoons CO(g) + 2H_2(g)$.For the reverse reaction,$K_P' = \frac{1}{K_P} = \frac{1}{200} = 0.005 = 5 \times 10^{-3} \, atm^{2}$.

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

Medium

For the equilibrium reaction $CO + 2H_2 \rightleftharpoons CH_3OH$ at $427 \, ^\circ C$,the partial pressures of $CH_3OH$,$CO$,and $H_2$ are $2.0 \, atm$,$1.0 \, atm$,and $0.1 \, atm$ respectively. What is the value of $K_P$ for the decomposition of $CH_3OH$?

A
$1 \times 10^{2} \, atm^{-2}$
B
$2 \times 10^{2} \, atm^{2}$
C
$50 \, atm^{2}$
D
$5 \times 10^{-3} \, atm^{2}$

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6-1.Equilibrium (Chemical Equilibrium)

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Kp and Kc Relationship

For the reaction $CO_{(g)} + 1/2 O_{2(g)} \rightleftharpoons CO_{2(g)}$,the value of $K_p/K_c$ is .....

Easy

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Consider the following reversible chemical reactions:
$A_{2(g)} + B_{2(g)} \overset {K_1} \leftrightarrows 2AB_{(g)} ......(1)$
$6AB_{(g)} \overset {K_2} \leftrightarrows 3A_{2(g)} + 3B_{2(g)} ......(2)$
The relation between $K_1$ and $K_2$ is:

DifficultJEE MAIN 2019

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At $298 \ K$,the value of $K_c$ for the following reaction is $x \ mol \ L^{-1}$. What is the approximate $K_p$ value for this reaction? $(R=0.082 \ L \ atm \ mol^{-1} \ K^{-1})$ $A_2O_{4(g)} \rightleftharpoons 2AO_{2(g)}$

MediumAP EAMCET 2025

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Value of $K_{p}$ for the equilibrium reaction $N_{2}O_{4(g)} \rightleftharpoons 2NO_{2(g)}$ at $288 \ K$ is $47.9$. The $K_{C}$ for this reaction at same temperature is $......$ (Nearest integer)
$(R=0.083 \ L \ \text{bar} \ K^{-1} \ mol^{-1})$

MediumJEE MAIN 2021

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For the reaction $N_{2(g)} + 3H_{2(g)} \rightleftharpoons 2NH_{3(g)}$,the value of $K_p = 41$ at $400 \ K$. Find out the value of $K_p$ for the following reaction at the same temperature: $2N_{2(g)} + 6H_{2(g)} \rightleftharpoons 4NH_{3(g)}$

Medium

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For the equilibrium reaction $CO + 2H_2 \rightleftharpoons CH_3OH$ at $427 \, ^\circ C$,the partial pressures of $CH_3OH$,$CO$,and $H_2$ are $2.0 \, atm$,$1.0 \, atm$,and $0.1 \, atm$ respectively. What is the value of $K_P$ for the decomposition of $CH_3OH$?

Similar Questions

For the reaction $CO_{(g)} + 1/2 O_{2(g)} \rightleftharpoons CO_{2(g)}$,the value of $K_p/K_c$ is .....

Consider the following reversible chemical reactions:$A_{2(g)} + B_{2(g)} \overset {K_1} \leftrightarrows 2AB_{(g)} ......(1)$$6AB_{(g)} \overset {K_2} \leftrightarrows 3A_{2(g)} + 3B_{2(g)} ......(2)$The relation between $K_1$ and $K_2$ is:

At $298 \ K$,the value of $K_c$ for the following reaction is $x \ mol \ L^{-1}$. What is the approximate $K_p$ value for this reaction? $(R=0.082 \ L \ atm \ mol^{-1} \ K^{-1})$ $A_2O_{4(g)} \rightleftharpoons 2AO_{2(g)}$

Value of $K_{p}$ for the equilibrium reaction $N_{2}O_{4(g)} \rightleftharpoons 2NO_{2(g)}$ at $288 \ K$ is $47.9$. The $K_{C}$ for this reaction at same temperature is $......$ (Nearest integer)$(R=0.083 \ L \ \text{bar} \ K^{-1} \ mol^{-1})$

For the reaction $N_{2(g)} + 3H_{2(g)} \rightleftharpoons 2NH_{3(g)}$,the value of $K_p = 41$ at $400 \ K$. Find out the value of $K_p$ for the following reaction at the same temperature: $2N_{2(g)} + 6H_{2(g)} \rightleftharpoons 4NH_{3(g)}$

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Consider the following reversible chemical reactions:
$A_{2(g)} + B_{2(g)} \overset {K_1} \leftrightarrows 2AB_{(g)} ......(1)$
$6AB_{(g)} \overset {K_2} \leftrightarrows 3A_{2(g)} + 3B_{2(g)} ......(2)$
The relation between $K_1$ and $K_2$ is:

Value of $K_{p}$ for the equilibrium reaction $N_{2}O_{4(g)} \rightleftharpoons 2NO_{2(g)}$ at $288 \ K$ is $47.9$. The $K_{C}$ for this reaction at same temperature is $......$ (Nearest integer)
$(R=0.083 \ L \ \text{bar} \ K^{-1} \ mol^{-1})$