(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 in equilibrium $N_2O_{4(g)} \rightleftharpoons 2NO_{2(g)}$,the equilibrium concentrations of $N_2O_4$ and $NO_2$ are $4.8 \times 10^{-2} \ mol/L$ and $1.2 \times 10^{-2} \ mol/L$,then $K_C$ is

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For the reaction $2NO_{2(g)} \rightleftharpoons 2NO_{(g)} + O_{2(g)}$,the equilibrium constant $K_c = 1.8 \times 10^{-6}$ at $184 \, ^\circ C$. Comparing $K_p$ and $K_c$ at $184 \, ^\circ C$,we find that:

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For the reaction $CaCO_{3(s)} \rightleftharpoons CaO_{(s)} + CO_{2(g)}$,the value of $K_p$ at $800 \ ^oC$ is $1.16 \ atm$. If $1 \ mol$ of $CaCO_{3(s)}$ is taken in a $1 \ L$ container to start the reaction,what will be the partial pressure of $CO_2$ at equilibrium in $atm$?

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$A$ schematic plot of $\ln K_{eq}$ versus inverse of temperature $(1/T)$ for a reaction is shown below. The reaction must be

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For which of the following equilibria are $K_P$ and $K_C$ different?

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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 $CH_3OH$?

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For the reaction in equilibrium $N_2O_{4(g)} \rightleftharpoons 2NO_{2(g)}$,the equilibrium concentrations of $N_2O_4$ and $NO_2$ are $4.8 \times 10^{-2} \ mol/L$ and $1.2 \times 10^{-2} \ mol/L$,then $K_C$ is

For the reaction $2NO_{2(g)} \rightleftharpoons 2NO_{(g)} + O_{2(g)}$,the equilibrium constant $K_c = 1.8 \times 10^{-6}$ at $184 \, ^\circ C$. Comparing $K_p$ and $K_c$ at $184 \, ^\circ C$,we find that:

For the reaction $CaCO_{3(s)} \rightleftharpoons CaO_{(s)} + CO_{2(g)}$,the value of $K_p$ at $800 \ ^oC$ is $1.16 \ atm$. If $1 \ mol$ of $CaCO_{3(s)}$ is taken in a $1 \ L$ container to start the reaction,what will be the partial pressure of $CO_2$ at equilibrium in $atm$?

$A$ schematic plot of $\ln K_{eq}$ versus inverse of temperature $(1/T)$ for a reaction is shown below. The reaction must be

For which of the following equilibria are $K_P$ and $K_C$ different?

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