(D) The equilibrium constant expression is $K_p = P_{CO_2} \times P_{H_2O}$.Since the stoichiometry of $CO_2$ and $H_2O$ is $1:1$,their partial pressu

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(D) The equilibrium constant expression is $K_p = P_{CO_2} \times P_{H_2O}$.Since the stoichiometry of $CO_2$ and $H_2O$ is $1:1$,their partial pressures are equal: $P_{CO_2} = P_{H_2O} = P$.Thus,$K_p = P^2 = 64 \ bar^2$,which gives $P = 8 \ bar$.The mole fraction of $CO_2$ is given by $X_{CO_2} = \frac{P_{CO_2}}{P_{total}} = 0.8$.Substituting the values: $0.8 = \frac{8 \ bar}{P_{total}}$.Therefore,$P_{total} = \frac{8}{0.8} = 10 \ bar$.

Class 11 Chemistry 6-1.Equilibrium (Chemical Equilibrium)Mix Examples- 6-1.Equilibrium (Chemical Equilibrium)

In a closed vessel,the decomposition of solid $Mg(HCO_3)_2$ is given as follows:
$Mg(HCO_3)_{2(s)} \rightleftharpoons MgCO_{3(s)} + CO_{2(g)} + H_2O_{(g)}$
Given $K_p = 64 \ bar^2$ and the mole fraction of $CO_2$ is $0.8$,calculate the total pressure at equilibrium. (in $bar$)

A
$16$
B
$20$
C
$8$
D
$10$

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6-1.Equilibrium (Chemical Equilibrium)

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Mix Examples- 6-1.Equilibrium (Chemical Equilibrium)

$2$ moles each of $A$ and $B$ were taken in a container and the following reaction takes place: $2 \ A_{(g)} + B_{(g)} \rightleftharpoons 2 \ C_{(g)} + D_{(g)}$. When the system attains equilibrium,which of the following is true?

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At a certain temperature and total pressure of $10^{5} \ Pa$,iodine vapour contains $40 \%$ by volume of $I$ atoms.
$I_{2(g)} \longleftrightarrow 2I_{(g)}$
Calculate $K_{p}$ for the equilibrium.

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The equilibrium constant at $298 \ K$ for a reaction $A + B \rightleftharpoons C + D$ is $100$. If the initial concentration of all the four species were $1 \ M$ each,then the equilibrium concentration of $D$ (in $mol \ L^{-1}$) will be:

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If the volume of the container for the reaction $2NO + O_2 \rightleftharpoons 2NO_2$ is reduced to half of its initial volume,the rate of the reaction will become .......

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For the reaction $PCl_5 \rightleftharpoons PCl_3 + Cl_2$,the forward reaction at constant temperature is favoured by

Medium

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In a closed vessel,the decomposition of solid $Mg(HCO_3)_2$ is given as follows:$Mg(HCO_3)_{2(s)} \rightleftharpoons MgCO_{3(s)} + CO_{2(g)} + H_2O_{(g)}$Given $K_p = 64 \ bar^2$ and the mole fraction of $CO_2$ is $0.8$,calculate the total pressure at equilibrium. (in $bar$)

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$2$ moles each of $A$ and $B$ were taken in a container and the following reaction takes place: $2 \ A_{(g)} + B_{(g)} \rightleftharpoons 2 \ C_{(g)} + D_{(g)}$. When the system attains equilibrium,which of the following is true?

At a certain temperature and total pressure of $10^{5} \ Pa$,iodine vapour contains $40 \%$ by volume of $I$ atoms.$I_{2(g)} \longleftrightarrow 2I_{(g)}$Calculate $K_{p}$ for the equilibrium.

The equilibrium constant at $298 \ K$ for a reaction $A + B \rightleftharpoons C + D$ is $100$. If the initial concentration of all the four species were $1 \ M$ each,then the equilibrium concentration of $D$ (in $mol \ L^{-1}$) will be:

If the volume of the container for the reaction $2NO + O_2 \rightleftharpoons 2NO_2$ is reduced to half of its initial volume,the rate of the reaction will become .......

For the reaction $PCl_5 \rightleftharpoons PCl_3 + Cl_2$,the forward reaction at constant temperature is favoured by

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In a closed vessel,the decomposition of solid $Mg(HCO_3)_2$ is given as follows:
$Mg(HCO_3)_{2(s)} \rightleftharpoons MgCO_{3(s)} + CO_{2(g)} + H_2O_{(g)}$
Given $K_p = 64 \ bar^2$ and the mole fraction of $CO_2$ is $0.8$,calculate the total pressure at equilibrium. (in $bar$)

At a certain temperature and total pressure of $10^{5} \ Pa$,iodine vapour contains $40 \%$ by volume of $I$ atoms.
$I_{2(g)} \longleftrightarrow 2I_{(g)}$
Calculate $K_{p}$ for the equilibrium.