(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)

$CH_3COCH_{3(g)} \rightleftharpoons C_2H_{6(g)} + CO_{(g)}$. The initial pressure of $CH_3COCH_3$ is $100 \ mm$. When equilibrium is set up,the mole fraction of $CO_{(g)}$ is $\frac{1}{4}$. Hence,the partial pressure of $CO$ is:

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In an equilibrium mixture at $1 \, atm$ pressure and $25 \, ^oC$,the partial pressures of $N_2O_4$ and $NO_2$ are $0.70 \, atm$ and $0.30 \, atm$ respectively. The partial pressure of $N_2O_4$ in the equilibrium mixture at $9 \, atm$ pressure and $25 \, ^oC$ will be ........... $atm$.

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For the reaction $P_{(g)} + 3Q_{(g)} \rightleftharpoons 4R_{(g)}$,the initial concentrations of $P$ and $Q$ are equal. If the equilibrium concentrations of $P$ and $R$ are equal,then the equilibrium constant $K_c$ for the reaction will be .....

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Which of the following equations is incorrect?

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Calculate the partial pressure of carbon monoxide from the following:
$CO_{2(g)} + C_{(s)} \rightleftharpoons 2CO_{(g)}$ ; $K_{p1} = 2$
$CaCO_{3(s)} \rightleftharpoons CaO_{(s)} + CO_{2(g)}$ ; $K_{p2} = 8 \times 10^{-2}$

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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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$CH_3COCH_{3(g)} \rightleftharpoons C_2H_{6(g)} + CO_{(g)}$. The initial pressure of $CH_3COCH_3$ is $100 \ mm$. When equilibrium is set up,the mole fraction of $CO_{(g)}$ is $\frac{1}{4}$. Hence,the partial pressure of $CO$ is:

In an equilibrium mixture at $1 \, atm$ pressure and $25 \, ^oC$,the partial pressures of $N_2O_4$ and $NO_2$ are $0.70 \, atm$ and $0.30 \, atm$ respectively. The partial pressure of $N_2O_4$ in the equilibrium mixture at $9 \, atm$ pressure and $25 \, ^oC$ will be ........... $atm$.

For the reaction $P_{(g)} + 3Q_{(g)} \rightleftharpoons 4R_{(g)}$,the initial concentrations of $P$ and $Q$ are equal. If the equilibrium concentrations of $P$ and $R$ are equal,then the equilibrium constant $K_c$ for the reaction will be .....

Which of the following equations is incorrect?

Calculate the partial pressure of carbon monoxide from the following:$CO_{2(g)} + C_{(s)} \rightleftharpoons 2CO_{(g)}$ ; $K_{p1} = 2$$CaCO_{3(s)} \rightleftharpoons CaO_{(s)} + CO_{2(g)}$ ; $K_{p2} = 8 \times 10^{-2}$

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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 $bar$)

Calculate the partial pressure of carbon monoxide from the following:
$CO_{2(g)} + C_{(s)} \rightleftharpoons 2CO_{(g)}$ ; $K_{p1} = 2$
$CaCO_{3(s)} \rightleftharpoons CaO_{(s)} + CO_{2(g)}$ ; $K_{p2} = 8 \times 10^{-2}$