(C) Initial pressure of $H_2$ is calculated using $PV = nRT$: $P_{H_2} = \frac{nRT}{V} = \frac{0.2 \times 0.0821 \times 363}{1} \approx 5.96 \, atm \a

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(C) Initial pressure of $H_2$ is calculated using $PV = nRT$: $P_{H_2} = \frac{nRT}{V} = \frac{0.2 \times 0.0821 \times 363}{1} \approx 5.96 \, atm \approx 6 \, atm$. For the reaction $H_{2(g)} + S_{(s)} \rightleftharpoons H_2S_{(g)}$,the equilibrium constant $K_p$ is given by: $K_p = \frac{P_{H_2S}}{P_{H_2}} = 6.8 \times 10^{-2}$. Let $x$ be the partial pressure of $H_2S$ at equilibrium. Then $P_{H_2} = (6 - x)$. $\frac{x}{6 - x} = 0.068$. $x = 0.068(6 - x) = 0.408 - 0.068x$. $1.068x = 0.408$. $x = \frac{0.408}{1.068} \approx 0.38 \, atm$.

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

Medium

In a $1.0 \, L$ vessel at $90 \, ^\circ C$,$0.2 \, mol$ of $H_{2(g)}$ and $2.0 \, mol$ of $S_{(s)}$ are mixed. For the reaction $H_{2(g)} + S_{(s)} \rightleftharpoons H_2S_{(g)}$; $K_p = 6.8 \times 10^{-2}$,the partial pressure of $H_2S_{(g)}$ at equilibrium will be ............ $atm$.

A
$6.8 \times 10^{-2}$
B
$0.19$
C
$0.38$
D
$0.6$

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

$A$ solid $XY$ kept in an evacuated sealed container undergoes decomposition to form a mixture of gases $X$ and $Y$ at temperature $T$. The equilibrium pressure is $10 \, bar$ in the vessel. $K_p$ for this reaction is

MediumJEE MAIN 2016

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The partial pressures of an equilibrium mixture of $H_2$,$N_2$,and $NH_3$ are $2 \, atm$,$1 \, atm$,and $3 \, atm$ respectively. If the value of $K_P$ for the reaction $N_2 + 3H_2 \rightleftharpoons 2NH_3$ at $725 \, K$ is $4.28 \times 10^{-5} \, atm^{-2}$,in which direction will the reaction proceed?

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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Consider the following chemical equilibrium of the gas phase reaction at a constant temperature: $A_{(g)} \rightleftharpoons B_{(g)} + C_{(g)}$. If $p$ is the total pressure,$K_p$ is the equilibrium constant,and $\alpha$ is the degree of dissociation,then which of the following is true at equilibrium?

MediumJEE MAIN 2025

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When $2 \ L$ of $CO_2$ is heated with graphite,the volume of gases collected is $3 \ L$. Calculate the number of moles of $CO$ produced at $STP$.

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In a $1.0 \, L$ vessel at $90 \, ^\circ C$,$0.2 \, mol$ of $H_{2(g)}$ and $2.0 \, mol$ of $S_{(s)}$ are mixed. For the reaction $H_{2(g)} + S_{(s)} \rightleftharpoons H_2S_{(g)}$; $K_p = 6.8 \times 10^{-2}$,the partial pressure of $H_2S_{(g)}$ at equilibrium will be ............ $atm$.

Similar Questions

$A$ solid $XY$ kept in an evacuated sealed container undergoes decomposition to form a mixture of gases $X$ and $Y$ at temperature $T$. The equilibrium pressure is $10 \, bar$ in the vessel. $K_p$ for this reaction is

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 $bar$)

When $2 \ L$ of $CO_2$ is heated with graphite,the volume of gases collected is $3 \ L$. Calculate the number of moles of $CO$ produced at $STP$.

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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 $bar$)