(B) The reaction is $N_2(g) + 3H_2(g) \rightleftharpoons 2NH_3(g).$ The reaction quotient $Q_P$ is given by the expression: $Q_P = \frac{(P_{NH_3})^2}

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(B) The reaction is $N_2(g) + 3H_2(g) \rightleftharpoons 2NH_3(g).$ The reaction quotient $Q_P$ is given by the expression: $Q_P = \frac{(P_{NH_3})^2}{(P_{N_2})(P_{H_2})^3}.$ Substituting the given partial pressures: $Q_P = \frac{(3)^2}{(1)(2)^3} = \frac{9}{8} = 1.125 \ atm^{-2}.$ Comparing $Q_P$ with $K_P$: $Q_P = 1.125$ and $K_P = 4.28 \times 10^{-5}.$ Since $Q_P > K_P,$ the reaction will proceed in the backward direction to reach equilibrium.

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

Medium

$A$ reaction mixture containing $H_2, N_2$ and $NH_3$ has partial pressures of $2 \ atm, 1 \ atm$ and $3 \ atm$ respectively at $725 \ K.$ If the value of $K_P$ for the reaction,$N_2(g) + 3H_2(g) \rightleftharpoons 2NH_3(g)$ is $4.28 \times 10^{-5} \ atm^{-2}$ at $725 \ K,$ in which direction will the net reaction proceed?

A
Forward
B
Backward
C
No net reaction
D
Direction of reaction cannot be predicted

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6-1.Equilibrium (Chemical Equilibrium)

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

$8 \ mol$ of $AB_{3(g)}$ are introduced into a $1.0 \ dm^3$ vessel. If it dissociates as $2AB_{3(g)} \rightleftharpoons A_{2(g)} + 3B_{2(g)}$. At equilibrium,$2 \ mol$ of $A_2$ are found to be present. The equilibrium constant of this reaction is

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$13.8 \,g$ of $N_{2}O_{4}$ was placed in a $1 \,L$ reaction vessel at $400 \,K$ and allowed to attain equilibrium.
$N_{2}O_{4(g)} \rightleftharpoons 2NO_{2(g)}$
The total pressure at equilibrium was found to be $9.15 \,bar$. Calculate $K_{c}$,$K_{p}$,and the partial pressures at equilibrium.

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Equivalent amounts of $H_2$ and $I_2$ are heated in a closed vessel till equilibrium is obtained. If $80\%$ of the hydrogen is converted to $HI$,the $K_c$ at this temperature is

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Consider the following gas phase reaction being carried out in a closed vessel at $25^\circ\text{C}$: $2A(g) \rightarrow 4B(g) + C(g)$. The table provides the total pressure of the system at different time intervals. Calculate the pressure of $C(g)$ at $30$ minutes time interval.
Time (min) Total pressure (mm Hg)
$30$ $300$
$\infty$ $600$

DifficultJEE MAIN 2026

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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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$8 \ mol$ of $AB_{3(g)}$ are introduced into a $1.0 \ dm^3$ vessel. If it dissociates as $2AB_{3(g)} \rightleftharpoons A_{2(g)} + 3B_{2(g)}$. At equilibrium,$2 \ mol$ of $A_2$ are found to be present. The equilibrium constant of this reaction is

$13.8 \,g$ of $N_{2}O_{4}$ was placed in a $1 \,L$ reaction vessel at $400 \,K$ and allowed to attain equilibrium.$N_{2}O_{4(g)} \rightleftharpoons 2NO_{2(g)}$The total pressure at equilibrium was found to be $9.15 \,bar$. Calculate $K_{c}$,$K_{p}$,and the partial pressures at equilibrium.

Equivalent amounts of $H_2$ and $I_2$ are heated in a closed vessel till equilibrium is obtained. If $80\%$ of the hydrogen is converted to $HI$,the $K_c$ at this temperature is

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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$13.8 \,g$ of $N_{2}O_{4}$ was placed in a $1 \,L$ reaction vessel at $400 \,K$ and allowed to attain equilibrium.
$N_{2}O_{4(g)} \rightleftharpoons 2NO_{2(g)}$
The total pressure at equilibrium was found to be $9.15 \,bar$. Calculate $K_{c}$,$K_{p}$,and the partial pressures at equilibrium.