(A) The balanced chemical equation is: $N_{2(g)} + 3H_{2(g)} \rightleftharpoons 2NH_{3(g)}$Initial moles: $N_2 = 2 \ mol$,$H_2 = 6 \ mol$,$NH_3 = 0 \

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(A) The balanced chemical equation is: $N_{2(g)} + 3H_{2(g)} \rightleftharpoons 2NH_{3(g)}$Initial moles: $N_2 = 2 \ mol$,$H_2 = 6 \ mol$,$NH_3 = 0 \ mol$Given that $50\%$ of $N_2$ reacts,the amount of $N_2$ reacted is $2 \times 0.5 = 1 \ mol$. Thus,$x = 1$.At equilibrium:$[N_2] = (2 - 1) = 1 \ mol/L$$[H_2] = (6 - 3 \times 1) = 3 \ mol/L$$[NH_3] = (2 \times 1) = 2 \ mol/L$$K_c = \frac{[NH_3]^2}{[N_2][H_2]^3} = \frac{(2)^2}{(1)(3)^3} = \frac{4}{27}$

Class 11 Chemistry 6-1.Equilibrium (Chemical Equilibrium)Kp and Kc Relationship

Difficult

$2 \ mol$ of $N_2$ is mixed with $6 \ mol$ of $H_2$ in a closed vessel of $1 \ L$ capacity. If $50\%$ of $N_2$ is converted into $NH_3$ at equilibrium,the value of $K_c$ for the reaction $N_{2(g)} + 3H_{2(g)} \rightleftharpoons 2NH_{3(g)}$ is

A
$4/27$
B
$27/4$
C
$1/27$
D
$24$

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6-1.Equilibrium (Chemical Equilibrium)

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Kp and Kc Relationship

For the reaction $2NOCl_{(g)} \rightleftharpoons 2NO_{(g)} + Cl_{2(g)}$,$K_C$ at $427\ ^oC$ is $3 \times 10^{-6}\ mol\ L^{-1}$. The value of $K_P$ is nearly $....... \times 10^{-4}$.

MediumAIIMS 2005

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The value of $\log \ K$ for the reaction $A \rightleftharpoons B$ at $298 \ K$ is (Nearest integer).
Given: $\Delta H^{\circ} = -54.07 \ kJ \ mol^{-1}$
$\Delta S^{\circ} = 10 \ J \ K^{-1} \ mol^{-1}$
(Take $2.303 \times 8.314 \times 298 = 5705$)

MediumJEE MAIN 2023

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At $1000\, K$ and $2\, atm$ pressure,a gaseous mixture of $CO$ and $CO_{2}$ in equilibrium with solid carbon has $84\%$ $CO_{(g)}$ by mass. Calculate $K_{p}$ for the reaction: $C_{(s)} + CO_{2_{(g)}} \rightleftharpoons 2CO_{(g)}$ at this temperature.

Difficult

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$K_{c}$ for the reaction $A_{2(g)} \rightleftharpoons B_{2(g)}$ is $39.0$. In a closed one litre flask,one mole of $A_{2(g)}$ was heated to $T \ K$. What are the concentrations of $A_{2(g)}$ and $B_{2(g)}$ (in $mol \ L^{-1}$) respectively at equilibrium?

EasyAP EAMCET 2024

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For the formation of ammonia gas from its constituent elements,the $K_{P} / K_{C}$ is

MediumTS EAMCET 2022

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$2 \ mol$ of $N_2$ is mixed with $6 \ mol$ of $H_2$ in a closed vessel of $1 \ L$ capacity. If $50\%$ of $N_2$ is converted into $NH_3$ at equilibrium,the value of $K_c$ for the reaction $N_{2(g)} + 3H_{2(g)} \rightleftharpoons 2NH_{3(g)}$ is

Similar Questions

For the reaction $2NOCl_{(g)} \rightleftharpoons 2NO_{(g)} + Cl_{2(g)}$,$K_C$ at $427\ ^oC$ is $3 \times 10^{-6}\ mol\ L^{-1}$. The value of $K_P$ is nearly $....... \times 10^{-4}$.

The value of $\log \ K$ for the reaction $A \rightleftharpoons B$ at $298 \ K$ is (Nearest integer).Given: $\Delta H^{\circ} = -54.07 \ kJ \ mol^{-1}$$\Delta S^{\circ} = 10 \ J \ K^{-1} \ mol^{-1}$(Take $2.303 \times 8.314 \times 298 = 5705$)

At $1000\, K$ and $2\, atm$ pressure,a gaseous mixture of $CO$ and $CO_{2}$ in equilibrium with solid carbon has $84\%$ $CO_{(g)}$ by mass. Calculate $K_{p}$ for the reaction: $C_{(s)} + CO_{2_{(g)}} \rightleftharpoons 2CO_{(g)}$ at this temperature.

$K_{c}$ for the reaction $A_{2(g)} \rightleftharpoons B_{2(g)}$ is $39.0$. In a closed one litre flask,one mole of $A_{2(g)}$ was heated to $T \ K$. What are the concentrations of $A_{2(g)}$ and $B_{2(g)}$ (in $mol \ L^{-1}$) respectively at equilibrium?

For the formation of ammonia gas from its constituent elements,the $K_{P} / K_{C}$ is

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The value of $\log \ K$ for the reaction $A \rightleftharpoons B$ at $298 \ K$ is (Nearest integer).
Given: $\Delta H^{\circ} = -54.07 \ kJ \ mol^{-1}$
$\Delta S^{\circ} = 10 \ J \ K^{-1} \ mol^{-1}$
(Take $2.303 \times 8.314 \times 298 = 5705$)