(B) The balanced chemical equation for the formation of $NH_3$ is: $N_2(g) + 3H_2(g) \rightleftharpoons 2NH_3(g)$.For the reverse reaction,the equatio

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(B) The balanced chemical equation for the formation of $NH_3$ is: $N_2(g) + 3H_2(g) \rightleftharpoons 2NH_3(g)$.For the reverse reaction,the equation is: $2NH_3(g) \rightleftharpoons N_2(g) + 3H_2(g)$.The equilibrium constant $K_C$ for the reverse reaction is given by the expression: $K_C = \frac{[N_2][H_2]^3}{[NH_3]^2}$.Substituting the given equilibrium concentrations:$K_C = \frac{(1.5 \times 10^{-2}) \times (3.0 \times 10^{-2})^3}{(1.2 \times 10^{-2})^2}$.$K_C = \frac{(1.5 \times 10^{-2}) \times (27.0 \times 10^{-6})}{1.44 \times 10^{-4}}$.$K_C = \frac{40.5 \times 10^{-8}}{1.44 \times 10^{-4}} = 28.125 \times 10^{-4} = 2.81 \times 10^{-3}$.

Class 11 Chemistry 1 Equilibrium: Chemical Equilibrium Kp and Kc Relationship

Medium

For the formation of $NH_3$ from $N_2$ and $H_2$ at $500 \ K$,the concentrations of $N_2, H_2$ and $NH_3$ at equilibrium are $1.5 \times 10^{-2} \ M, 3.0 \times 10^{-2} \ M$ and $1.2 \times 10^{-2} \ M$,respectively. The equilibrium constant for the reverse reaction is

TS EAMCET 2018 All TS EAMCET

A
$3.56 \times 10^2$
B
$2.81 \times 10^{-3}$
C
$3.56 \times 10^{-2}$
D
$2.81 \times 10^3$

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Class 11

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1 Equilibrium: Chemical Equilibrium

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Kp and Kc Relationship

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$9.2 \ g$ of $N_2O_{4(g)}$ is taken in a $1 \ L$ closed vessel and heated until the following equilibrium is attained:
${N_2}{O_{4(g)}} \rightleftharpoons 2N{O_{2(g)}}$
If $50\%$ of $N_2O_{4(g)}$ dissociates at equilibrium,what will be the equilibrium constant (in $mol \ L^{-1}$)? (Mol. wt. of $N_2O_4 = 92$)

Medium

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For the reaction at $25\,^{\circ}C$,$N_2O_{4(g)} \rightleftharpoons 2NO_{2(g)}$,if $\Delta G^{\circ}_f$ for $N_2O_4$ and $NO_2$ are $23.49 \, kcal$ and $12.39 \, kcal$ respectively,then $K_p$ for the reaction is:

Medium

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If $2 \ mol$ of $H_2$ and $I_2$ are taken initially in a $1 \ L$ vessel,and the equilibrium concentration of $HI$ is $2 \ mol/L$,find the $K_p$ for the reaction $H_{2(g)} + I_{2(g)} \rightleftharpoons 2HI_{(g)}$.

Easy

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$K_p$ for the following reaction is $3.0$ at $1000 \ K$.
$CO_{2(g)} + C_{(s)} \rightleftharpoons 2CO_{(g)}$
What will be the value of $K_c$ for the reaction at the same temperature?
(Given: $R = 0.083 \ L \ bar \ K^{-1} \ mol^{-1}$)

MediumNEET 2022

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Match List-$I$ (Hypothetical reaction) with List-$II$ (Ratio of $K_p/K_c$ for the given reaction) and select the correct answer using the options given below.

$(1)$ $A_{2(g)} + 3B_{2(g)} \rightleftharpoons 2AB_{3(g)}$ $(i)$ $(RT)^{-2}$

$(2)$ $A_{2(g)} + B_{2(g)} \rightleftharpoons 2AB_{(g)}$ $(ii)$ $(RT)^0$

$(3)$ $A_{(s)} + 1.5B_{2(g)} \rightleftharpoons AB_{3(g)}$ $(iii)$ $(RT)^{1/2}$

$(4)$ $AB_{2(g)} \rightleftharpoons AB_{(g)} + 0.5B_{2(g)}$ $(iv)$ $(RT)^{-1/2}$

Medium

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$(1)$ $A_{2(g)} + 3B_{2(g)} \rightleftharpoons 2AB_{3(g)}$	$(i)$ $(RT)^{-2}$
$(2)$ $A_{2(g)} + B_{2(g)} \rightleftharpoons 2AB_{(g)}$	$(ii)$ $(RT)^0$
$(3)$ $A_{(s)} + 1.5B_{2(g)} \rightleftharpoons AB_{3(g)}$	$(iii)$ $(RT)^{1/2}$
$(4)$ $AB_{2(g)} \rightleftharpoons AB_{(g)} + 0.5B_{2(g)}$	$(iv)$ $(RT)^{-1/2}$

For the formation of $NH_3$ from $N_2$ and $H_2$ at $500 \ K$,the concentrations of $N_2, H_2$ and $NH_3$ at equilibrium are $1.5 \times 10^{-2} \ M, 3.0 \times 10^{-2} \ M$ and $1.2 \times 10^{-2} \ M$,respectively. The equilibrium constant for the reverse reaction is

Similar Questions

For the reaction at $25\,^{\circ}C$,$N_2O_{4(g)} \rightleftharpoons 2NO_{2(g)}$,if $\Delta G^{\circ}_f$ for $N_2O_4$ and $NO_2$ are $23.49 \, kcal$ and $12.39 \, kcal$ respectively,then $K_p$ for the reaction is:

If $2 \ mol$ of $H_2$ and $I_2$ are taken initially in a $1 \ L$ vessel,and the equilibrium concentration of $HI$ is $2 \ mol/L$,find the $K_p$ for the reaction $H_{2(g)} + I_{2(g)} \rightleftharpoons 2HI_{(g)}$.

$K_p$ for the following reaction is $3.0$ at $1000 \ K$.$CO_{2(g)} + C_{(s)} \rightleftharpoons 2CO_{(g)}$What will be the value of $K_c$ for the reaction at the same temperature?(Given: $R = 0.083 \ L \ bar \ K^{-1} \ mol^{-1}$)

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$K_p$ for the following reaction is $3.0$ at $1000 \ K$.
$CO_{2(g)} + C_{(s)} \rightleftharpoons 2CO_{(g)}$
What will be the value of $K_c$ for the reaction at the same temperature?
(Given: $R = 0.083 \ L \ bar \ K^{-1} \ mol^{-1}$)