(C) Given: $K_C = 4.0 \times 10^{-6} \ mol \ L^{-1}$,$T = 1000 \ K$,$R = 0.083 \ L \ bar \ K^{-1} \ mol^{-1}$.For the reaction $2 \ NOCl_{(g)} \rightl

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(C) Given: $K_C = 4.0 \times 10^{-6} \ mol \ L^{-1}$,$T = 1000 \ K$,$R = 0.083 \ L \ bar \ K^{-1} \ mol^{-1}$.For the reaction $2 \ NOCl_{(g)} \rightleftharpoons 2 \ NO_{(g)} + Cl_{2(g)}$,the change in moles of gas is $\Delta n = (2 + 1) - 2 = 1$.The relationship between $K_P$ and $K_C$ is given by $K_P = K_C(RT)^{\Delta n}$.Substituting the values: $K_P = 4.0 \times 10^{-6} \times (0.083 \times 1000)^1$.$K_P = 4.0 \times 10^{-6} \times 83 = 3.32 \times 10^{-4}$.

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

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At $1000 \ K$,the equilibrium constant $K_C$ for the reaction $2 \ NOCl_{(g)} \rightleftharpoons 2 \ NO_{(g)} + Cl_{2(g)}$ is $4.0 \times 10^{-6} \ mol \ L^{-1}$. The $K_P$ (in bar) at the same temperature is $\left(R=0.083 \ L \ bar \ K^{-1} \ mol^{-1}\right)$

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A
$3.32 \times 10^{-6}$
B
$3.32 \times 10^4$
C
$3.32 \times 10^{-4}$
D
$3.32 \times 10^{-3}$

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Kp and Kc Relationship

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At $1000 \ K$,the equilibrium constant $K_C$ for the reaction $2 \ NOCl_{(g)} \rightleftharpoons 2 \ NO_{(g)} + Cl_{2(g)}$ is $4.0 \times 10^{-6} \ mol \ L^{-1}$. The $K_P$ (in bar) at the same temperature is $\left(R=0.083 \ L \ bar \ K^{-1} \ mol^{-1}\right)$

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For the reaction $PCl_{3(g)} + Cl_{2(g)} \rightleftharpoons PCl_{5(g)}$,the value of $K_c$ is $26$ at $250 \ ^oC$. The value of $K_p$ at this temperature will be ...........

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$2 SO_{2(g)} + O_{2(g)} \rightleftharpoons 2 SO_{3(g)}$In an equilibrium mixture,the partial pressures are$P_{SO_{3}} = 43 \ kPa$,$P_{O_{2}} = 530 \ Pa = 0.53 \ kPa$,and$P_{SO_{2}} = 45 \ kPa$. The equilibrium constant $K_{p} = ...... \times 10^{-2} \ kPa^{-1}$. (Nearest integer)

For the reaction $N_{2(g)} + O_{2(g)} \rightleftharpoons 2NO_{(g)}$,the value of $K_c$ at $800 \ ^oC$ is $0.1$. When the equilibrium concentrations of both the reactants are $0.5 \ M$,what is the value of $K_p$ at the same temperature?

The equilibrium concentrations of $N_2, H_2$ and $NH_3$ in the formation of $NH_3$ at $500 \ K$ are $1.25 \times 10^{-2} \ M, 4.0 \times 10^{-2} \ M$ and $1.6 \times 10^{-2} \ M$ respectively. The equilibrium constant $K_{p}$ at the same temperature is

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$2 SO_{2(g)} + O_{2(g)} \rightleftharpoons 2 SO_{3(g)}$
In an equilibrium mixture,the partial pressures are
$P_{SO_{3}} = 43 \ kPa$,$P_{O_{2}} = 530 \ Pa = 0.53 \ kPa$,and
$P_{SO_{2}} = 45 \ kPa$. The equilibrium constant $K_{p} = ...... \times 10^{-2} \ kPa^{-1}$. (Nearest integer)