(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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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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At $380 \ K$,$NH_4HS$ decomposes and the total pressure is $1.12 \ bar$. Find $K_p$ for the reaction: $NH_4HS_{(s)} \rightleftharpoons NH_{3(g)} + H_2S_{(g)}$ (in $bar^2$)

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The value of $K_P / K_C$ for the reaction at $T(K)$ is:
$CO_{(g)} + \frac{1}{2} O_{2(g)} \rightleftharpoons CO_{2(g)}$