(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 6-1.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 $\left(R=0.083 \ L \ bar \ K^{-1} \ mol^{-1}\right)$

AP EAMCET 2018 All AP EAMCET

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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6-1.Equilibrium (Chemical Equilibrium)

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Kp and Kc Relationship

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Consider the equilibria $(i)$ and $(ii)$ with equilibrium constants $K_1$ and $K_2$,respectively.
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$K_1$ and $K_2$ are related as

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For the following given equilibrium reaction,$\frac{K_{c}}{K_{p}}$ is equal to $1076$ at $T \ K$. What is the value of $T$ (in $K$)? $(R = 0.082 \ L \ atm \ K^{-1} \ mol^{-1})$
$N_{2(g)} + 3H_{2(g)} \rightleftharpoons 2NH_{3(g)}$

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For the reaction $H_{2(g)} + I_{2(g)} \rightleftharpoons 2HI_{(g)}$,$0.4 \ mol$ of $H_2$ and $I_2$ each are taken in a $2 \ L$ vessel. If $0.5 \ mol$ of $HI$ is formed at equilibrium,calculate the equilibrium constant $K_c$ and $K_p$.

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$A_{(g)} + 3B_{(g)} \rightleftharpoons 4C_{(g)}$. The starting concentrations of $A$ and $B$ are equal. At equilibrium,the concentrations of $A$ and $C$ are the same. The value of $K_c$ is:

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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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Consider the equilibria $(i)$ and $(ii)$ with equilibrium constants $K_1$ and $K_2$,respectively.$SO_{2(g)} + 1/2 O_{2(g)} \rightleftharpoons SO_{3(g)} ..... (i)$$2 SO_{3(g)} \rightleftharpoons 2 SO_{2(g)} + O_{2(g)} ..... (ii)$$K_1$ and $K_2$ are related as

For the following given equilibrium reaction,$\frac{K_{c}}{K_{p}}$ is equal to $1076$ at $T \ K$. What is the value of $T$ (in $K$)? $(R = 0.082 \ L \ atm \ K^{-1} \ mol^{-1})$$N_{2(g)} + 3H_{2(g)} \rightleftharpoons 2NH_{3(g)}$

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Consider the equilibria $(i)$ and $(ii)$ with equilibrium constants $K_1$ and $K_2$,respectively.
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For the following given equilibrium reaction,$\frac{K_{c}}{K_{p}}$ is equal to $1076$ at $T \ K$. What is the value of $T$ (in $K$)? $(R = 0.082 \ L \ atm \ K^{-1} \ mol^{-1})$
$N_{2(g)} + 3H_{2(g)} \rightleftharpoons 2NH_{3(g)}$