(A) The value of $\Delta n$ is calculated as $\Delta n = \sum n_p - \sum n_r$,where $n_p$ is the number of moles of gaseous products and $n_r$ is the

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(A) The value of $\Delta n$ is calculated as $\Delta n = \sum n_p - \sum n_r$,where $n_p$ is the number of moles of gaseous products and $n_r$ is the number of moles of gaseous reactants. For reaction $(1): C_2H_{6(g)} \rightleftharpoons C_2H_{4(g)} + H_{2(g)}$,$\Delta n = (1 + 1) - 1 = +1$. For reaction $(2): N_{2(g)} + O_{2(g)} \rightleftharpoons 2NO_{(g)}$,$\Delta n = 2 - (1 + 1) = 0$. For reaction $(3): H_{2(g)} + I_{2(g)} \rightleftharpoons 2HI_{(g)}$,$\Delta n = 2 - (1 + 1) = 0$. Therefore,$\Delta n$ is positive for reaction $(1)$.

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

Medium

For which of the following reactions will the value of $\Delta n = \sum n_p - \sum n_r$ be positive? $(1)$ $C_2H_{6(g)} \rightleftharpoons C_2H_{4(g)} + H_{2(g)}$ $(2)$ $N_{2(g)} + O_{2(g)} \rightleftharpoons 2NO_{(g)}$ $(3)$ $H_{2(g)} + I_{2(g)} \rightleftharpoons 2HI_{(g)}$

A
For $(1)$
B
For $(2)$
C
For $(3)$
D
None of these

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6-1.Equilibrium (Chemical Equilibrium)

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Kp and Kc Relationship

For the reaction, $2 SO_{2(g)} + O_{2(g)} \rightleftharpoons 2 SO_{3(g)}$ at $300 \ K$, the value of $\Delta G^{\circ}$ is $-690.9 R$. The equilibrium constant value for the reaction at that temperature is ($R$ is gas constant).

MediumWBJEE 2015

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Assertion : For reaction $N_{2(g)} + 3H_{2(g)} \rightleftharpoons 2NH_{3(g)}$,the unit of $K_C$ is $L^2 \, mol^{-2}$.
Reason : For the reaction $N_{2(g)} + 3H_{2(g)} \rightleftharpoons 2NH_{3(g)}$,the equilibrium constant $K_C = \frac{[NH_3]^2}{[N_2][H_2]^3}$.

MediumAIIMS 2008

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For the reaction $N_{2(g)} + O_{2(g)} \rightleftharpoons 2NO_{(g)}$,the equilibrium constant at temperature $T$ is $4 \times 10^{-4}$. Find the value of $K_c$ for the reaction $NO_{(g)} \rightleftharpoons \frac{1}{2} N_{2(g)} + \frac{1}{2} O_{2(g)}$.

Medium

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For the equilibrium reaction $CO + 2H_2 \rightleftharpoons CH_3OH$ at $427 \, ^\circ C$,the partial pressures of $CH_3OH$,$CO$,and $H_2$ are $2.0 \, atm$,$1.0 \, atm$,and $0.1 \, atm$ respectively. What is the value of $K_P$ for the decomposition of $CH_3OH$?

Medium

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At $1000 \, K$,for the reaction $A_{(g)} + 2B_{(g)} \rightleftharpoons 3C_{(g)} + D_{(g)}$,the value of $K_p$ is $0.05 \, atm$. What will be the value of $K_c$ in terms of $R$?

Medium

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For which of the following reactions will the value of $\Delta n = \sum n_p - \sum n_r$ be positive? $(1)$ $C_2H_{6(g)} \rightleftharpoons C_2H_{4(g)} + H_{2(g)}$ $(2)$ $N_{2(g)} + O_{2(g)} \rightleftharpoons 2NO_{(g)}$ $(3)$ $H_{2(g)} + I_{2(g)} \rightleftharpoons 2HI_{(g)}$

Similar Questions

For the reaction, $2 SO_{2(g)} + O_{2(g)} \rightleftharpoons 2 SO_{3(g)}$ at $300 \ K$, the value of $\Delta G^{\circ}$ is $-690.9 R$. The equilibrium constant value for the reaction at that temperature is ($R$ is gas constant).

Assertion : For reaction $N_{2(g)} + 3H_{2(g)} \rightleftharpoons 2NH_{3(g)}$,the unit of $K_C$ is $L^2 \, mol^{-2}$.Reason : For the reaction $N_{2(g)} + 3H_{2(g)} \rightleftharpoons 2NH_{3(g)}$,the equilibrium constant $K_C = \frac{[NH_3]^2}{[N_2][H_2]^3}$.

For the reaction $N_{2(g)} + O_{2(g)} \rightleftharpoons 2NO_{(g)}$,the equilibrium constant at temperature $T$ is $4 \times 10^{-4}$. Find the value of $K_c$ for the reaction $NO_{(g)} \rightleftharpoons \frac{1}{2} N_{2(g)} + \frac{1}{2} O_{2(g)}$.

For the equilibrium reaction $CO + 2H_2 \rightleftharpoons CH_3OH$ at $427 \, ^\circ C$,the partial pressures of $CH_3OH$,$CO$,and $H_2$ are $2.0 \, atm$,$1.0 \, atm$,and $0.1 \, atm$ respectively. What is the value of $K_P$ for the decomposition of $CH_3OH$?

At $1000 \, K$,for the reaction $A_{(g)} + 2B_{(g)} \rightleftharpoons 3C_{(g)} + D_{(g)}$,the value of $K_p$ is $0.05 \, atm$. What will be the value of $K_c$ in terms of $R$?

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Assertion : For reaction $N_{2(g)} + 3H_{2(g)} \rightleftharpoons 2NH_{3(g)}$,the unit of $K_C$ is $L^2 \, mol^{-2}$.
Reason : For the reaction $N_{2(g)} + 3H_{2(g)} \rightleftharpoons 2NH_{3(g)}$,the equilibrium constant $K_C = \frac{[NH_3]^2}{[N_2][H_2]^3}$.