(B) The reaction is $2 A \rightleftharpoons B + C$. The reaction quotient $Q$ is given by the expression: $Q = \frac{[B][C]}{[A]^2}$. Substituting the

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(B) The reaction is $2 A \rightleftharpoons B + C$. The reaction quotient $Q$ is given by the expression: $Q = \frac{[B][C]}{[A]^2}$. Substituting the given concentrations: $Q = \frac{(6 \times 10^{-5}) \times (6 \times 10^{-5})}{(6 \times 10^{-5})^2} = 1$. Since $Q = 1$ and $K_{eq} = 2 \times 10^{-3}$,we observe that $Q > K_{eq}$. When $Q > K_{eq}$,the reaction proceeds in the backward direction to reach equilibrium.

Class 11 Chemistry 6-1.Equilibrium (Chemical Equilibrium)Mix Examples- 6-1.Equilibrium (Chemical Equilibrium)

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For a given reaction,$2 A \rightleftharpoons B + C$,the equilibrium constant is $2 \times 10^{-3}$. If at any given time the composition of the reaction mixture is $[A]=[B]=[C]=6 \times 10^{-5} \ M$; predict in which direction the reaction will proceed and the correct value for reaction quotient.

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A
Forward direction and $1.0$
B
Backward direction and $1.0$
C
Forward direction and $3 \times 10^{-5}$
D
Backward direction and $3 \times 10^{-5}$

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6-1.Equilibrium (Chemical Equilibrium)

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Mix Examples- 6-1.Equilibrium (Chemical Equilibrium)

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For a given reaction,$2 A \rightleftharpoons B + C$,the equilibrium constant is $2 \times 10^{-3}$. If at any given time the composition of the reaction mixture is $[A]=[B]=[C]=6 \times 10^{-5} \ M$; predict in which direction the reaction will proceed and the correct value for reaction quotient.

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For the reaction $PCl_{5(g)} \rightleftharpoons PCl_{3(g)} + Cl_{2(g)}$,at equilibrium,the mole fraction of $PCl_5$ is $0.4$ and the mole fraction of $Cl_2$ is $0.3$. What will be the mole fraction of $PCl_3$?

$5 \ \text{moles}$ of $SO_2$ and $5 \ \text{moles}$ of $O_2$ are allowed to react to form $SO_3$ in a closed vessel. At the equilibrium stage,$60\%$ of $SO_2$ is used up. The total number of moles of $SO_2$,$O_2$,and $SO_3$ in the vessel now is:

For the reaction,$H_{2(g)} + I_{2(g)} \rightleftharpoons 2 HI_{(g)}$,the attainment of equilibrium is predicted correctly by:

At $550 \ K$,the $K_c$ for the following reaction is $10^4 \ mol^{-1} \ L$: $X_{(g)} + Y_{(g)} \rightleftharpoons Z_{(g)}$. At equilibrium,it was observed that $[X] = \frac{1}{2}[Y] = \frac{1}{2}[Z]$. What is the value of $[Z]$ (in $mol \ L^{-1}$) at equilibrium?

For the reaction $A_{(g)} \rightleftharpoons B_{(g)} + C_{(g)}$,$A$ is $33 \%$ dissociated at a total pressure $P$. The correct relation between $P$ and $K_{p}$ is

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