(C) The equilibrium reaction is $2HX_{(g)} \rightleftharpoons H_{2(g)} + X_{2(g)}$.The expression for the equilibrium constant $K$ is $K = \frac{[H_2]

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(C) The equilibrium reaction is $2HX_{(g)} \rightleftharpoons H_{2(g)} + X_{2(g)}$.The expression for the equilibrium constant $K$ is $K = \frac{[H_2][X_2]}{[HX]^2}$.Given $K = 1 \times 10^{-5}$,$[H_2] = 1.2 \times 10^{-3} \ M$,and $[X_2] = 1.2 \times 10^{-4} \ M$.Substituting the values: $10^{-5} = \frac{(1.2 \times 10^{-3}) \times (1.2 \times 10^{-4})}{[HX]^2}$.$[HX]^2 = \frac{1.44 \times 10^{-7}}{10^{-5}} = 1.44 \times 10^{-2}$.$[HX] = \sqrt{1.44 \times 10^{-2}} = 1.2 \times 10^{-1} \ M$.Converting to the format of the options: $1.2 \times 10^{-1} \ M = 12 \times 10^{-2} \ M$.

Class 11 Chemistry 6-1.Equilibrium (Chemical Equilibrium)Law of equilibrium and Equilibrium constant

Medium

The equilibrium constant for the equilibrium $2HX_{(g)} \rightleftharpoons H_{2(g)} + X_{2(g)}$ is $1 \times 10^{-5}$. What will be the equilibrium concentration of $HX$ if the equilibrium concentrations for $H_2$ and $X_2$ are $1.2 \times 10^{-3} \ M$ and $1.2 \times 10^{-4} \ M$ respectively?

A
$12 \times 10^{-4} \ M$
B
$12 \times 10^{-3} \ M$
C
$12 \times 10^{-2} \ M$
D
$12 \times 10^{-1} \ M$

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When $4 \ mol$ of $A$ is mixed with $4 \ mol$ of $B$,$2 \ mol$ of $C$ is formed at equilibrium. For the reaction $A + B \rightleftharpoons C + D$,the equilibrium constant is:

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Given that the equilibrium constant for the reaction,$2SO_{2(g)} + O_{2(g)} \rightleftharpoons 2SO_{3(g)}$ has a value of $278$ at a particular temperature. What is the value of the equilibrium constant for the following reaction at the same temperature? $SO_{3(g)} \rightleftharpoons SO_{2(g)} + \frac{1}{2} O_{2(g)}$

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For the reaction $CH_3COOH + H_2O \rightleftharpoons H_3O^{+} + CH_3COO^{-}$,the equilibrium constant $K$ is given by:

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The equilibrium constant for the reaction $PCl_{5(g)} \to PCl_{3(g)} + Cl_{2(g)}$ is $16$. If the volume of the container is reduced to one half its original volume,the value of $K_p$ for the reaction at the same temperature will be

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The dissociation of $SO_{3(g)}$ into $SO_{2(g)}$ and $O_{2(g)}$ is carried out in a closed container at a constant temperature $T$. The equilibrium constant for the reaction is $K_P = x \ atm$. The partial pressure variation for the three gases is as shown in the graph. The value of $x$ is

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The equilibrium constant for the equilibrium $2HX_{(g)} \rightleftharpoons H_{2(g)} + X_{2(g)}$ is $1 \times 10^{-5}$. What will be the equilibrium concentration of $HX$ if the equilibrium concentrations for $H_2$ and $X_2$ are $1.2 \times 10^{-3} \ M$ and $1.2 \times 10^{-4} \ M$ respectively?

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When $4 \ mol$ of $A$ is mixed with $4 \ mol$ of $B$,$2 \ mol$ of $C$ is formed at equilibrium. For the reaction $A + B \rightleftharpoons C + D$,the equilibrium constant is:

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The dissociation of $SO_{3(g)}$ into $SO_{2(g)}$ and $O_{2(g)}$ is carried out in a closed container at a constant temperature $T$. The equilibrium constant for the reaction is $K_P = x \ atm$. The partial pressure variation for the three gases is as shown in the graph. The value of $x$ is

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