(A) The reaction is $A + B \rightleftharpoons 2C$. Initial concentrations: $[A] = 1 \ M, [B] = 1 \ M, [C] = 1 \ M$. Let the change in concentration be

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(A) The reaction is $A + B \rightleftharpoons 2C$. Initial concentrations: $[A] = 1 \ M, [B] = 1 \ M, [C] = 1 \ M$. Let the change in concentration be $x$. At equilibrium: $[A] = 1 - x, [B] = 1 - x, [C] = 1 + 2x$. $K_c = \frac{[C]^2}{[A][B]} = \frac{(1+2x)^2}{(1-x)(1-x)} = 100$. Taking the square root on both sides: $\frac{1+2x}{1-x} = 10$. $1 + 2x = 10 - 10x$. $12x = 9$,so $x = \frac{9}{12} = 0.75$. Equilibrium concentration of $C = 1 + 2x = 1 + 2(0.75) = 1 + 1.5 = 2.5 \ M$. $2.5 \ M = 25 \times 10^{-1} \ M$. Thus,$X = 25$.

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

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For the reaction $A + B \rightleftharpoons 2C$,the value of equilibrium constant is $100$ at $298 \ K$. If the initial concentration of all the three species is $1 \ M$ each,then the equilibrium concentration of $C$ is $X \times 10^{-1} \ M$. The value of $X$ is $.....$ (Nearest integer)

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$25$
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$30$
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$35$
D
$40$

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For the reaction $A + B \rightleftharpoons 2C$,the value of equilibrium constant is $100$ at $298 \ K$. If the initial concentration of all the three species is $1 \ M$ each,then the equilibrium concentration of $C$ is $X \times 10^{-1} \ M$. The value of $X$ is $.....$ (Nearest integer)

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For the reaction $H_{2(g)} + I_{2(g)} \rightleftharpoons 2HI_{(g)}$,the value of $K_c$ at $440 \ ^oC$ is $50$. If the reaction is initiated in a $1 \ L$ flask with $1 \ mol$ of $H_2$,$2 \ mol$ of $I_2$,and $3 \ mol$ of $HI$,then the equilibrium concentration of $HI$ will be .......... $M$.

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The equilibrium constant for the following reaction is $1.6 \times 10^{5}$ at $1024 \, K$:
$H_{2(g)} + Br_{2(g)} \longleftrightarrow 2HBr_{(g)}$
Find the equilibrium pressure of all gases if $10.0 \, bar$ of $HBr$ is introduced into a sealed container at $1024 \, K$.