(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 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)

JEE MAIN 2021 All JEE MAIN

A
$25$
B
$30$
C
$35$
D
$40$

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

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Two equilibria,$AB \rightleftharpoons A^{+} + B^{-}$ and $AB + B^{-} \rightleftharpoons AB_2^-$,are simultaneously maintained in a solution with equilibrium constants $K_1$ and $K_2$ respectively. The ratio of $[A^{+}]$ to $[AB_2^-]$ in the solution is

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Match List-$I$ (Equations) with List-$II$ (Type of processes) and select the correct option.
List-$I$ (Equations) List-$II$ (Type of processes)
$A. K_p > Q$ $(i)$ Non-spontaneous
$B. \Delta G^\circ < RT \ln Q$ $(ii)$ Equilibrium
$C. K_p = Q$ $(iii)$ Spontaneous and endothermic
$D. T > \frac{\Delta H}{\Delta S}$ $(iv)$ Spontaneous

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When $1 \ mol$ of $H_2$ and $1 \ mol$ of $N_2$ are enclosed in a $5 \ L$ vessel and the reaction is allowed to attain equilibrium,it is found that at equilibrium there is $x \ mol$ of $H_2$. The number of moles of $NH_3$ would be

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List-$I$ (Equations)	List-$II$ (Type of processes)
$A. K_p > Q$	$(i)$ Non-spontaneous
$B. \Delta G^\circ < RT \ln Q$	$(ii)$ Equilibrium
$C. K_p = Q$	$(iii)$ Spontaneous and endothermic
$D. T > \frac{\Delta H}{\Delta S}$	$(iv)$ Spontaneous

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)

Similar Questions

Two equilibria,$AB \rightleftharpoons A^{+} + B^{-}$ and $AB + B^{-} \rightleftharpoons AB_2^-$,are simultaneously maintained in a solution with equilibrium constants $K_1$ and $K_2$ respectively. The ratio of $[A^{+}]$ to $[AB_2^-]$ in the solution is

$A$ plot of $\ln \ K$ against $\frac{1}{T}$ (abscissa) is expected to be a straight line with an intercept on the ordinate axis equal to:

$0.6 \ mol$ of $NH_3$ in a reaction vessel of $2 \ dm^3$ capacity was brought to equilibrium. The vessel was then found to contain $0.15 \ mol$ of $H_2$ formed by the reaction $2NH_{3(g)} \rightleftharpoons N_{2(g)} + 3H_{2(g)}$. Which of the following statements is true?

When $1 \ mol$ of $H_2$ and $1 \ mol$ of $N_2$ are enclosed in a $5 \ L$ vessel and the reaction is allowed to attain equilibrium,it is found that at equilibrium there is $x \ mol$ of $H_2$. The number of moles of $NH_3$ would be

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