(D) Let the initial concentration of $A$ be $a$ and $B$ be $1.5a$.Reaction: $A + 2B \rightleftharpoons 2C + D$Initial: $a, 1.5a, 0, 0$At equilibrium:

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(D) Let the initial concentration of $A$ be $a$ and $B$ be $1.5a$.Reaction: $A + 2B \rightleftharpoons 2C + D$Initial: $a, 1.5a, 0, 0$At equilibrium: $(a-x), (1.5a-2x), 2x, x$Given that at equilibrium,$[A] = [B]$,so $a-x = 1.5a-2x$.Solving for $x$: $x = 0.5a$.Equilibrium concentrations: $[A] = a - 0.5a = 0.5a$,$[B] = 1.5a - 2(0.5a) = 0.5a$,$[C] = 2(0.5a) = a$,$[D] = 0.5a$.Equilibrium constant $K_c = \frac{[C]^2 [D]}{[A] [B]^2} = \frac{(a)^2 (0.5a)}{(0.5a) (0.5a)^2} = \frac{a^2 \times 0.5a}{0.5a \times 0.25a^2} = \frac{0.5a^3}{0.125a^3} = 4$.

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

Medium

Consider the following equilibrium reaction in gaseous state at $T(K)$.
$A(g) + 2B(g) \rightleftharpoons 2C(g) + D(g)$
The initial concentration of $B$ is $1.5$ times that of $A$. At equilibrium,the concentrations of $A$ and $B$ are equal. The equilibrium constant for the reaction is

AP EAMCET 2025 All AP EAMCET

A
$6$
B
$16$
C
$12$
D
$4$

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6-1.Equilibrium (Chemical Equilibrium)

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Law of equilibrium and Equilibrium constant

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The equilibrium constant,$K_c$ for $3 C_2H_{2(g)} \rightleftharpoons C_6H_{6(g)}$ is $4 \, L^2 \, mol^{-2}$. If the equilibrium concentration of benzene is $0.5 \, mol \, L^{-1}$,the equilibrium concentration of acetylene in $mol \, L^{-1}$ is:

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At $T(K)$,$K_c$ for the reaction $A_{2(g)} \rightleftharpoons B_{2(g)}$ is $99.0$. Two moles of $A_{2(g)}$ were heated to $T(K)$ in a $1 \ L$ closed flask to reach the above equilibrium. What are the concentrations (in $mol \ L^{-1}$) of $A_{2(g)}$ and $B_{2(g)}$ respectively at equilibrium?

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Given the following equilibria:
$K_1 : N_2 + 3H_2 \rightleftharpoons 2NH_3$
$K_2 : N_2 + O_2 \rightleftharpoons 2NO$
$K_3 : H_2 + 1/2 O_2 \rightleftharpoons H_2O$
The equilibrium constant for the reaction $2NH_3 + 5/2 O_2 \rightleftharpoons 2NO + 3H_2O$ in terms of $K_1, K_2$,and $K_3$ is:

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At $400 \ K$ for the reaction $2NO_{2(g)} \rightleftharpoons N_{2}O_{4(g)}$,the concentration of $NO_{2}$ is $0.710 \ M$ and $N_{2}O_{4}$ is $0.145 \ M$. Find the equilibrium constant $K_{c}$. (in $M^{-1}$)

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$8 \, \text{mol}$ of $AB_3$ is added to a $1.0 \, \text{dm}^3$ container. If it dissociates according to the reaction $2AB_{3(g)} \rightleftharpoons A_{2(g)} + 3B_{2(g)}$ and $2 \, \text{mol}$ of $A_2$ are present at equilibrium,what is the equilibrium constant $(K_c)$ for this reaction?

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Consider the following equilibrium reaction in gaseous state at $T(K)$.$A(g) + 2B(g) \rightleftharpoons 2C(g) + D(g)$The initial concentration of $B$ is $1.5$ times that of $A$. At equilibrium,the concentrations of $A$ and $B$ are equal. The equilibrium constant for the reaction is

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The equilibrium constant,$K_c$ for $3 C_2H_{2(g)} \rightleftharpoons C_6H_{6(g)}$ is $4 \, L^2 \, mol^{-2}$. If the equilibrium concentration of benzene is $0.5 \, mol \, L^{-1}$,the equilibrium concentration of acetylene in $mol \, L^{-1}$ is:

At $T(K)$,$K_c$ for the reaction $A_{2(g)} \rightleftharpoons B_{2(g)}$ is $99.0$. Two moles of $A_{2(g)}$ were heated to $T(K)$ in a $1 \ L$ closed flask to reach the above equilibrium. What are the concentrations (in $mol \ L^{-1}$) of $A_{2(g)}$ and $B_{2(g)}$ respectively at equilibrium?

Given the following equilibria: $K_1 : N_2 + 3H_2 \rightleftharpoons 2NH_3$ $K_2 : N_2 + O_2 \rightleftharpoons 2NO$ $K_3 : H_2 + 1/2 O_2 \rightleftharpoons H_2O$ The equilibrium constant for the reaction $2NH_3 + 5/2 O_2 \rightleftharpoons 2NO + 3H_2O$ in terms of $K_1, K_2$,and $K_3$ is:

At $400 \ K$ for the reaction $2NO_{2(g)} \rightleftharpoons N_{2}O_{4(g)}$,the concentration of $NO_{2}$ is $0.710 \ M$ and $N_{2}O_{4}$ is $0.145 \ M$. Find the equilibrium constant $K_{c}$. (in $M^{-1}$)

$8 \, \text{mol}$ of $AB_3$ is added to a $1.0 \, \text{dm}^3$ container. If it dissociates according to the reaction $2AB_{3(g)} \rightleftharpoons A_{2(g)} + 3B_{2(g)}$ and $2 \, \text{mol}$ of $A_2$ are present at equilibrium,what is the equilibrium constant $(K_c)$ for this reaction?

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Consider the following equilibrium reaction in gaseous state at $T(K)$.
$A(g) + 2B(g) \rightleftharpoons 2C(g) + D(g)$
The initial concentration of $B$ is $1.5$ times that of $A$. At equilibrium,the concentrations of $A$ and $B$ are equal. The equilibrium constant for the reaction is

Given the following equilibria:
$K_1 : N_2 + 3H_2 \rightleftharpoons 2NH_3$
$K_2 : N_2 + O_2 \rightleftharpoons 2NO$
$K_3 : H_2 + 1/2 O_2 \rightleftharpoons H_2O$
The equilibrium constant for the reaction $2NH_3 + 5/2 O_2 \rightleftharpoons 2NO + 3H_2O$ in terms of $K_1, K_2$,and $K_3$ is: