(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 1 Equilibrium: Chemical Equilibrium Law of equilibrium and Equilibrium constant

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

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Law of equilibrium and Equilibrium constant

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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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For the reaction $2AB \rightleftharpoons A_2 + B_2$,the equilibrium constant is $49$. What will be the equilibrium constant for the reaction $AB \rightleftharpoons 1/2 A_2 + 1/2 B_2$?

For the reaction $CaCO_{3(s)} \rightleftharpoons CaO_{(s)} + CO_{2(g)}$,which of the following expressions for the equilibrium constant $K_p$ is correct?

The figure shows the change in concentration of species $A$ and $B$ as a function of time. The equilibrium constant $K_C$ for the reaction $2A_{(g)} \rightleftharpoons B_{(g)}$ is

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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