In the following reaction, 3A(g) + B(g) ⇌ 2C(g) + D(g), Initial moles of B is double of A. At equilibrium, moles of A and C are equal. Hence % dissociation of B is :

Question

In the following reaction, $3 A( g )+B( g ) \rightleftharpoons 2 C( g )+ D ( g )$,

Initial moles of $B$ is double of $A$. At equilibrium, moles of $A$ and $C$ are equal. Hence $\%$ dissociation of $B$ is :

(A) $10 \%$

(B) $20 \%$

(C) $40 \%$

(D) $5 \%$

Answer 1

The $\%$ dissociation of $B$ is $40%$. So, The correct option of this question will be (C).