The gas $A_2$ in the left flask allowed to react with gas $B_2$ present in right flask as $A_{2(g)}+

Question

The gas $A_2$ in the left flask allowed to react with gas $B_2$ present in right flask as $A_{2(g)}+B_{2(g)} \rightleftharpoons 2 A B_{(g)}$; $K_c=4$ at $27^{\circ} \mathrm{C}$. What is the concentration of $A B$ when equilibrium is established ?

Professor PC Thomas Classes · Answer

(c) :
$
A_{2(g)}+B_{2(g)} ightleftharpoons 2 A B_{(g)}
$
$
2-x \quad 4-x$        $2 x$
$
$Moles at equilibrium$  \ K_c=\frac{4 x^2}{(2-x)(4-x)}
$
$\begin{aligned} & \Rightarrow 4=\frac{4 x^2}{(2-x)(4-x)} \Rightarrow x=1.33 \mathrm{~mole} \ & {\left[A B_{(g)}ight]=\frac{2 	imes 1.33}{4}=0.66 \mathrm{M}}\end{aligned}$