The gas A2 in the left flask is allowed to react with gas B2 present in right flask as A2(g)+B2(g)⇌2AB(g),KC=4 at 27∘C. What is the concentration of AB when equilibrium is established?

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

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$1.33 M$

$0.66 M$

$0.33 M$

$2.66$

answer is B.

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Detailed Solution

$\begin{array}{l} A_{2} (g) + B_{2} (g) ⇌ 2 A B (g) \\ 2 - x 4 - x 2 x \\ \frac{4 x^{2}}{(2 - x) (4 - x)} 4 \\ x = \frac{4}{3} mole \\ [A B] = \frac{2 \times \frac{4}{3}}{4} = 0.66 M \end{array}$