Question

The gas $A_{2}$ in the left flask allowed to react with gas $B_{2}$ present in right flask as, $A_{2}\left(g\right)+B_{2}\left(g\right)\rightleftharpoons2AB\left(g\right)$ ; $Kc=4at27^\circ C$ . What is the concentration of $AB$ when equilibrium is established?

• A. $1.33M$
• B. $2.66M$
• C. $0.66M$
• D. $0.33M$

Answer 1

Answer: (C)

$K_{c}=\frac{\left[AB\right]^{2}}{\left[A_{2}\right] \left[B_{2}\right]}$
$\left(\text{K}\right)_{\text{c}}=\frac{4 \left(\text{x}\right)^{2}}{\left(2 - \text{x}\right) \left(4 - \text{x}\right)}$
$⇒ \, \, \text{x} = \frac{3 2}{2 4} = \text{1.33 mole}$
$\text{AB} \left(\text{g}\right) = \frac{2 \times \text{1} \text{.33}}{4} = \text{0} \text{.66 M}$