Question

The composition of the equilibrium mixture for the equilibrium $Cl_{2}\rightleftharpoons2Cl$ at $1470 \,K $ diffuses $1.16$ times as fast as Krypton $(84) $ under the same conditions. Find the degree of dissociation of $Cl_{2}$ at equilibrium.

• A. 0.14
• B. 0.41
• C. 0.91
• D. 0.24

Answer 1

Answer: (A)

$\underset{1 - x}{C l_{2}}\rightleftharpoons\underset{2 x}{2 C l}$
$M_\text{mix}=\frac{\left(\right. 1 - x \left.\right) 71 + 2 x \times 35.5}{\left(\right. 1 - x \left.\right) + 2 x}=\frac{71}{1 + x}$
$\frac{R_\text{mix}}{R_{K r}}=\sqrt{\frac{M_{K r}}{M_\text{mix}}}$
$1.16 = \sqrt{\frac{84}{\frac{71}{1 + \text{x}}}}$
On solving $x=0.14$