Question

2 moles of $PC{l}_5,$ were heated in a closed vessel of 2 litre capacity. At equilibrium, 40% of $PC{l}_5$ is dissociated into $PC{l}_{3}andC{l}_2.$ The value of equilibrium constant is

• A. 0.266
• B. 0.53
• C. 2.66
• D. 5.3

Answer 1

The correct option is A 0.266

$\underset{2}{PC{l}_5}\rightleftharpoons \underset{0}{PC{l}_3}+\underset{0}{C{l}_2}$
$\frac{2\times 60}{100}\frac{2\times 40}{100}\frac{2\times 40}{100}$

Volume of container = 2 litre.
$K_c=\frac{\frac{2\times 40}{100\times 2}\times \frac{2\times 40}{100\times 2}}{\frac{2\times 60}{100\times 2}}=0.266$