Chemical EquilibriumHard
Question
At 525 K, PCl5(g) is 80% dissociated at a pressure of 1 atm. Now, sufficient quantity of an inert gas at constant pressure is introduced into the above reaction mixture to produce inert gas partial pressure of 0.9 atm. What is the percentage dissociation of PCl5(g) when equilibrium is re-established?
Options
A.97.3%
B.80%
C.65.6%
D.4.7%
Solution
$K_{P} = \frac{\alpha^{2}.P}{1 - \alpha^{2}} \Rightarrow \frac{(0.3)^{2} \times 1}{1 - (0 - 3)^{2}} = \frac{\alpha^{2} \times 0.1}{1 - \alpha^{2}} \Rightarrow \alpha = 0.973$
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