Chemical EquilibriumHard

Question

One mole of pure PCl5 is placed in an evacuated container and maintained at 250°C. The equilibrium is established at total pressure of 2 atm. What is the partial pressure of chlorine at equilibrium?

PCl5(g) $\rightleftharpoons$ PCl3(g) + Cl2(g): KP = 1.6 atm

Options

A.0.4 atm
B.0.67 atm
C.0.80 atm
D.0.64 atm

Solution

PCl5(g) $\rightleftharpoons$ PCl3(g) + Cl2(g)

1 mole 0 0

Equilibrium (1 – x) mole x mole x mole

Equilibrium partial pressure (P = 2 atm)

$\frac{1 - x}{1 + x} \times P$ $\frac{x}{1 + x} \times P$ $\frac{x}{1 + x} \times P$

$K_{p} = \frac{\left( \frac{x}{1 + x}.P \right)\left( \frac{x}{1 + x}.P \right)}{\left( \frac{1 - x}{1 + x}.P \right)} = \frac{x^{2}.P}{1 - x^{2}}$

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