Chemical EquilibriumHard

Question

In a vessel of 1.0 L capacity, O2(g) at 0.25 atm pressure and HCl(g) at 1.0 atm pressure are allowed to react in the presence of liquid water at 57o C.

4HCl(g) + O2(g) $\rightleftharpoons$2Cl2(g) + 2H2O(g); KP = 5.0 × 1012 atm–1.

The volume occupied by liquid water is negligible but it is sufficient at achieve equilibrium with water vapour. The vapour pressure of water at 57o C is 0.4 atm. Select the correct statement(s) regarding the equilibrium mixture.

Options

A.The partial pressure of water vapour at any stage of reaction is 0.4 atm.
B.The partial pressure of Cl2(g) at equilibrium is 0.5 atm.
C.The partial pressure of O2(g) at equilibrium is 5.0 × 10–4 atm.
D.The partial pressure of HCl(g) at equilibrium is 2.0 × 10–3 atm.

Solution

4HCl(g) + O2(g) $\rightleftharpoons$ 2Cl2(g) + 2H2O(g)

Initial partial pressure 1.0 atm 0.25 atm 0 0.4 atm

On completion 0 0 0.5 atm 0.4 atm

Equ. partial pressure 4x atm x atm 0.5 atm 0.4 atm

$K_{p} = 5 \times 10^{12} = \frac{(0.5)^{2}(0.4)^{2}}{(4x)^{4} \times x} \Rightarrow x = 5 \times 10^{- 4}$

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