Chemical EquilibriumHard

Question

The Deacon reaction is the oxidation of HCl by O2 in the following reaction

HCl(g) + ¼ O2(g) $\rightleftharpoons$½ Cl2(g) + ½ H2O(g) at a pressure of 730 mm and with an initial mixture containing 8% of HCl and 92% of O2, the degree of decomposition of the HCl is 0.08. What is the equilibrium partial pressure of oxygen?

Options

A.671.6 mm
B.659.92 mm
C.537.28 mm
D.670.43 mm

Solution

HCl(g) + ¼ O2(g) $\rightleftharpoons$ ½ Cl2(g) + ½ H2O(g)

Initial partial pressure $730 \times \frac{8}{100}$ $730 \times \frac{92}{100}$

= 58.4 mm = 671.6 mm

Equilibrium partial pressure 58.4 – 58.4 × 0.08

$671.6 - \frac{58.4 \times 0.08}{4} = 670.432\text{ mm}$

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