Carbon monoxide and chlorine gas react to produce COCl2 gas. The Kp for the reaction is 1.49 × 108 at 100.0 °C: In an equilibrium mixture of the three gases, PCO, = PCl2 = 7.70 × 10-4 atm. The partial pressure of the product, phosgene (COCl2), is atm. Use the assumption that change in x is small so you do not have to use the quadratic.

Explanation:

Solution:

Fortheequilibrium

Theequilibrium constant is definedintermsofpartialpressure:

Introducingthenumericaldatagivenforpartialpressureofcarbonmonoxide 0 andchlorine 12,alsothevalueforequilibriumconstant:

Thepartialpressureoftheproduct,phosgene(COCl2),is29.4atm

88.34 atm

Explanation:

At equilibrium, carbon monoxide (CO) would react with chlorine gas according to the equation below:

CO (g) + Cl₂ (g)   ⇒ COCl₂ (g)

The equilibrium constant Kp, which is a ratio of the partial pressure of the product to that of the reactants is obtained from the equation below:

Kp = PCOCL / PCO.PCl₂

From the question given,

Kp = 1.49 x 10⁸ t 100° C

PCO = 7.70 X 10⁻⁴ atm

PCl₂ = 7.70 x 10⁻⁴ atm

It therefore implies that,

1.49 x 10⁸  = P(COCl₂) / (7.70 x 10⁻⁴). (7.70 x 10⁻⁴)

P(COCl₂) = 1.49 x 10⁸) . (7.70 x 10⁻⁴) . (7.70 x 10⁻⁴)

P (COCl₂) = 88.34 atm

The partial pressure P(COCl₂) of the product phosgene (COCl₂) is 88.34 atm

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