Question

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.

Answer 1

Answer:

Explanation:

Solution:

For the equilibrium

The equilibrium constant is defined in terms of partial pressure:

Introducing the numerical data given for partial pressureof carbon monoxide 0 and chlorine 12, also the value for equilibrium constant:

Answer:

The partial pressureof the product, phosgene (COCl2), is 29.4atm

Answer 2

Answer:

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