Question

Carbon monoxide and chlorine gas react to produce phosgene (COCl2) gas according to the following reaction at 100.0°C: CO(g)+Cl2(g)⟺COCl2(g)Kp=1.49×108 In an equilibrium mixture of the three gases, PCO = PCl2 = 4.83 x 10-4 atm, what is the equilibrium partial pressure (in atm) of phosgene?

Answer 1

Answer:

28.6

Explanation:

Step 1: Write the balanced reaction at equilibrium

CO(g) + Cl₂(g) ⟺ COCl₂(g)

Step 2: Calculate the equilibrium partial pressure (in atm) of phosgene?

We will use the expression for the pressure equilibrium constant (Kp)

Kp = pCOCl₂ / pCO × pCl₂

pCOCl₂ = Kp × pCO × pCl₂

pCOCl₂ = 1.49 × 10⁸ × 4.38 × 10⁻⁴ × 4.38 × 10⁻⁴ = 28.6