Carbon monoxide and chlorine gas react to produce COCl₂ gas.The for the reaction is 1.49 × 10⁸ at 100.0 °C: In an equilibrium mixture of the three gases, = = 7.70 × 10^-4 atm.The partial pressure of the product,phosgene ( ),is ________ atm.

Question

Quizplus · Accepted Answer

The balanced chemical equation for the reaction is:

CO(g) + Cl2(g) ⇌ COCl2(g)

The equilibrium constant expression is:

Kc = [COCl2]/([CO][Cl2])

Given:

Kc = 1.49 × 10^18 at 100.0 °C
[COCl2] = [CO]eq = [Cl2]eq = 7.70 × 10^-14 atm

Let's substitute the values into the expression and solve for [COCl2]:

1.49 × 10^18 = [COCl2]/([CO][Cl2])
1.49 × 10^18 = x/(7.70 × 10^-14)^2
x = 8.83 × 10^11

Therefore, the partial pressure of COCl2 (phosgene) is:

[COCl2] = x/V = (8.83 × 10^11)/(1 atm) = 8.83 × 10^11 atm

The answer is D, 8.83 × 10^11 atm.

Carbon Monoxide and Chlorine Gas React to Produce COCl2 Gas

Carbon Monoxide and Chlorine Gas React to Produce COCl₂ Gas