[Mr-E]

Question 3
When phosgene, COCl2, is introduced into a reactor, equilibrium is attained according to the reaction

COCl2(g) -> CO(g) + Cl2(g)

The chlorine gas is light green in colour, while the other gases are colourless.
0.30 mol of COCl2(g) and 0.20 mol of CO(g) are introduced in a 5.0 L container at 40°C. When equilibrium is
reached, 0.10 mol of Cl2(g) has formed. The temperature is maintained at 40°C throughout the experiment.
a. i. Calculate the numerical value of the equilibrium constant, K, for the forward reaction at 40°C.

The amount of moles of COCl at equilibrium is .1 or .2?
So at equilibrium the mole ratio is
.2 : .3 : .1 or .1 : .3 : .1
I hope that makes sense. Thanks

[curiouscat]

Desperate help please. Very easy Q

Contradiction in terms? 

[Dan]

Hint: How much phosgene would have to decompose to produce 0.1 mol Cl₂? How much did you start with? So, how much is left?

[Mr-E]

so the mole ratio will be .2 : .3 : .1?

[Dan]

Yes