# Consider the following reaction: COCl2(g) ⇌ CO(g) + Cl2(g) A reaction mixture initially contains 1.6 M COCl2.?

I feel like there is not enough information to solve this?

Consider the following reaction: COCl2(g) ⇌ CO(g) + Cl2(g) A reaction mixture initially contains 1.6 M COCl2. Determine the equilibrium concentration of CO if Kc for the reaction at this temperature is 8.33 × 10-4. Calculate this based on the assumption that the answer is negligible compared to 1.6.

the answer is supposed to be 3.7 × 10-2 M

• we have enough information and here is an excellent solution

COCl2(g) ⇌ CO(g) + Cl2(g) ICE table needed

I.....1.6...............0.........0

C....-x...............+x.........+x

E...1.6-x ...........x............x

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

Kc = x^2 / 1.6-x = 8.33 × 10-4

x is negligible compared to 1.6.so the denominator = 1.6

so x^2 = 1.6 * 8.33 × 10-4

x= 0.0365 M

[CO] = 0.0365 M

• I think you can, I haven't done this kind of ICE table math in a few years since AP Chem so I may make a mistake or two, but follow along and catch any mistakes if I make any, i doubt i will though. :/

COCl2 ----------> CO + Cl2

I 1.6......................0.........0

C -x.......................+x.......+x

E 1.6-x.................x............x

Kc = x^2 / 1.6-x

it tells you to assume x is negligible compared to 1.6 so...

Kc = x^2 / 1.6

8.33 x 10^-4 = x^2/1.6

(8.33 x 10^-4) (1.6) = x^2

solve for x

once you get x, plug into: 1.6 - x = answer