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
2 Answers
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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
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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
your answer will be in Molarity
Looks like it is solvable after all. 🙂
Source(s): some dude