[rainicorn]

Hi, I've been trying this question and I've been having difficulty finding the correct answer:

Consider the reaction:
CO(g)+2H2(g)⇌CH3OH(g)
A reaction mixture in a 5.23-L flask at 500 K contains 9.05 g of CO and 0.58 g of H2. At equilibrium, the flask contains 2.33 g of CH3OH.
Calculate the equilibrium constant at this temperature.

So far I have found the concentration of CO to be 0.0618 M, H₂ to be 0.0551 M, and CH₃OH. Then, I have made an ICE table:

I 0.0618 ---- 0.0551----- 0
C -x -------- -2x --------  +x
E 0.0618-x ----0.0551-2x --x

Then, I found: [CO] = 0.0479 M, [H₂]=0.0273 M, [CH₃OH]=0.0139 M

Then inserted these values into the equation Kc= [CH₃OH]/[CO] [H₂]^2, then Kc= 389.4.

Was my method correct?  Any help is much appreciated, thanks! 

[Borek]

Looks about right.