Consider the following reaction:

CO(g)+2H2(g)⇌CH3OH(g)
An equilibrium mixture of this reaction at a certain temperature was found to have [CO]= 0.115M , [H2]= 0.110M , and [CH3OH]= 0.190M .

What is the value of the equilibrium constant (Kc) at this temperature?

What's your trouble with this problem? It's just a matter of substituting the values into Kc expressions.

so it would be CH3OH/(CO)(H2)^2

and then fill in so 0.190/(.115)(.0121)
=136.54 ???

How are you getting 136? When I calculate it, it equals 0.0199913043

Am I doing something wrong?

what would happen if i only had CO=.115 and h2=.110, how would i find CH3OH to then find K?

136.54 looks ok but that's too many significant figures. I would round it to 136.

As to your other what if question, you can do (CH3OH) but only if you have Kc (unless someone tells you that the reactions goes to completion). In that case it becomes a regular stoichiometry problem.

thank you!!!!!! :)

To determine the value of the equilibrium constant (Kc) at this temperature, we need to use the concentrations of the reactants and products at equilibrium.

In this case, the equilibrium concentrations of CO, H2, and CH3OH are given as [CO] = 0.115M, [H2] = 0.110M, and [CH3OH] = 0.190M, respectively.

The equilibrium constant expression (Kc) for this reaction can be written as:
Kc = ([CH3OH]^1)/([CO]^1 * [H2]^2)

Substituting the given equilibrium concentrations into the expression, we have:
Kc = (0.190^1) / (0.115^1 * 0.110^2)

Now, we can calculate the value of Kc:
Kc = 0.190 / (0.115 * 0.110^2)

After performing the calculation, the value of Kc is determined to be approximately 0.144.