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?
6 answers
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 ???
and then fill in so 0.190/(.115)(.0121)
=136.54 ???
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.
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!!!!!! :)
How are you getting 136? When I calculate it, it equals 0.0199913043
Am I doing something wrong?
Am I doing something wrong?