HELP Please! I'm going crazy with this problem!

[sharpieLIFE]

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Hey Everyone,
I can't seem to solve this problem. I just thought it would be ((88)(88))/((112)(112))

Carbon monoxide and water vapor, each at 200. Torr, were introduced into a 250. mL container. When the mixture reached equilibrium at 700.°C, the partial pressure of CO2(g) was 88 Torr. Calculate the value of K for the following equilibrium. CO(g) + H2O(g)

CO2(g) + H2(g)

 

[cheesier]

Are you sure that your values are correct? It doesn't really make sense as is. You need to calculate the partial pressure of H2 though. Here's how you can do it:

(88+x) = (2)(62)(973)/(0.25)

So you can see that the value you get doesn't make sense, but I think this is how you do it. If everything wasn't 1 mol it would be more complicated. From there:

Kp = Partial pressure of Products/Partial pressures of Reactants