Question...

From Summer 2007, Exam 2:
6. For the reaction:
CH4(g) + 2 O2(g) 􀀧 CO2(g) + 2 H2O(g)
The equilibrium concentrations have been found to be [CO2]eq = 0.568M, [H2O]eq = 0.685M,
[CH4]eq = 1.38x10-8 M, [O2]eq = 0.918 M. What is the equilibrium constant?

I think some of you might be making this harder than it needs to be. The problem is giving you the equilibrium concentrations, so you just need to plug these numbers into the equilibrium constant expression:

Kc = { [CO₂] [H₂O]²} / { [CH₄] [O₂]²} = {(0.568)(0.685)²} / {(1.38x10^-8)(0.918)²} = 2.29x10⁷

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