(adsbygoogle = window.adsbygoogle || []).push({}); 1. The problem statement, all variables and given/known data

Consider the following reaction:

CH_{3}OH(g) <-> CO(g)+2H_{2}(g)

Calculate ΔG for this reaction at 298 K under the following conditions:

P_{CH3OH}=0.895atm

P_{CO}=0.115atm

P_{H2}=0.200atm

2. Relevant equations

ΔG=-R*T*ln(K)

where R is the gas constant 8.314 J/molK, T is 298 in this case, and K is determined from the partial pressures.

3. The attempt at a solution

I calculated K by (0.200^{2})(0.115)/0.895 and found it to be 0.00514.

This produced deltaG=-8.314*298*ln(0.00514)=-13.1 kJ, but this is incorrect according to the website. I'm really not sure what is going wrong; this is my last attempt on any of the pressure problems on this homework, so I'd like to get this figured out. My guess right now is that it's related to the # of moles not being used (as R suggests), but I'd appreciate input before I use my last attempt, especially so it's drilled into my brain after this assignment.

Thanks for any help!

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# Homework Help: Gibbs free energy from partial pressures

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