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The water - gas shift reaction plays an important role in the production of clean fuel from coal.

CO(g) + H20(g) <--> CO2(g) + H2 (g)

Given Data:

Substance = CO(g) H20(g) CO2(g) H2(g)

Delta H (KJ/Mol) -110.5 -241.8 -393.5 0

Delta S (J/Mol K) 197.7 188.8 213.7 130.7

Use the given data to find the equilibrium constant Kp at 700K?

I know that I am supposed to use the equation:
ln K = Delta G /-R*T. But I am having trouble with the set up required to solve for G using:
Delta G = sum n* delta G products - sum m* reactants.

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It shows how to calculate the equilibrium constant Kp given Gibbs free energy of the reaction. The solution is detailed and well presented.

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The water - gas shift reaction plays an important role in the production of clean fuel from coal.

CO(g) + H20(g) <--> CO2(g) + H2 (g)

Given Data:

Substance ...

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