calculate the equilibrium constant Kp
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.
https://brainmass.com/chemistry/energetics-and-thermodynamics/calculate-equilibrium-constant-kp-140467
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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 ...
Solution Summary
It shows how to calculate the equilibrium constant Kp given Gibbs free energy of the reaction. The solution is detailed and well presented.