The most important commercial process for generating hydrogen gas is the water-gas shift reaction:. CH4(g) + H2O(g) → CO(g) + 3H
2(g). Use tabulated thermodynamic data to find ΔG° for this reaction at the standard temperature of 25°C. i found this to be. =1.423×102 kJ. Now calculate ΔG°1200 for this process when it occurs at 1200 K
The Gibb's free energy at a certain temperature is calculated through the equation, ΔG = - RT(ln K) where K is constant. Substituting the values from the first set of the given, 1.423x10^2 = -(8.314)(25 + 273) x (ln K) Solving for the value of K gives us an answer of, K = 0.94418 Use the same equation to get the value of ΔG°1200 ΔG = - (8.314)(1200) x (ln 0.94418) The value of ΔG°1200 is approximately 573.05 kJ