Starting from the observation that the standard Gibbs free energy of reaction, G, is related to the equilibrium constant K by
G = -RT lnK
Show that
dlnK/dT = -ΔH/R T^2
Pure butane, CH4, is cracked at 600K to form ethylene, C2H4, and methane, CH4, according to the following reactions:
CH4 → C2H4 + CH4
(i) (ii)
Find the equilibrium constants for the two reactions. Hence, estimate the ratio of the amounts of propylene and ethylene produced at equilibrium. (ii) How might your calculation change if fugacity coefficients were not unity?
Data:
Energies of Formation at 298K (kJ/mol):
ΔH: -126.15, -17.15, 52.28, 68.12, -84.67, -32.89, 20.41, 62.72, -74.85, -50.79
ΔG: -126.15, -17.15, 52.28, 68.12, -84.67, -32.89, 20.41, 62.72, -74.85, -50.79
Heat Capacity (J/molK):
Cp: 16.08 + 0.0375T, 16.64 + 0.123T, 9.401, 0.160T, 13.61 + 0.189T, 14.15 + 0.075T
CH4, C2H4, CH6, CH4