Equilibrium Reaction: C3H8(g) + 6H2O(g) → 3CO2(g) + 10H2(g)
The methane used to obtain H2 for NH3 manufacture is impure and usually contains other hydrocarbons, such as propane, C3H8. Imagine the reaction of propane occurring in two steps:
C3H8(g) + 3H2O(g) ⥫⥬ 3CO(g) + 7H 2(g)
K p = 8.175×1015 at 1200. K
CO(g) + H2O(g) ⥫⥬ CO2(g) + H2(g)
K p = 0.6944 at 1200. K
(c) When 1.00 volume of C3H8 and 4.00 volumes of H2O, each at 1200. K and 5.0 atm, are mixed in a container, what is the final pressure? Assume the total volume remains constant, that the reaction is essentially complete, and that the gases behave ideally.
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