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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
(d) What percentage of the C3H8 remains unreacted?