# Problem: 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. KCO(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.

###### FREE Expert Solution

Equilibrium Reaction: C3H8(g) + 6H2O(g) → 3CO2(g) + 10H2(g)

0.2

0.8

###### Problem Details

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.