Question

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: \begin{equation}C₃H₈(g) + 3H₂O(g) ⇄ 3CO(g) + 7H₂(g) Kp = 8.175×10¹⁵ at 1200KCO(g) + H₂O(g) ⇄ CO₂(g) + H₂(g) Kp = 0.6944 at 1200k(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.

Answer 1

The ideal gas law states that the relationship between partial pressure and volume is inverse. Additionally, it relates temperature and moles in a direct proportion. The partial pressures of the gases are found to be PN2 = 0.094 atm, PH2 = 0.039 atm, and PNH3 = 0.003 atm in the following reaction at equilibrium at room temperature.

What is ideal gas law ?

PV = NkT, where P is a gas's absolute pressure, V is the volume it occupies, N is the quantity of atoms and molecules in the gas, and T is its absolute temperature, is the formula for the ideal gas law.

Equal volumes of two gases with the same temperature and pressure will contain an equal number of molecules, according to the law. The ideal gas law is the result of the union of all these relationships.

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