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(b) Calculate Kp for the overall process at 1200. K.

Answer 1

According to the ideal gas law, partial pressure is inversely proportional to volume. It is also directly proportional to moles and temperature. At equilibrium in the following reaction at room temperature, the partial pressures of the gases are found to be PN2 = 0.094 atm, PH2 = 0.039 atm, and PNH3 = 0.003 atm.

Equilibrium partial pressures

The initial partial pressures of CO and water are 4.0 bar and 4.0 bar respectively.

The equilibrium partial pressures (in the bar) of CO, H2​O, CO2​, and H2​ are 4−p,4−p, and respectively.

Let p bar be the equilibrium partial pressure of hydrogen.

The expression for the equilibrium constant is

Kp​=PCO​PH2​O​PCO2​​PH2​​​=(4−p)(4−p)p×p​=0.1

p=1.264−0.316p

p=0.96 bar.

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