Hydrogen is produced in the steam reforming of propane: C₃H₈ (g) + 3 H₂O (v) ? 3 CO₂ (g) + 7 H₂ (g) the water?gas shift reaction also takes place in the reactor, leading to the formation of additional hydrogen: CO (g) + H₂O (v) ? CO₂ (g) + H₂ (g) the reaction is carried out over a nickel catalyst in the tubes of a shell-and-tube reactor. The feed to the reactor contains steam and propane in a 6:1 molar ratio at 125?C, and the products emerge at 800?C. The excess steam in the feed assures essentially complete consumption of the propane. Heat is added to the reaction mixture by passing a hot gas over the outside of the tubes that contain the catalyst. The gas is fed at 4.94 m³/mol C₃H₈ entering the unit at 1400?C and 1 atm and leaving at 900?C. The unit may be considered adiabatic. Calculate the molar composition of the product gas assuming that the heat capacity of the heating gas is 0.040 kJ/ (mol??C).

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Heating gas 1400°C, 1 atm C3H₂(g) H₂O(v) 125°C Spent heating gas 900°C C3H₂(g) H₂O(v) CO(g) H₂(g) CO₂(8) 800°C