Q.3 Acetylene is hydrogenated to form ethane in the following reaction CH + 2H CH6. The feed to the reactor contains 1.25 mol H/mol CH. (a) Calculate the stoichiometric reactant ratio (mol H react/mol CH react) and the stoichiometric yield ratio (kmol CH6 formed/kmol H react). (b) Determine the limiting reactant and calculate the percentage by which the other reactant is in excess. (c) Calculate the mass feed rate of hydrogen (kg/s) required to produce 5x106 metric tons of ethane per year, assuming that the reaction goes to completion and that the process operates for 24 hours a day, 330 days a year. Q.4 At low to moderate pressures, the equilibrium state of the water-gas shift reversible reaction CO + HO CO + H is approximately described by the relation: 4020 = K (T) = 0.0247exp[T(K)- where T is the reactor temperature, Ke is the reaction equilibrium constant, and y; is mole fraction of species i in the reactor contents at equilibrium. The feed to a batch shift reactor contains 20.0 mole% CO, 10.0 % CO2, 40% water, and the balance an inert gas. The reactor is maintained at T = 1000 C. Assume a basis of 1 mol feed: (a) Draw and label a flowchart of this process. (b) Calculate the total moles of gas in the reactor at equilibrium and then the equilibrium mole fractions of each species in the product.

Q.3 Acetylene is hydrogenated to form ethane in the following reaction C2H2+2H2C2H6. The feed to the reactor contains 1.25molH2/molC2H2. (a) Calculate the stoichiometric reactant ratio ( molH2 react /mol2H2 react) and the stoichiometric yield ratio (kmolC2H6 formed /kmolH2 react). (b) Determine the limiting reactant and calculate the percentage by which the other reactant is in excess. (c) Calculate the mass feed rate of hydrogen (kg/s) required to produce 5106 metric tons of ethane per year, assuming that the reaction goes to completion and that process operates for 24 hours a day, 330 days a year. Q.4 At low to moderate pressures, the equilibrium state of the water-gas shift reversible reaction CO+H2OCO2+H2 is approximately described by the relation: yCOyH2OyCO2yH2=Ke(T)=0.0247exp[T(K)4020] where T is the reactor temperature, Ke is the reaction equilibrium constant, and yi is mole fraction of species i in the reactor contents at equilibrium. The feed to a batch shift reactor contains 20.0 mole %CO,10.0%CO2,40% water, and the balance an inert gas. The reactor is maintained at T=1000C. Assume a basis of 1 mol feed: (a) Draw and label a flowchart of this process. (b) Calculate the total moles of gas in the reactor at equilibrium and then the equilibrium mole fractions of each species in the product