Q1: The gas-phase reaction: 1/2N2+3/2H2NH3 is to be carried out in a batch or flow reactor. The molar feed ratio is 80%H2 and 20%N2. The initial (inlet) pressure is 10atm and temperature is 273K. 1) Choose the basis, and then determine CA0,, and ? 2) Construct the complete Stoichiometric Table for a batch system (Note: assuming the initial number of moles of the base element is NA0, and batch reactor is isothermal and isobaric at the initial condition); 3) Construct the Stoichiometric Table for a flow system (Note: assuming the initial flow rate of the base element is FA0, the outlet of flow reactor T=373K, and pressure =10.0 atm); 4) Find concentrations of NH3 and H2 at outlet of the flow reactor, when N2 conversion of is 60%. 5) Suppose the above listed reaction is elementary with kN2=10dm3/mol/s, Write the rate of reaction as a function of conversion for the flow reactor at the outlet conditions; 6) Suppose the reaction now is reversible and elementary: i.e. 1/2N2+3/2H2NH3, The thermodynamic equilibrium constant Kc=30 at the outlet condition and kN2=10 dm3/mol/s. Write the rate of reaction in terms of the concentration symbols (CN2,CNH3, CH2 ) only