A mixture of 80 mole% ethane (C2H) and 20 mole% hydrogen (H2) flowing at rate of 200 mol/h is burned with 30% excess air. 92% fractional conversions of C2H6 and 85% of H, are achieved with below reactions. 7 (reaction 1) C2H6 +592 2 CO2 + 3 H20 2 H2 + 02 2 H20 (reaction 2) Beside, the below undesired reaction also got carried out in the same reactor resulting to produce CO. Of the C2He that reacts, 85% formed CO2 and the balance reacted to form CO. Process flowchart is given. Solve for the following: 5 (undesired reaction) C2H6 + 302 2 CO + 3H20 n=200 (mol/h) C2H60.8 YHz=0.2 ng (mol/h) n (mol-CH/h) nair n2 (mol-H/h) Yo=0.21 n3 (mol-Co/h) ne (mol-co/h) VN2=0.79 ns (mol-H20/h) no (mol-oy/h) n (mol-Ny/h) a) Stoichiometric moles of O2 required b) Determine amount of air fed to the process (Nair) c) Prove that C3Hg is the limiting reactant d) Perform the degree-of-freedom analysis, based on molecular balance method, and comment of your results e) Calculate molar flowrates of C3H(ni), H2 (n2), CO2 (n3) and CO (n4) leaving the reactor. (Hint: use given process information) f) Calculate molar flowrates of effluent stream (ns) from the reactor using atomic balance method (Hint: input-output) g) Calculate the selectivity and yield of CO2 production (1 pt) (1 pt) (1 pt) (2 pt) (2 pt) (2 pt) (1 pt)