Consider that the equilibrium state of the water-gas shift reaction (CO+H2OCO2+H2) approximately described by the following relation yCOyH2OyCO2yH2=Ke(T)=0.0247exp[4020/T(K)] where Ke is the reaction equilibrium constant, and yi is the mole fraction of species i in the reactor contents at equilibrium. The feed to a shift reactor contains 20.0 mole %CO,10.0%CO2,40.0% water, and the balance an inert gas. The reactor is maintained at T=1123K. i. For a basis of 1mol feed and draw and label a flowchart. Carry out a degree-of-freedom analysis of the reactor based on extents of reaction and use it to prove that you have enough information to calculate the composition of the reaction mixture at equilibrium. You do not need to do calculation for this part (i) of this question. ii. Estimate the total moles of gas in the reactor at equilibrium and then the equilibrium mole fraction of hydrogen in the product. iii. A gas sample is drawn from the reactor and analyzed shortly after startup and the mole fraction of hydrogen is significantly different from the calculated value. Assuming that no calculation mistakes or measurement errors have been made, what is a likely explanation for the discrepancy between the calculated and measured hydrogen yields? iv. Construct a spreadsheet to take as input the reactor temperature and the feed component mole fractions yCO;yH2O, and yCO2 (assume no hydrogen is fed) and to calculate the mole fraction yH2 in the product gas when equilibrium is reached. The spreadsheet column headings should be The columns between Ke and y(H2) may contain intermediate quantities in the calculation of yH2. First test your program for the conditions of Part (a) and verify that it is correct. Then try a variety of values of the input variables and draw conclusions about the conditions (reactor temperature and feed composition) that maximize the equilibrium yield of hydrogen