At low moderate pressures, the equilibrium state of the water-gas shift reaction (co + h2o < --> co2 + h2) is approximately described by the reaction: (yco2yh2)/(ycoyh2o) = ke(t) = .0247 exp[4020/t(k)] where t is the reactor temperature, 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 batch 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=1123 k. a) assume a basis of 1 mole feed and draw and label a flowchart. carry out a degree of freedom analysis of the reactor based on extents of the reaction of the mixture at equilibrium. do no calculations. b) calculate the total moles of gas in the reactor at equilbrium (if it takes you more than 5 seconds youre missing the point) and then the equilibrium mole fraction of hydrogen in the product. (suggestion: begin writing expressions for the moles of each species in the product gas in terms of the extent of reaction, and then write expressions for the species mole fractions.) c) suppose a gas sample is drawn from the reactor and analyzed shortly after start up 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?