Water and carbon monoxide react to produce H2 and CO2 (reaction A) (see formation data below) H₂O(g) + CO(g) H₂(g) + CO2(g) (A) The reaction is known to proceed rapidly at

298 K and 5 atm pressure over an iron oxide (Fe3O4, magnetite) catalyst. Assuming a = stoichiometric feed of reactants and assuming that the heat of reaction is independent of temperature (i.e., no heat capacity terms needed) determine (a) If the equilibrium temperature was raised, would production of H₂ increase? (b) Calculate the mole fractions of CO2 and CO at equilibrium. (c) Does any liquid water exist at the equilibrium conditions? (d) Concern has been raised that under the equilibrium conditions for Reaction A (use concentrations calculated in part b), carbon may form from Reaction B (25 pts)/n(d) Concern has been raised that under the equilibrium conditions for Reaction A (use concentrations calculated in part b), carbon may form from Reaction B 2 CO CO₂ + C(s) = Show using equations if this fear is justified. Free energies of formation from the elements are available on page 686-687 of your textbook (also given below). Chemical Species Water T [C] 20 25 30 Formula H₂O DATA for Water Vapor Pressure H₂O [mm Hg] State gas 17.535 23.756 31.824 (B) AHE, 298K [J/mol] -241,818 P [g/ml] 0.9982 0.9970 0.9957 AG, 298K [J/mol] -228,572 ZOOM/nChemical Species Water Water Carbon Dioxide Carbon 25 30 Formula H₂O H₂O CO₂ CO State gas liquid gas gas 17.535 23.756 31.824 AH, 298K [J/mol] -241,818 -285,830 Page < -393,509 -110,525 6 0.9982 0.9970 0.9957 of 6 AGE, 298K [J/mol] -228,572 -237,129 -394,359 -137,169 0 | Monoxide Standard States: Gases-pure ideal gas at 1 bar and 25 C; Liquids-pure liquid at 1 bar and 25 C. - ZOOM