The oxidation of SO2 is to be carried out over a solid platinum catalyst in a packed bed reactor. As with almost all gas-solid catalytic reactions, the rate law is expressed in terms of partial pressures instead of concentrations. The rate law is found experimentally to be: −rSO2 ′ = k ൤PSO2ඥPO2 − PSO2 Kp ൨ ൫1 + ඥPO2 KO2 + PSO2 KSO2 ൯ 2 , mo SO2 oxidized(h −1 )(g catayst) −1 Where Pi (atm) is the partial pressure of species i. the reaction is to be carried out isothermally at 400 °C. At this temperature, the rate constant k, the adsorption constants for O2 (KO2 ) and SO2 (KSO2 ), are the pressure equilibrium constant (Kp) where found experimentally to be: k = 9.7 mol SO2/atm3/2/h/g-cat, KO2 = 38.5 atm-1 , KSO2 = 42.5atm-1 O2 and Kp = 930 atm-1/2 The total pressure is 14.7 atm. The inlet is a mixture of 28% SO2 and 72% air by mol. There is no pressure drop. Using Polymath (or Matlab), plot Fao −ra vs. W, for W ranging from W = 0 to 1000 g.