FeS is an important contaminant in iron after the ore is processed. A researcher is studying how to remove FeS in a batch reactor through direct oxidation. The UNBALANCED reaction is: FeS(s)+O2(g)FeO(s)+SO2(g) A sealed reactor is 'charged' with 1kg of solid FeS and pure pressurized oxygen. The internals are arranged so that the solid has intimate contact with the gas. The reactor is heated and held at a constant temperature. The pressure is monitored until the pressure stops falling. The reactor is then cooled and samples of the 2 phases are taken. The gas is found to be 100%SO2, and the solid product (slag) is 80 wt %FeO the balance FeS. a) Balance the reaction using integer stoichiometric coefficients. b) How would you characterize this reactor (batch? Continuous? Semi-batch?) Explain. c) After the initial heat up phase, why does the pressure in the reactor fall? What does it mean when the pressure stops changing? d) What is the limiting reactant? How do you know? e) Sketch the process. One way to do this is to present the reactor in 2 pictures, one before and 1 after the reaction. Show key information. f) Develop a stream table indicating species, MW, phase, mol fraction, and moles of each 'stream' (In this case, a 'stream' is either solid or gas, before or after the reaction). Enter what you know, without doing any calculations g) Determine the extent of the reaction. h) Determine the quantity (moles) of each of the 4 compounds both initially and finally. Complete your stream table