Carbon disulfide is widely used for the production of viscose rayon, rubber, and other organic materials and it is a feedstock for the synthesis of sulfuric acid. The primary industrial scale production of carbon disulfide is by the reaction between methane and sulfur vapor over a metal oxide catalyst at 700C : CH4(g)+4S(g)CS2(g)+2H2S(g)Hr(700C)kJ/mol 1mol feed of gaseous methane and sulfur are heated to 700C before entering the reactor in stoichiometric proportion. 80% conversion of methane is achieved and the reaction products emerge from the reactor at 800C. Constant heat capacities are assumed: Cp in J/molC:18.3 for S(s),29.4 for S(l),36.4 for S(g),71.4 for CH4(g),31.8 for CS2(g) and 44.8 for H2S(g). Temperatures and enthalpies of phase change for sulfur, Hm(113C)=10.04kJ/mol and Hv(444.6C)=83.7kJ/mol. The atomic weights of H,C,O and S are, respectively, 1,12,16 and 32. The standard heats of combustion of CH4(g),CS2(g) and H2S(g) as well as standard heat of formation of SO2(g) are given below: Hc0[CH4(g)]=890.36Hc0[(H2S(g)]=562.59kJ/molkJ/molHc0[CS2(g)]=1102.6Hf0[SO2(g)]=296.9kJ/molkJ/mol (a) Draw and label a flowchart of the process and calculate the molar amounts of process streams. [4 marks] (b) Establish the relationship between Hr(700C) in kJ/mol and Q in kJ/mol feed, the rate at which heat is transferred from the reactor, to achieve the specified conversion and product temperature. [7 marks] (c) Determine Hr(700C) in kJ/mol and Q in kJ/mol feed for the above sulfur reformation reaction. [9 marks]