Consider the following gas-phase reaction between methyl mercaptan (CH3SH) and hydrogen (in a desulfurization unit of a NG reforming process) to form methane and hydrogen sulfide (H2S). takes place in a fixed bed reactor. (desulfurization reaction) CH3SH+H2CH4+H2S (A) (B) (C) (D) At equilibrium, the mole fractions of the four reactive species are related by the reaction equilibrium constant (assumed value). Ky=yAyByCyD=4.87 (i) Draw and label a flow diagram of the desulfurization unit (only) (ii) Suppose the feed to the reactor consists of nA0;nB0;nCO and nD0, moles of A,B,C, and D, respectively. Write expressions for the moles of each species in the final product, nA,nB,nC, and nD in terms of incoming moles and the extent () be of the reaction. (iii) Then use these expressions and the given equilibrium constant to derive an equation for e, the equilibrium extent of reaction, in terms of nA0;nB0;nC0 and nD0. (iv) If the feed to the reactor contains equimolar quantities of mercaptan ( CH3SH) and hydrogen, calculate the equilibrium fractional conversion. (v) (iv) It is desired to produce 70mol of methane starting with 75mol of mercaptan ( CH3SH). If the reaction proceeds to equilibrium, how much hydrogen must be fed? What is the composition of the final product