(Solved): The reaction to produce ethylene oxide is as follows; C2H4+1/2O2C2H4O The reactio ...

The reaction to produce ethylene oxide is as follows; ${\mathrm{C}}_2{\mathrm{H}}_4+1/2{\mathrm{O}}_2?{\mathrm{C}}_2{\mathrm{H}}_4\mathrm{O}$ The reaction is an isothermal, isobaric, catalytic gas-phase oxidation reaction, where the feed consist of a stoichiometric mixture of ethylene and oxygen, enter the PBR at $6\mathrm{atm}$ and $260^{?}\mathrm{C}$. Set up a stoichiometric table for the reaction above. Express the concentration of each species in the reaction as a function of conversion evaluating all constants (e.g., $?,?)$. Then assume the reaction follows an elementary rate law, write the reaction rate solely as a function of conversion, i.e., $?r_A=f(X)$.