$1\mathrm{.}4,$ A reaction of carbon monoxide and hydrogen gives methanol as the only product when performed in a vapor phase reactor. The feed to the reactor is maintained at $25C$ and $1$atm pressure with a yolumetric flow rate measured as $100\frac{m^3}{h}.$ The proportions of gases in the feed is such that carbon monoxide and hydrogen are the two gases taken in stoichiometric proportions. The product stream in the vapor form emerges from the reactor at $115C.$ The rate of heat transfer from the renctor is $12\mathrm{.}05kW.$ Calculate the fractional conversion achieved and the bolumetric flow rate of the product stream in $\frac{m^3}{h}$ if the pressuse is maintained constant in the system. Heat of reaction $=-90\mathrm{.}68k\frac{J}{m}ol$

For CO$,$ Cp $(k{J}^{\text{m}\text{o}\text{l}}C)=28\mathrm{.}95{10}^{-3}+0\mathrm{.}4111$

For Hy'rogen,

For Meli.mol vapor, $Cp(k\frac{J}{m}olC)=42\mathrm{.}931l^3+8\mathrm{.}301{10}^{-5}T$