Calculate the conversion of benzene anc

Methanol oxidation using air produces carbon dioxide and water. In a reaction performed adiabatically, $100\%$ excess of air is used. Methanol is fed to the reactor at $25C$ whereas air is fed to the reactor at $100C.$ It is observed that the methanol is completely consumed in the reaction and the outlet temperature of the reactor is $1256C.$ The heat of reaction for methanol oxidation is $-726\mathrm{.}6k\frac{J}{m}ol$ of methanol consumed. Show the degrees of freedom analysis to justify the use of basis. The heat capacity of product gases is given by the following equation with $C_p$ in units of $k\frac{J}{m}olC$ and temperature in units of $C.$

$(C_p{)}_{C{O}_2}=0\mathrm{.}03611+4\mathrm{.}233{10}^{-5}T-2\mathrm{.}887{10}^{-8}{T}^2+7\mathrm{.}464{10}^{-12}{T}^3$

$(C_p{)}_{H_{2}O(8)}=0\mathrm{.}03346+0\mathrm{.}688{10}^{-5}T+0\mathrm{.}7604{10}^{-8}{T}^2-3\mathrm{.}593{10}^{-12}{T}^3$

$(C_p{)}_{O_2}=0\mathrm{.}02910+1\mathrm{.}158{10}^{-5}T-0\mathrm{.}6076{10}^{-8}{T}^2+1\mathrm{.}311{10}^{-12}{T}^3$

$(C_p{)}_{N_2}=0\mathrm{.}02900+0\mathrm{.}2199{10}^{-5}T+0\mathrm{.}5723{10}^{-8}{T}^2-2\mathrm{.}871{10}^{-12}{T}^3$

Specific enthalpy of air at $100C$ can be considered as $2\mathrm{.}191k\frac{J}{m}ol.$ Calculate the heat supplied or removed from the reactor.