$(25\%)$ Methanol can be made by catalytic oxidation of methane using the stoichiometric amount of $O_2$ as shown in the reaction below. A conversion of $30\%$ of the methane was obtained in the reactor. Determine the quantity of heat required to be added or removed from the reactor.

Basis of calculation: $1$ mole of methane fed.

$C{H}_4(g)+O_2(g)----C{H}_{3}OH(g)$

$($Given: the Constant heat capacity, $Cp,$ of $C{H}_4(g),O(g)$ and $C{H}_{3}OH(g)$ are $0\mathrm{.}08,0\mathrm{.}028$ and $0\mathrm{.}077k\frac{J}{m}olC$ respectively$).$ You can use $Cp02$ or table $8$ for calculation.

Feed temperature: $50C$ for Methane; $100C$ for Oxygen

Product temperature: $200C$

Standard Heat of reaction is $-126\mathrm{.}35k\frac{J}{m}ol$

Determine the molar flow rate of the product stream components based on the symbols used in the below inlet$-$outlet enthalpy table. You are required to use the heat of reaction method for the energy balance. Write the answers in the table below.

Reference states: at $25C$ latm