The methanol fuel $C{H}_{4}O($Liquid$)$ is burned with $134$ percent theoretical air, $(34$percent excess air$)$ at $298k$ at $1$atm at a rate of $0,5k\frac{g}{s}.$ Products are at $3$atm and $900K.$ An analysis of the combustion gases reveals that all the hydrogen in the fuel burns to $H_{2}O$ but Only $90$ percent of the corbon burns to $C{O}_2,$ with the remaining $10$ percent forming $CO$

a$)$ Write the combustion equation and find number of moles and $a_s(a_{+h}),$ and calculate?

b$)$ the mass flow rate of air $(k\frac{g}{s})?$

c$)$ The rate of heat transfer from the combustion chamber $($kw$)$ fuel