A furnace burns $26$ mole of methane with balance amount of oxygen. All the

methane is combusted according to the equation:

$C{H}_4(g)+2O_2(g)C{O}_2(g)+2H_{2}O(l)$

Methane and oxygen enter at $25C,$ while the products of the reaction $($combustion$)$

$($i$.$e$.$ the gas exiting through the exhaust of the furnace$)$ exit at $371C.$ Calculate the

energy released by the furnace $(kJ.$

Note : although $H_{2}O$ phase in the reaction equation is liquid, but the water that

comes out of the exhaust is in vapour phase. Boiling point of water at $1$atm is $100$

$C.$

Report your answer up to $1$ decimal point. Do not truncate any intermediate steps,

but only the final result

$C_{P,H2O(g)}=0\mathrm{.}035k\frac{J}{m}ol.C$

$C_{P,H2O(I)}=0\mathrm{.}0754k\frac{J}{m}ol.C$

$C_{P,CO2}=0\mathrm{.}042k\frac{J}{m}ol.C$

$C_{P,02}=0\mathrm{.}038k\frac{J}{m}ol.C$

$C_{P,CH4}=0\mathrm{.}043k\frac{J}{m}ol.C$