A furnace burns 28 mole of methane with balance amount of oxygen. All the methane is combusted according to the equation:

CH₄ (g)+ 2 O₂ (g) CO₂ (g) + 2 H₂O (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 336 C. Calculate the energy released by the furnace (kJ).

Note : although H₂O 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)} = 0.035 kJ/mol.C

C_{P, H2O (l)} = 0.0754 kJ/mol.C

C_{P, CO2} = 0.042 kJ/mol.C

C_{P, O2} = 0.038 kJ/mol. C

C_{P, CH4} = 0.043 kJ/mol.C