Nylon (C6H11NO) burns as a gas in air. There is 8 times the amount of stoichiometric air available by moles. The reaction takes place at constant pressure. The initial fuel temperature is 300 C and the air is at 25 C. The reaction produces CO2, H2O (gas) and HCN in the molar ratio, HCN=CO2 ¼ 1=5. Other properties: Heat of formation of nylon¼135 kJ/mole Species Molar specific heats at constant pressure ðJ=K moleÞ Nylon (gas) 136 H2O 50 CO2 60 HCN 90 N2 35 O2 35 (a) Compute the heat of combustion for this reaction using data in Table 2.2. (b) Compute the temperature of the final state of the products for an adiabatic process