Question 1 (20) Assume ideal gas properties, consider a 500 mL cylinder that contains a mixture of heptane and air at 350K, and 1 atm. C7H16 + 11027CO2 + 8H20 The oxygen is at 10% excess. 1. How many moles of oxygen, nitrogen and heptane are in the cylinder? 2. The gases are compressed adiabatically to a pressure of 11 atm. Use y = 1.4 for all the gases. What is the volume vad and temperature Tad? 3. The heptane is completely oxidized, find the composition of the products in moles (.e. carbon dioxide, steam, oxygen and nitrogen) k] 4. The heat of combustion of heptane is AH comb = 48 = 4.8MJ/mol. Use the specific heat capacities from the Table, calculate the rise in temperature from T'ad- gram Nitrogen 29.12 Steam 36 Oxygen 29.44 Carbon dioxide 37.35 Cp (J/mole/K) Heat released = AH combNheptane = =(ECp;n;)AT. The summation is over all the species in the table, AT is the rise in temperature due the combustion and Nheptane is the moles of heptane in the cylinder. 5. After the combustion reaction, the gases are at a temperature Tad +AT, and a volume of Vad: What is the pressure? (Remember to use the total moles after combustion in the calculation.)