A 1.02g sample of liquid nitroglycerin(C3H5N3O9) is placed in a 500.0ml steel container at 21°C and 1.00atm pressure (The density of nitroglycerin is 1.5931g/ml). The nitroglycerin explodes and the temperature rises to 425°C. The balanced equation for the reaction is:

4C3H5N3O9(l) → 12CO2(g) + 10H2O(g) + 6N2(g) + O2(g)

a. How many moles of nitroglycerin and how many moles of gas(air, assume no nitroglycerin vapors present)were in the container originally?

b. How many total moles of gas are in the container after the explosion?

c. What is the pressure(in atm) inside the container after the explosion assuming ideal behavior for the gases?

d. What is the partial pressure(in atm) of N2 in the container after the explosion?