Question

Assume that you have 1.60 g of nitroglycerin in a 657.0 mL steel container at 20.0 ∘C and 1.00 atm pressure. An explosion occurs, raising the temperature of the container and its contents to 425 ∘C. The balanced equation is
4C3H5N3O9(l)→12CO2(g)+10H2O(g)+6N2(g)+O2(g)
1. How many moles of nitroglycerin were in the container originally?

2.How many moles of gas (air) were in the container originally?

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

4.What is the pressure (in atmospheres) inside the container after the explosion according to the ideal gas law?

Answer 1

1. initial moles of nitroglycerin = w/Mwt = 1.6/227.1 = 0.007 mol

2. moles of gas (air) = PV/RT = 1*0.657/(0.0821*293) = 0.0273 mol

3. no of mol of gases produced = 0.007*(12/4)+0.007*(10/4)+0.007*(6/4)*+0.007*(1/4)

                               = 0.05 mol

   moles of gas (air) after explosion = gaseproduced + air

                                                        = 0.05+0.0273 mol

                                                         = 0.0773 mol

                                                         = 7.8*10^-2 mol

4. pressure after explosion(P) = nRT/V

                            = 0.078*0.0821*698.15/0.657

                            = 6.8 atm