Assume that you have 1.65g of nitroglycerin in a .614 L steel container at 293 K
ID: 753470 • Letter: A
Question
Assume that you have 1.65g of nitroglycerin in a .614 L steel container at 293 K and 1 atm pressure. An explosion occurs, raising the temperature of the container and its contents to 698 K. The balanced equation is: 4 C3H5N3O9 (l) -> 12 CO2 (g) + 10 H2O (g) + 6 N2 (g) +O2 (g) 1) How many moles of nitroglycerin were in the container orginally? I got this right: 7.27 X 10 ^-3mol 2) How many moles of gas (air) were in the container originally? I got this right. 2.55 X 10^-2 3) How many moles of gas are in the container after the explosion? Help!!! 4) What is the pressure (in atm) inside the container after the explosion according to the ideal gas law? Help!Explanation / Answer
. You know it was 1 atm at 293 degrees. You can assume it was filled with air, and you know the volume. Now you can calculate the moles of air. 3. That would be the air from part 2 plus the number of moles of gas generated from the reaction (.00705 times 12 +10 + 6 + 1). 4. Use the answer to 3 to correct the initial pressure for the increase in number of moles, and then correct for the temperature rise (*698/293).