The decomposition of sodium azide, 2 moles produce 3 moles of Nitrogen gas. If you do stoichiometry 33.4 grams of Sodium azide produces 0.771 moles of Nitrogen gas.

Use the equation PV= nRT

Volume = ?

n= 0.771

R= 0.082

T =273 + 26 = 299

P = 757 - 25.2 = 731. 8 torrYou need to subtract 25.2 because it is the vapor pressure of water and you need the volume of dry Nitrogen. The vapor pressure or aqueous tension of water at 26 degrees celsius is 25.2.

Now convert the pressure in atm. Pressure in mm of Hg must be converted into atm by dividing with 760 then the pressure in atm would be 0.963

0.963 atm * V = 0.771 mole * 0.082 lit- atm/kel-mol * 299

Solving for Volume in liters should be 19.63 liters

Can you please confirm the answer so that we do not need to redo it for someone else

Dawson H.

Yes, that is correct. The work makes sense too. Thank you!03/05/21