I keep getting this wrong. In a collision of sufficient force, automobile air bags respond by electrically triggering the explosive decomposition of sodium azide (NaN3) to its elements....

Question

A 33.4−g sample of sodium azide was decomposed, and the nitrogen gas generated was collected over water at 26°C. The total pressure was 757.0 mmHg. How many liters of dry N2 were generated? Do not answer in scientific notation.

The last answer I got was 17.24 L N₂ and it was incorrect.

Answer 1

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