Posted by Jim on .
The ¡°air¡± that fills the airbags installed in automobiles is actually nitrogen gas produced by the
decomposition of sodium azide, NaN3. Assuming that the decomposition of sodium azide produces both
nitrogen and sodium metal (Na), what volume, in litres, of nitrogen gas is released from the
decomposition of 1.88 g of sodium azide? The pressure is 755 torr and the temperature is 24oC.
Complete this question showing all of your work

Chemistry 
DrBob222,
Write and balance the equation.
Convert 1.88 g NaN3 to mols. mol = grams/molar mass.
Using the coefficients in the balanced equation, convert mols NaN3 to mols N2.
Now convert mols N2 at the conditions listed by using PV = nRT and solving for L. Remember P must be in atm and T in kelvin. 
Chemistry 
Jo,
Answer is 1.104L

Chemistry 
Jo,
Answer is 1.104L Oh remember that there are 0.028 mol in 1.88g of NaN2. Final, in 0.028mol of NaN3, there is 0.042 mol of N2. This is your n.
so, V= ( nRT)/P remember, you are given R, T and P
Hope this helps:)