Question

Automotive air bags inflate when a sample of Sodium Azide NaN3 is very rapidly decomposed.

Answer 1

Answer: 1424 grams

Explanation:

$2NaN_3\rightarrow 2a+3N_2$

$Density=\frac{mass}{Volume}$

$1.25g/L=\frac{mass}{736L}$

$Mass=920g$

Thus mass of nitrogen produced is 920 g.

$\text{Number of moles}=\frac{\text{Given mass}}{\text{Molar mass}}$

$\text{Number of moles of nitrogen}=\frac{920g}{28g/mol}=32.8moles$

According to stoichiometry:

3 mole of $N_2$ are produced from= 2 mole of $NaN_3$

Thus 32.8 moles of $N_2$ are produced from=$\frac{2}{3}\times 32.8=21.9moles$ of $NaN_3$

Mass of $NaN_3=moles\times {\text {molar mass}}=21.9\times 65=1424g$

Thus 1424 grams of sodium azide is required to produce 736 L of Nitrogen gas with the density of 1.25 g/L.