Question

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

2NaN3 ? 2Na +3N2
what mass of Sodium Azide is required to produce 2.6 feet3 (736 L) of Nitrogen gas with the density of 1.25 g/L?

Answer 1

141 g

Step-by-step explanation:

Answer 2

Answer: 1424 grams

Step-by-step explanation:

`2NaN_3\rightarrow 2a+3N_2`

`Density=(mass)/(Volume)`

`1.25g/L=(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}=(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=
`(2)/(3)* 32.8=21.9moles` of
`NaN_3`

Mass of
`NaN_3=moles* {\text {molar mass}}=21.9* 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.