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3 years ago

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

Chemistry

1 answer:

Andru [333]3 years ago

6 0

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.

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Number of O atoms in 0.20 moles Ba(OH)2 = 2*0.20 = 0.40 moles O atom

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