Automotive air bags are inflated when a sample of sodium azide $(NaN_{3})$ is very rapidly decomposed as : $2 NaN_{3} (s) \to 2 Na (s) + 3 N_{2} (g)$ .
What mass of sodium azide is required to produce 336 litre of N₂(g) with density 1.25 g/L

Question

Automotive air bags are inflated when a sample of sodium azide $(NaN_{3})$ is very rapidly decomposed as : $2 NaN_{3} (s) \to 2 Na (s) + 3 N_{2} (g)$ .

What mass of sodium azide is required to produce 336 litre of N₂(g) with density 1.25 g/L

TestHub · Accepted Answer

Given, V N 2 ​ ​ = 336 L , ρ = 1.25 g / L . m ( N 2 ​ ) = 336 × 1.25 = 420 g n ( N 2 ​ ) = 28 420 ​ = 15 m o l The reaction is 2 N a N 3 ​ → 3 N 2 ​ . From the stoichiometry, n ( N a N 3 ​ ) = 3 2 ​ × 15 = 10 m o l . The molar mass of N a N 3 ​ is M ( N a N 3 ​ ) = 23 + 3 ( 14 ) = 65 g / m o l . Therefore, m ( N a N 3 ​ ) = 10 × 65 = 650 g = 0.65 k g .

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