The chemical most commonly used in airbags is sodium azide, NaN3; it breaks down into solid sodium and nitrogen gas: 2NaN3 --> 2Na + 3N2 If an airbag has a volume of 55 L, what mass of sodium azide would be needed?

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anor277 Share
Feb 10, 2018

Approx. $250 \cdot g$ of azide are required....the gas is assumed expand to 1 atmosphere or slightly over...

Explanation:

Given $N a {N}_{3} \left(s\right) \rightarrow N a \left(s\right) + \frac{3}{2} {N}_{2} \left(g\right)$...

...we need a mass of sodium azide so as to fill a $60 \cdot L$ volume at room temperature, and one atmosphere pressure....in other words we solve for volume in the Ideal Gas equation...

$V = \frac{n R T}{P}$...and so $n = \frac{P V}{R T}$

$\frac{1 \cdot a t m \times 60 \cdot L}{0.0821 \cdot \frac{L \cdot a t m}{K \cdot m o l} \times 298 \cdot K} = 2.45 \cdot m o l$.

But given the stoichiometry of the reaction, we need 2/3 equiv with respect to sodium azide... a mass of....

2.45*molxx2/3xx65.01*g*mol^-1=??*g

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