# Question 91cb4

Feb 28, 2016

$2 N a {N}_{3} \left(s\right) \rightarrow 2 N a \left(s\right) + 3 {N}_{2} \left(g\right)$. Dinitrogen volume is approx. $34$ $L$.
This reaction is apparently used to fill car air bags in the event of an accident. If there are $\frac{60.0 \cdot g}{65.01 \cdot g \cdot m o {l}^{-} 1}$ $=$ $0.923$ $m o l$, sodium azide, $1.38$ $m o l$ dinitrogen gas are evolved.
Now, I assume a standard temperature of $298$ $K$ and a standard pressure of $1$ $a t m$ (perhaps this is unjustified, but further information is absent). Under these circumstances, $1$ $m o l$ of gas has a volume of $24.5$ $L$. Under other conditions of temperature I could use the Ideal Gas equation: $V = \frac{n R T}{P}$.
So, $24.5$ $L \cdot m o {l}^{-} 1$ $\times$ $1.38$ $m o l$ $=$ ??# $L$. Hopefully this is enough volume to stop your nut being banged into the dashboard.