# How does sodium azide, used in air-bags, decompose?

$\text{Natrium azide}$ decomposes according..........
$\text{Natrium azide}$ decomposes according to the following stoichiometric equation:
$N a {N}_{3} \left(s\right) \rightarrow N a \left(s\right) + \frac{3}{2} {N}_{2} \left(g\right) \uparrow$
Given the stoichiometry, $\text{1.5 equiv}$ of dinitrogen gas are evolved per $\text{equiv}$ of the azide. We had $1.50 \cdot m o l$ azide, hence, $1.5 \times 1.5 \cdot m o l = 2.25 \cdot m o l$ $\text{dinitrogen gas}$. This is certainly enuff gas to fill an airbag under standard conditions, and hopefully prevent your nut from hitting the dash. Under standard conditions of $1 \cdot a t m$, and $298 \cdot K$, what volume would this gas occupy?