# A technician is designing an airbag for a new model car. She wants to use 72.0g of sodium azide (NaN_3) to inflate the bag at 22.0°C and 1.00 atm. What is the maximum volume of the airbag under these conditions?

Mar 10, 2016

Approx $40$ $L$. Hopefully, this is enough to stop you banging your nut on the dash.

#### Explanation:

We need the azide decomposition reaction:

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

else,

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

I divided the soithciometric coefficients to make things a bit easier on myself.

So, moles of sodium azide $=$ $\frac{72.0 \cdot g}{65.01 \cdot g \cdot m o {l}^{-} 1}$ $=$ $1.11 \cdot m o l$.

So $1.66$ $m o l$ dinitrogen gas can be evolved under these conditions.

And, $V$ $=$ (1.66*cancel(mol)xx0.0821*L*cancel(atm)*cancel(K^-1)*cancel(mol^-1)xx295cancelK)/(1*cancel(atm) $=$ ?? $\text{litres}$