Question #91cb4

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Question #91cb4

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Answer 1 · 2016-02-28T19:15:35

$2 N a N_{3} (s) \to 2 N a (s) + 3 N_{2} (g)$ $2NaN_3(s) rarr 2Na(s) + 3N_2(g)$ . Dinitrogen volume is approx. $34$ $34$ $L$ $L$ .

Explanation:

This reaction is apparently used to fill car air bags in the event of an accident. If there are $\frac{60.0 \cdot g}{65.01 \cdot g \cdot m o l^{- 1}}$ $(60.0*g)/(65.01*g*mol^-1)$ $=$ $=$ $0.923$ $0.923$ $m o l$ $mol$ , sodium azide, $1.38$ $1.38$ $m o l$ $mol$ dinitrogen gas are evolved.

Now, I assume a standard temperature of $298$ $298$ $K$ $K$ and a standard pressure of $1$ $1$ $a t m$ $atm$ (perhaps this is unjustified, but further information is absent). Under these circumstances, $1$ $1$ $m o l$ $mol$ of gas has a volume of $24.5$ $24.5$ $L$ $L$ . Under other conditions of temperature I could use the Ideal Gas equation: $V = \frac{n R T}{P}$ $V=(nRT)/P$ .

So, $24.5$ $24.5$ $L \cdot m o l^{- 1}$ $L*mol^-1$ $\times$ $xx$ $1.38$ $1.38$ $m o l$ $mol$ $=$ $=$ $? ?$ $??$ $L$ $L$ . Hopefully this is enough volume to stop your nut being banged into the dashboard.

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Question #91cb4

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