Physics

Automobiles air bags are inflated with $$N_{2}$$ gas which is formed by the decomposition of solid sodium azide $$(NaN_{3})$$. The other product is $$Na - metal$$. Calculate the volume of $$N_{2}$$ gas at $$27^{\circ}C$$ and $$756\ Torr$$ formed by the decomposing of $$125\ gm$$ of sod azide.


SOLUTION
Sodium azide $$(NaN_3)$$ decomposes as:
$$2NaN_3\rightleftharpoons 2Na+3N_2$$
Here, we see that at STP,
$$2$$ moles of sodium azide produces $$3$$ moles of $$N_2=(22.4\times3)=67.2L$$ of $$N_2.$$
Or,
$$130g$$ of $$NaN_3$$ produces $$67.2$$ of $N_2$$ gas.
Here, $$P_1=1atm,T_1=273K, V_1=64.5L$$
Also given that, $$P_2=756$$ for  $$r=0.9atm.$$
$$T_2=27+273=300K$$
We have, $$\cfrac{P_1V_1}{T_1}=\cfrac{P_2V_2}{T_2}\\ \cfrac{1\times 64.6}{273}=\cfrac{0.9\times V_2}{300}\\\text{Volume of }N_2\text{ gas}=78.8L$$
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Subjective Medium Published on 18th 08, 2020
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