The chemical most commonly used in airbags is sodium azide, NaN3; it breaks down into solid sodium and nitrogen gas: 2NaN3 --> 2Na + 3N2 If an airbag has a volume of 55 L, what mass of sodium azide would be needed?

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anor277 Share
Feb 10, 2018

Answer:

Approx. #250*g# of azide are required....the gas is assumed expand to 1 atmosphere or slightly over...

Explanation:

Given #NaN_3(s) rarrNa(s) + 3/2N_2(g)#...

...we need a mass of sodium azide so as to fill a #60*L# volume at room temperature, and one atmosphere pressure....in other words we solve for volume in the Ideal Gas equation...

#V=(nRT)/P#...and so #n=(PV)/(RT)#

#(1*atmxx60*L)/(0.0821*(L*atm)/(K*mol)xx298*K)=2.45*mol#.

But given the stoichiometry of the reaction, we need 2/3 equiv with respect to sodium azide... a mass of....

#2.45*molxx2/3xx65.01*g*mol^-1=??*g#

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