New automobiles are now equipped with airbags. Many that inflate with N2 use the

Question

New automobiles are now equipped with airbags. Many that inflate with N2 use the rapid reaction of NaN3 + Fe2O3 which is initiated by a spark. How many grams of NaN3 (sodium azide) would be required to provide 75.0 L of N2 at 25 degrees C and 748 mmHg? 6 NaN3 (s) + Fe2O3 (s) --> 3 Na2O (s) + 2 Fe (s) + 9 N2 (g) 9. New automobiles are now equipped with airbags. Many that inflate with N2 use the rapid reaction of NaN3 + Fe203 which is initiated by a spark. How many grams of NaN's (sodium azide) would be required to provide 75.0 L of N2 at 25°C and 748 mmHg? of NaN3 (sodium azide) would be 6 NaNs ) Fe203 6) 6 NaN3 (s) Fe203 (s) 3 Na20 () + 2 Fe (6)9 N2(8)

Explanation / Answer

P = 748 mm Hg

   = 0.98 atm

V= 75 L

T = 273 + 25 =298 K

R = universal gas constant = 0.0821 L-atm / K mol

PV = n RT

n = PV / RT

    = 0.98 x 75 / 0.0821 x 298

     = 3 moles

nitrogen moles =3

6 NaN3 (s) + Fe2O3 (s) --------------> 3 Na2O (s) + 2 Fe (s) + 9 N2 (g)

6 mole NaN3       = 9 moles N2 (from balanced equation)

   2 moles NaN3 = 3 moles N2   (calculated)

mole = weight / molecular weight

2 = weight / 65

weight = 130 g

weight of NaN3 = 130 g

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