Automobiles are equipped with air bags that inflate on collision to protect the

Question

Automobiles are equipped with air bags that inflate on collision to protect the occupants from injury. Many such air bags are inflated with nitrogen, N2, using the rapid reaction of sodium azide, NaN3, and iron (III) oxide, Fe2O3, which is initiated by a spark. The overall reaction is

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

A: How many grams of sodium azide would be required to provide 74.6 L of nitrogen gas at 26 degrees celsius and 743 mmHg?

B: What is the pressure of nitrogen gas in atmospheres and the temperature of the gas in kelvin?

Explanation / Answer

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

PV   = nRT

   n = W/M

M = 28 g/mole for N2

V = 74.6L

P = 743mmHg   = 743/760 = 0.977atm

T = 26C0 = 26+273 = 299K

PV = WRT/M

W = PVM/RT

     = 0.977*74.6*28/0.0821*299   = 83.13g

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

6 moles of NaN3 produces 9 moles of N2

6*65g of NaN3 produces 9*28g of N2

6*65*83.13/9*28 = g of NaN3 produces 83.13g of N2

128.65g of NaN3 >>>> answer

B.

760mmHg   = 1atm

743mmHg = 1atm*743/760 = 0.977atm

C0 + 273 = K0

26+ 273 = 299K

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