The reaction below is used to produce nitrogen gas to inflate air bags in automobiles. Calculate how many grams of sodium azidide, NaN3, are needed to produce 4.1 mol nitrogen gas, which is the equivalent of inflating a 50 L air bag to a pressure of 2.0 atm at 300K.

10 NaN3 (s) + 2 KNO3 (s) => 16 N2 (g) + K2O (s) + 5 Na2O (s)

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Deanna HettingerLv2

17 Dec 2019

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Automotive air bags inflate when sodium azide, NaN₃, rapidly decomposes to its component elements:

2 NaN₃(s) 2 Na(s) + 3 N₂(g)
(a) How many moles of N₂ are produced by the decomposition of 1.50 mol of NaN₃?
(b) How many grams of NaN₃ are required to form 10.0 g of nitrogen gas?
(c) How many grams of NaN₃ are required to produce 10.0 ft³ of nitrogen gas, about the size of an automotive air bag, if the gas has a density of 1.25 g/L?

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Here is the overall reaction in an automobile air bag: 20 NaN3 (s)+ 6SiO2(s)+ 4KNO3(s) 32N2(g)+ 5Na4SiO4(s)+ K4SiO4 (s). Calculate how many grams of sodium azide (NaN3) are needed to inflate a 4.0 times 10^1 times 4.0 times 10^1 times 20 cm bag to a pressure of 1.15 atm at a temerature of 20 C. How much sodium azide is needed if the air bag must produce the same pressure at 10 C

"Air" bags for automobiles are inflated during a collision by the explosion of sodium azide, NaN₃. The equation for the decomposition is
2NaN₃(s) â 2Na(s) + 3N₂(g). What mass of sodium azide would be needed to inflate a 11.6-L bag to a pressure of 1.0 atm at 25Â°C?

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