The air bags in cars are inflated when a collision triggers the explosive, highly exothermic decomposition of sodium azide (NaN3): 2NaN3(s) → 2Na(s) + 3N2(g) The passenger-side air bag in a typical car must fill a space approximately four times as large as the driver-side bag to be effective. Calculate the mass of sodium azide required to fill a 113-L air bag. Assume the pressure in the car is 1.00 atm and the temperature of N2 produced is 85°C.

Answer : The mass of required is, 166.4 grams.

Explanation :

First we have to calculate the moles of nitrogen gas.

Using ideal gas equation:

where,

P = Pressure of gas = 1.00 atm

V = Volume of gas = 113 L

n = number of moles  = ?

R = Gas constant =

T = Temperature of gas =

Putting values in above equation, we get:

Now we have to calculate the moles of sodium azide.

The balanced chemical reaction is,

From the balanced reaction we conclude that

As, 3 mole of produced from 2 mole of

So, 3.84 moles of produced from moles of

Now we have to calculate the mass of

Molar mass of = 65 g/mole

Therefore, the mass of required is, 166.4 grams.

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