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.

water is used to store them because it would keep the radiation from getting out in the open and causing harm to the workers