Question

The "air bags" that are currently installed in automobiles to prevent injuries in the event of a crash are equipped with sodium azide, NaN₃, which decomposes when activated by an electronic igniter to produce nitrogen gas that fills the bag. How many liters of nitrogen, measured at 25°C and 1.00 atm, will be produced by 100.0 g of NaN₃?

Answer 1

0.0177 L of nitrogen will be produced

Step-by-step explanation:

The decomposition reaction of sodium azide will be:

`2NaN_(3)(s)--->2Na(s)+3N_(2)(g)`

As per the balanced equation two moles of sodium azide will give three moles of nitrogen gas

The molecular weight of sodium azide = 65 g/mol

The mass of sodium azide used = 100 g

The moles of sodium azide used =
`(mass)/(molarmass)=(100)/(65)=1.54mol`

so 1.54 moles of sodium azide will give =
`(3X1.54)/(2)=2.31`mol

the volume will be calculated using ideal gas equation

PV=nRT

Where

P = Pressure = 1.00 atm

V = ?

n = moles = 2.31 mol

R = 0.0821 L atm / mol K

T = 25 °C = 298.15 K

Volume =
`(P)/(nRT)=(1)/(2.31X0.0821X298.15)=0.0177L`