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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?

Respuesta :

Answer:

0.0177 L of nitrogen will be produced

Explanation:

The decomposition reaction of sodium azide will be:

[tex]2NaN_{3}(s)--->2Na(s)+3N_{2}(g)[/tex]

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 = [tex]\frac{mass}{molarmass}=\frac{100}{65}=1.54mol[/tex]

so 1.54 moles of sodium azide will give = [tex]\frac{3X1.54}{2}=2.31[/tex]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 = [tex]\frac{P}{nRT}=\frac{1}{2.31X0.0821X298.15}=0.0177L[/tex]

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