Airbags and Chemistry?

Question

Here is the problem: In a certain car if 135g of solid sodium azide(NaN3<--subscript) is completely reacted.. how many liters of nitrogen gas is blown into the airbag? Balance the equation as well. Thanks to anyone for the effort!

The balanced equation is 2NaN3(subscript) --> 2Na+ 3N2(also a subsricpt)

Answer 1

The balanced equation is 2NaN3(subscript) --> 2Na+ 3N2(also a subsricpt)

Step 1: Determine the number of moles of N2 released.
2 moles of NaN3 creates 3 moles of N2, so 1 mole of NaN3 creates 1.5 moles N2.
NaN3's molar mass is 23 + 14*3 = 65 g/mol
135g / 65 g/mol = 2.077 mol NaN3 -> 3.114 mol N2

Step 2: Use the ideal gas law to find volume. Also, assume STP (Standard Temperature and Pressure)
Ideal gas law: PV = nRT
V = nRT/P
Where:
R = gas constant
T = temperature in Kelvin (273.15 K = 0C)
P = Pressure (100 kPa = 100000 N/m^2)
n = number of moles

V = 3.114 mol * 8.314472 (N * m /k*mol) * 273.15 K / 100000 N/m^2
V = 0.070722 m^3 * 1 L/0.001 M^3
V = 70.7 L N2 (solution!)