One of the main components of an airbag is the gas that fills it. as part of the design process, you need to determine the exact amount of nitrogen that should be produced. calculate the number of moles of nitrogen required to fill the airbag. show your work. assume that the nitrogen produced by the chemical reaction is at a temperature of 495°c and that nitrogen gas behaves like an ideal gas. use this fact sheet to review the ideal gas law.
n N2(g) = 15.367 mol
airbags generally vary between 35 and 60 liters in volume and for the airbag system to activate, it takes about 20 Kgf/cm² of pressure; with this data taken from literature and knowing the temperature of reaction (495 °C), we determine the moles of nitrogen needed from the ideal gas law.
ideal gas law:PV = RTn
∴ P = 20 Kgf/cm² * ( 0.9678 atm / Kgf/cm² ) = 19.356 atm
∴ V = 50 L average volume
∴ R = 0.082 atm * L / K * mol
∴ T = 495°C + 273 = 768 K
⇒ n = PV / RT
⇒ n = ((19.356 atm) * (50 L)) / ((0.082atm*L/K*mol) * (768K))
⇒ n = 15.367 mol N2(g)
Nowadays cars have common availability of airbags installed in it for safety purposes. The main ingredients for producing hydrogen gas inside the bags are , and .The temperature at collision increases and is converted into sodium metal and Nitrogen gas which fills the bag.
One mole of any in three will contain three molecules of Nitrogen
N=3 x NA
Nitrogen is an inert gas a normal air bag require 70 liters of Nitrogen which means the approximate amount of needed will be 130g.