Calculate the equilibrium concentration of [N2] if the initial concentrations are 2.23 M N2 and 0.55 M O2. (This N2/O2 concentration ratio is the ratio found in air.) Express your answer to three significant figures and include the appropriate units.

n N2(g) = 15.367 mol

Explanation:

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:

∴ 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)