In this activity, you are tasked with designing an airbag for a company that creates airbags for automobiles. You must design the driver’s front airbag for a specific car model so it will protect the driver as effectively as possible. For this car, the airbag must have a volume of 58 liters when fully inflated. To provide an adequate cushion for the driver’s head, the air pressure inside the airbag should be 4.4 psi. This pressure value is in addition to the normal atmospheric pressure of 14.7 psi, giving a total absolute pressure of 19.1 psi, which equals 1.30 atmospheres.

PART B

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.

PV = nRT

P(58) = nRT

P = 1.3 atm
V = 58 liters
n = ?
R = .082 (L - atm) / (mol * k)
T = 768 k
1.3 * 58 = n * .082 * 768 (1/mol)
75.8 / ( .082 * 768 ) moles = n
n = 1.19728 moles of N2

For anyone who has this I have the answers for the unit activity, feel free to ask me for the other ones too.