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For an air bag to work, it has to inflate full of nitrogen incredibly fast-within to
milliseconds of the collision. For a 60-liter cylindrical air bag to work property, the
nitrogen gas has to reach a pressure of 2.37 atm. At 25°G, how many moles of
nitrogen gas are needed to pressurize the air bag? Given, 0.0821 L-atm/mol-Kl

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tanisharawat014

5.8 moles of nitrogen gas are needed to pressurize the air bag.

What's the expression of Ideal gas equation?

  • Ideal gas equation is PV=nRT
  • P= pressure, V = volume, n= no. of moles of gas, R= universal gas constant, T = temperature of the gas

What's the no. of moles of nitrogen present in a 60L air bag at 2.37 atm pressure and 25°C temperature?

  • P= 2.37 atm, V = 60L, R= 0.0821 L-atm/mol-K, T = 25°C = 298K
  • n= PV/RT

= (2.37×60)/(0.0821×298)

= 5.8 moles

Thus, we can conclude that 5.8 moles of nitrogen gas are needed to pressurize the air bag.

Learn more about the ideal gas here:

brainly.com/question/20348074

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