Calculating Pressure w/ Nitrogen Molecules: Where to Start?

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SUMMARY

The discussion centers on calculating the pressure exerted by 6 x 1022 nitrogen molecules with an rms speed of 450 m/s in a volume of 2 x 103 cm3. The Ideal Gas Law and equations from the kinetic theory of gases are essential for this calculation. Participants emphasize the importance of understanding molecular speed and mass, specifically noting that nitrogen molecules have a mass of 28 amu. Utilizing these principles will lead to an accurate determination of pressure.

PREREQUISITES
  • Understanding of the Ideal Gas Law
  • Familiarity with kinetic theory of gases
  • Knowledge of root mean square (rms) speed
  • Basic concepts of molecular mass and units of measurement
NEXT STEPS
  • Study the Ideal Gas Law and its applications
  • Learn about the kinetic theory of gases and relevant equations
  • Explore calculations involving root mean square speed
  • Review unit conversions for pressure and volume in gas calculations
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Students in physics or chemistry, educators teaching gas laws, and anyone interested in thermodynamics and molecular behavior of gases.

cuddlylover
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If 61022 nitrogen molecules with an rms speed of 450m=s occupy a volume of 2103 cm3, what
is the pressure? Nitrogen molecules have a mass of 28 amu.


I have been giving this but have no idea where to start. Can somebody point me to a starting point so i can have a go at it.
 
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Ideal gas law i would guess
 
Have you met any of the equations from the kinetic theory of gases?
There are a couple that relate pressure of a gas to molecular speed etc.
 

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