Real vs Ideal Gas: Pressure & Temperature Effects

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SUMMARY

A sample of air under high pressure and high temperature is classified as a real gas, as real gases exhibit molecular interactions that ideal gases do not. At elevated pressures, gas molecules are closer together, leading to interactions that deviate from ideal gas behavior. Conversely, at high temperatures, the kinetic energy of gas molecules increases, allowing them to behave more like ideal gases. Thus, the ideal gas laws provide a better approximation at low pressures.

PREREQUISITES
  • Understanding of gas laws, specifically the Ideal Gas Law
  • Knowledge of molecular interactions in gases
  • Familiarity with kinetic molecular theory
  • Basic concepts of thermodynamics
NEXT STEPS
  • Research the Ideal Gas Law and its limitations
  • Explore the concept of real gas behavior using Van der Waals equation
  • Study the effects of temperature on gas behavior in detail
  • Learn about kinetic molecular theory and its applications
USEFUL FOR

Students of chemistry, physicists, and anyone interested in thermodynamics and gas behavior will benefit from this discussion.

s.p.q.r
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If a sample of air had high pressure and high temperature, would it be a real or ideal gas?
 
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If it's air it is a real gas.
Generally at higher pressures gases become less 'real' as the molecules are closer together they interact - which ideal gases don't do.
In other words at low pressures the ideal gas laws are a better approximation.

Similairly at high temperatures the gas is moving around more so most of it's energy is kinetic rather than in any chemical properties of the molecules so it behaves more like an ideal gas.
 

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