Does air behave like an ideal gas

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SUMMARY

Air behaves similarly to an ideal gas under normal conditions, such as room temperature and standard atmospheric pressure. While air is composed of various molecules, it can be approximated as an ideal gas for many engineering applications. This approximation holds true as long as the temperature, pressure, and volume remain within typical ranges. Understanding the properties of ideal gases is essential for accurate modeling in engineering contexts.

PREREQUISITES
  • Understanding of ideal gas laws
  • Familiarity with basic thermodynamics
  • Knowledge of atmospheric pressure and temperature conditions
  • Basic principles of molecular behavior in gases
NEXT STEPS
  • Research the Ideal Gas Law and its applications in engineering
  • Study the differences between real gases and ideal gases
  • Explore the impact of temperature and pressure on gas behavior
  • Learn about the kinetic molecular theory of gases
USEFUL FOR

Engineering students, physicists, and anyone interested in thermodynamics and gas behavior in practical applications.

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Homework Statement


Simple question, does air behave like an ideal gas. I have researched online and flipped through 3 textbooks but cannot find a simple explanation.

Homework Equations


none

The Attempt at a Solution


The closest answer i came up with is air is made up of molecules that behave similar to an ideal gas. I think the problem is I am not exactly sure what an ideal gas is. There's a lot of explanations with regards to chemical structure and what not but I am an engineering student.
 
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I think you can get away with assuming air is an ideal gas most of the time, as long as temperatures, pressures, and volumes are normal (like room temperature, etc.), but my answer might be kind of vague.
 

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