Average kinetic energy of all gases are the same

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SUMMARY

The average kinetic energy of all gases is indeed the same at a given temperature, regardless of their molecular weights. This principle is rooted in the kinetic molecular theory, which states that temperature is a measure of the average kinetic energy of gas molecules. While gases like hydrogen and oxygen exhibit different molecular weights, their average kinetic energy remains constant at the same temperature, although individual molecules can possess a wide range of energies.

PREREQUISITES
  • Kinetic molecular theory
  • Understanding of temperature as a measure of energy
  • Basic knowledge of molecular weights
  • Familiarity with gas laws
NEXT STEPS
  • Study the kinetic molecular theory in detail
  • Explore the relationship between temperature and kinetic energy
  • Investigate the implications of molecular weight on gas behavior
  • Learn about the ideal gas law and its applications
USEFUL FOR

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

Amith2006
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Sir,
Is it true that the average kinetic energy of all gases are the same at the same temperature? For example at the same temperature the molecules of hydrogen, oxygen,etc. have the same energy irrespective of their different atomic weights.
 
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Amith2006 said:
Sir,
Is it true that the average kinetic energy of all gases are the same at the same temperature? For example at the same temperature the molecules of hydrogen, oxygen,etc. have the same energy irrespective of their different atomic weights.
Different gases (ie different molecular weights) have the same average molecular kinetic energy if they are at the same temperature. This is quite different than the molecules all having the same energy. The molecules individually can have almost any energy.

AM
 

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