What is the Relationship Between Gas Volume and Its Properties?

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SUMMARY

The discussion centers on the relationship between gas volume and its properties, specifically addressing the definitions and behaviors of ideal and real gases. It clarifies that the volume of a gas is not simply the sum of atomic volumes, as gases occupy the entire space available to them. The conversation also highlights that temperature relates to the average kinetic energy of gas molecules rather than direct collisions. Furthermore, it explains that deviations from ideal gas behavior occur due to intermolecular attractions and the intrinsic volume of gas molecules, impacting compressibility under high pressure.

PREREQUISITES
  • Understanding of ideal gas laws and real gas behavior
  • Familiarity with kinetic molecular theory
  • Knowledge of thermodynamic principles, particularly temperature and pressure
  • Basic concepts of molecular interactions and compressibility
NEXT STEPS
  • Research the Van der Waals equation for real gases
  • Explore the concept of compressibility factors in gas behavior
  • Study the differences between isothermal and adiabatic processes in gases
  • Learn about the implications of intermolecular forces on gas properties
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Students of chemistry and physics, researchers in thermodynamics, and professionals in fields involving gas behavior and properties will benefit from this discussion.

f24u7
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Hi, I have a few question about gas and its volume

1. How to define the volume of gas (is it the sum of the volume of each atom)?

2. If ideal gas does not consider atom to occupy space, then how does it accounts for
the basic definition of temperature (the collision of atoms)

3. What is the deviations between ideal gas and real gas ( I really don't get this even
though I read the textbook several times, I will assume that the attraction between
atoms must play a big role in the deviations for I don't see the relations between the
deviations and finite volume)
 
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f24u7 said:
1. How to define the volume of gas (is it the sum of the volume of each atom)?

Voulme of atoms is constant, so this sum will be constant as well. Obviously it is not, so this definition sounds incorrect.

2. If ideal gas does not consider atom to occupy space, then how does it accounts for the basic definition of temperature (the collision of atoms)

I am not sure if I follow - temperature is not directly related to collisions. It is related to average energy of the gas atoms (molecules). Could be you have no idea to collide two atoms that don't have a size - you may try to imagine they interact like identical charges, repelling itself.

3. What is the deviations between ideal gas and real gas ( I really don't get this even though I read the textbook several times, I will assume that the attraction between
atoms must play a big role in the deviations for I don't see the relations between the
deviations and finite volume)

If atoms (molecules) don't have intrinsic volume, gas can be compressed into as small volume as you wish, you just have to use pressure high enough. However, if they have some intrinsic volume, at some point increasing the pressure will not change volume of the substance, its compressibility will abruptly change from close to 1 to much closer to zero. That's the end of ideality.
 
if my assumption for number 1 is incorrect then how do we define the volume of gas ( the space in which the gas is allow to move? then wouldn't it be infinity ?)
 
f24u7 said:
if my assumption for number 1 is incorrect then how do we define the volume of gas ( the space in which the gas is allow to move? then wouldn't it be infinity ?)

Yes; at equilibrium a gas fills its available volume.
 

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