Thermal Physics -> Chapter 4 ( Kinetic Theory of Gases )

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Last updated 4:41 AM on 10/11/26
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6 Terms

1
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State the assumptions behind the kinetic theory of gases.

  • Gas molecules behave as perfectly elastic spheres.

  • The volume of the gas molecule is negligible compared to the volume of the container in which the gas is contained.

  • Intermolecular attractive forces between the molecules are negligibly small.

  • The time of collision of a molecule with the wall of the container is negligibly small when compared with the time between two collisions of a molecule.


2
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State the formula for the kinetic theory of gases.

where P → pressure of gas, V → volume of gas, m → mass of a gas molecule, N → total number of molecules, v²̄ → mean square speed of the molecules

<p>where P → pressure of gas, V → volume of gas, m → mass of a gas molecule, N → total number of molecules, v²̄ → mean square speed of the molecules</p>
3
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Relationship between the density of a gas and its root mean square.

where vrms → root mean square speed, P → pressure of gas, ρ → density of gas

<p>where v<sub>rms</sub> → root mean square speed, P → pressure of gas, ρ → density of gas</p>
4
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Relationship between the absolute temperature of a gas and its root mean square.

where vrms → root mean square speed, R → universal gas constant, T → absolute temperature of the gas, M → molar mass of the gas

<p>where v<sub>rms</sub> → root mean square speed, R → universal gas constant, T → absolute temperature of the gas, M → molar mass of the gas</p>
5
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Mean kinetic energy of a gas molecule.

where NA → Avagadro’s constant, R → universal gas constant, T → absolute temperature of gas

<p>where N<sub>A</sub> → Avagadro’s constant, R → universal gas constant, T → absolute temperature of gas</p>
6
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Mean kinetic energy of a gas mole.

where R → universal gas constant, T → absolute temperature of the ga

<p>where R → universal gas constant, T → absolute temperature of the ga</p>