An ideal gas or perfect gas is a hypothetical gas consisting of identical particles of zero volume, with no intermolecular forces, where the constituent atoms or molecules undergo perfectly elastic collisions with the walls of the container and each other and are in constant random motion. Real gases do not behave according to these exact properties, although the approximation is often good enough to describe real gases.
These four properties that constitute an ideal gas can be easily remembered by the acronym PRIE, which stands for;
- Point masses (molecules occupy no volume)
- Random Motion (molecules are in constant random motion)
- Intermolecular forces (there are NO intermolecular forces between the particles)
- Elastic collisions (the collisions involving the gas molecules are totally elastic)
The ideal gas law is the equation of state of a hypothetical ideal gas, first stated by Benoît Paul Émile Clapeyron in 1834.
The state of an amount of gas is determined by its pressure, volume, and temperature
- n = number of moles
- R = universal gas constant = 8.3145 J/mol K
- N = number of molecules
- k = Boltzmann constant = 1.38066 x 10-23 J/K = 8.617385 x 10-5 eV/K
- k = R/NA
- NA = Avogadro's number = 6.0221 x 1023 /mo
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