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Why are the constants a and b independent of temperature in gas properties?
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[QUOTE="BvU, post: 6016812, member: 499340"] Hello, indeed it is. But that is a 'different volume'. the ##b## in the [URL='http://hyperphysics.phy-astr.gsu.edu/hbase/Kinetic/waal.html']van der Waals equation of state[/URL] refers to the 'actual' volume of the molecules themselves. In other words: the equivalent volume of the molecules if they are considered as hard spheres. The volume the gas assumes under a given pressure and at a given temperature is much greater: most of that is simply empty space trough which the molecules move at considerable speeds. ##b## follows when you go to zero Kelvin and classically the molecules don't move any more. ##a## is a first correction on the pressure: in the [URL='http://hyperphysics.phy-astr.gsu.edu/hbase/Kinetic/ktcon.html#c1']ideal gas law[/URL] there are no intermolecular forces and ##pV = nRT##. In a real gas there is a small, almost always attractive, force between the molecules that reduces the pressure. [/QUOTE]
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Why are the constants a and b independent of temperature in gas properties?
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