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What is the relationship between an ideal gas pressure and its volume?


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January 21, 2008 4:37AM

Firstly, an ideal gas is one consisting of identical particles with no volume. These particles feel no intermolecular forces and undergo perfectly elastic collisions with the all of the container. It is important to note that real gases do not exhibit these characteristics and that it merely provides an approximation. Though the heading "Ideal Gas" can be separated into two board sections, the classical thermodynamic ideal gas and the ideal quantum Boltzmann gas; from the question wording I'll assume it's the former we're dealing with (both are essentially the same, except that the classical thermodyamic ideal gas is based on classical thermodynamics alone). The classical ideal gas pressure, p, and its volume, V, are related in the following way: pV=nRT where n is the amount of gas in moles , R is the gas constant, 8.314J•K-1mol-1 (Joule Kelvin per mole) and T is the absolute temperature in Kelvin. Put simply : the relationship between pressure and volume is the that the change in pressure is inversly proportional to the volume. p= a/V where a is a constant; in this case (nRT).