# Difference between revisions of "Ideal Gas Law"

m (remove fractions for better look (only takes up one line now)) |
m |
||

Line 7: | Line 7: | ||

*P is the [[pressure]] of gas; | *P is the [[pressure]] of gas; | ||

*V the [[volume]] the gas occupies; | *V the [[volume]] the gas occupies; | ||

− | *T the absolute [[temperature]] (meaning it must be in [[Kelvin]] or [[Rankine]]; | + | *T the absolute [[temperature]] (meaning it must be in [[Kelvin]] or [[Rankine]]); |

*n is the number of moles of the gas occupying the volume V; | *n is the number of moles of the gas occupying the volume V; | ||

*R is the [[gas constant]]. | *R is the [[gas constant]]. |

## Revision as of 17:21, 11 October 2007

The **ideal gas law**, is an equation of state for an ideal gas. It combines three gas laws (Dalton’s Law, Boyle’s Law and Charles' Law) into one equation:

- PV = nRT

where

- P is the pressure of gas;
- V the volume the gas occupies;
- T the absolute temperature (meaning it must be in Kelvin or Rankine);
- n is the number of moles of the gas occupying the volume V;
- R is the gas constant.

The gas constant can be expressed in any number of units, but the most common representations are 0.0821 or 8.314

## Ideal Gas

The equation is valid only for an ideal gas, the hypothetically perfect embodiment of a gas in which the particles (atoms or molecules) in the gas are spherical, identical, have no volume, and experience no intermolecular forces between them. All collisions between the particles or the particles and the container are perfectly elastic.

Since this is just a model, real gases only obey the ideal gas law approxamately, not perfectly. Generally, the ideal gas assumption is accurate for unreactive gases at high temperature and/or low pressure. A good rule of thumb is that the assumption can be used above room temperature and below 1 atmosphere of pressure.