# Difference between revisions of "Ideal Gas Law"

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where | where | ||

− | * | + | *<math>P</math> is the [[pressure]] of gas; |

− | * | + | *<math>V</math> the [[volume]] the gas occupies; |

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

− | * | + | *<math>n</math> is the number of [[Mole (chemistry)|moles]] of the gas; |

− | * | + | *<math>R</math> is the ideal gas constant. |

+ | |||

+ | It can also be expressed in terms of the number of [[molecules]], <math>N</math> and the Boltzmann constant, <math>k_B</math> as: | ||

+ | :<math>PV = N k_B T</math> | ||

The ideal gas constant can be expressed in any number of units, but the most common representations are <math>0.0821\,L \cdot atm \cdot mole^{-1} \cdot K^{-1}</math> or <math>8.314\,J \cdot mole^{-1} \cdot K^{-1}</math> | The ideal gas constant can be expressed in any number of units, but the most common representations are <math>0.0821\,L \cdot atm \cdot mole^{-1} \cdot K^{-1}</math> or <math>8.314\,J \cdot mole^{-1} \cdot K^{-1}</math> |

## Revision as of 15:23, 22 November 2016

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:

where

- is the pressure of gas;
- the volume the gas occupies;
- the absolute temperature (meaning it must be in Kelvin or Rankine);
- is the number of moles of the gas;
- is the ideal gas constant.

It can also be expressed in terms of the number of molecules, and the Boltzmann constant, as:

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

## 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 point particles (have no volume) and experience no intermolecular forces. 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 approximately, 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.

## Density

With the molar mass (*M*), the ideal gas law can be used to calculate the density of a gas, .