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## Charles's law
*At constant pressure, the volume of a given mass of an ideal gas increases or decreases by the same factor as its temperature (in kelvin) increases or decreases.*
## Additional recommended knowledgeThe law was first published by Joseph Louis Gay-Lussac in 1802, but he referenced unpublished work by Jacques Charles from around 1787. This reference has led to the law being attributed to Charles. The relationship had been anticipated by the work of Guillaume Amontons in 1702. Charles's Law, Boyle's law, and Gay-Lussac's Law form the combined gas law. The three gas laws in combination with Avogadro's law can be generalized by the ideal gas law. ## DerivationThe formula for the law is: where: *V*is the volume of the gas*T*is the temperature of the gas (measured in Kelvins)*k*is a constant.
In other more thermodynamics-based definitions, the relationship between the fixed mass of a gas at constant pressure is inversely proportional to the temperature applied to the system, which can be further used by stipulating a system where α represents cubic expansivity of a gas, with θ representing the temperature measured of the system in Kelvins: *V*=*V*_{o}(1 + αθ)
To maintain the constant, - .
Therefore, as temperature increases, the volume of the gas increases. Theoretically as a gas reaches absolute zero the volume will also reach a point of zero. ## See alsoCategories: Thermodynamics | Gas laws |

This article is licensed under the GNU Free Documentation License. It uses material from the Wikipedia article "Charles's_law". A list of authors is available in Wikipedia. |