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## Gas constant
The mole (rather than energy per kelvin per particle).
Its value is: *R*= 8.314472(15) J · K^{-1}· mol^{-1}
The two digits in parentheses are the uncertainty (standard deviation) in the last two digits of the value. The gas constant occurs in the simplest equation of state, the ideal gas law, as follows: where *P*is the pressure*T*is (absolute) temperature-
*V*is the volume the gas occupies -
*n*is the amount of gas (loosely*number of moles*) -
*V*_{m}is the molar volume
## Additional recommended knowledge
## Relationship with the Boltzmann constantThe Boltzmann constant k) may be used in place of the gas constant by working in pure particle count, N, rather than number of moles, n, since R = N_{A}k_{B}, where N_{A} is Avogadro's number. For example, the ideal gas law in terms of Boltzmann's constant is:
## Specific gas constantThe It is common to represent the specific gas constant by the symbol The specific gas constant of dry air is ## US Standard AtmosphereThe US Standard Atmosphere, 1976 (USSA1976) defines the Universal Gas Constant as: The USSA1976 does recognize, however, that this value is not consistent with the cited values for the Avogadro constant and the Boltzmann constant. ## See also## References |
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This article is licensed under the GNU Free Documentation License. It uses material from the Wikipedia article "Gas_constant". A list of authors is available in Wikipedia. |