Gas laws
From Freepedia
The gas laws are a set of laws that describe the relationship between thermodynamic temperature (T), pressure (P) and volume (V) of gases. Three of these laws, Boyle's law, Charles's law, and Gay-Lussac's law come together to form the combined gas law, which with the addition of Avogadro's law later gave way to the ideal gas law. Other important gas laws include Dalton's law of partial pressures. The kinetic theory of gases, Graham's law of effusion, and root mean square velocity all explain how individual molecules in a gas act and their relation to pressure, volume, and temperature.
A gas which obeys these gas laws exactly is hypothetical and is known as an ideal gas (or perfect gas). An ideal gas does not exist, however: some gases follow the laws more closely than others given standard conditions.
The most important gas law is the ideal gas law which states that:
- <math>\qquad\qquad P V = n R T</math>
-where:
- P is pressure in atmospheres (atm) or kilopascals (kPa)
- V is volume in liters
- n is the number of moles of gas
- R is the ideal gas constant in L atm/mol K or Pa m³/mol K
- T is temperature in kelvins.
Other gas laws, such as van der Waals equation, seek to eliminate the value differences between the ideal gas laws and the actual gases. The van der Waals equation alters the ideal gas law to more truely reflect how actual gases function using a series of calculated values called van der Waals constants.
See also
References
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