Boyle's law: Difference between revisions

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== Further Reading ==
== Further Reading ==
see [[Ideal gas law]]
see [[Ideal gas law]]
== Related topics  ==
[[Amonton's law]]
[[Avogadro's law]]
[[Boyle's law]]
[[Charles's law]]
[[Dalton's law of partial pressure]]
[[Ideal gas law]]
[[Gay-Lussac's law]]
[[Law of combining volumes]]
[[van der Waals equation]]
== References ==
"General Chemistry, 2nd Ed.", pp 103-117, D. D. Ebbing & M. S. Wrighton, Houghton Mifflin, Boston, 1987.
"General Chemistry with Qualitative Analysis, 2nd Ed.", pp. 263-278, Saunders College Publishing, Philadelphia, 1984.




[[Category:CZ Live]]
[[Category:CZ Live]]
[[Category:Chemistry Workgroup]]
[[Category:Physics Workgroup]]

Revision as of 08:33, 19 December 2007

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Boyle's law is a special case of the ideal gas law from which one may calculate either the pressure or the volume of gas. It was developed by Robert Boyle in the 1660s and describes an inverse relationship between the pressure (P) and the volume (V) of a fixed amount of gas at a fixed temperature. This law is only valid if BOTH temperature and the amount of gas is held constant.

Boyle's law (at fixed temperature and amount of gas)


Example Problem

Two liters of gas at 1 atm and 25C is placed under 5 atm of pressure at 25C. What is the final volume of gas?


or

Further Reading

see Ideal gas law