Boyle's law: Difference between revisions

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== 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?


<math> \left(P_\mathrm{i}V_\mathrm{i}\right) = \left(constant\right) = \left(P_\mathrm{f}V_\mathrm{f}\right) </math> or
<math> \left(V_\mathrm{f}\right) = \left(\frac{P_\mathrm{i}V_\mathrm{i}}{P_\mathrm{f}}\right) </math>
<math> \left(V_\mathrm{f}\right) = \left(\frac{(1 atm)(2 L)}{(5 atm)}\right) = 0.4 L </math>


== Further reading ==
== Further reading ==

Revision as of 13:13, 19 March 2008

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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)



Further reading

see Ideal gas law

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