Boyle's Law simply describes the relationship between the pressure and volume of an enclosed gas when Temperature remains constant. That relationship, usually expressed as P1V1 = P2V2, just means that the product of pressure x volume remains unchanged as either or both are changed.
Since pressure x volume remains constant, for example, doubling the pressure on an enclosed gas will reduce its volume to 1/2 its previous size. Tripling the pressure will reduce its volume to 1/3, and so on. Alternatively, if you double the volume available to an enclosed gas, pressure is halved.
The simplest demonstration of Boyle's Law is a hand bicycle pump. By pushing down on the
piston, the reduced volume increases the pressure of the air inside so that it is forced
into the tire. Because pressure changes will have an affect on temperature (feel the pump after a few seconds of pumping), temperature must be allowed to return to its prior value
for Boyle's Law to hold true.
Paul Walorski, B.A., Part-time Physics/Astronomy Instructor
Boyle's Law is a statement of the relationship between the pressure and volume of gasses. Specifically it states that under isothermic conditions, the product of the pressure and volume remains constant, or
P1 x V1 = P2 x V2
where P1 is the pressure before some change, V1 is the volume before the change, P2 and V2 are the new values after the change. Another way of thinking about this law is that the values of pressure and volume are inversely proportional; if one goes up, the other must decrease by the same factor. If you trap gas in a cylinder, and then reduce the internal volume of the cylinder to half its original value, the pressure will double.
Why does this happen? If you squeeze those gas molecules from the above example into half the volume, you would expect them to be packed closer together and to slam into the sides of the container more often. The sum of all those little collisions is what we call pressure.
Rob Landolfi, Science Teacher, Washington, DC
'If one wishes to obtain a definite answer from Nature one must attack the question from a more general and less selfish point of view.'