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Termsisothermin thermodynamics, a curve on a p-V diagram for an isothermal processBoyle’s lawthe absolute pressure and volume of a given mass of confined gas are inversely proportional, while the temperature remains unchanged within a closed systemideal gasa theoretical gas composed of a set of randomly-moving, non-interacting point particles

## Boyle’s Law

Boyle’s Law (sometimes referred to as the Boyle-Mariotte Law) states that the absolute pressure and volume of a given mass of confined gas are inversely proportional, provided the temperature remains unchanged within a closed system. This can be stated mathematically as follows:

## History and Derivation of Boyle’s Law

The law was named after chemist and physicist Robert Boyle, who published the original law in 1662. Boyle showed that the volume of air trapped by a liquid in the closed short limb of a J-shaped tube decreased in exact proportion to the pressure produced by the liquid in the long part of the tube.

Boyle’s LawAn animation of Boyle’s Law, showing the relationship between volume and pressure when mass and temperature are held constant.The trapped air acted much like a spring, exerting a force opposing its compression. Boyle called this effect “the spring of the air” and published his results in a pamphlet with that title. The difference between the heights of the two mercury columns gives the pressure (76 cm = 1 atm), and the volume of the air is calculated from the length of the air column and the tubing diameter.

The law itself can be stated as follows: for a fixed amount of an ideal gas kept at a fixed temperature, P (pressure) and V (volume) are inversely proportional—that is, when one doubles, the other is reduced by half.

Remember that these relations hold true only if the number of molecules (n) and the temperature (T) are both constant.

**Interactive: The Volume-Pressure Relationship**Gases can be compressed into smaller volumes. How does compressing a gas affect its pressure? Run the model, then change the volume of the containers and observe the change in pressure. The moving wall converts the effect of molecular collisions into pressure and acts as a pressure gauge. What happens to the pressure when the volume changes?

## Example

In an industrial process, a gas confined to a volume of 1 L at a pressure of 20 atm is allowed to flow into a 12-L container by opening the valve that connects the two containers. What is the final pressure of the gas?

Set up the problem by setting up the known and unknown variables. In this case, the initial pressure is 20 atm (P1), the initial volume is 1 L (V1), and the new volume is 1L + 12 L = 13 L (V2), since the two containers are connected. The new pressure (P2) remains unknown.

P1V1 = P2V2

(20 atm)(1 L) = (P2)(13 L).

20 atom = (13) P2.

P2 = 1.54 atm.

The final pressure of the gas is 1.54 atm.

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**Boyle**An introduction to the relationship between pressure and volume, and an explanation of how to solve gas problems with Boyle’s Law.

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