Watch
Watching this resources will notify you when proposed changes or new versions are created so you can keep track of improvements that have been made.
Favorite
Favoriting this resource allows you to save it in the “My Resources” tab of your account. There, you can easily access this resource later when you’re ready to customize it or assign it to your students.
Boyle's Law: Volume and Pressure
Boyle's Law describes the inverse relationship between the pressure and volume of a fixed amount of gas at a constant temperature.
Learning Objectives

Describe Boyle's Law and its underlying assumptions

Apply Boyle's Law using mathematical calculations.
Key Points
 According to Boyle's Law, an inverse relationship exists between pressure and volume.
 Boyle's Law holds true only if the number of molecules (n) and the temperature (T) are both constant.
 Boyle's Law is used to predict the result of introducing a change in volume and pressure only, and only to the initial state of a fixed quantity of gas.
 The relationship for Boyle's Law can be expressed as follows: P1V1 = P2V2, where P1 and V1 are the initial pressure and volume values, and P2 and V2 are the values of the pressure and volume of the gas after change.
Terms

Boyle's law
the absolute pressure and volume of a given mass of confined gas are inversely proportional, while the temperature remains unchanged within a closed system

isotherm
in thermodynamics, a curve on a pV diagram for an isothermal process

ideal gas
a theoretical gas composed of a set of randomlymoving, noninteracting point particles
Full Text
Boyle's Law
Boyle's Law (sometimes referred to as the BoyleMariotte 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 Jshaped tube decreased in exact proportion to the pressure produced by the liquid in the long part of the tube.
Boyle's Law
An 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 VolumePressure 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 12L 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 (P_{1}), the initial volume is 1 L (V_{1}), and the new volume is 1L + 12 L = 13 L (V_{2}), since the two containers are connected. The new pressure (P_{2}) remains unknown.
P_{1}V_{1} = P_{2}V_{2}
(20 atm)(1 L) = (P_{2})(13 L).
20 atom = (13) P_{2}.
P_{2} = 1.54 atm.
The final pressure of the gas is 1.54 atm.
Boyle
An introduction to the relationship between pressure and volume, and an explanation of how to solve gas problems with Boyle's Law.
Key Term Reference
 Pressure
 Appears in these related concepts: SI Units of Pressure, Physics and Engineering: Fluid Pressure and Force, and Surface Tension and Capillary Action
 atom
 Appears in these related concepts: The Law of Multiple Proportions, Stable Isotopes, and John Dalton and Atomic Theory
 gas
 Appears in these related concepts: Osmotic Pressure, Bond Order, and New Energy Sources
 liquid
 Appears in these related concepts: Viscosity, The Halogens (Group 17), and Three States of Matter
 molecule
 Appears in these related concepts: Molecular Formulas, Levels of Organization of Living Things, and Chemical Reactions and Molecules
 system
 Appears in these related concepts: Exact Numbers, Definition of Management, and Comparison of Enthalpy to Internal Energy
 temperature
 Appears in these related concepts: Concentration of Cells, Capillary Action, and Temperature
 volume
 Appears in these related concepts: Volumes, Cylindrical Shells, and Line
Sources
Boundless vets and curates highquality, openly licensed content from around the Internet. This particular resource used the following sources:
Cite This Source
Source: Boundless. “Boyle's Law: Volume and Pressure.” Boundless Chemistry. Boundless, 21 Jul. 2015. Retrieved 22 Jul. 2015 from https://www.boundless.com/chemistry/textbooks/boundlesschemistrytextbook/gases5/gaslaws51/boyleslawvolumeandpressure2548360/