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Boyle’s Law Relate to Gas Compression

Boyle's law, also referred to as the Boyle–Mariotte law in France, is an experimental gas principle that describes how a gas's pressure is proportional to its volume.

Boyle’s law, also referred to as the Boyle–Mariotte law in France, is an experimental gas principle that describes how a gas’s pressure is proportional to its volume. It explains how the gas pressure rises when the container’s capacity decreases. In modern scientific terms, it could be described as follows: If the amount of gas and temperature remain constant in a closed system, the relative pressure applied by a given mass of the ideal gas is inversely proportional to the volume.

What is Boyle’s law?

According to Boyle’s law, “within a closed system, the absolute pressure which is exerted by a mass of an ideal gas is inversely proportional to the volume occupied by it if the quantity of the gas and temperature of the gas remain unchanged.”

Boyle’s law can be expressed as,

P ∝ 1/V

Above, P is a pressure of a gas 

V is the volume of gas.

It means that if temperature is kept constant and no. moles or volume of gas is kept constant, the volume of gas would reduce when the pressure is increased, and the volume of the gas will expand when the pressure is reduced.

When we remove the proportionality by using constant k

PV = k

P1V1 = P2V2 = P3V3 = k (Constant)

P1 denoted the initial pressure

V1 denoted the initial volume

P2 denoted the final pressure

V2 denoted the final volume

This statement states that if the temperature is constant, the system will receive the same quantity of energy during its operation, and hence the significance of the value of k would always remain constant. Because pressure is calculated as the perpendicular force applied and probabilistic like of colliding with other atoms using the concept of the theory of collision, the application of the power to the surface may not be always constant for the values of v. Still, it might have the limits when comparing such a value over time. When vol. V of a certain quantity of the gas is forced to increase while the gas temperature remains constant, the pressure (denoted by p) would fall accordingly.

To put another way, decreasing volume of gas puts more pressure. The law of the Boyle is used to predict the outcome of changing initial state of the constant quantity of the gas only in volume and pressure. We use and apply this concept or idea in our daily lives, even when we make the food in the pressure cooker. When the inside of the cooker boils completely, the rice is supposed to cook. At atmospheric pressure, we all dwell on Earth, which is equivalent  to the weight of 13mm of the Mercury. Water to cook rice boils at just 100 degrees C under atmospheric pressure. By raising the weight the pressure inside that vessel rises up quickly, and the water in a large thick metal cooking pot is forced to boil at  lower temperature. As a result, the water quickly reaches a boiling point above 100 degrees Cel., and rice is cooked in the fraction of the time it would take in an uncovered vessel.

What are the examples of Boyle’s law?

When you squeeze an inflated balloon, the volume of the air within the balloon shrinks. As a result of Boyle’s law, this is characterised by an elevation in the pressure imposed by air in the balloon. As the balloon is pushed tighter, the pressure builds up until it pops. Below is a diagram that depicts the increase in blood pressure that occurs when the vol. of the gas decreases. The decrease in pressure caused by a scuba diver quickly ascending from a deep zone to the sea’s surface can induce the gas molecules in their body to expand. These gas bubbles can harm the diver’s organs and perhaps cause death. Another example of Boyle’s law is expanding the gas generated by the scuba diver’s ascent. Another similar example is deep-sea fish that die after approaching the water’s surface.


Boyle’s law is a fundamental concept in physics. This post focused on a deep examination of what the law is all about and how it works. The post also highlighted some crucial facts to remember that demonstrate Boyle’s law’s application. Above we read about the concept of an ideal gas, the meaning of a closed system, and the link between the terms of volume and temperature. An ideal gas is a theoretical gas made up of a large number of randomly movable discrete particles whose only connections are entirely elastic collisions. As it fulfils the ideal gas equation, a reduced equation of state, and is subject to statistical mechanics analysis, the ideal gas theory is beneficial. We hope that by reading this article, you gained a better understanding of Boyle’s law and were able to conclude from the numerous examples we discussed.


Frequently asked questions

Get answers to the most common queries related to the NEET UG Examination Preparation.

What is the most suitable example of Boyle's law?

Ans. A balloon exemplifies Boyle’s law in action. By pumping air into the balloon, air pressure pushes on the ...Read full

How does Boyle's law relate to gas compression?

Ans. Boyle’s law is like a hand pump for a bicycle. The volume of the gas diminishes as the piston is pushed d...Read full

What other laws can states of matter have that are important?

Ans. Main states of matter laws are Boyle’s law, Charles law, Gay-lussac’s law, Avogadro’s law.

Write the ideal gas equation in density and molar mass form.

Ans. PM=dRT  Where,  ...Read full

Is there another way to derive ideal gas laws instead of from Boyle’s Law, Charles’s Law, Avogadro’s Law and Gay-Lussac’s Law?

Ans. Yes. Ideal gas law can also be derived from the kinetic theory of gas.