Gas Laws

Gas laws state the relationship between the pressure, volume, and temperature of a gas.

Before starting the description of gas laws, we will learn about the basic properties of gases.

Properties of Gases:

  • Gases do not have a specific shape. It takes the shape in which it is stored.
  • Density is less compared to solids and liquids.
  • They expand when heated.
  • When pressure is applied to the gas, it compresses, and its volume decreases.

In this article, we will learn the three most important gas laws as listed below.

  1. Boyle’s Law
  2. Charle’s law
  3. Gay Lussac’s law

Let us discuss all these gas laws one by one.

1. Boyle’s Law

At constant temperature, the pressure P of a gas varies inversely with its volume V, or PV = k, where k is a constant.

2. Charle’s law

at constant pressure, the volume V of a gas is directly proportional to its absolute (Kelvin) temperature T, or V/T = k.

3. Gay Lussac’s law

The pressure of a fixed mass of gas is directly proportional to its absolute temperature if the volume is kept constant.

P1/T1 = P2/T2

Ideal Gas Equation:

Boyle’s law and Charle’s law can be joined to shape the ideal gas law, solitary speculation of the conduct of gases known as an equation of state, PV = nRT, where n is the number of gram-moles of gas and R is known as the universal gas constant. In spite of the fact that this law depicts the conduct of an ideal gas, it intently approximates the conduct of real gases.

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