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.
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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.
- Boyle’s Law
- Charle’s law
- 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.