Author: workhouse123

The ideal gas law (PV = nRT) relates the macroscopic properties of ideal gases. An ideal gas is a gas in which the particles (a) do not attract or repel one another and (b) take up no space (have no volume).

The gas particles are equally sized and do not have intermolecular forces, such as attraction or repulsion, with other gas particles.

Helium Helium ( ) behave as an ideal gas. Due to the completely filled outer electron shell, it has a low tendency to react with other atoms also, It exists as a single atom, so the van der Waals dispersion forces are very less.

For example, the set of integers (ℤ) forms a ring with ordinary addition and multiplication. The set 3ℤ formed by multiplying each integer by 3 forms an ideal, and the quotient ring ℤ/3ℤ has only three elements: 0 + 3ℤ = 3ℤ = {0, ±3, ±6, ±9,…}

Examples of Ideal gases are – Hydrogen, Oxygen, Nitrogen and noble gases like Helium and Neon. These gases show behaviour that is very close to that of ideal gases at conditions of standard temperature and pressure (STP).

The properties of IDEAL gases are that:

Real Gas Examples Any gas that exists in nature is a real gas. Oxygen, hydrogen, carbon dioxide, helium, carbon monoxide, etc., are all examples of real gases. Ideal gas laws are derived by following certain conditions which do not support the existence of particles like gas molecules and their interactions

An ideal gas is a theoretical gas composed of many randomly moving point particles that are not subject to interparticle interactions. The ideal gas concept is useful because it obeys the ideal gas law, a simplified equation of state, and is amenable to analysis under statistical mechanics.