Difference Between Ideal Gas And Real Gas

we can categories gases into two types: ideal gas and real gas. an ideal gas fulfills all the laws of gas at all conditions of pressure and temperature. on the other hand, real gas does not follow all gas laws at temperature and pressure. it does not behave like assumptions of the kinetic molecular theory of gases. the basic difference between Ideal Gas And Real Gas is that in an ideal gas, the volume occupied by molecules is negligible, does not obey the gas laws at also a force of attractions between molecules is negligible while in real gas occupied volume of gas molecules is not negligible, doe not obeys the gas laws, and attraction forces between molecules are not negligible.

Difference Between Ideal Gas And Real Gas in tabular Form

Ideal Gas Real Gas
Ideal gas obeys all gas laws Real gas obeys gas laws only at conditions of low pressure and high temperature.
An ideal gas has no definite volume real gas has a definite volume
Elastic collision Non-elastic collisions
There are no intermolecular forces of attraction between the molecules of gases. Either attractive or repulsive forces are present between the particles
no mass real gas has mass
No energy is involved during the collision of particles The collision of particles in real gas has to attract energy

Real Gas Vs. Ideal Gas – Overview

Real gases are the different gases around us. Ideal gas obeys all gas laws at all conditions of temperature and pressure. it is an imaginary concept developed to enhance our thinking on how these gases behave. No gas is ideal in the real world. An ideal gas does not condense.

Ideal Gas

In an ideal gas the pressure P, temperature T, and volume V are related by the gas law:

PV = nRT

Where R is the ideal gas constant and n is the number of moles of the gas. The ideal gas has molecules of negligible size with an average molar kinetic energy depends only on temperature. Most gases behave enough like ideal gases at low temperatures that the gas law can be applied for this. It is also known as a perfect gas. In the ideal gas, the molecules collide with each other elastically. The volume occupied by the molecules in an ideal gas is negligible as compared to the total volume. Intermolecular forces are not present between the molecules of gas. Ideal gases have high pressure and also obey PV =nRT.

Real Gas

Real gases do not behave like ideal gas due to interactions between gas molecules. It is also considered a nonideal gas as the behavior of a real gas is only approximated by the ideal gas law. Real gas at ordinary pressure behaves like an ideal gas, increasing its temperature or pressure increases the interactions between molecules, resulting in real gas behavior that cannot be predicted reliably using the ideal gas law.

A real gas does not obey gas laws at all standard pressure and temperature. These gases condense when cooled to their boiling point. Velocity, mass, and volume exist in real gases. The molecules of gas collide with each other inelastically. Either repulsive or attractive forces are present between the gas particles. A real gas exists in nature around us. According to ideal gas law, the van der Waals equation improves by adding two terms: one term for the volume of the gas molecules and the other terms for the forces of attraction between the gas molecules. Real gas obeys:


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