Behaviour of Real Gas like an Ideal Gas
Real gases are non-ideal gases because real gases' molecules occupy space and interact, contravening the ideal gas law. The following factors must be considered in order to comprehend how real gases behave: variable specific heat capacity, van der Waals forces, non-equilibrium thermodynamic effects, problems with molecular dissociation, and elementary reactions with variable composition are just a few of the effects of compressibility.
- The ideal gases are the classical or Maxwell–Boltzmann ideal gas, the ideal quantum Fermi gas, and the ideal quantum Bose gas.
- The ideal gas model can fail at higher pressures or lower temperatures.
- The failure is possible for many refrigerants and for gases with strong intermolecular forces.
An ideal gas has the following characteristics:
- They are tiny, point-sized molecules with negligible volume.
- The gas-particle interactions are not influenced by an attractive or repelling force.
- The collision between the gases and the container's walls needs to be completely elastic (there is no loss of energy).
- It adheres to the gas law, i.e. P V = n R T (where P is the gas pressure, V is volume, n is moles, R is the universal gas constant of 8.314 J/mol-K, and T is temperature).
A Real Gas Behaves Like an Ideal Gas at
A real gas behaves like an ideal gas at higher temperatures and lower pressure. It happens because the potential energy starts to pale in comparison to the kinetic energy. Additionally, the distance between molecules becomes more important than the size of the molecules themselves. Some gases like oxygen, nitrogen, carbon dioxide, hydrogen, noble gases, and mixtures such as air can be considered ideal gases within reasonable tolerances.