Ideal gas law states that there are no inter molecular attractions between gas molecules and that ideal gas does not occupy space therefore having no volume. However, a real gas does have intermolecular attractions and does have a volume.
A 'real' gas would occupy a higher volume as compared to the same amount of gas would have when 'idealistically' calculated by the 'ideal' gas law. The 'eigen' volume (its own molecular dimension) is to be taken in account at high pressure.
The volume of gas in a cubic meter is one cubic meter. But perhaps that is not the real question?
The volume of a gas is dependent on the pressure and temperature of the gas.
The gas molecules interact with one another
No. As a gas contracts you are only reducing the volume between the atoms/molecules. The atoms/molecules of a real gas have their own volume that does not change with temperature.
The molecules of real gas have some volume and some attraction for each other.
It is less
No, that's why you call it real gas. For an ideal gas the size of the particle, that means the volume of interaction is zero, for real gases not. An effect of real gases is the cool down (or heat up) of an gas which is expanded (compressed). Another effect is that you can get liquids.
Ideal gas law states that there are no inter molecular attractions between gas molecules and that ideal gas does not occupy space therefore having no volume. However, a real gas does have intermolecular attractions and does have a volume.
An ideal gas would have zero volume at zero kelvin. This is an idealization, and it won't happen with a real gas. Also, real substances can't be cooled down to zero kelvin.
they have no volume and their molecular force of attraction is negligible
A 'real' gas would occupy a higher volume as compared to the same amount of gas would have when 'idealistically' calculated by the 'ideal' gas law. The 'eigen' volume (its own molecular dimension) is to be taken in account at high pressure.
The volume of gas in a cubic meter is one cubic meter. But perhaps that is not the real question?
The volume of a gas - at constant pressure - is proportional to the absolute temperature, that is, to the temperature expressed in Kelvin. This relationship is only approximate for real gases, but it is close enough for most practical purposes.
Real gases are those we encounter in the real world- hydrogen oxygen, nitrogen, argon, water vapour. An ideal gas is one that obeys the ideal gas law, usually expressed as PV=nRT. No real world gas follows this law although it is a good predictor of their behaviour as pressure, P, volume, V, temperature, T and number of moles, n, change.
The volume of a gas is dependent on the pressure and temperature of the gas.