The kinetic theory assumes that, for an ideal gas, the volume taken up by the molecules themselves is entirely negligible compared with the volume of the container. For a real gas, that assumption isn't true. The molecules themselves do take up a proportion of the space in the container. The space in the container available for things to move around in is less than the measured volume of the container.
After reading the above, my interpretation of volume of gas is that the space for the molecules to move around. When we consider the volume of molecules, then the space for it to move around reduces. But according to my interpretation the volume of real gas must be lower than the volume of ideal gas which is not true.
When we talk about volume of gas, is it the sum of volume of molecules and space between them?
If that is the case then,
- When we talk about volume of ideal gas, we are considering the volume of the container which is the sum of volume of molecules and the space in between them. Then what do we take into account when we say volume of molecule is negligible as compared to volume of container?
It might be a basic question, but I didn't get any answer to it till now(from my teachers and other websites). Hope i'll get it cleared in CSE.