Real gas molecules do occupy volume and it does have an impact on the behavior of the gas. These particles are in rapid, random, constant straight line motion. This motion can be described by well-defined and established laws of motion. There are no attractive forces between gas molecules or between molecules and the sides of the container with which they collide. In a real gas, there actually is attraction between the molecules of a gas.
Molecules collide with one another and the sides of the container.
Energy is conserved in these collisions, although one molecule may gain energy at the expense of the other. Energy can be transferred in collisions among molecules. Energy is distributed among the molecules in a particular fashion known as the Maxwell-Boltzmann Distribution. At any paticular instant, the molecules in a given sample of gas do not all possess the same amount of energy. The average kinetic energy of all the molecules is proportional to the absolute temperature.