Answer :
None of the above. There is no force of attraction between gas particles and between the particles and the container walls. Interactions with the package's walls and gas particle collisions are both completely elastic.
Because the observed connections between a gas's pressure, volume, and temperature are typically not perfect, the gas laws do not adequately account for these interactions. In this section, the reasons for these aberrations from the conduct of an inert gas are considered.
Gas molecules behave almost exactly like ideal gas particles at relatively low pressures because they are (on average) so widely apart and have virtually no attraction for one another. However, the force of attraction is also no longer negligible at higher pressures. This force marginally reduces the pressure (assuming the volume is constant) or decreases the volume by drawing the molecules closer together (at constant pressure). Due to the molecules' lower KE in comparison to the attractive forces, which makes them less able to overcome these forces after interacting with one another, this change is more pronounced at low temperatures.
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