Respuesta :
None of the above. Between gas particles or between the particles and the container walls, there is no force of attraction. Gas particle collisions and impacts with the container's walls are both fully elastic.
The observed correlations between a gas's pressure, volume, and temperature are frequently not ideal, which means that the gas laws do not fully capture these interactions. The causes of these departures from the behavior of an ideal gas are taken into account in this section.
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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