What happens to real gases under high pressure according to deviations from ideal gas laws?

Under conditions of high pressure, real gases do not behave according to ideal gas laws, and one significant deviation observed is related to the volume of the gas particles themselves. In ideal gas behavior, it is assumed that gas particles have no volume and do not interact with each other. However, at high pressures, the actual volume of the gas particles becomes significant compared to the volume of the container.

As the pressure increases, the distances between particles decrease, and the finite size of these particles cannot be ignored. Therefore, their collective volume takes up a more substantial portion of the total volume available in the container, leading to deviations from the behavior predicted by the ideal gas law. This is why the correct answer is that the volume of the particles is significant under high pressure conditions.

In contrast, under high pressure, the other statements about the behaviors of gases would not hold true. For instance, the idea that gas behaves more like an ideal gas would generally contradict the observed behavior since real gases diverge from the ideal model when subjected to high pressures. Similarly, while the volume of particles becomes more relevant, significant temperature increases are not a necessary consequence of high pressure in the context of ideal versus real gas behaviors.