What conditions must be fulfilled for an ideal gas?

For an ideal gas to be described accurately by the ideal gas law, certain conditions must be met, primarily involving low pressure and high temperature. Under these conditions, the gas particles are far apart, and the volume occupied by the individual gas molecules becomes negligible compared to the volume of the container. This allows for the assumptions of the ideal gas law, which include negligible intermolecular forces and elastic collisions, to hold true.

At high temperatures, the kinetic energy of the gas molecules is increased, which means the gas particles move more rapidly. This minimizes the impact of intermolecular forces, which are more prominent at lower temperatures and higher pressures. On the other hand, low pressure influences the ideal gas behavior by ensuring that the gas molecules do not experience significant collisions with one another, thus behaving as an ideal gas.

In contrast, high pressure tends to bring gas particles closer together, which can result in non-ideal behavior due to increased molecular interactions. Low temperature, especially as it approaches the condensation point, increases the likelihood of attractive forces influencing the behavior of the gas, leading to deviations from the ideal gas law. Therefore, the combination of low pressure and high temperature is essential for achieving the ideal gas behavior.