Real gases tend to show ideal gas behavior under certain conditions of temperature and pressure. The conditions under which real gases behave ideally are typically high temperature and low pressure. Specifically, as the temperature increases and the pressure decreases, the behavior of real gases starts to approximate that of an ideal gas.
The ideal gas law, PV = nRT, describes the relationship between the pressure (P), volume (V), number of moles (n), gas constant (R), and temperature (T) for an ideal gas. Real gases deviate from ideal behavior due to intermolecular forces and the finite size of gas molecules.
At high temperatures, the kinetic energy of the gas molecules increases, resulting in more rapid and energetic motion. This increased molecular motion helps overcome the attractive forces between the gas molecules, reducing their impact on gas behavior. Consequently, real gases behave more ideally at higher temperatures.
At low pressures, the gas molecules are more spaced out, and the probability of molecular interactions decreases. As a result, the impact of intermolecular forces diminishes, and real gases approach ideal behavior.
It is important to note that no gas is truly ideal under all conditions, but some gases, such as noble gases, exhibit behavior close to ideal over a wider range of temperatures and pressures compared to other gases.