Among the four gases mentioned (H2, He, N2, and CO2), carbon dioxide (CO2) is known to exhibit greater non-ideal behavior compared to the others.
Non-ideal behavior in gases typically arises due to intermolecular interactions between gas molecules. In an ideal gas, the gas particles are assumed to have negligible volume and no intermolecular forces. However, in reality, gas molecules do interact with each other to some extent, and these interactions can lead to deviations from ideal gas behavior.
Carbon dioxide (CO2) has a relatively larger molecular size compared to hydrogen (H2) and helium (He), which are both composed of single atoms. Additionally, CO2 molecules possess dipole moments due to the presence of polar carbon-oxygen bonds. These factors contribute to stronger intermolecular interactions in carbon dioxide.
Carbon dioxide exhibits deviations from ideal gas behavior at high pressures and low temperatures. At these conditions, the intermolecular forces between CO2 molecules become significant, resulting in deviations from ideal gas laws such as Boyle's law and the ideal gas equation.
In contrast, hydrogen (H2) and helium (He) are both composed of single atoms and have weaker intermolecular forces. Nitrogen (N2) is a diatomic molecule like CO2, but it has nonpolar bonds, resulting in weaker intermolecular interactions compared to CO2.
Therefore, among the gases mentioned, carbon dioxide (CO2) is expected to show greater non-ideal behavior due to its larger molecular size and polar nature, leading to stronger intermolecular interactions.