Which of the following gases would you predict to be most non-ideal? CO_(2)(g) He(g) CH_(4)(g) N_(2)(g)

The question is asking which of the given gases would deviate the most from ideal gas behavior. Ideal gases are hypothetical gases that perfectly obey the ideal gas law, PV = nRT, where P is pressure, V is volume, the number of moles, R is the ideal gas constant, and T is temperature. In reality, no gas perfectly follows this law, but gases that are monatomic and have low molar mass tend to behave more like an ideal gas. On the other hand, gases with strong intermolecular forces or those that can form temporary dipoles (like CO2) will deviate more from ideal behavior.<br /><br />Among the given options, CO2 is a linear molecule with a permanent dipole moment, which means it has strong intermolecular forces. These forces cause CO2 to deviate more from ideal gas behavior compared to the other gases listed, which are either monatomic (He) or have weaker intermolecular forces (CH4 and N2).