The behaviour of a gas most closely approaches that of an ideal gas at

Step-by-step solution

An ideal gas assumes that the intermolecular forces of attraction between gas molecules are zero and the volume occupied by the molecules is negligible compared to the total volume of the gas. At low pressure, the total volume of the gas is very large, making the volume of the individual gas molecules negligible. At high temperature, the kinetic energy of the gas molecules is very high, which effectively overcomes the intermolecular forces of attraction. Therefore, a real gas behaves most closely like an ideal gas