The correct answer is B. Low pressure and high temperature.
An ideal gas is a theoretical gas composed of a set of randomly moving, non-interacting point particles. The ideal gas concept is useful because it obeys the ideal gas law, a good approximation to the behavior of many gases under many conditions.
Real gases, on the other hand, do interact with each other and do not behave exactly like ideal gases. The extent to which a real gas deviates from ideal gas behavior depends on the temperature and pressure of the gas.
At low pressures and high temperatures, the molecules of a real gas are moving very quickly and have a lot of space between them. This means that the intermolecular forces between the molecules are weak and the molecules can be considered to be non-interacting. Under these conditions, a real gas will behave very much like an ideal gas.
At high pressures and low temperatures, the
molecules of a real gas are moving more slowly and have less space between them. This means that the intermolecular forces between the molecules are stronger and the molecules cannot be considered to be non-interacting. Under these conditions, a real gas will deviate more from ideal gas behavior.In conclusion, a real gas can act as an ideal gas in low pressure and high temperature conditions.