Final answer:
A gas can be considered ideal at low pressure and high temperature, where molecule volume is negligible and intermolecular forces are minimal. Real gases approximate ideal behavior under such conditions, although they deviate at very high pressures or very low temperatures.
Step-by-step explanation:
A gas can be considered as an ideal gas under certain conditions. Primarily, these conditions include situations of low pressure and high temperature, where the behavior of the gas aligns well with the assumptions made in the ideal gas law. At low pressures, the volume occupied by gas molecules is insignificant compared to the volume of their container, and intermolecular forces become negligible. Conversely, at high temperatures, the kinetic energy of the gas molecules is high enough to overcome any attractive forces between them. Thus, under these conditions, the gas behaves ideally and the deviations from the ideal gas law are minimal.
It is important to note that while no real gas is truly ideal, many gases approximate ideal behavior closely enough under these conditions that the ideal gas law can be effectively used to predict their behavior. However, at very high pressures or very low temperatures, real gases deviate significantly from ideal behavior, and the ideal gas law may no longer provide an accurate description.