Final answer:
The ideal gas law is best applied when pressure is low, volume is high, and temperature is high, as real gases approximate the behavior of ideal gases under these conditions. Therefore the correct answer is d) All of the above
Step-by-step explanation:
We give preference to the ideal gas law for making calculations when the pressure is low, the volume is high, and the temperature is high. This is because an ideal gas is a theoretical gas composed of many randomly moving point particles that do not interact except when they collide elastically. The ideal gas law assumes that these collisions between particles are perfectly elastic and that there are no intermolecular attractive or repulsive forces.
Practically, we find that real gases behave approximately as ideal gases under low pressure and high temperature conditions. The reason is that under these conditions, the molecules are generally far enough apart that intermolecular forces become negligible, and the volume of the individual gas molecules is much less than the total volume of the gas.
The ideal gas law combines several empirical laws, including Boyle's law, Charles's law, Avogadro's law, and the Combined Gas Law, relating pressure, volume, temperature, and the number of moles of a gas into a single equation. This equation is used to calculate the state of a gas under a set of conditions. However, the ideal gas law is most accurate when the gas is at a low density, which typically corresponds to a low pressure and a high temperature.