What is the Difference Between Ideal Gas and Real Gas?

The main difference between an ideal gas and a real gas lies in the assumptions made about the particles of the gas and their behavior. Here are the key differences:

• Theoretical vs. Actual: An ideal gas is a theoretical concept, while a real gas is an actual substance. Ideal gases are used as a simplified model to describe the behavior of real gases under certain conditions.
• Particle Volume and Interactions: Ideal gas particles are assumed to have no volume and to not interact with each other except during collisions. In contrast, real gas particles have volume and interactions between them.
• Applicability of Ideal Gas Law: The ideal gas law (PV = nRT) works for all ideal gases, regardless of their chemical identity, and applies under certain conditions. However, real gases deviate from the ideal gas law, especially at low temperatures and high pressures.
• Intermolecular Forces: Real gases have intermolecular forces that can be strong or weak, depending on the substance. The strength of these forces affects how closely a real gas behaves like an ideal gas. Gases with weak intermolecular forces, such as neon, are more ideal than those with strong forces, like water vapor.

In summary, an ideal gas is a theoretical concept that follows the assumptions of the kinetic-molecular theory, while a real gas is an actual substance that deviates from these assumptions due to factors such as particle volume, interactions, and intermolecular forces. Ideal gas laws work well for real gases at low pressures and high temperatures, but they become less accurate at extreme conditions.

Comparative Table: Ideal Gas vs Real Gas

The main differences between ideal and real gases can be summarized in the following table:

An ideal gas is a hypothetical substance that obeys the gas laws at all conditions of pressure and temperature, with molecules that have no volume and no intermolecular forces. In contrast, a real gas is a substance that does not obey the gas laws at all standard pressure and temperature, with molecules that have volume and intermolecular forces. Real gases deviate from the ideal gas behavior, especially at high pressures and low temperatures.