differences between ideal gases and real gases

In thermodynamics, ideal gases and real gases are two different concepts that help simplify the study of gases and their behavior. Here are the key differences between ideal gases and real gases:

Ideal Gas

1. Molecular Model: Ideal gases are based on a simplified molecular model where gas particles are considered as point masses with no volume and no intermolecular forces.
2. Pressure and Volume: The ideal gas law, PV = nRT, accurately describes the behavior of ideal gases. It relates pressure (P), volume (V), the number of moles (n), the ideal gas constant (R), and temperature (T).
3. Applicability: Ideal gases are an approximation that works well under low pressure and high-temperature conditions. They are most accurate at high temperatures and low pressures.
4. Specific Heat: Ideal gases have constant specific heat capacities.
5. Real-World Use: Ideal gases are often used in theoretical and mathematical calculations as a simplification of real gases.

Real Gas

1. Molecular Model: Real gases consider the actual molecular characteristics of gas particles, including their volume and intermolecular forces. They do not assume point masses.
2. Pressure and Volume: Real gases do not strictly follow the ideal gas law, especially at high pressures and low temperatures.
3. Applicability: Real gases are a more accurate representation of the behavior of gases under a wide range of conditions, including high pressures and low temperatures.
4. Specific Heat: The specific heat capacities of real gases can vary with temperature and pressure.
5. Real-World Use: Real gases are used in practical applications, especially when dealing with gases at non-ideal conditions, such as liquefied gases or gases under high pressure.