Real gases deviate from ideal gas behavior due to intermolecular forces and the finite volume occupied by gas molecules, especially under high pressure and low temperature conditions. These deviations are described by equations like the Van der Waals equation, which adjusts for these factors to better predict the behavior of real gases.

Real Gas

Real gases

ideal gas behavior

Intermolecular forces are the forces of attraction or repulsion between neighboring molecules, crucial for determining the physical properties of substances such as boiling and melting points. These forces, while weaker than intramolecular forces (bonds within molecules), play a significant role in the behavior of liquids, solids, and gases.

intermolecular forces

The finite volume method is a numerical technique used for solving partial differential equations by dividing the domain into discrete volumes and applying conservation laws. It is particularly effective for fluid dynamics problems because it ensures the conservation of fluxes across the boundaries of each control volume.

finite volume

Gas molecules are in constant, random motion and exhibit elastic collisions with each other and the walls of their container, leading to pressure being exerted. The behavior of gas molecules can be described by the ideal gas law under standard temperatures and pressures, but real gas behavior varies significantly under different conditions.

gas molecules

High pressure conditions

low temperature conditions

Deviations from ideal gas behavior

The Van der Waals equation is an adjustment of the ideal gas law that accounts for the finite size of molecules and the attraction between them, providing a more accurate description of real gas behavior. It introduces two parameters, 'a' and 'b', which correct for intermolecular forces and molecular volume, respectively, making it particularly useful for understanding gases at high pressures and low temperatures.

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