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Van der Waals Interactions

Van der Waals Interactions

Atoms and molecules interact with each other through intermolecular forces. These electrostatic forces arise from attractive or repulsive interactions between particles with permanent, partial, or temporary charges. The intermolecular forces between neutral atoms and molecules are ion–dipole, dipole–dipole, and dispersion forces, collectively known as van der Waals forces.Polar molecules have a partial positive charge on one end and a partial negative charge on the other end of the molecule,...

Real Gases: Effects of Intermolecular Forces and Molecular Volume Deriving Van der Waals Equation

Real Gases: Effects of Intermolecular Forces and Molecular Volume Deriving Van der Waals Equation

Thus far, the ideal gas law, PV = nRT, has been applied to a variety of different types of problems, ranging from reaction stoichiometry and empirical and molecular formula problems to determining the density and molar mass of a gas. However, the behavior of a gas is often non-ideal, meaning that the observed relationships between its pressure, volume, and temperature are not accurately described by the gas laws.

Intermolecular Forces

Intermolecular Forces

Atoms and molecules interact through bonds (or forces): intramolecular and intermolecular. The forces are electrostatic as they arise from interactions (attractive or repulsive) between charged species (permanent, partial, or temporary charges) and exist with varying strengths between ions, polar, nonpolar, and neutral molecules. The different types of intermolecular forces are ion–dipole, dipole–dipole, hydrogen bonds, and dispersion; among these, dipole–dipole, hydrogen bonds, and dispersion...

Intermolecular Forces

Intermolecular Forces

Atoms and molecules interact through bonds (or forces): intramolecular and intermolecular. The forces are electrostatic as they arise from interactions (attractive or repulsive) between charged species (permanent, partial, or temporary charges) and exist with varying strengths between ions, polar, nonpolar, and neutral molecules. The different types of intermolecular forces are ion–dipole, dipole–dipole, hydrogen bonds, and dispersion; among these, dipole–dipole, hydrogen bonds, and dispersion...

Van der Waals Equation

Van der Waals Equation

The ideal gas law is an approximation that works well at high temperatures and low pressures. The van der Waals equation of state (named after the Dutch physicist Johannes van der Waals, 1837−1923) improves it by considering two factors.
First, the attractive forces between molecules, which are stronger at higher densities and reduce the pressure, are considered by adding to the pressure a term equal to the square of the molar density multiplied by a positive coefficient a. Second, the volume...

The Van der Waals Equation

The Van der Waals Equation

The ideal gas law is based on two simplifying assumptions: first, that there are no intermolecular attractions between gas molecules, and second, that the volume occupied by the molecules themselves is negligible compared with the volume of the container. However, these assumptions don't hold up under all conditions - specifically, at high pressures and low temperatures, as gas tends to deviate from ideal gas behavior.The van der Waals equation is an enhanced version of the ideal gas law,...

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An Analog Macroscopic Technique for Studying Molecular Hydrodynamic Processes in Dense Gases and Liquids

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Published on: December 4, 2017

Dynamic van der Waals theory.

¹Department of Physics, Kyoto University, Kyoto 606-8502, Japan.

Physical Review. E, Statistical, Nonlinear, and Soft Matter Physics

|May 16, 2007

Summary

This summary is machine-generated.

This study introduces a dynamic van der Waals theory for gas-liquid transitions, explaining phenomena like heat pipes and boiling. The new hydrodynamic model captures density gradient stress for improved fluid dynamics simulations.

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Area of Science:

Fluid Dynamics
Thermodynamics
Statistical Mechanics

Background:

Existing hydrodynamic theories often simplify gas-liquid transitions and temperature nonuniformities.
Accurately modeling interfacial phenomena like evaporation and condensation remains a challenge.

Purpose of the Study:

To develop a dynamic van der Waals theory incorporating gradient contributions to entropy and energy functionals.
To establish a general scheme for two-phase hydrodynamics applicable to nonuniform temperature conditions.
To numerically investigate complex hydrodynamic processes involving phase transitions.

Main Methods:

Formulation of a dynamic van der Waals theory with gradient energy and entropy functionals.
Derivation of hydrodynamic equations that include stress from density gradients.
Numerical examination of six distinct hydrodynamic processes: spinodal decomposition, piston effect, droplet behavior in heat flow, latent heat transport, boiling, and liquid spreading/evaporation.

Main Results:

The theory successfully models stress induced by density gradients in hydrodynamic equations.
Numerical simulations elucidated various complex phenomena including efficient latent heat transport (heat pipe mechanism) and boiling dynamics.
The model provides a unified framework for understanding gas-liquid transitions in nonuniform temperature fields.

Conclusions:

The dynamic van der Waals theory offers a robust framework for studying two-phase hydrodynamics.
The inclusion of gradient contributions enhances the accuracy of modeling phase transitions and interfacial phenomena.
This work has implications for understanding heat pipes, boiling, and other complex fluid behaviors.