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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,...

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.

Deviation from Ideal Behaviour

Deviation from Ideal Behaviour

Real gases do not perfectly obey the ideal gas laws, especially at high pressures and low temperatures or when they are about to condense to a liquid. These deviations occur due to intermolecular forces between gas molecules. Repulsive forces aid expansion and are significant when molecules are very close together, typically at high pressure. Attractive forces assist compression and have a longer range, being effective over several molecular diameters. They become significant when molecules are...

Nonideal Two-Component Liquid Solutions

Nonideal Two-Component Liquid Solutions

Nonideal liquid solutions, also known as real solutions, do not strictly follow Raoult's law. Raoult's law is a rule of thumb in physical chemistry. However, not all mixtures adhere to this law due to varying molecular interactions. For example, in an acetone/chloroform solution, the individual vapor pressures of the components are lower than expected, resulting in a total vapor pressure below that predicted by Raoult's law, causing a negative deviation.On the other hand, in an ethanol/water...

Ideal Gas Equation

Ideal Gas Equation

The ideal gas equation is an equation of state that relates the state variables pressure, volume, temperature, and the number of moles of a hypothetical gas. This equation is a combination of four empirical laws, namely Boyle’s Law, Charles’s Law, Avogadro’s Law, and Gay-Lussac’s Law. When the proportionalities of the above four empirical laws are combined, it results in a single proportionality constant known as the universal gas constant.

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Related Experiment Video

Updated: Jul 3, 2026

Experimental Investigation of Secondary Flow Structures Downstream of a Model Type IV Stent Failure in a 180° Curved Artery Test Section

Experimental Investigation of Secondary Flow Structures Downstream of a Model Type IV Stent Failure in a 180° Curved Artery Test Section

Published on: July 19, 2016

A non-ideal replacement for the Boyle van't Hoff equation.

Richelle C Prickett¹, Janet A W Elliott, Shamina Hakda

¹Department of Chemical and Materials Engineering, Room 536, Chemical & Materials Engineering Building, University of Alberta, Edmonton, AB, Canada T6G2G6.

|August 5, 2008

Summary

This summary is machine-generated.

A new non-ideal osmotic equilibrium equation accurately describes cell volume, improving upon the Boyle van't Hoff equation. This revised model reduces the calculated osmotically inactive cell fraction by 20% for human erythrocytes.

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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

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Last Updated: Jul 3, 2026

Experimental Investigation of Secondary Flow Structures Downstream of a Model Type IV Stent Failure in a 180° Curved Artery Test Section

Experimental Investigation of Secondary Flow Structures Downstream of a Model Type IV Stent Failure in a 180° Curved Artery Test Section

Published on: July 19, 2016

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

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

Published on: December 4, 2017

Area of Science:

Cell biology
Physical chemistry
Biophysics

Background:

The Boyle van't Hoff equation is widely used to model cell volume regulation.
This equation is thermodynamically valid only for ideal, dilute solutions.
It often overestimates the osmotically inactive cell fraction.

Purpose of the Study:

To propose a more accurate non-ideal osmotic equilibrium equation for living cells.
To replace the Boyle van't Hoff equation for describing cell volume.
To re-evaluate the osmotically inactive cell fraction.

Main Methods:

Development of a non-ideal osmotic equilibrium equation.
Analysis of experimental osmotic equilibrium data using the new equation.
Comparison of results with the Boyle van't Hoff equation.

Main Results:

The proposed equation provides a more accurate description of cell volume.
Inferred osmotically inactive fraction for human erythrocytes was reduced by ~20%.
The new equation overcomes limitations of ideal solution assumptions.

Conclusions:

The non-ideal osmotic equilibrium equation is a superior model for cell volume.
It yields more accurate estimates of the osmotically inactive cell fraction.
This advancement impacts our understanding of cell volume regulation.