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Ideal Solutions

Ideal Solutions

According to Raoult’s law, the partial vapor pressure of a solvent in a solution is equal or identical to the vapor pressure of the pure solvent multiplied by its mole fraction in the solution. However, Raoult's Law is only valid for ideal solutions. For a solution to be ideal, the solvent-solute interaction must be just as strong as a solvent-solvent or solute-solute interaction. This suggests that both the solute and the solvent would use the same amount of energy to escape to the vapor phase...

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.

Gas Solubility

Gas Solubility

Gas solubility in liquids forms liquid-gas solutions, such as soft drinks, where carbon dioxide is dissolved in water, and the ocean, where the solubility of oxygen and carbon dioxide supports marine life. The ability of oceans to dissolve gases impacts weather conditions in the troposphere.However, gas-liquid interactions vary. For instance, hydrogen chloride gas is highly soluble in water, while oxygen's solubility is much lower. Because these solutions are non-ideal, Raoult’s law, which...

Physical Properties Affecting Solubility

Physical Properties Affecting Solubility

Solutions of Gases in Liquids
As for any solution, the solubility of a gas in a liquid is affected by the attractive intermolecular forces between solute and solvent species. Unlike solid and liquid solutes, however, there is no solute-solute intermolecular attraction to overcome when a gaseous solute dissolves in a liquid solvent since the atoms or molecules comprising a gas are far separated and experience negligible interactions. Consequently, solute-solvent interactions are the sole...

Thermodynamic Properties of Ideal Solutions

Thermodynamic Properties of Ideal Solutions

For an ideal liquid solution, the standard state of each component is defined as the pure liquid at the temperature and pressure of the solution. Similarly, for solid solutions, the standard state is the pure solid. The chemical potentials of the components in the ideal solution are compared to the chemical potentials of the pure substances in their standard states. These standard states provide a reference point for calculating the thermodynamic properties of ideal solutions.For ideal...

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...

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Nonideal gas solvation thermodynamics.

Dor Ben-Amotz¹, B Widom

¹Department of Chemistry, Purdue University, West Lafayette, Indiana 47907-1393, USA. bendor@purdue.edu

The Journal of Chemical Physics

|March 17, 2007

Summary

This study provides general thermodynamic expressions for nonideal gas mixtures, detailing equations of state and solvation functions. These findings reveal how solutes impact nonideal solvents, differing from ideal gas behavior.

Area of Science:

Physical Chemistry
Thermodynamics
Statistical Mechanics

Background:

Understanding the thermodynamic properties of nonideal gas mixtures is crucial for chemical processes.
Existing models often simplify interactions or assume ideal behavior, limiting their applicability.
Solvation effects in complex mixtures require detailed theoretical treatment.

Purpose of the Study:

To derive general expressions for the thermodynamic properties of nonideal gases with arbitrary composition.
To analyze the equation of state and solvation thermodynamic functions of mixtures.
To investigate solute-induced changes in solvent properties and chemical equilibria.

Main Methods:

Developed general expressions for thermodynamic properties, expanded to first order in total number density.

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Utilized binary second virial coefficients, linked to binary interaction potential energy functions.

Decomposed solvation thermodynamic functions into solute-solvent and solvent-reorganization components.

Main Results:

Obtained general equations of state and solvation thermodynamic functions for multicomponent nonideal gas mixtures.
Expressed results using binary second virial coefficients and potential energy functions.
Quantified solute-solvent and solvent-reorganization contributions to solvation.
Identified solute effects on solvent reorganization energy and chemical potential, distinct from ideal gas behavior.

Conclusions:

The derived expressions offer a comprehensive framework for nonideal gas mixture thermodynamics.
Solvation functions can be experimentally resolved into distinct contributions.
Solute interactions in nonideal solvents exhibit unique thermodynamic consequences compared to ideal systems.