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Related Concept Videos

Entropy02:39

Entropy

36.0K
Salt particles that have dissolved in water never spontaneously come back together in solution to reform solid particles. Moreover, a gas that has expanded in a vacuum remains dispersed and never spontaneously reassembles. The unidirectional nature of these phenomena is the result of a thermodynamic state function called entropy (S). Entropy is the measure of the extent to which the energy is dispersed throughout a system, or in other words, it is proportional to the degree of disorder of a...
36.0K
Entropy01:18

Entropy

3.6K
The first law of thermodynamics is quantitatively formulated via an equation relating the internal energy of a system, the heat exchanged by it, and the work done on it. A quantitative formulation of the second law of thermodynamics leads to defining a state function, the entropy.
When an ideal gas expands isothermally, the disorder in the gas increases. From the molecular perspective, the gas molecules have more volume to move around in.
Consider an infinitesimal step in the expansion, which...
3.6K
Standard Entropy Change for a Reaction03:00

Standard Entropy Change for a Reaction

24.5K
Entropy is a state function, so the standard entropy change for a chemical reaction (ΔS°rxn) can be calculated from the difference in standard entropy between the products and the reactants.
24.5K
Nomenclature of Aromatic Compounds with Multiple Substituents01:11

Nomenclature of Aromatic Compounds with Multiple Substituents

10.4K
When more than one substituent is present on the benzene ring, the IUPAC nomenclature depends on the number of substituents present.
For disubstituted benzene derivatives, with two groups attached to the benzene ring, three constitutional isomers are possible. For example, consider dimethyl benzene, often called xylene, where the second methyl group can be substituted at the second, third, or fourth carbon. The relative position of the substituents is represented by prefixes ortho, meta, or...
10.4K
Solubility Equilibria03:07

Solubility Equilibria

57.4K
Solubility equilibria are established when the dissolution and precipitation of a solute species occur at equal rates. These equilibria underlie many natural and technological processes, ranging from tooth decay to water purification. An understanding of the factors affecting compound solubility is, therefore, essential to the effective management of these processes. This section applies previously introduced equilibrium concepts and tools to systems involving dissolution and precipitation.
The...
57.4K
Entropy and Solvation02:05

Entropy and Solvation

8.4K
The process of surrounding a solute with solvent is called solvation. It involves evenly distributing the solute within the solvent. The rule of thumb for determining a solvent for a given compound is that like dissolves like. A good solvent has molecular characteristics similar to those of the compound to be dissolved. For example, polar solutions dissolve polar solutes, and apolar solvents dissolve apolar solutes. A polar solvent is a solvent that has a high dielectric constant (ϵ...
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Entropy in multiple equilibria, compounds with different sites.

Gion Calzaferri1

  • 1Department of Chemistry and Biochemistry, Freiestrasse 3, 3012 Bern, Switzerland. gion.calzaferri@dcb.unibe.ch.

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|November 20, 2018
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Summary
This summary is machine-generated.

This study simplifies complex chemical equilibria by showing entropy contributions can be calculated using just two constants. This offers new tools for understanding adsorption and ion exchange phenomena.

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Area of Science:

  • Physical Chemistry
  • Chemical Thermodynamics
  • Surface Chemistry

Background:

  • Investigating entropy's role in multiple chemical equilibria is crucial for understanding complex systems.
  • Existing models often require numerous equilibrium constants, hindering quantitative analysis.
  • The binding enthalpy of species is assumed to be constant within site types and independent of existing bonds.

Purpose of the Study:

  • To develop a simplified method for evaluating entropy contributions to free reaction enthalpy in systems with multiple, distinct binding sites.
  • To provide a framework for quantitatively analyzing complex chemical equilibria, including adsorption and ion exchange.
  • To offer new tools for describing and testing isotherms based on physical principles.

Main Methods:

  • Decomposing free reaction enthalpy into particle distribution and other contributions for each site type.
  • Developing a model where numerous equilibrium constants are expressed as a function of only two fundamental constants.
  • Analyzing systems with varying numbers of coordination sites (n1, n2) using a generalized notation (Xrc1{n1ABn2}Xrc2).

Main Results:

  • A significant reduction in the number of required equilibrium constants, from many to just two, for describing complex systems.
  • Demonstrated that entropy-driven fractional equilibrium coverage can be represented as a linear combination of individual Langmuir isotherms.
  • Provided explicit solutions for systems with 2 to 12 coordination sites, applicable to diverse chemical scenarios.

Conclusions:

  • The simplified approach provides a powerful and transparent method for quantitative analysis of complex chemical equilibria.
  • The findings offer new insights and tools for understanding adsorption and ion exchange isotherms.
  • This work facilitates both experimental and theoretical studies of systems previously difficult to handle.