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Entropy02:39

Entropy

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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...
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Entropy01:18

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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...
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Entropy and the Second Law of Thermodynamics01:20

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The second law of thermodynamics can be stated quantitatively using the concept of entropy. Entropy is the measure of disorder of the system.
The relation  between entropy and disorder can be illustrated with the example of the phase change of ice to water. In ice, the molecules are located at specific sites giving a solid state, whereas, in a liquid form, these molecules are much freer to move. The molecular arrangement has therefore become more randomized. Although the change in average...
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Second Law of Thermodynamics02:49

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In the quest to identify a property that may reliably predict the spontaneity of a process, a promising candidate has been identified: entropy. Processes that involve an increase in entropy of the system (ΔS > 0) are very often spontaneous; however, examples to the contrary are plentiful. By expanding consideration of entropy changes to include the surroundings, a significant conclusion regarding the relation between this property and spontaneity may be reached. In thermodynamic models, the...
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Second Law of Thermodynamics00:53

Second Law of Thermodynamics

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The Second Law of Thermodynamics states that entropy, or the amount of disorder in a system, increases each time energy is transferred or transformed. Each energy transfer results in a certain amount of energy that is lost—usually in the form of heat—that increases the disorder of the surroundings. This can also be demonstrated in a classic food web. Herbivores harvest chemical energy from plants and release heat and carbon dioxide into the environment. Carnivores harvest the...
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Third Law of Thermodynamics02:38

Third Law of Thermodynamics

21.0K
A pure, perfectly crystalline solid possessing no kinetic energy (that is, at a temperature of absolute zero, 0 K) may be described by a single microstate, as its purity, perfect crystallinity,and complete lack of motion means there is but one possible location for each identical atom or molecule comprising the crystal (W = 1). According to the Boltzmann equation, the entropy of this system is zero.
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Effects of Structural Relaxation of Glass-Forming Melts on the Overall Crystallization Kinetics in Cooling and Heating.

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An Analog Macroscopic Technique for Studying Molecular Hydrodynamic Processes in Dense Gases and Liquids
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Entropy and the Tolman Parameter in Nucleation Theory.

Jürn W P Schmelzer1, Alexander S Abyzov2, Vladimir G Baidakov3

  • 1Institute of Physics, University of Rostock, Albert-Einstein-Strasse 23-25, 18059 Rostock, Germany.

Entropy (Basel, Switzerland)
|December 3, 2020
PubMed
Summary

This study enhances nucleation theory by linking surface tension to entropy changes, enabling accurate predictions for phase transitions. The new model describes surface tension

Keywords:
boilingcondensationcrystallizationcurvature dependence of the surface tensionnucleationsegregation

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Area of Science:

  • Thermodynamics
  • Physical Chemistry
  • Materials Science

Background:

  • Classical nucleation theory relies on Gibbs' theory of interfacial phenomena to define critical cluster properties.
  • Accurate prediction of nucleation rates requires understanding the size and curvature dependence of surface tension.
  • Existing models often use entropy or enthalpy changes (latent heat) to describe surface tension in phase transitions.

Purpose of the Study:

  • To expand the Stefan-Skapski-Turnbull rule for describing surface tension of critical clusters and its size dependence.
  • To generalize the application of Tolman's equation for surface tension curvature dependence to various phase formation scenarios.
  • To develop a unified approach for surface tension's size dependence across the metastable range from binodal to spinodal curves.

Main Methods:

  • Utilizing the Stefan-Skapski-Turnbull rule to determine surface tension's dependence on pressure and temperature.
  • Applying Tolman's equation to describe surface tension's curvature dependence in one-component and multi-component systems.
  • Comparing the developed approach with alternative methods for specifying the Tolman parameter and surface tension size dependence.

Main Results:

  • A novel method is presented to determine the size dependence of surface tension based on the Stefan-Skapski-Turnbull rule.
  • The generalized Tolman equation is shown to be applicable for describing surface tension in condensation and boiling.
  • A relation for surface tension's curvature dependence is derived, covering the entire metastable region of initial states.

Conclusions:

  • The expanded Stefan-Skapski-Turnbull rule provides a robust framework for understanding surface tension in nucleation.
  • The generalized Tolman equation offers a versatile tool for analyzing phase transitions across diverse systems and conditions.
  • This work advances the thermodynamic theory of nucleation, improving predictions of phase formation phenomena.