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Related Concept Videos

Entropy02:39

Entropy

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...
Entropy01:18

Entropy

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...
Third Law of Thermodynamics02:38

Third Law of Thermodynamics

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.
Entropy Changes Accompanying Specific Processes01:21

Entropy Changes Accompanying Specific Processes

Entropy, a measure of disorder in a system, changes during phase transitions like freezing or boiling. At the transition temperature Ttrs, where two phases are in equilibrium, the phase transition is a reversible process. The entropy change can be calculated from a substance's enthalpy of transition using the equation ΔStrs = ΔtrsH /Ttrs.When a perfect gas expands isothermally from one volume to another, entropy increases logarithmically with volume. Conversely, isothermal compression results...
Second Law of Thermodynamics02:49

Second Law of Thermodynamics

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...
Second Law of Thermodynamics00:53

Second Law of Thermodynamics

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 chemical energy...

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Related Experiment Video

Updated: Jun 16, 2026

Experimental Investigation of Secondary Flow Structures Downstream of a Model Type IV Stent Failure in a 180&#176; Curved Artery Test Section
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Excess entropy and structural transitions in a two-dimensional square-shoulder fluid.

Murari Singh1, Hongjun Liu, Sanat K Kumar

  • 1School of Physical Sciences, Jawaharlal Nehru University, New Delhi 110067, India.

The Journal of Chemical Physics
|February 23, 2010
PubMed
Summary

Metropolis Monte Carlo simulations reveal thermodynamic signatures of phase transitions in a square-shoulder fluid. The residual multiparticle entropy (RMPE) rule predicts structure formation but fails in coexistence regions.

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Area of Science:

  • Thermodynamics
  • Statistical Mechanics
  • Computational Physics

Background:

  • Understanding phase transitions in simple fluids is crucial for materials science.
  • The square-shoulder fluid model provides a simplified yet relevant system for studying complex phase behavior.
  • Previous studies identified low-density solid and stripe phases at zero temperature.

Purpose of the Study:

  • To investigate temperature-dependent thermodynamic properties of the square-shoulder fluid.
  • To identify thermodynamic signatures of structural phase transitions.
  • To evaluate the predictive power of the residual multiparticle entropy (RMPE) for phase ordering.

Main Methods:

  • Metropolis Monte Carlo simulations were employed.
  • Simulations were performed on the square-shoulder fluid model.
  • Analysis focused on excess entropy, heat capacity, and configurational energy along isochores.

Main Results:

  • Thermodynamic signatures of phase transitions were observed along multiple isochores.
  • Competition between cluster and stripe formation was identified as a key mechanism for free energy minimization.
  • The RMPE rule generally predicted ordered structure formation but showed limitations in coexistence regions.

Conclusions:

  • Finite temperature simulations confirm and extend zero-temperature findings on phase behavior.
  • The RMPE rule is a useful, albeit approximate, predictor for phase transitions in systems with limited phase coexistence.
  • The study highlights the interplay of different ordering mechanisms in dense fluids.