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Related Concept Videos

Entropy01:18

Entropy

2.7K
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...
2.7K
Entropy Change in Reversible Processes01:10

Entropy Change in Reversible Processes

2.7K
In the Carnot engine, which achieves the maximum efficiency between two reservoirs of fixed temperatures, the total change in entropy is zero. The observation can be generalized by considering any reversible cyclic process consisting of many Carnot cycles. Thus, it can be stated that the total entropy change of any ideal reversible cycle is zero.
The statement can be further generalized to prove that entropy is a state function. Take a cyclic process between any two points on a p-V diagram.
2.7K
Entropy and the Second Law of Thermodynamics01:20

Entropy and the Second Law of Thermodynamics

3.0K
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...
3.0K
Standard Entropy Change for a Reaction03:00

Standard Entropy Change for a Reaction

20.7K
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.
20.7K
Third Law of Thermodynamics02:38

Third Law of Thermodynamics

19.3K
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.
19.3K
Second Law of Thermodynamics02:49

Second Law of Thermodynamics

24.1K
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...
24.1K

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Unraveling Entropic Rate Acceleration Induced by Solvent Dynamics in Membrane Enzymes
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Resolving entropy contributions in nonequilibrium transitions.

Benjamin Sorkin1, Joshua Ricouvier2, Haim Diamant1

  • 1School of Chemistry and Center for Physics and Chemistry of Living Systems, Tel Aviv University, 69978 Tel Aviv, Israel.

Physical Review. E
|February 17, 2023
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Summary
This summary is machine-generated.

This study introduces a new functional to calculate entropy from microscopic correlations, applicable both in and out of equilibrium. It identifies key degrees of freedom and characterizes dynamic transitions in systems like jammed emulsions.

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Area of Science:

  • Statistical Mechanics
  • Soft Matter Physics
  • Non-equilibrium Thermodynamics

Background:

  • Understanding entropy in complex systems, especially out of equilibrium, is challenging.
  • Microscopic correlations often dictate macroscopic system behavior and phase transitions.

Purpose of the Study:

  • To derive a universal functional for entropy based on measurable microscopic pair correlations.
  • To develop a method for identifying key degrees of freedom and characterizing dynamic transitions.
  • To apply this formalism to non-equilibrium systems like jammed emulsions.

Main Methods:

  • Derivation of a general entropy functional from pair correlation functions.
  • Application of the functional to experimental data of jammed bidisperse emulsions.
  • Analysis of cross-correlations between droplet positions and sizes.

Main Results:

  • The derived functional quantifies entropy from microscopic correlations, applicable in and out of equilibrium.
  • The method successfully captures dynamic transitions, such as the crossover in jammed emulsions.
  • Cross-correlations between droplet positions and sizes are identified as crucial for disordered hyperuniform state formation.

Conclusions:

  • The developed formalism provides a powerful tool for entropy estimation and transition characterization in disordered and non-equilibrium systems.
  • Microscopic correlations offer a fundamental link to macroscopic properties and system dynamics.
  • This approach has significant implications for understanding complex materials and phase transitions.