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Reversible and Irreversible Processes01:14

Reversible and Irreversible Processes

The thermodynamic processes can be classified into reversible and irreversible processes. The processes that can be restored to their initial state are called reversible processes. It is only possible if the process is in quasi-static equilibrium, i.e., it takes place in infinitesimally small steps, and the system remains at equilibrium However, these are ideal processes and do not occur naturally. An ideal system undergoing a reversible process is always in thermodynamic equilibrium within...
Absolute Entropies and the Third Law of Thermodynamics01:23

Absolute Entropies and the Third Law of Thermodynamics

Ludwig Edward Boltzmann developed a definition for entropy, which stated that absolute entropy is proportional to the natural logarithm of the number of possible combinations of particles. Entropy stands alone among state functions as the only one whose absolute values can be determined.Consider a gas sample confined to a container. As the container expands, the energy levels of gas molecules become more closely spaced. This increases the number of available energy states, thereby increasing...
Entropy and the Second Law of Thermodynamics01:26

Entropy and the Second Law of Thermodynamics

Consider an isolated system in which a hot object is placed in contact with a cold one. This is an irreversible process that eventually leads both objects to reach the same equilibrium temperature. It is crucial to note that the constituents of any substance exhibit increased disorder at higher temperatures. As a cold substance absorbs heat, its constituents become more disordered. The energy transfer from a hotter object to a cooler one increases the system's disorder or randomness. This...
Entropy and the Second Law of Thermodynamics01:20

Entropy and the Second Law of Thermodynamics

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...
Limits of the First Law of Thermodynamics01:22

Limits of the First Law of Thermodynamics

Spontaneous processes, like a rock falling to the ground or sodium reacting with chlorine, occur without external work and often involve a decrease in the system‘s energy. However, certain endothermic processes, such as the dissolution of sodium chloride in water, occur spontaneously even though they increase the energy of the system. This limitation suggests that the First Law of Thermodynamics, which states that the total energy of a system is constant in an isolated system, cannot fully...
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...

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An Analog Macroscopic Technique for Studying Molecular Hydrodynamic Processes in Dense Gases and Liquids
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An Analog Macroscopic Technique for Studying Molecular Hydrodynamic Processes in Dense Gases and Liquids

Published on: December 4, 2017

Current trends in finite-time thermodynamics.

Bjarne Andresen1

  • 1Niels Bohr Institute, University of Copenhagen, Denmark. andresen@nbi.ku.dk

Angewandte Chemie (International Ed. in English)
|March 5, 2011
PubMed
Summary

Finite-time thermodynamics explores the trade-off between speed and efficiency. It offers methods to minimize costs like energy or entropy production, even in rapid processes.

Area of Science:

  • Thermodynamics
  • Physical Chemistry
  • Engineering

Background:

  • Reversible processes offer maximum efficiency but are impractically slow.
  • Real-world processes incur costs (energy, entropy, money) for speed.
  • Finite-time thermodynamics addresses this fundamental trade-off.

Purpose of the Study:

  • To introduce the core concepts of finite-time thermodynamics.
  • To explain its application in minimizing the costs associated with rapid processes.
  • To present methods for calculating optimal operational paths.

Main Methods:

  • Analyzing the "price of haste" in various systems (chemical, mechanical, economic).
  • Developing strategies to limit extra expenditure (energy, entropy, money).

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Cooling an Optically Trapped Ultracold Fermi Gas by Periodical Driving
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An Analog Macroscopic Technique for Studying Molecular Hydrodynamic Processes in Dense Gases and Liquids
11:03

An Analog Macroscopic Technique for Studying Molecular Hydrodynamic Processes in Dense Gases and Liquids

Published on: December 4, 2017

Cooling an Optically Trapped Ultracold Fermi Gas by Periodical Driving
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Cooling an Optically Trapped Ultracold Fermi Gas by Periodical Driving

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  • Utilizing time-varying environments to guide system evolution.

    • Main Results:

    • Demonstrates that finite-time thermodynamics provides a framework for optimizing speed-efficiency trade-offs.
    • Identifies methods to minimize energy and entropy production in non-ideal, time-dependent processes.
    • Shows how to determine optimal operating paths for accelerated processes.

    Conclusions:

    • Finite-time thermodynamics is crucial for understanding and optimizing real-world processes where speed is essential.
    • The field provides practical approaches to reduce costs associated with haste.
    • Optimal system control using time-varying environments is a key strategy.