Related Experiment Video
Updated: Sep 22, 2025

05:39
Scalable Quantum Integrated Circuits on Superconducting Two-Dimensional Electron Gas Platform
Published on: August 2, 2019
9.8K
Upper bound for quantum entropy production from entropy flux
1Unidade de Educação a Distância e Tecnologia, Universidade Federal Rural de Pernambuco, 52171-900 Recife, Pernambuco, Brazil.
Physical Review. E
|May 20, 2022
Summary
This study introduces a new method to estimate entropy production in complex quantum systems. The derived upper bound, based on entropy flux, simplifies calculations for nonequilibrium processes.
Area of Science:
- Quantum thermodynamics
- Statistical mechanics
- Non-equilibrium systems
Background:
- Entropy production quantifies irreversibility in systems not at equilibrium.
- Calculating entropy production is challenging, especially in quantum systems with complex reservoirs.
- Standard methods fail for generic non-equilibrium reservoirs.
Purpose of the Study:
- To derive a practical upper bound for entropy production.
- To relate entropy production to entropy flux for specific systems.
- To provide a tool for estimating entropy production in quantum systems.
Main Methods:
- Derivation of an upper bound for entropy production.
- Utilizing entropy flux as a computable quantity.
- Analysis of systems where flux is an observable.
Main Results:
- An upper bound for entropy production is established in terms of entropy flux.
- The bound is applicable to systems with observable fluxes.
- Demonstrated utility in a three-level maser engine and a system with a squeezed bath.
Conclusions:
- The derived bound offers a practical approach to estimate entropy production.
- This method is valuable for systems where currents (fluxes) are accessible.
- Applicable to diverse quantum non-equilibrium phenomena.
Related Concept Videos
Entropy and the Second Law of Thermodynamics
3.2K
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...
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...
3.2K
Entropy
2.9K
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...
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...
2.9K
The Second Law of Thermodynamics
5.8K
In the quest to identify a property that may reliably predict the spontaneity of a process, a promising candidate has been identified: entropy. Scientists refer to the measure of randomness or disorder within a system as entropy. High entropy means high disorder and low energy. To better understand entropy, think of a student’s bedroom. If no energy or work were put into it, the room would quickly become messy. It would exist in a very disordered state, one of high entropy. Energy must be...
5.8K
Second Law of Thermodynamics
24.4K
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...
24.4K
Third Law of Thermodynamics
19.6K
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.
19.6K
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.
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

