Inverse Thermodynamic Uncertainty Relation and Entropy Production
View abstract on PubMed
Summary
This summary is machine-generated.This study introduces the inverse thermodynamic uncertainty relation (iTUR) to set an upper bound on nonequilibrium current fluctuations. The iTUR prohibits perpetual superdiffusion in systems with finite entropy production and spectral gap.
Area Of Science
- Non-equilibrium physics
- Statistical mechanics
- Complex systems
Background
- Non-equilibrium current fluctuations are central to physics.
- The thermodynamic uncertainty relation (TUR) bounds fluctuations using entropy production and average current.
- Existing bounds primarily focus on lower bounds for fluctuations.
Purpose Of The Study
- To derive and analyze an upper bound for current fluctuations, termed the inverse thermodynamic uncertainty relation (iTUR).
- To establish a universal iTUR expression applicable to both continuous and discrete systems.
- To investigate the implications of iTUR for phenomena like perpetual superdiffusion and giant diffusion.
Main Methods
- Derivation of a universal iTUR expression for continuous-variable systems (overdamped Langevin equations).
- Derivation of a universal iTUR expression for discrete-variable systems (Markov jump processes).
- Analysis of the conditions under which current fluctuations can diverge, relating them to spectral gap closure and entropy production.
Main Results
- A universal inverse thermodynamic uncertainty relation (iTUR) is derived.
- iTUR establishes a no-go theorem against perpetual superdiffusion for systems with finite entropy production and spectral gap.
- Divergence of current fluctuations requires either a vanishing spectral gap or diverging entropy production.
Conclusions
- The iTUR provides a crucial upper bound on fluctuations in non-equilibrium systems.
- The findings highlight the interplay between spectral gap and entropy production in determining fluctuation behavior.
- The iTUR framework offers insights into phenomena like giant diffusion and limits on anomalous transport.
Related Concept Videos
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...
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...
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...
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...
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...
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...

