Related Experiment Video
Updated: Nov 8, 2025

09:42
Unraveling Entropic Rate Acceleration Induced by Solvent Dynamics in Membrane Enzymes
Published on: January 16, 2016
9.2K
Improved bounds on entropy production in living systems
Dominic J Skinner1, Jörn Dunkel2
1Department of Mathematics, Massachusetts Institute of Technology, Cambridge, MA 02139.
Summary
Living systems defy the second law of thermodynamics by consuming energy to create order, increasing environmental entropy. This study introduces an improved method to estimate entropy production rates from partial biological data.
Area of Science:
- Thermodynamics
- Biophysics
- Cellular Biology
Background:
- Living systems locally decrease entropy by consuming free energy, increasing environmental entropy.
- Estimating entropy production rates is crucial for understanding cellular process efficiency.
- Existing methods struggle with systems where many degrees of freedom are unobserved.
Purpose of the Study:
- To develop an improved method for estimating entropy production rates in biological systems using partial measurements.
- To provide provably optimal estimates under specific measurable transition statistics.
- To reveal nonzero entropy production in systems that appear time-symmetric.
Main Methods:
- Reformulating entropy production estimation within an optimization framework.
- Inferring improved bounds on entropy production from partial system measurements.
- Utilizing measurable transition statistics for optimal estimation.
Main Results:
- Developed an improved estimator for entropy production rates from partial biological data.
- Demonstrated that the new method can detect entropy production in time-symmetric nonequilibrium processes.
- Achieved provably optimal estimates under defined measurement conditions.
Conclusions:
- The novel optimization framework offers a more robust way to quantify entropy production in complex biological systems.
- This approach enhances our understanding of energy consumption and thermodynamic efficiency in life.
- Applicable to diverse biological systems, including molecular motors and cellular oscillations.
Related Concept Videos
Entropy within the Cell
12.2K
A living cell's primary tasks of obtaining, transforming, and using energy to do work may seem simple. However, the second law of thermodynamics explains why these tasks are harder than they appear. None of the energy transfers in the universe are completely efficient. In every energy transfer, some amount of energy is lost in a form that is unusable. In most cases, this form is heat energy. Thermodynamically, heat energy is defined as the energy transferred from one system to another that...
12.2K
Second Law of Thermodynamics
65.9K
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...
65.9K
Second Law of Thermodynamics
25.4K
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 models, the...
25.4K
Entropy and the Second Law of Thermodynamics
3.5K
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...
3.5K
Entropy
32.7K
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...
32.7K
Entropy
3.1K
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...
3.1K

