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Phase Transitions02:31

Phase Transitions

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Whether solid, liquid, or gas, a substance's state depends on the order and arrangement of its particles (atoms, molecules, or ions). Particles in the solid pack closely together, generally in a pattern. The particles vibrate about their fixed positions but do not move or squeeze past their neighbors. In liquids, although the particles are closely spaced, they are randomly arranged. The position of the particles are not fixed—that is, they are free to move past their neighbors to...
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Phase Transitions: Sublimation and Deposition02:33

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Some solids can transition directly into the gaseous state, bypassing the liquid state, via a process known as sublimation. At room temperature and standard pressure, a piece of dry ice (solid CO2) sublimes, appearing to gradually disappear without ever forming any liquid. Snow and ice sublimate at temperatures below the melting point of water, a slow process that may be accelerated by winds and the reduced atmospheric pressures at high altitudes. When solid iodine is warmed, the solid sublimes...
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Phase Transitions: Melting and Freezing02:39

Phase Transitions: Melting and Freezing

15.2K
Heating a crystalline solid increases the average energy of its atoms, molecules, or ions, and the solid gets hotter. At some point, the added energy becomes large enough to partially overcome the forces holding the molecules or ions of the solid in their fixed positions, and the solid begins the process of transitioning to the liquid state or melting. At this point, the temperature of the solid stops rising, despite the continual input of heat, and it remains constant until all of the solid is...
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Phase Transitions: Vaporization and Condensation02:39

Phase Transitions: Vaporization and Condensation

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The physical form of a substance changes on changing its temperature. For example, raising the temperature of a liquid causes the liquid to vaporize (convert into vapor). The process is called vaporization—a surface phenomenon. Vaporization occurs when the thermal motion of the molecules overcome the intermolecular forces, and the molecules (at the surface) escape into the gaseous state. When a liquid vaporizes in a closed container, gas molecules cannot escape. As these gas phase molecules...
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Third Law of Thermodynamics02:38

Third Law of Thermodynamics

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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.
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Second Law of Thermodynamics02:49

Second Law of Thermodynamics

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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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Orientational Transition in a Liquid Crystal Triggered by the Thermodynamic Growth of Interfacial Wetting Sheets
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Phase transition in thermodynamically consistent biochemical oscillators.

Basile Nguyen1, Udo Seifert1, Andre C Barato2

  • 1II. Institut für Theoretische Physik, Universität Stuttgart, 70550 Stuttgart, Germany.

The Journal of Chemical Physics
|August 3, 2018
PubMed
Summary
This summary is machine-generated.

Biochemical oscillations emerge from a nonequilibrium phase transition, driven by thermodynamic force. The number of coherent oscillations is a better measure of precision than the Fano factor.

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Area of Science:

  • Biophysics
  • Chemical Kinetics
  • Non-equilibrium Thermodynamics

Background:

  • Biochemical oscillations are fundamental to life, occurring in autonomous systems out of equilibrium.
  • Understanding the emergence and precision of these oscillations is crucial for biological process comprehension.

Purpose of the Study:

  • To elucidate the generic nonequilibrium phase transition underlying biochemical oscillations.
  • To establish a robust metric for quantifying the precision of biochemical oscillations.

Main Methods:

  • Analysis of a generic nonequilibrium phase transition.
  • Characterization of critical behavior using thermodynamic force, flux, diffusion coefficient, and stationary distribution.
  • Comparison of Fano factor and number of coherent oscillations as precision metrics.
  • Thermodynamically consistent modeling using Brusselator, activator-inhibitor, and KaiC models.

Main Results:

  • Biochemical oscillations arise from a generic nonequilibrium phase transition requiring a threshold thermodynamic force.
  • Critical behavior is defined by thermodynamic flux, diffusion coefficient, and species distribution.
  • The number of coherent oscillations is a more appropriate measure of precision than the Fano factor.

Conclusions:

  • Biochemical oscillations are a universal phenomenon governed by nonequilibrium thermodynamics.
  • The number of coherent oscillations provides a reliable quantification of oscillation precision.
  • The study offers a theoretical framework applicable to diverse biochemical oscillating systems.