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Related Concept Videos

Phase Transitions02:31

Phase Transitions

22.9K
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...
22.9K
Phase Transitions: Sublimation and Deposition02:33

Phase Transitions: Sublimation and Deposition

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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

14.8K
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

20.8K
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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Thermochemical Equations02:55

Thermochemical Equations

35.8K
For a chemical reaction (the system) carried out at constant pressure – with the only work done caused by expansion or contraction – the enthalpy of reaction (also called the heat of reaction, ΔHrxn) is equal to the heat exchanged with the surroundings (qp).
35.8K
Maxwell-Boltzmann Distribution: Problem Solving01:20

Maxwell-Boltzmann Distribution: Problem Solving

2.8K
Individual molecules in a gas move in random directions, but a gas containing numerous molecules has a predictable distribution of molecular speeds, which is known as the Maxwell-Boltzmann distribution, f(v).
This distribution function f(v) is defined by saying that the expected number N (v1,v2) of particles with speeds between v1 and v2 is given by
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Related Experiment Video

Updated: Jan 27, 2026

Optogenetic Phase Transition of TDP-43 in Spinal Motor Neurons of Zebrafish Larvae
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Phase Transition in the Boltzmann-Vlasov Equation.

A C Fowler1,2

  • 11MACSI, University of Limerick, Limerick, Ireland.

Journal of Statistical Physics
|April 2, 2019
PubMed
Summary

This study shows that strong inter-molecular attraction can destabilize uniform gas states, explaining phase transitions. The research uses a modified Boltzmann equation for typical gas densities.

Area of Science:

  • Statistical Mechanics
  • Kinetic Theory
  • Thermodynamics

Background:

  • Phase transitions are crucial phenomena in physics.
  • Understanding the kinetic theory basis of phase transitions is complex.
  • Previous models often simplified inter-molecular interactions.

Purpose of the Study:

  • To explain phase transitions using a modified Boltzmann equation.
  • To investigate the role of inter-molecular attraction in gas stability.
  • To analyze the conditions under which a uniform gas state becomes unstable.

Main Methods:

  • Studied a form of the Boltzmann equation incorporating a Vlasov term for inter-molecular attraction.
  • Analyzed the evolution equation for the one-particle distribution function.
Keywords:
Boltzmann equationPhase transitionStability theory

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Combining Microfluidics and Microrheology to Determine Rheological Properties of Soft Matter during Repeated Phase Transitions
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Combining Microfluidics and Microrheology to Determine Rheological Properties of Soft Matter during Repeated Phase Transitions

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Patterning via Optical Saturable Transitions - Fabrication and Characterization
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Patterning via Optical Saturable Transitions - Fabrication and Characterization

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  • Utilized an approximation valid for typical gas densities where the ratio of molecular diameter to mean inter-particle distance is small.

    • Main Results:

    • Demonstrated that a uniform gas state becomes unstable when inter-molecular attraction is sufficiently strong.
    • Showed that the collision term is negligible for fluctuations at the molecular spacing scale.
    • An explicit approximate solution was derived and its validity discussed.

    Conclusions:

    • Inter-molecular attraction is a key factor in destabilizing uniform gas states, leading to phase transitions.
    • The derived approximation provides a foundation for understanding these phenomena.
    • Future work can extend these results to finite amplitude effects.