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Related Concept Videos

Phase Transitions: Melting and Freezing02:39

Phase Transitions: Melting and Freezing

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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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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...
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Heating and Cooling Curves02:44

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When a substance—isolated from its environment—is subjected to heat changes, corresponding changes in temperature and phase of the substance is observed; this is graphically represented by heating and cooling curves.
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Phase Transitions: Vaporization and Condensation02:39

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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...
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States of Water01:23

States of Water

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Water exists in any one of the three classical states: solid (ice), liquid (water), and gas (steam or water vapor). The state of water depends on i) the intermolecular forces that draw molecules together and ii) the kinetic energy that leads to movements that pull them apart.
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Freezing Point Depression and Boiling Point Elevation03:12

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Boiling Point Elevation
The boiling point of a liquid is the temperature at which its vapor pressure is equal to ambient atmospheric pressure. Since the vapor pressure of a solution is lowered due to the presence of nonvolatile solutes, it stands to reason that the solution’s boiling point will subsequently be increased. Vapor pressure increases with temperature, and so a solution will require a higher temperature than will pure solvent to achieve any given vapor pressure, including one...
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Ice Generation and the Heat and Mass Transfer Phenomena of Introducing Water to a Cold Bath of Brine
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Ice Generation and the Heat and Mass Transfer Phenomena of Introducing Water to a Cold Bath of Brine

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Supercooled water escaping from metastability.

Francesco Aliotta1, Paolo V Giaquinta2, Rosina C Ponterio1

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Scientific Reports
|November 28, 2014
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This summary is machine-generated.

Supercooled water

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Area of Science:

  • Thermodynamics
  • Phase transitions
  • Fluid dynamics

Background:

  • Supercooled water exists below its freezing point without solidifying.
  • The transition from supercooled water to ice is an irreversible adiabatic process in large samples.
  • Understanding this transition is crucial for various scientific and industrial applications.

Purpose of the Study:

  • To investigate the dynamics of supercooled water transitioning to a stable equilibrium.
  • To analyze the role of temperature, energy, and density fluctuations during freezing.
  • To identify critical thresholds governing the transition process.

Main Methods:

  • Utilized fast imaging techniques to observe the phenomenon in water.
  • Synchronously monitored local temperature evolution during the freezing process.
  • Analyzed spatial coexistence of solid and liquid phases at different temperatures.

Main Results:

  • Observed large energy and density fluctuations during water's freezing process.
  • Identified a sharp dynamic transition at approximately 266.6 K, separating fast and slow decay regimes.
  • Correlated heat transfer dynamics and convective motion suppression with a percolation threshold.

Conclusions:

  • The transition dynamics are governed by heat transfer from solid/liquid regions to supercooled liquid.
  • Convective motions are suppressed when the nucleated solid fraction exceeds a percolation threshold at low temperatures.
  • This study provides insights into the fundamental physics of water freezing and phase transitions.