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Related Concept Videos

Phase Transitions02:31

Phase Transitions

20.6K
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...
20.6K
Phase Diagram01:19

Phase Diagram

6.2K
The phase of a given substance depends on the pressure and temperature. Thus, plots of pressure versus temperature showing the phase in each region provide considerable insights into the thermal properties of substances. Such plots are known as phase diagrams. For instance, in the phase diagram for water (Figure 1), the solid curve boundaries between the phases indicate phase transitions (i.e., temperatures and pressures at which the phases coexist).
6.2K
Phase Transitions: Sublimation and Deposition02:33

Phase Transitions: Sublimation and Deposition

18.3K
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...
18.3K
Phase Changes01:19

Phase Changes

4.6K
Phase transitions play an important theoretical and practical role in the study of heat flow. In melting or fusion, a solid turns into a liquid; the opposite process is freezing. In evaporation, a liquid turns into a gas; the opposite process is condensation.
A substance melts or freezes at a temperature called its melting point and boils or condenses at its boiling point. These temperatures depend on pressure. High pressure favors the denser form of the substance, so typically, high pressure...
4.6K
States of Matter and Phase Changes00:59

States of Matter and Phase Changes

1.4K
The internal energy of a substance—the total kinetic energy of all its molecules and the potential energy of their associated forces—depends on the strength of the intermolecular forces in the condensed phases and the pressure exerted on the substance. The internal energy of a substance is the highest in the gaseous state, the lowest in the solid state, and intermediate in the liquid state. Phase transitions are caused by changes in physical conditions, such as temperature and...
1.4K
Heating and Cooling Curves02:44

Heating and Cooling Curves

24.4K
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.
For instance, the addition of heat raises the temperature of a solid; the amount of heat absorbed depends on the heat capacity of the solid (q = mcsolidΔT). According to thermochemistry, the relation between the amount of heat absorbed or released by a substance, q, and its...
24.4K

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Enhanced weak superconductivity in trigonal<i>γ</i>-PtBi<sub>2</sub>.

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Phase Behavior of Charged Vesicles Under Symmetric and Asymmetric Solution Conditions Monitored with Fluorescence Microscopy
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Phase Behavior of Charged Vesicles Under Symmetric and Asymmetric Solution Conditions Monitored with Fluorescence Microscopy

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First-Order Phase Transformation at Constant Volume: A Continuous Transition?

Víctor F Correa1, Facundo J Castro1

  • 1Consejo Nacional de Investigaciones Científicas y Técnicas (CONICET), Centro Atómico Bariloche (CNEA) and Instituto Balseiro (U. N. Cuyo), Av. Bustillo 9500, Bariloche 8400, Rio Negro, Argentina.

Entropy (Basel, Switzerland)
|January 21, 2022
PubMed
Summary

First-order phase transitions at constant volume exhibit unique behaviors, with transformations occurring over a range of temperatures and pressures. Thermodynamic potentials remain continuous, and heat capacity shows discrete jumps, not divergence.

Keywords:
first-order phase transitionisochoric processmechanical actuatorthermodynamicswater

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Area of Science:

  • Thermodynamics
  • Physical Chemistry
  • Materials Science

Background:

  • First-order phase transitions are typically studied under constant pressure conditions.
  • Understanding phase transitions under different constraints is crucial for fundamental science and applications.

Purpose of the Study:

  • To investigate the characteristics of a first-order phase transition under constant volume (isochoric) conditions.
  • To contrast isochoric transitions with isobaric transitions and clarify distinctions between continuous and discontinuous transitions.

Main Methods:

  • Theoretical analysis of a simple system undergoing a first-order phase transition at constant volume.
  • Application of thermodynamic principles to analyze potential behavior and heat capacity.
  • Modeling the ice VI-liquid water transition and a mechanical actuator based on isochoric phase transitions.

Main Results:

  • Isochoric first-order phase transitions occur over a finite temperature and pressure range.
  • Extensive thermodynamic potentials (U, H, F, G) and entropy (S) remain continuous across the transition.
  • Constant-volume heat capacity exhibits discrete jumps, without divergence.

Conclusions:

  • Controlling thermodynamic variables (volume vs. pressure) is critical for correctly identifying the nature of phase transitions.
  • Isochoric phase transitions offer distinct thermodynamic signatures compared to isobaric transitions.
  • The principles of isochoric phase transitions can be applied to engineer devices like mechanical actuators.