Investigating global phase diagrams (GPDs) with reentrant transition behavior
Jude Simons Bayor1, Baohua Teng2, Lingli Wang2
1Department of Applied Physics, Faculty of Applied Sciences, University for Development Studies, Navrongo Campus, Tamale, Ghana.
Plos One
|July 13, 2018
Summary
This study calculates global phase diagrams and closed-loop behavior for physical system phase transitions using the transverse field Ising model. Results reveal reentrant phase behavior and correlate theoretical calculations with experimental phenomena.
Area of Science:
- Condensed matter physics
- Statistical mechanics
Background:
- Phase transitions are fundamental in physical systems.
- Understanding closed-loop behavior is crucial for predicting system dynamics.
Purpose of the Study:
- To calculate global phase diagrams and closed-loop behavior for phase transitions.
- To investigate the reentrant phase behavior in physical systems.
- To correlate theoretical models with experimental observations.
Main Methods:
- Utilizing the transverse field Ising model with nearest neighbor interaction.
- Generating 3D graphs of physical parameters to visualize system behavior.
Main Results:
- Successfully calculated global phase diagrams and closed-loop behavior.
- Demonstrated clear appreciation and qualitative understanding of reentrant phase behavior.
- Showcased a close correlation between theoretical calculations and experimental phenomena.
Conclusions:
- The transverse field Ising model effectively describes closed-loop phase transitions.
- Theoretical predictions align well with observed experimental behaviors.
- This work provides a robust framework for studying complex phase transitions.
Related Concept Videos
Phase Diagrams
50.3K
A phase diagram combines plots of pressure versus temperature for the liquid-gas, solid-liquid, and solid-gas phase-transition equilibria of a substance. These diagrams indicate the physical states that exist under specific conditions of pressure and temperature and also provide the pressure dependence of the phase-transition temperatures (melting points, sublimation points, boiling points). Regions or areas labeled solid, liquid, and gas represent single phases, while lines or curves represent...
50.3K
Phase Transitions
23.2K
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...
23.2K
Phase Transitions: Sublimation and Deposition
20.2K
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...
20.2K
Phase Diagram
7.0K
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).
7.0K
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...
15.2K
Phase Transitions: Vaporization and Condensation
21.5K
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...
21.5K


