Related Experiment Video
Updated: May 16, 2026

06:26
Orientational Transition in a Liquid Crystal Triggered by the Thermodynamic Growth of Interfacial Wetting Sheets
Published on: May 15, 2017
Thermodynamic geometry, phase transitions, and the Widom line
G Ruppeiner1, A Sahay, T Sarkar
1Division of Natural Sciences, New College of Florida, 5800 Bay Shore Road, Sarasota, Florida 34243-2109, USA. ruppeiner@ncf.edu
Physical Review. E, Statistical, Nonlinear, and Soft Matter Physics
|December 11, 2012
Summary
A new method using thermodynamic curvature (R) characterizes liquid-gas phase transitions. This approach accurately determines coexistence curves and the Widom line without problematic constructions.
Area of Science:
- Thermodynamics
- Phase Transitions
- Statistical Mechanics
Background:
- First-order liquid-gas phase transitions are fundamental in physical chemistry.
- The Maxwell equal area construction is conventionally used but has limitations.
- Characterizing the supercritical regime, including the Widom line, remains an active research area.
Purpose of the Study:
- To propose a novel microscopic characterization for first-order liquid-gas phase transitions.
- To develop a method for determining liquid-gas coexistence curves without the Maxwell construction.
- To enable direct determination of the Widom line in the supercritical regime.
Main Methods:
- Utilizing thermodynamic curvature (R) as a microscopic characterization parameter.
- Proposing that R is equal in coexisting phases near the critical point.
- Relating R to the correlation volume (ξ(3)) near the critical point.
Main Results:
- A new method for determining liquid-gas coexistence curves is presented, avoiding the Maxwell equal area construction.
- The relationship |R| ~ ξ(3) allows for direct determination of the Widom line in the supercritical region.
- The proposed method is illustrated using the van der Waals model and NIST Chemistry WebBook data.
Conclusions:
- Thermodynamic curvature offers a robust framework for analyzing liquid-gas phase transitions.
- The proposed method provides a more accurate and direct approach to phase transition characterization.
- This work advances the understanding of critical phenomena and supercritical fluid behavior.
Related Concept Videos
Phase Diagram
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).
Phase Diagram
A phase diagram is a graphical representation of the physical states of a substance under different conditions of temperature and pressure. It shows the boundaries between solid, liquid, and gas phases and the conditions at which these phases coexist in equilibrium. An area in a phase diagram represents a single phase, whereas lines or phase boundaries represent the equilibrium between two phases.In the phase diagram of water, the boundary line between the solid and liquid states illustrates...
Phase Transitions
A phase transition is the process in which a substance changes from one state of matter to another, like from a solid to a liquid, liquid to gas, or vice versa, at a specific temperature and under given pressure conditions. This change is spontaneous and is affected by alterations in temperature and pressure. These parameters impact the strength of the forces between molecules (intermolecular forces) in the substance.During a phase transition, both the initial and final phases of the substance...
Phase Transitions
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 occupy...
Entropy Changes Accompanying Specific Processes
Entropy, a measure of disorder in a system, changes during phase transitions like freezing or boiling. At the transition temperature Ttrs, where two phases are in equilibrium, the phase transition is a reversible process. The entropy change can be calculated from a substance's enthalpy of transition using the equation ΔStrs = ΔtrsH /Ttrs.When a perfect gas expands isothermally from one volume to another, entropy increases logarithmically with volume. Conversely, isothermal compression results...
Phase Changes
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...
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...

