Related Experiment Video
Updated: May 5, 2026

08:02
Fabricating High-viscosity Droplets using Microfluidic Capillary Device with Phase-inversion Co-flow Structure
Published on: April 17, 2018
9.9K
Vapor condensation onto a non-volatile liquid drop
Levent Inci1, Richard K Bowles
1Department of Chemistry, University of Saskatchewan, Saskatoon, Saskatchewan S7N 5C9, Canada.
The Journal of Chemical Physics
|December 11, 2013
Summary
Molecular dynamics simulations reveal how vapor condenses onto liquid drops. For miscible and partially miscible mixtures, distinct behaviors like film formation and solubility transitions were observed, impacting nucleation theory.
Area of Science:
- Physical Chemistry
- Materials Science
- Computational Chemistry
Background:
- Vapor condensation onto liquid drops is crucial in various physical and chemical processes.
- Understanding the dynamics and thermodynamics of this process is key for applications like atmospheric science and materials design.
- Previous studies often simplified mixture behavior or focused on specific conditions.
Purpose of the Study:
- To investigate the condensation dynamics and thermodynamics of binary Lennard-Jones mixtures onto a non-volatile liquid drop.
- To explore the influence of miscibility on adsorption, film formation, and core mixing.
- To develop and validate a theoretical model for solubility transitions in partially miscible systems.
Main Methods:
- Utilizing molecular dynamics simulations in the canonical ensemble.
- Analyzing systems with varying volume and miscibility (miscible and partially miscible).
- Developing a capillarity approximation-based model for non-volatile liquid drops.
Main Results:
- Observed submonolayer adsorption at large volumes with minor solvent mixing in miscible systems.
- Identified complete film formation at smaller volumes, driven by cluster-cluster coalescence.
- Discovered a solubility transition in partially miscible systems below a critical volume, accompanied by hysteresis.
- Validated simulation findings with the developed theoretical model.
Conclusions:
- The study elucidates the complex interplay between miscibility, system volume, and condensation behavior.
- A novel model successfully captures solubility transitions and hysteresis, relevant to deliquescence phenomena.
- Findings contribute to refining classical nucleation theory for systems with low free energy barriers.
Related Concept Videos
Phase Transitions: Vaporization and Condensation
16.9K
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...
16.9K
Vaporization
33.3K
The physical form of a substance changes by 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. For vaporization to occur, kinetic energy must be greater than the intermolecular forces that keep molecules bonded. The amount of energy needed to vaporize a quantity of liquid at a given pressure and a constant temperature is called the heat of vaporization. When...
33.3K
Distillation: Vapor–Liquid Equilibria
4.1K
Distillation is a separation technique that takes advantage of the boiling point properties of disparate elements in a mixture. To perform distillation, we begin by heating a miscible mixture of two liquids with a significant difference in boiling points (at least 20°C). As the solution heats up and reaches the bubble point of the more volatile component, some molecules of the more volatile component transition into the gas phase and travel upward into the condenser, which is a glass tube...
4.1K
Vapor Pressure
30.3K
When a liquid vaporizes in a closed container, gas molecules cannot escape. As these gas phase molecules move randomly about, they will occasionally collide with the surface of the condensed phase, and in some cases, these collisions will result in the molecules re-entering the condensed phase. The change from the gas phase to the liquid is called condensation. When the rate of condensation becomes equal to the rate of vaporization, neither the amount of the liquid nor the amount of the vapor...
30.3K
Sublimation
4.4K
Sublimation is the direct transformation of a solid to a gaseous state. For instance, at standard pressure and room temperature, solid carbon dioxide sublimes to gaseous carbon dioxide. The phase diagram depicts the conditions required for sublimation. This process occurs at the solid-gas phase boundary and is not observed above the triple point of the substance. The reverse of sublimation is called deposition, where a gaseous substance condenses directly into a solid. Sublimation and...
4.4K
Vapor Pressure Lowering
25.2K
The equilibrium vapor pressure of a liquid is the pressure exerted by its gaseous phase when vaporization and condensation are occurring at equal rates: Dissolving a nonvolatile substance in volatile liquid results in a lowering of the liquid’s vapor pressure. This phenomenon can be explained by considering the effect of added solute molecules on the liquid's vaporization and condensation processes. To vaporize, solvent molecules must be present at the surface of the solution. The...
25.2K

