Related Experiment Video
Updated: Feb 15, 2026

13:02
Microfabrication of Nanoporous Gold Patterns for Cell-material Interaction Studies
Published on: July 15, 2013
11.9K
Three-dimensional bicontinuous nanoporous materials by vapor phase dealloying
Zhen Lu1,2, Cheng Li1, Jiuhui Han1
1Advanced Institute for Materials Research, Tohoku University, Sendai, 980-8577, Japan.
Nature Communications
|January 20, 2018
Summary
A new green vapor-phase dealloying method fabricates 3D bicontinuous open nanoporous materials universally. This eco-friendly technique recovers elements and offers tunable pore sizes for catalysis and energy storage.
Area of Science:
- Materials Science
- Nanotechnology
- Chemical Engineering
Background:
- Three-dimensional bicontinuous open (3DBO) nanoporosity is crucial for catalysis, sensing, and energy storage.
- Conventional dealloying methods (electrochemical, liquid-metal) have limitations in alloy applicability and generate chemical waste.
Purpose of the Study:
- To develop a green and universal method for fabricating 3DBO nanoporous materials.
- To overcome the limitations of existing dealloying techniques.
Main Methods:
- Utilizing vapor pressure differences between alloy elements for selective component removal.
- Employing a vapor-phase dealloying approach.
Main Results:
- Fabrication of nanoporous materials from a wide range of elements, irrespective of chemical activity.
- Achieved tunable pore sizes in the resulting nanoporous structures.
- Demonstrated full recovery of evaporated components, highlighting the method's sustainability.
Conclusions:
- Vapor-phase dealloying is an environmentally friendly and versatile technique for producing 3DBO nanoporous materials.
- This method enables broad applications in catalysis, sensing, and energy storage.
- The ability to recover elements makes this approach highly sustainable.
More Related Videos
Related Concept Videos
Phase Transitions: Vaporization and Condensation
21.6K
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...
21.6K
Vapor Pressure
41.2K
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...
41.2K
Vaporization
38.5K
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...
38.5K
Vapor Pressure Lowering
31.6K
The equilibrium vapor pressure of a liquid is the pressure exerted by its gaseous phase when vaporization and condensation are occurring at equal rates:
31.6K
Phase Diagrams
50.6K
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...
50.6K
Phase Transitions: Sublimation and Deposition
20.4K
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...
20.4K

