Related Experiment Video
Updated: Dec 10, 2025

11:16
Preparation of Silver-Palladium Alloyed Nanoparticles for Plasmonic Catalysis under Visible-Light Illumination
Published on: August 18, 2020
5.8K
Reduction of carbon dioxide at a plasmonically active copper-silver cathode.
Elizabeth R Corson1, Ananya Subramani, Jason K Cooper
1Department of Chemical and Biomolecular Engineering, University of California, Berkeley, California 94720, USA. bmcclosk@berkeley.edu.
Summary
This study demonstrates how silver-coated copper nanostructures can enhance carbon dioxide (CO2) reduction selectivity using light. Plasmonic enhancement under illumination selectively promotes specific CO2 reduction products over hydrogen evolution.
Area of Science:
- Materials Science
- Electrochemistry
- Catalysis
Background:
- Electrochemical reduction of carbon dioxide (CO2) is a key technology for renewable energy storage.
- Copper-based catalysts are widely studied for CO2 reduction but often suffer from poor selectivity.
- Plasmonic materials offer potential for enhancing catalytic reactions through light-matter interactions.
Purpose of the Study:
- To develop a plasmonically active cathode for enhanced CO2 reduction selectivity.
- To investigate the effect of light illumination on CO2 reduction pathways at silver-coated copper nanostructures.
- To elucidate the role of plasmonic effects in directing CO2 reduction product distribution.
Main Methods:
- Electrochemical deposition of copper nanostructures.
- Coating copper nanostructures with silver to create plasmonic cathodes.
- Illumination of the cathode with 365 nm light during CO2 reduction.
- Analysis of CO2 reduction products using gas chromatography and other analytical techniques.
- Temperature-dependent control experiments to rule out thermal effects.
Main Results:
- Illumination selectively enhanced 5 out of 14 observed CO2 reduction products.
- Hydrogen evolution was suppressed under illumination.
- At low overpotentials, carbon monoxide (C1 product) was promoted.
- At high overpotentials, ethylene, methane, formate, and allyl alcohol (C2/C3 products) were enhanced.
- Selective promotion of C1 products and C2/C3 products with double carbon bonds was observed under illumination.
- Temperature-dependent studies confirmed that local heating was not responsible for the observed selectivity changes.
Conclusions:
- Plasmonic enhancement using light can significantly improve the selectivity of CO2 reduction at copper electrodes.
- The study demonstrates a novel approach to tune CO2 reduction pathways using plasmonically active materials.
- Further research is needed to fully understand the underlying plasmonic mechanisms for selective CO2 reduction.
More Related Videos
Related Concept Videos
Electrodeposition
1.1K
Electrodeposition is a technique used to separate an analyte from interferents by electrochemical processes. Here, the analyte is a metal ion that can be deposited on an electrode immersed in the sample solution. The electrochemical setup consists of an anode and a cathode. When an electric current is applied to the setup, oxidation occurs at the anode. At the cathode, which consists of a large metal surface, metal ions undergo reduction and deposit onto the surface.
Electrodeposition can...
Electrodeposition can...
1.1K
Voltaic/Galvanic Cells
62.2K
Spontaneous Chemical Reactions
Spontaneous redox reactions occur abundantly in nature. The chemical reaction occurring in a disposable AA battery powering our remote controls is one such example of a spontaneous redox reaction. Another example is the immersion of coiled copper wire into an aqueous silver nitrate solution. The reaction shows a gradual, visually impressive color change from colorless to bright blue and the formation of a grey precipitate on the copper wire. In this experiment,...
Spontaneous redox reactions occur abundantly in nature. The chemical reaction occurring in a disposable AA battery powering our remote controls is one such example of a spontaneous redox reaction. Another example is the immersion of coiled copper wire into an aqueous silver nitrate solution. The reaction shows a gradual, visually impressive color change from colorless to bright blue and the formation of a grey precipitate on the copper wire. In this experiment,...
62.2K

