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Related Concept Videos

Electrodeposition01:08

Electrodeposition

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...
Extraction: Advanced Methods00:56

Extraction: Advanced Methods

Metal ions can be separated from one another by complexation with organic ligands–the chelating agent– to form uncharged chelates. Here, the chelating agent must contain hydrophobic groups and behave as a weak acid, losing a proton to bind with the metal. Since most organic ligands used in this process are insoluble or undergo oxidation in the aqueous phase, the chelating agent is initially added to the organic phase and extracted into the aqueous phase. The metal-ligand complex is formed in...
Ladder Diagrams: Redox Equilibria01:30

Ladder Diagrams: Redox Equilibria

Ladder diagrams are useful tools for understanding redox equilibrium reactions, especially the effects of concentration changes on the electrochemical potential of the reaction. The vertical axis in the redox ladder diagrams represents the electrochemical potential, E. The area of predominance is demarcated using the Nernst equation.
Consider the Fe3+/Fe2+ half-reaction, which has a standard-state potential of +0.771 V. At potentials more positive than +0.771 V, Fe3+ predominates, whereas Fe2+...
Types of Reversible Electrodes01:24

Types of Reversible Electrodes

For electrode reversibility to be maintained, all the reactants and products involved in the half-reaction must be present at the electrode. There are several types of reversible electrodes (half-cells).In metal-metal-ion electrodes, a metal balances electrochemically with a solution of its own ions. Examples are Cu2+|Cu and Zn2+|Zn. Metals that react with the solvent, like group 1 and most group 2 metals, which react with water, and zinc, which reacts with aqueous acidic solutions, cannot be...
Processes at Electrodes01:30

Processes at Electrodes

The electrode interacts with ions in the electrolyte solution at its interface. The rate of oxidation and reduction depends on the speed at which electrons can transfer through this interface. As ions attach to or leave the electrode surface, the electrode acquires a charge, and an electrical potential forms across the interface, making the process more difficult to reach equilibrium. The charge on the electrode affects the local ion concentrations in the solution, though thermal motion...
Redox Reactions01:24

Redox Reactions

Oxidation-reduction or redox reactions involve the transfer of electrons from one molecule or atom to another. When an atom gains an electron, another atom must lose an electron, meaning oxidation and reduction must occur together. Since the redox occurs in pairs, the atom that gets oxidized is also called the reducing agent or reductant, and the atom that is reduced is also called the oxidizing agent or oxidant. A straightforward way to remember the definitions of oxidation and reduction is...

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Hydrogenation of CO<sub>2</sub> to Methanol Catalyzed by In<sub>2</sub>O<sub>3</sub>: Oxygen Vacancies, Surface Hydroxyl Groups, and Temperature Dependence for Reactivity Revealed by <sup>17</sup>O NMR.

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Stabilization of Atomic CoO<sub><i>x</i></sub> Clusters on Oxygen Vacancy-Rich TiO<sub>2</sub> for Enhanced Photocatalytic CO<sub>2</sub> to Methanol.

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Controllable synthesis of perovskite solid solutions as novel energetic materials <i>via</i> thermodynamic equilibrium.

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Synergistic Catalysis in Fe─In Diatomic Sites Anchored on Nitrogen-Doped Carbon for Enhanced CO<sub>2</sub> Electroreduction.

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Construction of "Metal Defect/Oxygen Defect Junction" in ZnFe<sub>2</sub>O<sub>4</sub>-NiCo<sub>2</sub>O<sub>4</sub> Heterostructures for Enhancing Electrocatalytic Oxygen Evolution.

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Updated: Jun 4, 2026

Solar-Driven Electrochemical Green Fuel Production from CO2 and Water Using Ti3C2Tx MXene-Supported CuZn and NiCo Catalysts
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Solar-Driven Electrochemical Green Fuel Production from CO2 and Water Using Ti3C2Tx MXene-Supported CuZn and NiCo Catalysts

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Electron-Rich In2O3-Cu Interfaces Drive Selective and Stable CO2 Electroreduction.

Anyu Zhang1, Jian Wang1, Junxin Guo1

  • 1National Engineering Research Center of Industry Crystallization Technology, School of Chemical Engineering and Technology, Tianjin University, Tianjin 300072, China.

The Journal of Physical Chemistry Letters
|June 3, 2026
PubMed
Summary

Researchers developed an inverse indium oxide/copper (In2O3/Cu) catalyst for efficient carbon dioxide electroreduction (CO2RR). This novel design enhances selectivity and stability, achieving 95% CO selectivity over 90 hours.

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Magnetometric Characterization of Intermediates in the Solid-State Electrochemistry of Redox-Active Metal-Organic Frameworks
06:53

Magnetometric Characterization of Intermediates in the Solid-State Electrochemistry of Redox-Active Metal-Organic Frameworks

Published on: June 9, 2023

Area of Science:

  • Electrochemistry
  • Materials Science
  • Catalysis

Background:

  • Metal-oxide interfaces are crucial for steering CO2 electroreduction (CO2RR) on copper catalysts.
  • Conventional supported catalysts face interfacial degradation issues under operating potentials.

Purpose of the Study:

  • To design a stable and highly selective catalyst for CO2RR.
  • To investigate the role of inverse oxide-metal architecture in mitigating interfacial degradation and enhancing catalytic performance.

Main Methods:

  • Fabrication of an inverse In2O3/Cu architecture with dispersed In2O3 domains on porous Cu.
  • Electrochemical performance testing for CO2RR.
  • In situ infrared spectroscopy and density functional theory (DFT) calculations.

Main Results:

  • The optimized 5In2O3/Cu catalyst demonstrated a CO Faradaic efficiency of ~95%.
  • Stable operation exceeding 90 hours was achieved.
  • Interface stabilization of water structure and dual active sites were identified, suppressing hydrogen evolution reaction (HER) and lowering COOH formation barrier to 0.51 eV.

Conclusions:

  • Inverse catalyst design is an effective strategy for achieving high selectivity and long-term stability in CO2RR.
  • Strong oxide-metal interactions in the In2O3/Cu system stabilize interfaces and create an electron-rich Cu microenvironment.