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Related Concept Videos

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...
Heterogeneous Catalysis01:22

Heterogeneous Catalysis

Heterogeneous catalysis involves a catalyst in a different phase from the reactants. It is a process where the catalyst and the reactants are in distinct phases, typically solid and gas or liquid.Most heterogeneous catalysts are metals, metal oxides, or acids. The list includes transition metals like iron (Fe), cobalt (Co), nickel (Ni), palladium (Pd), platinum (Pt), chromium (Cr), manganese (Mn), tungsten (W), silver (Ag), and copper (Cu). These metals possess partially vacant d orbitals that...
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...
Standard Electrode Potentials03:02

Standard Electrode Potentials

On comparing the reactivity of silver and lead, it is observed that the two ionic species, Ag+ (aq) and Pb2+ (aq), show a difference in their redox reactivity towards copper: the silver ion undergoes spontaneous reduction, while the lead ion does not. This relative redox activity can be easily quantified in electrochemical cells by a property called cell potential. This property is commonly known as cell voltage in electrochemistry, and it is a measure of the energy which accompanies the charge...
Electrochemical Cells01:28

Electrochemical Cells

Electrochemical cells are systems that convert chemical energy into electrical energy or use electrical energy to drive chemical reactions. They consist of two electrodes in contact with an electrolyte, where redox reactions enable electron transfer. Most electrochemical cells include two half-cells connected by an external wire for electron flow and a salt bridge for ion flow. The salt bridge contains an electrolyte solution and maintains charge neutrality by allowing ions—not electrons—to...
Catalysis02:50

Catalysis

The presence of a catalyst affects the rate of a chemical reaction. A catalyst is a substance that can increase the reaction rate without being consumed during the process. A basic comprehension of a catalysts’ role during chemical reactions can be understood from the concept of reaction mechanisms and energy diagrams.

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Synthesis and Performance Characterizations of Transition Metal Single Atom Catalyst for Electrochemical CO2 Reduction
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Heterogeneous consecutive electron transfer at graphite electrodes under steady state.

Xiaoquan Lu1, Ping Sun, Dongna Yao

  • 1Key Laboratory of Bioelectrochemistry & Environmental Analysis of Gansu Province, College of Chemistry & Chemical Engineering, Northwest Normal University, Lanzhou, 730070, China. luxq@nwnu.edu.cn

Analytical Chemistry
|September 22, 2010
PubMed
Summary

Thin-layer cyclic voltammetry (TLCV) effectively models consecutive electron transfer (ET) at the interface between two immiscible electrolyte solutions (ITIES). Numerical simulations and experiments confirm TLCV

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Area of Science:

  • Electrochemistry
  • Physical Chemistry
  • Chemical Interfaces

Background:

  • Investigating electron transfer (ET) at the interface between two immiscible electrolyte solutions (ITIES) is crucial for understanding complex electrochemical processes.
  • Consecutive or multistep electron transfer at ITIES presents unique challenges for theoretical and experimental analysis.

Purpose of the Study:

  • To develop and experimentally verify a theoretical model for consecutive electron transfer (ET) at the interface between two immiscible electrolyte solutions (ITIES) using thin-layer cyclic voltammetry (TLCV).
  • To predict voltammetric responses for multistep ET at ITIES via numerical simulations and examine the influence of key parameters on current-voltage curves.

Main Methods:

  • Development of a theoretical framework based on thin-layer cyclic voltammetry (TLCV).
  • Numerical simulations to predict voltammetric responses for multistep electron transfer.
  • Experimental verification using a model system (ZnTPP/[Fe(CN)₆]⁴⁻).
  • Analysis of empirical parameters, including reactant concentration ratios and thin-layer thickness.

Main Results:

  • The developed TLCV theory for consecutive ET at ITIES is well-established and experimentally validated.
  • Numerical simulations accurately predict voltammetric responses, showing excellent agreement with experimental data.
  • The study elucidates the impact of concentration ratios and thin-layer thickness on multistep ET.
  • The Butler-Volmer (B-V) theory is confirmed as suitable for describing consecutive electron transfer in the model system.

Conclusions:

  • Thin-layer cyclic voltammetry (TLCV) is a powerful and validated technique for studying heterogeneous consecutive electron transfer (ET) at the interface between two immiscible electrolyte solutions (ITIES).
  • The combination of theoretical modeling, numerical simulation, and experimental verification provides robust insights into the kinetics of complex electrochemical reactions at ITIES.
  • The findings support the applicability of established electrochemical theories, like Butler-Volmer, to multistep ET processes at ITIES.