Related Experiment Video

Updated: Jul 11, 2026

Determination of Thermodynamic Properties of Alkaline Earth-liquid Metal Alloys Using the Electromotive Force Technique
12:02

Determination of Thermodynamic Properties of Alkaline Earth-liquid Metal Alloys Using the Electromotive Force Technique

Published on: November 3, 2017

Free energy and temperature dependence of electron transfer at the metal-electrolyte interface

C E Chidsey

    Science (New York, N.Y.)
    |February 22, 1991
    PubMed

    More Related Videos

    Characterizing Electron Transport through Living Biofilms08:52

    Characterizing Electron Transport through Living Biofilms

    Published on: June 1, 2018

    Asymmetric Thermoelectrochemical Cell for Harvesting Low-grade Heat under Isothermal Operation09:09

    Asymmetric Thermoelectrochemical Cell for Harvesting Low-grade Heat under Isothermal Operation

    Published on: February 5, 2020

    Related Concept Videos

    Electrochemical Systems01:24

    Electrochemical Systems

    Electrochemical systems provide a fascinating insight into the dynamic interplay of charged species within various phases. One notable example is the interaction between a membrane permeable to K⁺ ions but not to Cl⁻ ions, separating an aqueous KCl solution from pure water. As K⁺ ions diffuse through the membrane, they generate net charges on each phase, leading to a potential difference between them.Similarly, when a piece of Zn is immersed in an aqueous ZnSO₄ solution, the Zn metal, composed...
    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...
    Applications of EMF Measurements01:26

    Applications of EMF Measurements

    Electromotive force (EMF) measurements have a broad range of applications in various fields, including chemistry and physics. The electrochemical series, an arrangement of elements in order of their standard electrode potentials, can be determined through EMF measurements. Elements with lower standard potentials can reduce ions of elements with higher standard potentials.The standard cell potential, E°, allows for the calculation of the standard reaction Gibbs energy, ΔG°, and the equilibrium...
    The Nernst Equation02:59

    The Nernst Equation

    Nonstandard Reaction Conditions
    The interconnection between standard cell potentials and various thermodynamic parameters such as the standard free energy change ΔG° and equilibrium constant K has been previously explored. For example, a redox reaction involving zinc(II) and tin(II) ions at 1 M concentration with Eºcell = +0.291 V and ΔG° = −56.2 kJ is spontaneous.
    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+...
    Redox Equilibria: Overview01:23

    Redox Equilibria: Overview

    A reduction-oxidation reaction is commonly called a redox reaction. In a redox reaction, electrons are transferred from one species to another rather than being shared between or among atoms. The reducing agent or reductant is the species that loses electrons and gets oxidized in the process. The species that gains electrons and gets reduced in the process is the oxidizing agent or oxidant. Redox reactions are represented as two separate equations called half-reactions, where one equation...