Lecture

Electrochemistry: Principles and Applications in Thermodynamics

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In course

PHYS-106(b): General physics : thermodynamics

Le but du cours de Physique générale est de donner à l'étudiant les notions de base nécessaires à la compréhension des phénomènes physiques. L'objectif est atteint lorsque l'étudiant est capable de prévoir quantitativement les conséquences de ces phénomène ...

Description

This lecture covers the fundamental concepts of electrochemistry, including electrochemical potential, oxidation and reduction reactions, and the Nernst potential. The instructor explains the electrochemical potential as a generalization of chemical potential, incorporating electrostatic energy. The lecture details oxidation and reduction processes, highlighting the reactions involving zinc and copper, and the role of electrodes in these reactions. The instructor also discusses the construction and functioning of the Daniell cell, illustrating how oxidation at the zinc anode and reduction at the copper cathode generate electric current. The Nernst equation is introduced to explain the relationship between concentration differences and electrochemical potential. Practical experiments, such as the deposition of copper on electrodes and the operation of a lemon battery, are demonstrated to reinforce theoretical concepts. The lecture concludes with applications of electrochemistry in various systems, emphasizing its relevance in thermodynamics and energy conversion processes.

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Instructors (2)

Sylvain Bréchet

Sylvain Bréchet was born on October 13th, 1981 in Moudon (legal origin Epesses, VD, Switzerland). He obtained a Master of Science in physics at EPFL in 2005. He went on to Cambridge for his PhD studies in theoretical cosmology from 2005 to 2009 under the supervision of Prof. Lasenby (FRS) and Prof. Michael Hobson at the Cavendish Laboratory of the University of Cambridge. He went back to EPFL where he is since 2010 university lecturer and research scientist in the Institute of Condensed Matter Physics. He taught classical mechanics, special relativity and thermodynamics to mechanical, electrical engineering students and physics students. He is currently writing a textbook in thermodynamics.

Nicolas Grandjean

Nicolas Grandjean received a PhD degree in physics from the University ofNice Sophia Antipolis in 1994 and shortly thereafter joined the French National Center for Scientific Research (CNRS) as a permanent staff member. In 2004, he was appointed tenure-track assistant professor at the École polytechnique fédérale de Lausanne (EPFL) where he created the Laboratory for advanced semiconductors for photonics and electronics. He was promoted to full professor in 2009. He was the director of the Institute of Condensed Matter Physics from 2012 to 2016 and then moved to the University of California at Santa Barbara where he spent 6 months as a visiting professor. Since 2018, he is the head of the School of Physics at the EPFL. He was awarded the Sandoz Family Foundation Grant for Academic Promotion, received the “Nakamura Lecturer” Award in 2010, the "Quantum Devices Award” at the 2017 Compound Semiconductor Week, and “2016 best teacher” award from the EPFL Physics School. His research interests are focused on the physics of nanostructures and III-V nitride semiconductor quantum photonics.

Official source

Ontological neighbourhood

Chemistry

Physical chemistry: Electrochemistry

Physics

Thermodynamics: Statistical mechanics

Related concepts (32)

Electrochemical cell

An electrochemical cell is a device that generates electrical energy from chemical reactions. Electrical energy can also be applied to these cells to cause chemical reactions to occur. Electrochemical cells which generate an electric current are called voltaic or galvanic cells and those that generate chemical reactions, via electrolysis for example, are called electrolytic cells. Both galvanic and electrolytic cells can be thought of as having two half-cells: consisting of separate oxidation and reduction reactions.

Galvanic cell

A galvanic cell or voltaic cell, named after the scientists Luigi Galvani and Alessandro Volta, respectively, is an electrochemical cell in which an electric current is generated from spontaneous Oxidation-Reduction reactions. A common apparatus generally consists of two different metals, each immersed in separate beakers containing their respective metal ions in solution that are connected by a salt bridge or separated by a porous membrane. Volta was the inventor of the voltaic pile, the first electrical battery.

Reduction potential

Redox potential (also known as oxidation / reduction potential, ORP, pe, , or ) is a measure of the tendency of a chemical species to acquire electrons from or lose electrons to an electrode and thereby be reduced or oxidised respectively. Redox potential is expressed in volts (V). Each species has its own intrinsic redox potential; for example, the more positive the reduction potential (reduction potential is more often used due to general formalism in electrochemistry), the greater the species' affinity for electrons and tendency to be reduced.

Standard electrode potential

In electrochemistry, standard electrode potential , or , is a measure of the reducing power of any element or compound. The IUPAC "Gold Book" defines it as: "the value of the standard emf (electromotive force) of a cell in which molecular hydrogen under standard pressure is oxidized to solvated protons at the left-hand electrode". The basis for an electrochemical cell, such as the galvanic cell, is always a redox reaction which can be broken down into two half-reactions: oxidation at anode (loss of electron) and reduction at cathode (gain of electron).

Electrochemical potential

In electrochemistry, the electrochemical potential (ECP), , is a thermodynamic measure of chemical potential that does not omit the energy contribution of electrostatics. Electrochemical potential is expressed in the unit of J/mol. Each chemical species (for example, "water molecules", "sodium ions", "electrons", etc.) has an electrochemical potential (a quantity with units of energy) at any given point in space, which represents how easy or difficult it is to add more of that species to that location.

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