Lecture

Chemical Equilibrium: Principles and Applications

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In course

MSE-101(a): Materials:from chemistry to properties

Ce cours permet l'acquisition des notions essentielles relatives à la structure de la matière, aux équilibres et à la réactivité chimique en liaison avec les propriétés mécaniques, thermiques, électriques et magnétiques des matériaux. ...

Description

This lecture introduces the concepts of chemical equilibrium, focusing on the principles of equilibrium, Le Chatelier's principle, and the relationship between free energy and equilibrium constant. It explains how reversible reactions reach a point of equilibrium when the forward and reverse reactions occur at the same rate. The lecture also covers the factors influencing chemical equilibrium, such as concentration, temperature, and volume/pressure. Additionally, it discusses the effects of changing concentrations and pressures on equilibrium shifts. The importance of equilibrium constants and the behavior of reactions under different conditions are highlighted.

Instructor

Véronique Michaud

Background: 1994 Habilitation à diriger des recherches ( INPG, France) 1991 PhD in Materials Engineering ( MIT, USA) 1987 Ingénieur Civil des Mines ( Ecole des Mines de Paris, France) Activities: Since January 2018: Associate Dean of Engineering, in charge of Education June 2012-Dec.2017: Head of the Materials Science and Engineering Section Since April 2017: Associate Professor at EPFL 2009-2017 : Professeur Titulaire at EPFL 1997-2009: Researcher at EPFL 1994-1997 : Chef de Travaux au laboratoire MSS-MAT, Ecole Centrale Paris (France) 1991-1994 : Post-doctoral research associate, MIT (USA) Author of about 300 publications of which 140 in peer-reviewed journals

Official source

Ontological neighbourhood

Physics

Thermodynamics: Statistical mechanics

Related concepts (32)

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Reversible reaction

A reversible reaction is a reaction in which the conversion of reactants to products and the conversion of products to reactants occur simultaneously. \mathit aA{} + \mathit bB \mathit cC{} + \mathit dD A and B can react to form C and D or, in the reverse reaction, C and D can react to form A and B. This is distinct from a reversible process in thermodynamics. Weak acids and bases undergo reversible reactions. For example, carbonic acid: H2CO3 (l) + H2O(l) ⇌ HCO3−(aq) + H3O+(aq).

Solubility equilibrium

Solubility equilibrium is a type of dynamic equilibrium that exists when a chemical compound in the solid state is in chemical equilibrium with a solution of that compound. The solid may dissolve unchanged, with dissociation, or with chemical reaction with another constituent of the solution, such as acid or alkali. Each solubility equilibrium is characterized by a temperature-dependent solubility product which functions like an equilibrium constant. Solubility equilibria are important in pharmaceutical, environmental and many other scenarios.

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Dynamic equilibrium

In chemistry, a dynamic equilibrium exists once a reversible reaction occurs. Substances transition between the reactants and products at equal rates, meaning there is no net change. Reactants and products are formed at such a rate that the concentration of neither changes. It is a particular example of a system in a steady state. In physics, concerning thermodynamics, a closed system is in thermodynamic equilibrium when reactions occur at such rates that the composition of the mixture does not change with time.

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