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Equations \ (\ref {10.1}\) and \ (\ref {10.2}\) represent the same chemical reaction system in which the roles of the components are reversed, and both yield the same mixture of components when the change is completed. This is central to the concept of chemical equilibrium.
Equilibrium chemistry is concerned with systems in chemical equilibrium. The unifying principle is that the free energy of a system at equilibrium is the minimum possible, so that the slope of the free energy with respect to the reaction coordinate is zero.
In a chemical reaction, chemical equilibrium is the state in which both the reactants and products are present in concentrations which have no further tendency to change with time, so that there is no observable change in the properties of the system. [1]
Unit 7: Chemical equilibrium This unit is part of the Chemistry library. Browse videos, articles, and exercises by topic.
Learn about the condition and equation of chemical equilibrium, where a reversible reaction reaches a state of dynamic balance. Find out how the equilibrium constant and the standard Gibbs free energy are related to the reaction.
- The Editors of Encyclopaedia Britannica
In a chemical equilibrium, the forward and reverse reactions occur at equal rates, and the concentrations of products and reactants remain constant. If we run a reaction in a closed system so that the products cannot escape, we often find the reaction does not give a 100% yield of products.
Learn about the concepts and applications of chemical equilibrium, such as dynamic equilibrium, reversible reactions, equilibrium constants, reaction quotients, Le Chatelier's principle, and Gibb's free energy. Test your knowledge with quizzes and practice questions.
