Le Chatelier principle

Học thuật
Thân thiện
Definition

Noun: - Le Chatelier's Principle: A fundamental principle in chemistry stating that if a system at equilibrium experiences a change in concentration, temperature, volume, or pressure, the system will adjust its equilibrium position to counteract the effect of that change and establish a new equilibrium.

Usage

This principle is used to predict the directional shift of a chemical equilibrium in response to an external stress. - According to Le Chatelier's principle, increasing the pressure will shift the equilibrium toward the side with fewer moles of gas. - When applying Le Chatelier's principle to an exothermic reaction, lowering the temperature favors the forward reaction.

Advanced Usage
  • Qualitative Predictions: The principle provides a qualitative, not quantitative, framework for predicting equilibrium behavior. It explains "why" a shift occurs, not "how much."
    • While Le Chatelier's principle correctly predicts the direction of shift, it does not provide the new equilibrium concentrations; that requires calculation.
  • Broad Application: Though rooted in chemistry, the principle's conceptual framework is sometimes applied analogously in economics, biology, and other fields describing systems in dynamic balance.
    • One can think of market forces using a concept similar to Le Chatelier's principle, where supply and demand adjust to external pressures.
Variants and Related Words
  • Le Chatelier's Law: An alternative name for the same principle.
  • Equilibrium Principle: A more general term that can encompass Le Chatelier's principle.
  • Chatelier's Principle: A common shortened form (though "Le Chatelier's" is standard).
Synonyms
  • Equilibrium Law: A less common synonym emphasizing its role as a governing rule for equilibria.
  • Principle of Mobile Equilibrium: A descriptive synonym highlighting the system's tendency to adjust.
Related Phrases/Concepts
  • Common Ion Effect: An application of Le Chatelier's principle where adding an ion common to an equilibrium suppresses the dissociation of a weak electrolyte.
    • The decrease in solubility due to a common ion is explained by Le Chatelier's principle.
  • Effect of a Catalyst: It is crucial to note that while a catalyst speeds up the attainment of equilibrium, it does not shift the equilibrium position itself, a point clarified by Le Chatelier's principle.
    • Le Chatelier's principle reminds us that a catalyst affects only the rate, not the equilibrium constant.
Noun
  1. the principle that if any change is imposed on a system that is in equilibrium then the system tends to adjust to a new equilibrium counteracting the change

Từ đồng nghĩa