Chapter 6: Equilibrium
Dynamic equilibrium describes a state where the rates of the forward and reverse reactions are equal, resulting in constant concentrations of reactants and products. Le Chatelier's Principle explains how a system at equilibrium reacts to changes in concentration, pressure, and temperature, shifting to maintain balance. Understanding the equilibrium constant (K) allows for predicting the extent of reactions and involves calculations related to both concentrations and partial pressures. The relationship between Gibbs free energy change (ĪG) and K further links thermodynamics to chemical equilibria.
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Sections
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What we have learnt
- The characteristics and significance of dynamic equilibrium in reversible reactions.
- How Le Chatelier's Principle predicts the shifts in equilibrium position due to changes in conditions.
- The definition and implications of the equilibrium constant (K) in determining the extent of reaction.
Key Concepts
- -- Dynamic Equilibrium
- A state in which the forward and reverse reactions occur at equal rates, resulting in constant concentrations of reactants and products.
- -- Le Chatelier's Principle
- A principle that states that if the conditions of a system at equilibrium are changed, the system will adjust to counteract the change and establish a new equilibrium.
- -- Equilibrium Constant (K)
- A ratio that expresses the concentrations or partial pressures of products to those of reactants at equilibrium, providing a measure of the extent of the reaction.
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