chemical equilibrium le chatelier
Overview
This lesson explores the dynamic nature of chemical equilibrium, where forward and reverse reaction rates are equal, resulting in constant macroscopic properties. We will delve into how various factors can shift the position of this equilibrium, as predicted by Le Chatelier's Principle, and understand its industrial significance.
Introduction to Reversible Reactions and Equilibrium
Most chemical reactions are reversible, meaning that products can react to reform reactants. When a reversible reaction occurs in a closed system, it eventually reaches a state of **chemical equilibrium**. At equilibrium, the **rate of the forward reaction is exactly equal to the rate of the reverse...
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Key Concepts
- Reversible Reaction: A reaction that can proceed in both the forward and reverse directions simultaneously.
- Chemical Equilibrium: A dynamic state where the rates of the forward and reverse reactions are equal, and the net concentrations of reactants and products remain constant.
- Le Chatelier's Principle: If a change of condition is applied to a system in equilibrium, the system will shift in a direction that relieves the stress.
- Equilibrium Constant (Kc/Kp): A value that expresses the ratio of product concentrations to reactant concentrations at equilibrium, indicating the extent of a reaction.
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Exam Tips
- →Always state Le Chatelier's Principle when explaining shifts in equilibrium, then apply it to the specific stress.
- →Remember that catalysts only affect the rate of reaction, not the position of equilibrium or the value of Kc/Kp.
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