About this video

• Video Title: Le Chatelier's Principle
• Channel: The Organic Chemistry Tutor
• Speakers: [None specified in the transcript]
• Duration: 00:26:40

Overview

This video explains Le Chatelier's Principle, which states that if a system at equilibrium is subjected to a change, the system will shift in a direction that counteracts that change. The video uses chemical reaction examples to illustrate how changes in concentration, pressure, and volume affect the equilibrium position.

Key takeaways

• Le Chatelier's Principle: When a system at equilibrium experiences a disturbance (stress), it will shift in a way that minimizes or counteracts that stress.
• Dynamic Equilibrium: In a chemical reaction at equilibrium, the forward and reverse reactions occur at equal rates, resulting in constant concentrations of reactants and products.
• Effect of Concentration Changes: Increasing the concentration of a reactant or product will cause the equilibrium to shift away from that substance. Conversely, decreasing the concentration will cause a shift towards that substance to restore equilibrium.
• Effect of Volume/Pressure Changes: For reactions involving gases, changing the volume or pressure will shift the equilibrium towards the side with fewer moles of gas if pressure increases (volume decreases) and towards the side with more moles of gas if pressure decreases (volume increases).
• Inert Substances: Changes in the amount of substances in the solid or liquid phase, as well as the addition of inert gases, do not affect the position of equilibrium.
• Catalysts: Catalysts speed up both the forward and reverse reactions equally, thus they do not shift the position of equilibrium.