LeChatelier's Principle
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General Chemistry 1
Summary
The essence of the content revolves around explaining Le Chatelier's principle and its application in predicting the effects of various changes on a chemical equilibrium.
- Le Chatelier's principle states that a chemical system at equilibrium will adjust to counteract any imposed change, aiming to re-establish equilibrium.
- Adding or removing reactants or products, changing pressure, or altering temperature can shift the equilibrium position either to the right (towards products) or to the left (towards reactants).
- The concept of a seesaw is introduced as a visual aid to understand how changes in reactant or product concentrations, pressure, and temperature influence the direction of the equilibrium shift.
- The impact of adding a catalyst or a noble gas on the equilibrium position is discussed, highlighting that neither changes the position of equilibrium.
- Specific examples, including the addition of sodium bicarbonate and changes in pH, illustrate how to apply Le Chatelier's principle to predict the outcome of changes in a chemical system.
Chapters
00:00
Understanding Le Chatelier's Principle
03:03
Applying Pressure and Temperature Changes
10:34
Exceptions to Equilibrium Shifts