5 Questions
Which of the following is the definition of Le Chatelier's principle?
Changing the conditions of a reversible reaction will shift the position of equilibrium to counteract that change.
What does it mean if the equilibrium lies to the left?
There are more reactants than products at equilibrium.
What does it mean if the equilibrium lies to the right?
There are more products than reactants at equilibrium.
What is the purpose of Le Chatelier's principle?
To predict the outcome of a reaction when conditions are changed.
What is the reaction being used as an example in the video?
The production of ammonia from nitrogen and hydrogen.
Study Notes
Le Chatelier's Principle
- Le Chatelier's principle states that when a system in equilibrium is subjected to a change, the equilibrium will shift in a direction that tends to counteract the change.
Equilibrium Shift
- If the equilibrium lies to the left, it means that the reaction favors the reactants, indicating that the concentration of reactants is higher than the concentration of products.
- If the equilibrium lies to the right, it means that the reaction favors the products, indicating that the concentration of products is higher than the concentration of reactants.
Purpose of Le Chatelier's Principle
- The purpose of Le Chatelier's principle is to predict how a system in equilibrium will respond to changes in concentration, pressure, or temperature.
Example Reaction
- The reaction being used as an example in the video is not specified in the given text, but it is likely to be a reversible reaction that illustrates the concept of equilibrium and Le Chatelier's principle.
Test your knowledge on Le Chatelier's principle and its impact on the position of equilibrium. This quiz covers the effects of temperature, pressure, and concentration on reversible reactions. Evaluate your understanding of reactant and product particle ratios at equilibrium.
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