Le Chatelier's Principle Part 1

The video explains Le Chatelier's Principle, which describes how a system at equilibrium responds to stresses such as changes in concentration, pressure, and temperature. Using examples, it illustrates how equilibrium shifts to counteract these stresses, ensuring the system returns to equilibrium. The principle is applied to both concentration and pressure changes, with specific focus on gaseous systems.

What is the primary goal of a system at equilibrium when it is subjected to stress?

• To decrease the temperature

• To increase the pressure

• To restore equilibrium

• To increase the concentration of reactants

When additional reactants are added to a system at equilibrium, in which direction does the equilibrium shift?

• It remains unchanged

• It oscillates back and forth

• To the right

• To the left

If the concentration of products in a reaction is decreased, what happens to the equilibrium?

• It shifts to the right

• It becomes unstable

• It shifts to the left

• It remains unchanged

How does an increase in pressure affect the equilibrium of a gaseous reaction?

• It shifts to the side with fewer moles

• It causes the reaction to stop

• It shifts to the side with more moles

• It remains unchanged

What happens to the equilibrium when the pressure is decreased in a gaseous system?

• It causes the reaction to reverse

• It remains unchanged

• It shifts to the side with fewer moles

• It shifts to the side with more moles