Le Chatelier's Principle and Its Effects on Chemical Equilibrium

Professor Dave explains Le Chatelier's principle, which describes how a system at equilibrium responds to stress. He discusses three types of stress: changes in concentration, temperature, and volume/pressure. For concentration, adding reactants or products shifts equilibrium to restore balance. Temperature changes depend on whether a reaction is exothermic or endothermic, affecting equilibrium by treating heat as a reactant or product. Volume and pressure changes, especially in gases, shift equilibrium based on particle count. The video concludes with a comprehension check and encourages further learning.

What does Le Chatelier's Principle primarily describe?

• The behavior of gases under pressure

• The shift in equilibrium due to applied stress

• The formation of chemical bonds

• The rate of chemical reactions

If more reactants are added to a system at equilibrium, what is the expected shift?

• The equilibrium shifts to the left

• The equilibrium remains unchanged

• The equilibrium shifts to the right

• The reaction stops

What happens to the equilibrium if products are removed from the system?

• The equilibrium shifts to the right

• The equilibrium shifts to the left

• The reaction stops

• The equilibrium remains unchanged

How does an exothermic reaction respond to an increase in temperature?

• The equilibrium shifts to the right

• The equilibrium shifts to the left

• The reaction rate decreases

• The reaction stops

In an endothermic reaction, what role does heat play?

• Heat is a product

• Heat is a reactant

• Heat is a catalyst

• Heat is irrelevant

What is the effect of cooling down an exothermic reaction?

• The equilibrium shifts to the left

• The reaction stops

• The equilibrium shifts to the right

• The reaction rate increases

According to Boyle's Law, what happens to pressure when volume decreases?

• Pressure decreases

• Pressure remains constant

• Pressure increases

• Pressure becomes zero

In a gaseous equilibrium, if the volume is increased, which direction does the equilibrium shift?

• The reaction stops

• The equilibrium remains unchanged

• Towards the side with fewer particles

• Towards the side with more particles

What happens to the equilibrium when pressure is increased in a system with more moles of gas on one side?

• The equilibrium shifts towards the side with more moles

• The equilibrium remains unchanged

• The reaction stops

• The equilibrium shifts towards the side with fewer moles

In a reaction involving gases, what is the effect of decreasing the volume?

• The reaction stops

• The equilibrium remains unchanged

• The equilibrium shifts towards the side with more particles

• The equilibrium shifts towards the side with fewer particles