Le Chatelier's Principle and Equilibrium

The video tutorial explores Le Chatelier's principle, explaining how chemical reactions at equilibrium respond to various stresses such as changes in concentration, temperature, and pressure. It illustrates how systems adjust to maintain balance, using examples to demonstrate shifts in equilibrium. The tutorial also provides insights into exothermic and endothermic reactions, and how volume and pressure changes influence gaseous equilibria. The video concludes with a call for questions and additional resources for further learning.

What is the main idea behind Le Chatelier's Principle?

• It describes how systems at equilibrium respond to stress.

• It explains the rate of chemical reactions.

• It measures the temperature of reactions.

• It predicts the color change in reactions.

How does adding more reactants affect the equilibrium of a reaction?

• The equilibrium shifts to the right.

• The equilibrium remains unchanged.

• The reaction stops completely.

• The equilibrium shifts to the left.

What happens to the equilibrium when more products are added to a reaction?

• The equilibrium remains unchanged.

• The equilibrium shifts to the left.

• The reaction speeds up.

• The equilibrium shifts to the right.

In an exothermic reaction, how is heat treated according to Le Chatelier's Principle?

• As a reactant.

• As a catalyst.

• As a product.

• As an inhibitor.

What is the effect of increasing temperature on an endothermic reaction?

• The equilibrium shifts to the left.

• The equilibrium shifts to the right.

• The reaction stops.

• The equilibrium remains unchanged.

What is the role of Delta H in determining the nature of a reaction?

• It indicates the speed of the reaction.

• It predicts the pressure change in a reaction.

• It shows whether a reaction is exothermic or endothermic.

• It measures the color change in a reaction.

How does decreasing the volume of a container affect the pressure in a gaseous equilibrium?

• The pressure remains the same.

• The pressure decreases.

• The pressure increases.

• The reaction stops.

When the volume is increased in a gaseous equilibrium, towards which side does the equilibrium shift?

• The reaction stops.

• The equilibrium remains unchanged.

• Towards the side with more particles.

• Towards the side with fewer particles.

According to Le Chatelier's Principle, what happens when pressure is increased in a system with different moles on each side?

• The equilibrium shifts towards the side with more moles.

• The equilibrium shifts towards the side with fewer moles.

• The equilibrium remains unchanged.

• The reaction stops.

What should you do if you have additional questions about Le Chatelier's Principle?

• Ignore them.

• Search online for answers.

• Leave them in the comments section.

• Ask a friend.