Chemical Equilibrium and Reaction Yield

This video tutorial by Mr. Andersen covers Le Chatelier's Principle, explaining how it applies to reversible reactions. The principle states that if a system at equilibrium experiences a disturbance, it will adjust to counteract the change. The video provides examples, such as the Haber process, to illustrate how changes in concentration, pressure, volume, and temperature affect equilibrium. It also discusses strategies to increase reaction yield by manipulating these factors.

What does Le Chatelier's Principle primarily address in a chemical reaction?

• The speed of the reaction

• The color change in the reaction

• The formation of new compounds

• The counteraction of disturbances in equilibrium

In the Haber process, what happens when there is an increase in hydrogen concentration?

• The reaction remains unchanged

• The reaction shifts to the right, increasing ammonia

• The reaction shifts to the left, decreasing ammonia

• The reaction shifts to the left, increasing nitrogen

In the context of Le Chatelier's Principle, what does an increase in reactants typically cause?

• A shift to the left

• A decrease in product formation

• A shift to the right

• No change in equilibrium

How does a decrease in volume affect the equilibrium of a gas reaction?

• It has no effect on the equilibrium

• It increases the pressure and shifts the reaction to the side with more moles

• It increases the pressure and shifts the reaction to the side with fewer moles

• It decreases the pressure and shifts the reaction to the right

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

• The reaction shifts to the left

• The reaction becomes exothermic

• The reaction shifts to the right

• The reaction rate decreases

What happens to the color of nitrogen dioxide when the temperature is increased?

• It remains the same

• It turns blue

• It becomes darker

• It becomes colorless

In an exothermic reaction, how can you increase the yield of the product?

• Add more products

• Increase the volume

• Decrease the temperature

• Increase the temperature

How can you increase the yield of ammonia in the Haber process by changing pressure?

• Decrease the pressure

• Increase the pressure

• Add more nitrogen

• Add more ammonia

What is the result of decreasing the temperature in an exothermic reaction?

• The reaction shifts to the right

• The reaction shifts to the left

• The reaction rate increases

• The reaction becomes endothermic

What is a common strategy to increase the yield of a product in a chemical reaction?

• Decrease the concentration of reactants

• Increase the concentration of reactants

• Increase the concentration of products

• Decrease the pressure