Le Chatelier's Principle

Mr. Anderson explains Le Chatelier's Principle, which describes how reversible reactions respond to disturbances in equilibrium. He uses examples like the Haber process to illustrate how changes in concentration, pressure, and temperature can shift reactions to re-establish equilibrium. The video also covers strategies to increase yield in chemical reactions by manipulating these factors.

What does Le Chatelier's Principle predict when a system at equilibrium experiences a disturbance?

• The reaction will shift to counteract the disturbance.

• The reaction will stop completely.

• The reaction will become irreversible.

• The reaction will speed up indefinitely.

In the Haber process, what happens to the concentration of ammonia when there is an influx of hydrogen?

• It becomes zero.

• It increases.

• It remains unchanged.

• It decreases.

How does decreasing the volume of a gas mixture affect the equilibrium according to Le Chatelier's Principle?

• It increases the number of moles of gas.

• It decreases the pressure.

• It causes the reaction to shift towards the side with fewer moles of gas.

• It has no effect on the equilibrium.

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

• The reaction shifts to the right.

• The reaction shifts to the left.

• The reaction becomes exothermic.

• The reaction rate decreases.

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

• Add more products.

• Decrease the temperature.

• Increase the volume.

• Increase the temperature.

What happens to the color of a gas mixture when the temperature is increased in an endothermic reaction?

• It becomes colorless.

• It becomes lighter.

• It becomes darker.

• It remains the same.

How can pressure changes be used to increase the yield of ammonia in the Haber process?

• By increasing the pressure to favor the side with more moles.

• By increasing the pressure to favor the side with fewer moles.

• By decreasing the pressure to favor the side with fewer moles.

• By decreasing the pressure to favor the side with more moles.