Le Chatelier's Principle: Part 2

The video explains how a system at equilibrium responds to temperature changes, guided by Le Chatelier's principle. It discusses the energetics of reactions, highlighting the exothermic and endothermic nature of forward and reverse reactions. The video uses the example of nitrogen dioxide dimerization to illustrate how temperature changes affect equilibrium, favoring either the exothermic or endothermic reaction. It also clarifies that catalysts speed up reactions without altering equilibrium positions. An analogy of digging and refilling a hole is used to explain the concept of equilibrium.

What happens to a system at equilibrium when the temperature is increased?

• The exothermic reaction is favored.

• The reaction stops completely.

• The endothermic reaction is favored.

• The system remains unchanged.

In the reaction between nitrogen dioxide and dinitrogen tetroxide, what visual change occurs when the temperature is decreased?

• The mixture becomes more viscous.

• The mixture becomes paler.

• The mixture turns green.

• The mixture becomes darker brown.

How does an increase in temperature affect the production of nitrogen dioxide in the given reaction?

• More nitrogen dioxide is produced.

• Less nitrogen dioxide is produced.

• The amount of nitrogen dioxide remains the same.

• Nitrogen dioxide is completely consumed.

What is the effect of adding a catalyst to a system at equilibrium?

• It shifts the equilibrium position.

• It stops the reaction.

• It slows down the reaction.

• It speeds up the attainment of equilibrium.

In the metaphor of digging a hole, what does giving larger shovels represent?

• Decreasing the temperature.

• Increasing the temperature.

• Removing a reactant.

• Adding a catalyst.