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 that an increase in temperature favors endothermic reactions, while a decrease favors exothermic ones. The video uses the example of nitrogen dioxide dimerization to illustrate color changes with temperature variations. It also clarifies that catalysts speed up reactions but do not alter equilibrium positions. The video concludes by summarizing these concepts.

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

• The system remains unchanged.

• The reaction stops completely.

• The endothermic reaction is favored.

• The exothermic reaction is favored.

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

• The mixture turns blue.

• The mixture becomes paler.

• The mixture becomes darker brown.

• The mixture remains the same color.

What is the effect of increasing temperature on the nitrogen dioxide and dinitrogen tetroxide reaction?

• More dinitrogen tetroxide is produced.

• The reaction rate decreases.

• More nitrogen dioxide is produced.

• The reaction stops.

How does a catalyst affect the position of equilibrium in a chemical reaction?

• It has no effect on the position of equilibrium.

• It shifts the equilibrium to the left.

• It stops the reaction.

• It shifts the equilibrium to the right.

What is the role of a catalyst in a chemical reaction at equilibrium?

• It increases the rate of the reverse reaction only.

• It decreases the rate of both reactions.

• It increases the rate of the forward reaction only.

• It increases the rate of both forward and reverse reactions.