Dynamic Equilibrium in Chemical Reactions

The video introduces dynamic equilibrium, a key concept in chemistry, using water evaporation and condensation as an example. It explains the conditions necessary for equilibrium, such as a closed system and equal rates of forward and backward reactions. A generic reaction is used to illustrate how equilibrium is established, emphasizing that the rate, not the quantity, of reactants and products is equal. An escalator analogy helps visualize the concept, and the video concludes with key points and a summary.

What is the primary reason dynamic equilibrium is significant in chemistry?

• It only occurs in laboratory settings.

• It is only applicable to gaseous reactions.

• It occurs in almost every chemical reaction.

• It is a rare phenomenon.

In a closed system, what is crucial for establishing dynamic equilibrium?

• Reactants and products cannot escape.

• Reactants and products must be able to escape.

• The system must be open to the environment.

• The system must be at a constant temperature.

What does the term 'dynamic' in dynamic equilibrium refer to?

• The system is constantly changing in composition.

• The forward and backward reaction rates are equal.

• The temperature of the system is fluctuating.

• The system is static.

When a system is in equilibrium, what should remain unchanged?

• The volume of the system.

• The pressure of the system.

• The temperature of the system.

• The color and density of the system.

How can equilibrium be established in a chemical reaction?

• Only when the system is heated.

• Only from the forward direction.

• Only from the backward direction.

• From either the forward or backward direction.

In the generic example of A + B ⇌ C + D, what happens initially?

• The products are immediately formed in large quantities.

• The reaction is fast due to high reactant concentration.

• The reaction is slow due to low reactant concentration.

• The reaction does not occur.

What is the key point about the rates of reactions in equilibrium?

• The rates of the forward and backward reactions are equal.

• The backward reaction rate is always higher.

• The forward reaction rate is always higher.

• The rates of the forward and backward reactions are different.

In the escalator analogy, what does standing still on the escalator represent?

• The reaction is moving towards equilibrium.

• The reaction is in equilibrium with equal reaction rates.

• The reaction is in equilibrium with equal amounts of reactants and products.

• The reaction is not in equilibrium.

What common mistake do students make regarding equilibrium?

• Assuming the amounts of reactants and products are equal.

• Assuming the system must be open.

• Assuming the temperature must be constant.

• Assuming the reaction stops completely.

What does the escalator analogy help illustrate about equilibrium?

• The importance of temperature in equilibrium.

• The concept of equal reaction rates.

• The role of pressure in equilibrium.

• The need for a closed system.