Chemical Equilibrium Concepts Assessment

The video tutorial explores the concept of chemical equilibria, starting with a standard reaction of magnesium and hydrochloric acid, which is a one-directional reaction. It then introduces reversible reactions using hydrogen and iodine, explaining how these reactions can move in both directions, leading to a dynamic equilibrium. The tutorial describes dynamic equilibrium as a state where the rate of the forward reaction equals the rate of the reverse reaction, using a treadmill analogy to illustrate the concept. It emphasizes the importance of a closed system for maintaining equilibrium, where matter cannot enter or escape, ensuring constant concentrations of reactants and products.

What happens to a one-directional chemical reaction when one of the reactants is completely used up?

• The reaction reverses.

• The reaction speeds up.

• The reaction continues indefinitely.

• The reaction stops.

In a reversible reaction, what does the reversible arrow indicate?

• The reaction is irreversible.

• The reaction is instantaneous.

• The reaction can proceed in both forward and reverse directions.

• The reaction can only proceed in one direction.

What term is used to describe a process that never stops in chemistry?

• Reversible

• Equilibrium

• Dynamic

• Static

At what point do we say a reaction is in dynamic equilibrium?

• When the reaction stops completely.

• When the rates of the forward and reverse reactions are equal.

• When the reverse reaction is faster than the forward reaction.

• When the forward reaction is faster than the reverse reaction.

In the treadmill analogy, what does the runner represent?

• The closed system

• The equilibrium state

• The forward reaction

• The reverse reaction

What remains constant at equilibrium in a chemical reaction?

• The concentrations of all species

• The volume

• The pressure

• The temperature

Why is it important for a chemical equilibrium to be in a closed system?

• To allow energy to escape

• To prevent matter from entering or escaping

• To increase the reaction rate

• To decrease the reaction rate

What can pass in and out of a closed system in chemical equilibria?

• Matter

• Energy

• Both matter and energy

• Neither matter nor energy

What would happen to the equilibrium if the system was not closed?

• The reaction would reverse.

• The reaction would stop.

• The equilibrium would be disrupted.

• The equilibrium would remain unchanged.

What is the role of the sealed container in maintaining equilibrium?

• It speeds up the reaction.

• It ensures matter cannot enter or escape.

• It prevents energy from entering.

• It allows matter to escape.