Reversible Reactions and Dynamic Equilibrium Explained

The video tutorial covers reversible reactions and dynamic equilibrium. It begins by explaining the difference between reversible and irreversible reactions, highlighting the role of chemical equations. The tutorial then delves into the concept of dynamic equilibrium, illustrating how forward and backward reactions reach a balance. It discusses the importance of a closed system for achieving equilibrium and explores how changes in temperature, pressure, and concentration can shift the equilibrium position. The tutorial concludes with examples and graphical representations to reinforce understanding.

What distinguishes a reversible reaction from an irreversible one?

• Irreversible reactions require more energy.

• Reversible reactions have arrows pointing in both directions.

• Reversible reactions only form products.

• Irreversible reactions can go in both directions.

In a reversible reaction, if one direction is exothermic, what is true about the other direction?

• It is also exothermic.

• It is endothermic.

• It requires no energy.

• It stops the reaction.

What is dynamic equilibrium?

• A state where reactions stop completely.

• A state where the forward and backward reaction rates are equal.

• A state where only products are formed.

• A state where only reactants are present.

Why is a closed system necessary for dynamic equilibrium?

• To keep the total amount of reactants and products constant.

• To allow gases to escape.

• To increase the reaction rate.

• To decrease the reaction rate.

How can the position of dynamic equilibrium be changed?

• By changing the color of the reactants.

• By removing all reactants.

• By altering the temperature, pressure, or concentration.

• By adding more products.

What happens when you increase the temperature in a reversible reaction?

• The reaction shifts towards the exothermic direction.

• The reaction stops.

• The reaction shifts towards the endothermic direction.

• The reaction becomes irreversible.

What is the effect of increasing pressure on a gaseous equilibrium system?

• It favors the side with more moles of gas.

• It has no effect on the equilibrium.

• It stops the reaction completely.

• It favors the side with fewer moles of gas.