What Is Dynamic Equilibrium?

The video tutorial explains dynamic equilibrium using a digging analogy, where two processes occur at the same rate, resulting in no observable change. It outlines the criteria for equilibrium: a reversible process in a closed system. An example of hydrogen and iodine reacting to form hydrogen iodide is provided, illustrating how equilibrium is achieved when forward and reverse reactions occur at the same rate. The video also covers phase change equilibrium using bromine as an example. In summary, equilibrium is when the forward and reverse reaction rates are equal, with no observable changes.

What happens to the size of the hole if you and your friend dig and refill at the same speed?

• The hole disappears completely.

• The size of the hole remains unchanged.

• The hole gets smaller.

• The hole gets larger.

Which of the following is NOT a requirement for a chemical system to reach equilibrium?

• The process must occur in a closed system.

• The system must be closed.

• The system must be open.

• The process must be reversible.

In the reaction between hydrogen and iodine, what happens to the concentrations of reactants and products at equilibrium?

• The concentrations of both remain constant.

• The concentrations of products decrease.

• The concentrations of reactants increase.

• The concentrations of both increase.

What would happen to the equilibrium of the hydrogen and iodine reaction if the container lid is removed?

• The system remains at equilibrium.

• The reaction stops completely.

• The system reaches a new equilibrium.

• The system is no longer at equilibrium.

What is the result when liquid bromine equilibrates to gaseous bromine at room temperature?

• The gaseous bromine completely condenses.

• There is no observable macroscopic change.

• The liquid bromine completely evaporates.

• The system becomes unstable.