Chemical Equilibrium & Dynamic Equilibrium

The video explains chemical equilibrium, using the formation of hydrogen iodide as an example. It describes how reactions can be reversible, leading to a state of dynamic equilibrium where reactants and products coexist with constant concentrations. The video also differentiates between forward and backward reactions, emphasizing that at equilibrium, their rates are equal.

What is the nature of the reaction between hydrogen and iodine to form hydrogen iodide?

• It is a reversible reaction.

• It is a spontaneous reaction.

• It is an irreversible reaction.

• It is a non-reversible reaction.

What happens to the concentrations of reactants and products at dynamic equilibrium?

• They both increase.

• They both decrease.

• They remain constant.

• They fluctuate randomly.

In a dynamic equilibrium, how do the forward and backward reactions proceed?

• Only the forward reaction occurs.

• Both reactions occur simultaneously.

• Only the backward reaction occurs.

• Both reactions stop.

What is the forward reaction in a chemical equilibrium?

• Conversion of products into reactants.

• Conversion of reactants into products.

• No conversion occurs.

• Conversion of reactants into energy.

At dynamic equilibrium, how do the rates of forward and backward reactions compare?

• The rates are equal.

• The backward reaction is faster.

• The forward reaction is faster.

• The reactions do not have rates.