Chemical Equilibrium Concepts and Calculations

Mr. Andersen explains chemical equilibrium using a water demonstration. He discusses the concepts of Q and K values, their role in predicting reaction direction, and how to calculate equilibrium constants. The video also introduces ICE tables for solving equilibrium problems, using the Haber process as an example.

What does it mean for a chemical reaction to be at equilibrium?

• The reaction only proceeds in one direction.

• The reaction has stopped completely.

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

• The concentrations of reactants and products are equal.

In the context of equilibrium, what does the term 'reversible reaction' mean?

• The reaction can only proceed in one direction.

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

• The reaction only occurs under certain conditions.

• The reaction stops once products are formed.

In the Haber process, what are the initial concentrations of products?

• Unknown

• High

• Equal to reactants

• Zero

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

• They continue to change.

• They remain constant.

• They become equal.

• They become zero.

What does a Q value less than K indicate about the direction of a reaction?

• The reaction will move to the left.

• The reaction is at equilibrium.

• The reaction will stop.

• The reaction will move to the right.

What does a Q value greater than K suggest about a reaction?

• The reaction will stop.

• The reaction is at equilibrium.

• The reaction will move to the right.

• The reaction will move to the left.

How can you determine the direction of a reaction using Q and K values?

• By comparing their magnitudes.

• By adding them together.

• By subtracting Q from K.

• By multiplying them.

How is the equilibrium constant (K) calculated?

• By adding the concentrations of reactants and products.

• By dividing the concentration of products by reactants.

• By multiplying the concentrations of reactants and products.

• By subtracting the concentration of reactants from products.

What is the significance of the equilibrium constant (K) remaining the same?

• It means the concentrations are equal.

• It indicates the reaction has stopped.

• It shows the reaction is irreversible.

• It confirms the reaction is at equilibrium.

What is the role of stoichiometry in an ICE table?

• It only affects the equilibrium constant.

• It is not used in ICE tables.

• It guides the changes in concentration.

• It determines the initial concentrations.