Equilibrium Constants and Reactions

Mr. Andersen explains chemical equilibrium using a water demonstration, illustrating how reactants and products reach a state of balance. He introduces equilibrium constants (K) and reaction quotients (Q), using the Haber process as an example. The video covers calculating K and Q values, using ICE tables for equilibrium calculations, and solving equilibrium problems with given data. Key concepts include reversible reactions, stoichiometry, and the use of graphs to predict reaction directions.

What does the water demonstration in the video represent?

• The rate of reaction

• The formation of precipitates

• The process of dilution

• The concept of chemical equilibrium

In a reversible reaction at equilibrium, what is true about the rates of the forward and reverse reactions?

• The rates are equal

• The rates are zero

• The reverse reaction rate is higher

• The forward reaction rate is higher

What does the equilibrium constant (K) represent?

• The temperature of the reaction

• The speed of the reaction

• The ratio of products to reactants at equilibrium

• The ratio of reactants to products at equilibrium

If Q < K for a reaction, in which direction will the reaction proceed?

• It will stop completely

• It will remain unchanged

• To the right, forming more products

• To the left, forming more reactants

In the Haber process, what are the reactants used to produce ammonia?

• Ammonia and oxygen

• Nitrogen and oxygen

• Hydrogen and oxygen

• Nitrogen and hydrogen

What does a graph showing the concentration of reactants and products over time at equilibrium look like?

• Reactants increase and products decrease until they level off

• Reactants and products both decrease

• Reactants decrease and products increase until they level off

• Reactants and products both increase

How do you calculate the equilibrium constant (K) for a given reaction?

• By dividing the concentration of products by the concentration of reactants

• By multiplying the concentration of reactants

• By dividing the concentration of reactants by the concentration of products

• By adding the concentration of reactants and products

What is the purpose of an ICE table in equilibrium calculations?

• To determine the pH of the solution

• To calculate the speed of the reaction

• To track the initial, change, and equilibrium concentrations

• To measure the temperature change

If the initial concentration of a reactant is 1 M and it decreases by 0.5 M, what is the change in concentration?

• 0.5 M

• 1.5 M

• 0.25 M

• 1 M

When given initial concentrations and the equilibrium constant, what can you determine using an ICE table?

• The final temperature

• The final pressure

• The equilibrium concentrations

• The reaction rate