Chemical Equilibrium Dynamics Through Water Jar Demonstrations

Mr. Andersen explains chemical equilibrium using a water demonstration, illustrating how reactants and products reach a state of balance. He introduces the concepts of Q and K values, showing how they predict reaction direction. Graphs are used to depict equilibrium states and reaction rates. The video covers calculating equilibrium constants and using ICE tables to solve equilibrium problems, with examples from the Haber process.

What does the demonstration with water jars illustrate in terms of chemical reactions?

• The temperature of the reaction

• The speed of a reaction

• The concept of equilibrium

• The amount of reactants used

In the Haber process, what happens to the concentrations of reactants and products over time?

• They increase indefinitely

• They decrease indefinitely

• They fluctuate randomly

• They reach a constant state

What does it mean when the concentrations of reactants and products remain constant over time?

• The reaction has reached equilibrium

• The reaction is slowing down

• The reaction is speeding up

• The reaction is incomplete

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

• The reaction will move to the right

• The reaction will move to the left

• The reaction will stop

• The reaction is at equilibrium

What happens if the Q value is greater than the K value?

• The reaction will stop

• The reaction is at equilibrium

• The reaction will move to the left

• The reaction will move to the right

How can you determine the direction of a reaction using a number line?

• By placing only Q on the line

• By placing only K on the line

• By placing K and Q on the line and moving towards Q

• By placing K and Q on the line and moving towards K

How is the equilibrium constant (K) calculated for a reaction?

• By adding the concentrations of reactants

• By subtracting the concentrations of products

• By dividing the concentration of products by reactants

• By multiplying the concentrations of reactants

In the equilibrium formula, what does the exponent represent?

• The speed of the reaction

• The moles of each substance

• The pressure of the system

• The temperature of the reaction

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

• To calculate the speed of reaction

• To determine the color change

• To track changes in concentration

• To measure the temperature change

Why are stoichiometric coefficients important in ICE tables?

• They affect the concentration changes

• They change the color of the solution

• They determine the temperature

• They increase the reaction speed