proceeds to equilibrium. Enter the initial molarities (values must be >= 0 and <= 5.0) and the temperature in degrees Kelvin and then click the "Enter" button. Plots of the molarities of A, B, and C versus time are displayed along with the equilibrium molarities and the value of K_c.

    Use the applet in the design and performance of experiments to answer the following questions. See the Tutorial for Experiment: Chemical Equilibrium II for an example and help.

1. If 4.0 mol/L of A and 4.0 mol/L of B are placed initially in the reaction container at 25^oC, what will be the change in the mol/L of A, B, and C?
2. What evidence do you have to confirm that the reaction has reached equilibrium?
3. If 1.0 mol/L of A, 1.0 mol/L of B, and 3.0 mol/L of C are placed initially in the reaction container at 25^oC, what will be the change in the mol/L of A, B, and C?
4. Does the equilibrium lie to the left or right?
5. If the reaction is at equilibrium and 1.0 mol/L of B is added to the container at 25^oC, will the reaction go to the left or to the right to reestablish the equilibrium?
6. If the reaction is at equilibrium and 1.0 mol/L of C is added to the container at 25^oC, will the reaction go to the left or to the right to reestablish the equilibrium?
7. If the reaction is at equilibrium and 1.0 mol/L of A and 1.0 mol/L of C are added to the container at 25^oC, will the reaction go to the left or right to reestablish the equilibrium?
8. If the reaction is at equilibrium and the temperature is increased by 100 degrees, does the equilibrium molarity of C increase or decrease?
9. Is the reaction exothermic or endothermic?

    Include data from your experiments to support your answers to the questions.

    If you have preformed all of the experiments, answered all of the questions, and completed the report to be submitted for credit, then you may check the Answers to Chemical Equilibrium II Questions