Calculations and Analysis: Looking at the graphs provided in the experiment, describe what is happening at the point where all lines are horizontal:
in terms of reaction rate
in terms of concentration
in terms of reaction completion

Create a general graph representing concentration vs. time for trial 6.
Remember, this is a qualitative graph showing a general comparison of concentrations observed in the reaction. There are no data values to be plotted on the graph.
Be sure to label each axis and line on the graph.
Conclusion:
Write a conclusion statement that addresses the following questions:
Explain what the color change indicated about the changes in the concentrations of Co(H2O)62+ and CoCl42– in each trial.
Do your data support or fail to support your hypothesis (include examples)?
How do you think the investigation can be explored further?
Post-Lab Reflection Questions
Answer the reflection questions using what you have learned from the lesson and your experimental data. It will be helpful to refer to your chemistry journal notes. Answer questions in complete sentences.
How did the change of stress (adding or removing reactants or products) cause a shift in the equilibrium system of your solutions? Use data to support your answer. Make sure you discuss all four stress changes:
Adding a reactant
Adding a product
Removing a reactant
Removing a product

Concentration is just one stress that can affect the equilibrium position. Another is temperature. Describe how you would design this experiment to test for the effects of temperature on equilibrium position. Include a description of the experiment and describe what you would look for to see changes in the equilibrium position.

The equilibrium system Co(H2O)62+ + 4Cl– ⇌ CoCl42– + 6H2O is endothermic as written, meaning heat is a reactant for the forward reaction and a product for the reverse reaction. Based on that information and your findings from this experiment, predict what you would expect to observe in the experiment you described above when you tested the effects of temperature on an equilibrium position.