07_06_lab_report

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Equilibrium Lab Report Instructions: For this investigative phenomenon, you will observe the changes that result when you add more of, or take away some of, one of the components of the equilibrium (known as a stress) and determine if there are trends in the behavior of equilibrium systems. Record your observation in the lab report below. You will submit your completed report. Title: Equilibrium Lab Objective(s): Be able to determine the effect of altering the concentration, either increasing or decreasing it, on the equilibrium. Hypothesis: If the amount of reactant increases, the rate of the forward reaction will decrease to reach a new equilibrium. If the amount of reactant decreases, the rate of the forward reaction will increase to reach a new equilibrium. Procedure: Access the virtual lab and complete the inquiry experiment. List your controlled variables, independent variables, and dependent variables. Explain why these are the variables. Summarize the steps of the experimental procedure. Materials: Equilibrium Virtual Lab Variables: Remember, controlled variables are factors that remain the same throughout the experiment. An independent (test) variable changes so that the experimenter can see the effect on other variables. The dependent (outcome) variable will change in response to the test variable. Controlled variables: concentrations Independent variable: added reactants Dependent variable: color of the product Summary of Steps: Include a summary of steps here. We have included the first two important steps to get you started. You can summarize the rest from the virtual lab.

1. Write down the equilibrium equation you are investigating using the information provided by the introduction within the virtual lab activity Equilibrium reaction: Co( H 2 O ¿ ¿ 2 + ¿ ¿ +4C l − ¿ ¿ CoC ⇆ l 4 2 − ¿¿ +6 H 2 O 2. Select each control test tube to compare the concentrations of reactants and products. Write down what each indicator color means about the concentrations of reactants and products in solution. Pink means: Co( H 2 O ¿ ¿ 2 + ¿ ¿ Blue means: CoC l 4 2 − ¿¿ Purple means: C l − ¿ ¿ 3. select each test tube and add or remove the appropriate stress changes, stir with a clean and dry rod. repeat. 4. note the color before and after the reaction in the data table. Data: For each trial, make sure you record the initial color of the solution, what is added to the test tube (a description of the stress), and what happened after the substance was added. Also include a screenshot , sketch, or description of each graph of each trial. Initial Color End Color Screenshot, sketch, or description Trial One: Tube 1 Adding HCL purple light blue

Trial Two: Tube 1 Adding AgNO 3 light blue light pink Trial Three: Tube 2 Adding H 2 O purple bubblegu m pink

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Trial Four: Tube 3 Adding NaCl purple lavender Trial Five: Tube 3 Adding H 2 O Lavender bubblegu m pink

Trial Six: Tube 2 Adding CaCl 2 bubblegu m pink lavender Calculations and Analysis: 1. 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 The graphs show that at the point where all lines are horizontal, the reaction rates of the reactions are equal. ● in terms of concentration The graphs show that at the point where all lines are horizontal, the concentration of the reactants and products are equal. ● in terms of reaction completion The graphs show that at the point where all lines are horizontal, the reaction is not progressing towards completion due to the dynamic equilibrium being achieved. 2. 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(H 2 O) 6 2+ and CoCl 4 2– 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? When there was an increase of the concentration of Co(H 2 O) 6 2+ in a trial the result was a color change to pink while an increase in the concentration of CoCl 4 2– in a trial resulted in a color change to blue. My data supported my hypothesis that if the amount of reactant increases, the rate of the forward reaction will decrease to reach a new equilibrium and if the amount of reactant decreases, the rate of the forward reaction will increase to reach a new equilibrium. This is seen in the reactions where an increase in reactant concentration slows the progression of the reaction allowing it to reach a new equilibrium such as in the first trial. This investigation could be explored further with the addition of concentrations of varying qualities or different chemical combinations to see if other reactions occur when different substances and concentrations reach new equilibriums. 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.

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1. 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: a. Adding a reactant b. Adding a product c. Removing a reactant d. Removing a product Adding a reactant will increase the concentration of reactants and the reaction will try to reverse the increase by shifting the reaction towards the products to the right. Adding a product will increase the concentration of products and the reaction will attempt to reverse this and restore equilibrium which causes a shift to the left. Removing a reactant will decrease the concentration of causes a shift to the left as the reaction will work to find a new equilibrium while attempting to restore the previous equilibrium. Removing product will cause a decrease in the concentration of products and force the reaction to try and return to its previous equilibrium which it will be unable to do and causes a shift to the right. These are all seen in different trials with the addition and subtraction of both reactants and products. 2. 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. I would design an experiment to test for the effects of temperature on equilibrium by choosing solutions that were heated to different temperatures and compare the effects of the temperature to a room temperature control solution to analyze how the equilibrium shifts. You could look for if the solution changes color or if it reaches a boiling point at relatively the same time as the other solutions or something of that nature. 3. The equilibrium system Co(H 2 O) 6 2+ + 4Cl – ⇌ CoCl 4 2– + 6H 2 O 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. I predict that if heat was added to an endothermic reaction such as Co(H 2 O) 6 2+ + 4Cl – ⇌ CoCl 4 2– + 6H 2 O, then the equilibrium position would shift to the right as heat is considered to be a reactant and would shift depending on the increase or decrease of temperature.

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