Experimeni 25 PROCEDURE 1. Obtain and wear pouples 2. Set up the data collection system, Connect a LabPro or CBL 2 interface to the computer or handheld with the proper cable, a. Connect a Colorimeter to Channel 1 of your interface, b. Start the data collection program e. Set up the Time Graph data collection for 5 seconds per sample and 24 mmples, 3. Set up and calibrate the Colorimeter a. Prepare a blank by filling an empty cuvette % full with distilled water. Place the blank in the cuvette slot of the Colorimeter and close the lid b. If your Colorimeter has a CAL button, set the wavelength on the Colorimeter to 430 nm, press the CAL button and proceed directly to Step 4. If your Colorimeter does not have a CAL button, calibrate your Colorimeter manually for the Blue LED, 4. Obtain the materials you will need to conduct this experiment, • Three 25 ml graduated cylinders. . Approximately 100 mL of 0.020 M KI solution in a 100 mL beaker, Approximately 100 ml of 0.020 M FeCl, solution in a separate 100 mL beaker, CAUTION: The FeCTz solution in this experiment is prepared in 0.7 M HCl and should be handled with care. • Approximately 60 ml of distilled water in a third 100 ml beaker, 5. During this experiment you will conduct 5 trials. This step describes the process for conducting the trials using the Trial I volumes. When you repeat this process, use the correct yolume for each trial based on the table below. Feci, (ml) 20.0 KI (mL) 20.0 HO (mL) 00 1 200 10.0 100 10.0 20.0 10.0 4 160 10.0 15.0 10.0 160 15.0 CHANGES Color a. Measure 20.0 ml of FeCl, solution into a 100 ml beaker, b. Measure 20.0 ml of KI solution into a second 100 ml beaker, e. Remove the cuvette from the Colorimeter and pour out the distilled water, d. Add the 20.0 mL of FeCl, solution to the beaker of KI solution. Swirl the beaker to mix. e. Rinse the cuvette twice with l-ml amounts and then fill it full, Wipe the outside of the cuvette with a tissue, place it in the Colorimeter, and close the lid. 6. Begin collecting absorbance data. Data will be gathered for 2 minutes. Observe the progress of the reaction in the beaker, 7. When the data collection is complete, carefully remove the cuvette from the Colorimeter. Dispose of the contents of the beaker and cuvette as directed. Rinse and clean the beakers and the cuyette for the next trial. 25.2 Advanced Chemistry with Pernier The Rate and Order of a Chemical Reaction 8. Examine the graph of the reaction Select a linear region of the graph that covers 30-40 seconds of the reaction and represents the entire graph. Calculate the best fit line, or linear regression, equation for this region Record the slope, in your data table, as the initial rate the reaction 9. Repeat the necessary steps to conduct Trials 2-5. DATA TABLE Trial [Feco IKO Initial rate (s) 3 5 DATA ANALYSIS 1. Calculate the molar concentration of Fech, and Ki for each reaction and record the values in the table above. Provide one example to show how you completed the calculation 2. What is the order of the reaction in FeCl, and KI? Explain. 3. Write the rate law expression for the reaction. 4. Is it possible to calculate the rate constant, k, from your data? If so, calculate the rate constant. If not, explain why not. 25 Advanced Chemistry with Vernier 2000 T-Mobile LTE 1:59 PM 10 20% o х то Experiment 25 INTROR The Rate and Order of a Chemical Reaction A basic kinetic study of a chemical reaction often involves conducting the reaction at varying concentrations of reactants. In this way, you can determine the order of the reaction in each species, and determine a rate law expression. Once you select a reaction to examine, you must decide how to follow the reaction by measuring some parameter that changes regularly as time passes, such as temperature, pH, pressure, conductance, or absorbance of light. In this experiment you will conduct the reaction between solutions of potassium iodide and iron (III) chloride. The reaction equation is shown below, in ionic form. 21 (aq) + 2 Fe+ (aq) — 12 (aq) + 2 Fe2+ (aq) As this reaction proceeds, it undergoes a color change that can be precisely measured by a Colorimeter (see Figure 1). By carefully varying the concentrations of the reactants, you will determine the effect each reactant has on the rate of the reaction, and consequently the order of the reaction. From this information, you will write a rate law expression for the reaction. OBJECTIVES In this experiment, you will • Conduct the reaction of KI and FeCl3 using various concentrations of reactants. • Determine the order of the reaction in KI and FeCl3. • Determine the rate law expression for the reaction. Light SOURCE Detector Figure 1 MATERIALS LabPro or CBL 2 interface computer or handheld device Vernier Colorimeter two 100 mL beakers plastic cuvettes five plastic Beral pipets 0.020 M potassium iodide, KI, solution 0.020 M iron (III) chloride, FeCl3, solution, in 0.10 M HCI distilled water three 25 ml graduated cylinders 25-1 Advanced Chemistry with Vernier Vernier Software & Technology
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