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AP Chem Lab 6 Kinetics Lab.docx

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Department
Chemistry
Course
CHEM 1951
Professor
Dr.Acio
Semester
Fall

Description
Curt Kim, Jonathan Lee, Keshav Mantha, Bobbie Sheng AP Chemistry, Period 1 2/11/13 Title: Study of the Kinetics of a Reaction Goal: The goal of this experiment was to conduct the reaction between KI and Fe(NO 3 3ith varying concentrations of reactants, to determine the order of the reaction, and to find a rate law equation for the reaction. Procedure: To begin this lab, the spectrophotometer was set to a wavelength of 470 nm and calibrated to display transmittance. The first combination of reactants (10 mL of Fe(3 3) , 10 mL of KI, and 0 mL of water) was measured out and mixed together into a test tube. The test tube was immediately placed in the spectrophotometer machine and transmittance data was recorded every five seconds for 200 seconds. The test tube was then removed from the machine and washed, after which the process was repeated again with each of the other four reactant combinations (10 mL of Fe(NO ) 3 3 mL of KI, and 5 mL of water; 5 mL of Fe(NO ) ,3 3 mL of KI, and 5 mL of water; 7.5 mL of Fe(NO ) , 5 mL of KI, and 7.5 mL of water; 5 mL of 3 3 Fe(NO )3 37.5 mL of KI, and 7.5 mL of water; and 7.5 mL of Fe(NO )3 37.5 mL of KI, and 5 mL of water) Data: Transmittance data (%) Time (secs) Exp. 1 Exp. 2 Exp. 3 Exp. 4 Exp. 5 Exp. 6 5 55.1 88.1 80.2 87.2 83.6 81.2 10 52.6 86.1 75.9 85.8 81.4 78.6 15 50.1 84.7 71.1 84.4 79.0 74.8 20 47.5 83.0 68.4 83.2 76.4 72.6 25 45.0 81.5 65.5 82.0 74.2 69.2 30 43.3 79.8 62.5 80.6 72.2 67.0 35 41.1 79.1 59.8 79.2 70.2 64.6 40 39.4 77.4 57.5 77.8 68.2 62.6 45 37.7 76.2 55.7 76.8 66.4 60.0 50 36.0 75.2 53.8 75.6 65.0 58.0 55 34.7 73.6 52.1 74.4 63.2 56.0 60 33.7 72.4 50.6 73.2 61.6 54.2 65 32.5 71.0 49.0 72.2 60.0 52.4 70 31.3 70.0 47.4 71.2 58.6 50.6 75 30.3 69.2 46.3 70.2 57.2 49.0 80 29.2 68.2 44.9 69.2 56.0 47.4 85 28.6 67.0 43.9 68.2 54.6 45.8 90 27.7 66.4 42.8 67.2 53.4 44.2 95 26.8 65 41.7 66.6 52.4 42.8 100 26.1 64.1 40.7 65.6 51.4 41.6 105 25.2 63.4 39.8 64.6 50.2 40.2 110 24.5 62.5 38.9 63.8 49.2 39.4 115 24 61.7 38.0 62.8 48.2 38.2 120 23.6 61.0 37.3 62.0 47.2 37.2 125 22.8 60.0 36.6 61.4 46.2 36.0 130 22.3 59.2 35.8 60.4 45.4 35.0 135 21.7 58.5 35.3 59.6 44.4 34.2 140 21.3 57.7 34.4 58.8 43.6 33.2 145 20.7 57.0 33.9 58.0 42.8 32.2 150 20.3 56.5 33.3 57.4 42.0 31.4 155 19.9 55.7 32.7 56.6 41.2 30.6 160 19.5 55.0 32.1 56.0 40.6 29.8 165 19.1 54.5 31.6 55.2 39.8 29.0 170 18.7 54.0 31.0 54.4 39.2 28.2 175 18.3 53.1 30.6 53.8 38.4 27.2 180 17.9 52.5 30.1 53.4 37.8 26.6 185 17.6 52.0 29.5 52.6 37.2 25.8 190 17.3 51.4 29.2 51.8 36.6 25.2 195 17.0 50.8 28.8 51.2 35.8 24.6 200 16.7 50.4 28.3 50.6 35.2 24.0 This transmittance data was converted to absorbance data using the formula % Abs = (2-log(% Trans)) * 100%. Exp. 1 Exp. 2 Exp. 3 Exp. 4 Exp. 5 Exp. 6 5 25.9 5.5 9.6 5.9 7.8 9 10 27.9 6.5 12 6.7 8.9 10.5 15 30 7.2 14.8 7.4 10.2 12.6 20 32.3 8.1 16.5 8 11.7 13.9 25 34.7 8.9 18.4 8.6 13 16 30 36.4 9.8 20.4 9.4 14.1 17.4 35 38.6 10.2 22.3 10.1 15.4 19 40 40.5 11.1 24 10.9 16.6 20.3 45 42.4 11.8 25.4 11.5 17.8 22.2 50 44.4 12.4 26.9 12.1 18.7 23.7 55 46 13.3 28.3 12.8 19.9 25.2 60 47.2 14 29.6 13.5 21 26.6 65 48.8 14.9 31 14.1 22.2 28.1 70 50.4 15.5 32.4 14.8 23.2 29.6 75 51.9 16 33.4 15.4 24.3 31 80 53.5 16.6 34.8 16 25.2 32.4 85 54.4 17.4 35.8 16.6 26.3 33.9 90 55.8 17.8 36.9 17.3 27.2 35.5 95 57.2 18.7 38 17.7 28.1 36.9 100 58.3 19.3 39 18.3 28.9 38.1 105 59.9 19.8 40 19 29.9 39.6 110 61.1 20.4 41 19.5 30.8 40.5 115 62 21 42 20.2 31.7 41.8 120 62.7 21.5 42.8 20.8 32.6 42.9 125 64.2 22.2 43.7 21.2 33.5 44.4 130 65.2 22.8 44.6 21.9 34.3 45.6 135 66.4 23.3 45.2 22.5 35.3 46.6 140 67.2 23.9 46.3 23.1 36.1 47.9 145 68.4 24.4 47 23.7 36.9 49.2 150 69.3 24.8 47.8 24.1 37.7 50.3 155 70.1 25.4 48.5 24.7 38.5 51.4 160 71 26 49.3 25.2 39.1 52.6 165 71.9 26.4 50 25.8 40 53.8 170 72.8 26.8 50.9 26.4 40.7 55 175 73.8 27.5 51.4 26.9 41.6 56.5 180 74.7 28 52.1 27.2 42.3 57.5 185 75.4 28.4 53 27.9 42.9 58.8 190 76.2 28.9 53.5 28.6 43.7 59.9 195 77 29.4 54.1 29.1 44.6 60.9 200 77.7 29.8 54.8 29.6 45.3 62 “Examine the graph of the first trial. Select a linear region of the graph that covers about 30-45 seconds of the reaction. Record the slope as the initial rate of the trial 1 reaction, in your data data. Graph trials 2 through 5 as well.” -1 Initial Reaction Rate = Slope = 0.4221 sec Initial Reaction Rate = Slope = 0.1579 sec -1 -1 Initial Reaction Rate = Slope = 0.4071 sec Initial Reaction Rate = Slope = 0.1395 sec -1 Initial Reaction Rate = Slope = 0.255 sec -1 -1 Initial Reaction Rate = Slope = 0.3288 sec Analysis: 1. Calculate the molar concentration of Fe(NO3)3 and KI for each experiment. Density of Fe(NO3)3 = 1.68 g/mL MM of Fe(NO3)3 = 241.8597 g/mol mol/mL of a 100% Fe(NO3)3 = Density/MM = (1.68 g/mL)/(241.8597 g/mol) = 0.0069461758 mol/mL Density of KI = 1.72 g/mL MM of KI = 166.6026 g/mol mol/mL of a 100% KI = Density/MM = (1.72 g/mL)/(166.6026 g/mol) = 0.0103239685 mol/mL mol Fe(NO3)3 = mol/mL Fe(NO3)3 * ml Fe(NO3)3 = 0.0069461758 mol/mL * mL Fe(NO3)3 mol KI = mol/mL KI * mL KI = 0.0103239685 mol/mL * mL KI Experiment 1: mol Fe(NO3)3 = 0.0069461758 mol/mL * 10.0 mL Fe(NO3)3 = 0.069461758 mol Fe(NO3)3 mol KI = 0.0103239685 mol/mL * 10.0 mL KI = 0.103239685 mol KI Experiment 2: mol Fe(NO3)3 = 0.0069461758 mol/mL * 10.0 mL Fe(NO3)3 = 0.069461758 mol Fe(NO3)3 mol KI = 0.0103239685 mol/mL * 5.00 mL KI = 0.0516198425 mol KI Experiment 3: mol Fe(NO3)3 = 0.0069461758 mol/mL * 5.0 mL Fe(NO3)3 = 0.034730879 mol Fe(NO3)3 mol KI = 0.0103239685 mol/mL * 10.0 mL KI = 0.103239685 mol KI Experiment 4: mol Fe(NO3)3 = 0.0069461758 mol/mL * 7.5 mL Fe(NO3)3 = 0.0520963185 mol Fe(NO3)3 mol KI = 0.0103239685 mol/mL * 5.00 mL KI = 0.0516198425 mol KI Experiment 5: mol Fe(NO3)3 = 0.0069461758 mol/mL * 5.0 mL Fe(NO3)3 = 0.034730879 mol Fe(NO3)3 mol KI = 0.0103239685 mol/mL * 7.5 mL KI = 0.07742976375 mol KI Experiment 6: mol Fe(NO3)3 = 0.0069461758 mol/mL * 7.5 mL Fe(NO3)3 = 0.0520963185 mol Fe(NO3)3 mol KI = 0.0103239685 mol/mL * 7.5 mL KI = 0.07742976375 mol KI M = mol/L Experiment 1: Volume of solution = 10.0 mL Fe(NO3)3 + 10.0 mL KI + 0.0 mL H2O = 20.0mL = .0200L 0.069461758 mol Fe(NO3)3 / 0.0200L = 3.4730879M → 3.47M 0.103239685 mol KI / 0.0200L = 5.16198425M → 5.16M Experiment 2: Volume of solution = 10.0 mL Fe(NO3)3 + 5.0 mL KI + 5.0 mL H2O = 20.0mL = .0200L 0.069461758 mol Fe(NO3)3 / 0.0200L = 3.4730879M → 3.47M 0.0516198425 mol KI / 0.0200L = 2.580992125M → 2.58M Experiment 3: Volume of solution = 5.0 mL Fe(NO3)3 + 10.0 mL KI + 5.0 mL H2O = 20.0mL = .0200L 0.034730879 mol Fe(NO3)3 / 0.0200L = 1.73654395M → 1.737M 0.103239685 mol KI / 0.0200L = 5.16198425M → 5.16M Experiment 4: Volume of solution = 7.5mL Fe(NO3)3 + 5.0mL KI + 7.5 mL H2O = 20.0mL = 0.0200L 0.0520963185 mol Fe(NO3)3 / 0.0200L = 2.604815925M → 2.60M 0.0516198425 mol KI / 0.0200L = 2.580992125M → 2.58M Experiment 5: Volume of solution = 5.0mL Fe(NO3)3 + 7.5mL KI + 7.5 mL H2O = 20.0mL = 0.0200L 0.034730879 mol Fe(NO3)3 / 0.0200L = 1.73654395M → 1.737M 0.07742976375 mol KI / 0.0200L = 3.871488188M → 3.87M Experiment 6: Volume of solution = 7.5mL Fe(NO3)3 + 7.5mL KI + 5.0 mL H2O = 20.0mL = 0.0200L 0.0520963185 mol Fe(NO3)3 / 0.0200L = 2.604815925M → 2.60M 0.07742976375 mol KI / 0.0200L = 3.871488188M → 3.87M The following is a table that shows each experiments reactant concentrations and initial rates Experiment [Fe(NO3)3] [KI] Initial rate (sec ) 1 3.47M 5.16M 0.4221 2 3.47M 2.58M
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