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3. Plot In tin versus 1/T and determine the activation energy for the reaction from the slope. Include the graphs in your report.

3. Plot In tin versus 1/T and determine the activation energy for the reaction from the slope. Include the graphs in your report.

Chemistry: The Molecular Science
Chemistry: The Molecular Science
5th Edition
ISBN:9781285199047
Author:John W. Moore, Conrad L. Stanitski
Publisher:John W. Moore, Conrad L. Stanitski
Chapter11: Chemical Kinetics: Rates Of Reactions
Section: Chapter Questions
Problem 113QRT
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THE ACTIVATION ENERGY OF THE REACTION BETWEEN PERSULFATE AND IODIDE IONS, During the reaction of the persulfate ion with the iodide ion, iodine is produced. The molar relationship between the persulfate ion and iodine is 1:1. Iodine turns the colour of starch indicator from colourless to blue. If we add starch indicator to the reagent solutions, we see a blue colour as soon as the reaction starts, and products are formed. If we want to measure a rate constant, we want to remove some of the iodine until, for example, one quarter of the persulfate has reacted. This we can achieve by adding a predetermined amount of thiosulfate to the reagent solutions, because thiosulfate reacts with iodine as follows to form iodide and tetrathionate: 2 S₂03² + 1₂ = 21 +S406 ² A certain amount, which we can calculate to be 1/4 of the initial persulfate concentration of the iodine is thus removed, and at the same time iodide is produced, so that the iodide ion concentration remains constant. Concentrations of solutions of 0.5 M KI, 0.01 M K₂S₂Os, and 0.01 M Na₂S₂O3-5H₂O Volume of KI used = 20ml Volume of K₂S₂O = 20ml Volume of Na2S₂O3 = 10ml Results Experiment 1 1 2 3 4 5 6 Temperature of solution (K) 273 278 288 293 298 303 Time taken for color change (s) 1456 1027 618 358 221 165 3. Plot In t₁/n versus 1/T and determine the activation energy for the reaction from the slope. Include the graphs in your report. 4. Determine the pre-exponential factor A from the intercept of your graph. 5. Determine the rate constants k1 and k2 at 25°C. 6. Comment on the suitability of the experiment to determine the activation energy and the rate constant of the reaction
Transcribed Image Text:THE ACTIVATION ENERGY OF THE REACTION BETWEEN PERSULFATE AND IODIDE IONS, During the reaction of the persulfate ion with the iodide ion, iodine is produced. The molar relationship between the persulfate ion and iodine is 1:1. Iodine turns the colour of starch indicator from colourless to blue. If we add starch indicator to the reagent solutions, we see a blue colour as soon as the reaction starts, and products are formed. If we want to measure a rate constant, we want to remove some of the iodine until, for example, one quarter of the persulfate has reacted. This we can achieve by adding a predetermined amount of thiosulfate to the reagent solutions, because thiosulfate reacts with iodine as follows to form iodide and tetrathionate: 2 S₂03² + 1₂ = 21 +S406 ² A certain amount, which we can calculate to be 1/4 of the initial persulfate concentration of the iodine is thus removed, and at the same time iodide is produced, so that the iodide ion concentration remains constant. Concentrations of solutions of 0.5 M KI, 0.01 M K₂S₂Os, and 0.01 M Na₂S₂O3-5H₂O Volume of KI used = 20ml Volume of K₂S₂O = 20ml Volume of Na2S₂O3 = 10ml Results Experiment 1 1 2 3 4 5 6 Temperature of solution (K) 273 278 288 293 298 303 Time taken for color change (s) 1456 1027 618 358 221 165 3. Plot In t₁/n versus 1/T and determine the activation energy for the reaction from the slope. Include the graphs in your report. 4. Determine the pre-exponential factor A from the intercept of your graph. 5. Determine the rate constants k1 and k2 at 25°C. 6. Comment on the suitability of the experiment to determine the activation energy and the rate constant of the reaction
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4. Determine the pre-exponential factor A from the intercept of your graph.

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