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The rate of a chemical reaction is the derivative of the extent of the reaction with respect to time, to measure the effect of concentration upon the rate of the reaction of peroxydisulfate ion with iodine ion; to determine the order of the reaction with respect to the reactant concentrations; and to obtain the rate law for the chemical reaction. Four reaction solutions are prepare as: 1 - Dilute 5 mL of 0. 2 M KI solution with 10 mL of distilled water in a test tube, add 3 drops of starch solution and mix thoroughly, and then add 5 mL of 0. 2 M (NH 4) S 2 O 8 solution. Mix. Wait a while and observe color changes. 2 - Repeat the procedure in (1), but when the solution changes color add 4 drops of 0. 4 M Na 2 S 2 O 3, mix the solution, and note the effect that the addition of Na 2 S 2 O 3 has on the color. Prepare solution 1 in a 250 -mL Erlenmeyer flask that has been scrupulously cleaned and dried. Pipet 25. 0 mL of (NH 4) 2 S 2 O 8 solution into a clean, dry 100 -mL beaker.
Be ready to begin timing the reaction when the solutions are mixed. The reaction starts the moment the solutions are mixed! Be prepare! ZERO TIME!
Quickly pour the 25. 0 mL of (NH 4) 2 S 2 O 8 solution into solution 1 and swirl vigorously note the time you being mixing to the nearest second. At the instant when the blue black color appears, 2 x 10 - 4 mole of S 2 O 8 - 4 has reacted. IMMEDIATELY (be prepare! ) add a 1 -mL aliquot of Na 2 S 2 O 3 solution from the pipet and swirl the solution; the color will disappear. Record the time for the reappearance of the blue black color. Add an other 1 mL aliquot of Na 2 S 2 O 3 solution and note the time for the reappearance of the color. The time interval being measured is that between the appearance of the black color.
For good results, these aliquots of Na 2 S 2 O 3 must measured as quickly, accurately, and reproducibly as possible. Continue this procedure until you have added seven (7) aliquots to solution 1. You are finished with solution 1 when you have recorded all your times on the report sheet. (the time intervals are cumulative. ) Solution 2, 3, 4 should be treated in exactly the same manner except that 50. 0 mL portions of (NH 4) 2 S 2 O 8 solution should be added to solution 3. (CAUTION: Be on guard- solution 3 will react much more rapidly than solution 1. ) In each of these reactions the final total solution volume is 100 mL. Solution 1 solution 2 solution 3 solution 4 Time 3. 23 2. 26 1. 27 4. 55 (sec) 6. 49 6. 01 3. 06 9. 55 interval 10. 30 9. 41 4. 48 15. 0 2 I- + S 4 O 6 - 2 slope = = 2. 0 x 10 - 5 mole / sec slope = = 1. 06 x 10 - 5 mole / sec Slope = = 2. 0 x 10 - 5 mole / sec slope = = 1. 3 x 10 - 5 mole / sec Since temperature is really a measure of the average kinetic energy of the molecules of a substance, a higher temperature translates into higher kinetic energy which leads to faster moving molecules.
Since the molecules are moving faster, they have a higher chance of successfully colliding and completing a chemical reaction. Thus, a higher temperature allows for a faster rate of chemical reaction. Bibliography:
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