kinetics of the iodince clock

kinetics of the iodince clock - John Warwick Lab AI: Amanda...

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John Warwick Lab AI: Amanda Le Sueur April 13, 2011 Kinetics of the Iodine Clock Reaction Table 1: Data for Runs #1-3, Experimental Trial, and Run #1 at 0 O C and 40 O C Run # Test Tube A Test Tube B Time Trial 1 (sec.) Time Trial 2 (sec.) Ave. Time (sec.) Initial [KI] Initial [K 2 S 2 O 8 ] 1 2 mL KI 1 mL Na 2 S 2 O 3 2 mL K 2 S 2 O 8 42 43 42.5 0.088 M 0.072 M 2 2 mL KI 2 mL K 2 S 2 O 8 n/a n/a n/a 0.11 M 0.09 M 3 2 mL KI 2 mL Na 2 S 2 O 3 2 mL K 2 S 2 O 8 114 113 113.5 0.072 M 0.06 M Trial 2 mL KI 1 mL Na 2 S 2 O 3 1 mL KNO 3 2 mL K 2 S 2 O 8 92 93 92.5 0.072M 0.06M 0 O C 2 mL KI 1 mL Na 2 S 2 O 3 2 mL K 2 S 2 O 8 215 210 212.5 0.088 M 0.072 M 40 O C 2 mL KI 1 mL Na 2 S 2 O 3 2 mL K 2 S 2 O 8 8 10 9 0.088 M 0.072 M Determination of Reaction Order Reaction 1 was studied because of the fact that it takes place on the order of seconds or minutes while the second reaction takes place instantaneously. In order to calculate the rate of the reaction the time that the reaction took place is necessary. Using reaction 1 an experiment was created to find the order of the reactants in the iodine clock reaction. Table #1, shows the differences in the molar concentrations of KI and in the three trials. Run 3 and the trial run were used to determine any difference in overall
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reaction time. The times of those runs doubled with the corresponding change in
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kinetics of the iodince clock - John Warwick Lab AI: Amanda...

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