Iodine-Clock Reaction

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CHEMICAL KINETICS: IODINE-CLOCK REACTION DATE SUBMITTED: 14 DECEMBER 2012 DATE PERFORMED: 7 DECEMBER 2012 ABSTRACT Chemical kinetics involving reaction rates and mechanisms is an essential part of our daily life in the modern world. It helps us understand whether particular reactions are favorable and how to save time or prolong time during each reaction. Experiment demonstrated the how concentration, temperature and presence of a catalyst can change the rate of a reaction. 5 runs of dilution and reaction were made to show the effect of concentration on chemical reactions. A certain run from the previous task was twice duplicated to for a “hot and cold” test for reaction rate. The prior run was again duplicated for a test with…show more content…
The contents of the beakers are mixed, and the reaction was timed until the solution turns blue. Catalyst Another run 2 was made and the set-up where the reaction will take place was ensured to be at room temperature. 4 drops of CuSo4 was added immediately after Beaker A was poured to Beaker B. The reaction was timed until it turned to blue. After the experiment, dispose all the Cu(II) solutions in inorganic waste jars and all the other solutions can be discarded in the sink with copious running water. RESULTS AND DISCUSSION Table 2. Concentration Effect | [S2O82-] | [I-] | Time (s) | Rate (M·s-1) | k (M-1·s-1) | 1 | 2.00 x10-2 | 8.00 x10-2 | 52 | 1.92 x10-2 | 12.0 | 2 | 2.00 x10-2 | 4.00 x10-2 | 118.5 | 8.43 x10-3 | 10.5 | 3 | 2.00 x10-2 | 2.00 x10-2 | 227.2 | 4.40 x10-3 | 11.0 | 4 | 3.00 x10-2 | 4.00 x10-2 | 20.5 | 1.41 x10-2 | 11.75 | 5 | 4.00 x10-2 | 4.00 x10-2 | 45.7 | 2.19 x10-2 | 13.7 | Table 2 shows the concentrations of S2O8-2 and I- and the time of each reaction for each run. Rate of the reaction was calculated by dividing 1M with the time it took to complete the reaction. The constant k was calculated using the rate law (4), the x and y value was determined by the graphs below. Considering most of the k’s calculated by our laboratory class, the supposed real value of k must be 10/Ms for that reaction. No outlier was found, so the
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