Determination of Rate Law

1530 WordsMar 26, 20127 Pages
Abstract: The reaction used to determine the experimental rate law of is 2I-(aq) + H2O2(aq) I2(aq) + 2H2O2(l). The rate law determined experimentally is rate= k[I-]1.017[H2O2]0.927. Additionally by performing essentially the same experiments but with temperature changes one can determine how k is affected by temperature changes and the new activation energy. Also, from graphs the activation energy was determined to be 33.3 kJ/mol. INTRODUCTION: The rate of a chemical reaction often depends on reactant concentrations, temperature, and the presence of a catalyst. Additionally, the rate law is determined mathematically only from experimental data. The reaction investigated in this experiment is: 2I-(aq) + H2O2(aq) I2(aq) +…show more content…
Calculations Data For Graph (Reference Calculations Section) Run # | Temp. (K) | K (L/mol*sec) | 1/T | Ln(k) | 1 | 273.5 | 1.321E-06 | 3.66E-03 | -1.35E+01 | 2 | 273 | 2.456E-06 | 3.66E-03 | -1.29E+01 | 3 | 312.5 | 1.141E-05 | 3.20E-03 | -1.14E+01 | 4 | 317 | 1.102E-05 | 3.15E-03 | -1.14E+01 | 5 | 305 | 1.579E-05 | 3.28E-03 | -1.11E+01 | 6 | 303 | 6.093E-06 | 3.30E-03 | -1.20E+01 | K Average from Part 1 | 296.97 | 8.545E-06 | 3.37E-03 | -1.17E+01 | Figure 3: 1/T V. Ln(k) Ea (kJ/mol) | 33.389024 | SAMPLE CALCULATIONS: Part 1 and Part 2 To determine the amount of moles of S2O32- are contained in the delivered amount of 0.0200 M Na2S2O3: To determine how many moles of I2 are needed to react completely with the number of moles of S2O32- formed above: (Reference equation (3) to get mole to mole ratio used) This answer is equivalent to the number of moles formed from equation (1) To determine the concentration of I2 in moles per liter use the total volume of the solution for that specific run (in this case Run 1 Total volume =39.52mL): To determine the average rate of an experimental run: Using the delivered amount of 0.300M KI and the final
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