Determining The Rate Law Variable Concentration Experiments 1 Initial Concentrations And Rates Include A Spreadsheet 1 (93.01 KiB) Viewed 38 times
Determining The Rate Law Variable Concentration Experiments 1 Initial Concentrations And Rates Include A Spreadsheet 2 (79.42 KiB) Viewed 38 times
Determining the Rate Law: Variable-Concentration Experiments 1. Initial Concentrations and Rates: Include a spreadsheet (as a separate file) with the result of all of your calculations of initial concentrations and rates for each variable-concentration experiment. The data in your spreadsheet will be used in the rest of your analysis. In the space below, show a full sample calculation for the sample data given below. As in your experimental data, assume that sufficient water was added to make the total volume of the reaction 10.00 mL. NOTE: This data is for your sample calculation onfy? Do not use this data for any other part of your analysis! Show how you use the stock concentrations (blue-shaded box) and the volumes of reactants and reaction time (redshaded box) to find the initial concentrations of all reactants and the initial reaction rate (yellow-shaded box). 0.0519×0.46/10=2.39×10∧−3 1.04×1.81/10=1.88×10×1 1.14×0.98/10=1.12×10n−1 2. Using your experimental data from D2L, determine the reaction order with respect to each of the reactants. You have been given enough data to do this numerous ways, be sure to explain how you determined the orders and exactly what data you used in that process. 3. After you have determined the correct orders with respect to each reactant, calculate the value of the rate law constant, k, for every variable concentration experiment. (This is a constant; the values should be approximately constant.) Show how you calculate k for one of these experiments. Report an average k based upon your experimental data including error and appropriate units. Comment on the magnitude of the experimental error and how it affects your level of confidence in the value of k that you are reporting.
Determining the Activation Energy: Variable-Temperature Experiments 4. Initial Concentrations and Rates: For the variable temperature experiments, calculate the initial concentrations and rates for each reaction. You should do these calculations in MSExcel; copy and paste your results here. Because these are the same type of calculation as in #1 above, you do not need to show additional sample calculations. 5. For each variable-temperature experiment, calculate the value of the rate law constant, k. You have already shown a sample calculation of this type in #3, so you can just include the k values in your table for #4 NOTE: The value of k is temperature-dependent so you should not expect these value to be the samel 6. Why does the reaction rate change when the temperature of the reaction changes? 7. Using the comparative form of the Arrhenius equation, determine the activation energy for this reaction using at least 3 different pairs of temperature data. Report the average activation energy with error. Comment on the magnitude of the experimental error and how it affects your level of confidence in the value of Ea that you are reporting. 8. Using all of the variable-temperature data, determine the activation energy of the reaction using the linear form of the Arrhenius equation. Paste your properly-formatted Arrhenius plot below and show/explain how you determined the activation energy. 9. Comment on the agreement or disagreement between the activation energy calculated using the comparative Arrhenius equation and the activation energy calculated using the linear Arrhenius equation. Is one of them more reliable than the other? Why or why not? What are the advantages and/or disadvantages of each approach?
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