5 T6 Data Enter the data from the lab in the file. Perform the calculations in t

Question

5 T6 Data Enter the data from the lab in the file. Perform the calculations in the clock:Aterkabxlsx file, including making an Amhenius Law plotto determine the activation enery of the reaction. Results The rate law for Equation was experimentally determined to be The activation energy (Ea) for Equation (l) was experimentally determined to be Discussion Follow-up Questions Compare the average reaction time for Trial I from PartI(without a catalyst) to the reaction time ofTrial l from Part III (with a catalyst), include the values. How did the addition of a catalyst affect the rate of reaction? Write in full sentences.using proper grammar. Compare your average reaction time for Run lat room temperature to your reaction times at the colder and hotter temperatures. What effect does changing the temperature have on the rate of reaction? Write in full sentences, using proper grammar. Theoretical Error: What assumptions or approximations may have contributed to emor in your results? Procedural Error: What parts of the experimental procedure may have contributed significantly to error in your results? Human Error: What failures on your part to effectively follow the procedure as written do you think may have contributed to error in yourresults? Thereshould not be anything to write here, but if you did mess up and for some reason did not redo the portion(s) of the experiment required to obtain uncorrupted data, the mistake(s) should be identified here)

Explanation / Answer

compare run1 and run 2. Here concentration of KBrO3 is kept constant while the concentration of KI is increased two times. rate of the reaction is also increases about two times. So, the reaction is 1st order with respect to concentration of I-.

Compare run 1 and run 3. Here concentration of KI and H+ is kept constant while concentration of KBrO3 is doubled. The is also doubled. So, the reaction is first order with respect to concentration of KBrO3

Compare run 1 and 4. Here concentration of KI and KBrO3 is kepr constant while concentration of H+ is doubled. As a result rate of the reaction is incraesed four fold. So, the reaction is second order with respect to concentration of H+.

rate = k[KI][KBrO3][H+]^2

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slope =- Ea/R

or, Ea = -(14272.33) *8.314 J/K/mol =118660.15 J/mol

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