b For each of the successive trials we used 40 mL of the catalase fluid and 10

B for each of the successive trials we used 40 ml of

• Lab Report
• 15

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b. For each of the successive trials we used 40 mL of the catalase fluid and 10 mL of hydrogen peroxide c. We will keep the catalase sample stable by placing it in ice/water bath preventing the denaturing of the enzymes. d. We can prepare another sample of the catalase solution, depending on how much lettuce we are given of course. It can affect the results possibly because of the process of straining, or discrepancies in the amount of catalase or hydrogen peroxide used. 2. Determine the partial order with respect to the peroxide, in the presence of the catalyst catalase, in the rate law. a. To determine partial order we need the initial rate, which can be found out just after the reaction begins. We will also need the value of k( rate constant x concentration of catalase), which can be determined using the calculated activation energy on which temperature is dependent. b. The initial rate and the constant are dependent. The concentration of hydrogen peroxide as well as the temperature are variables that are independent. c. We will measure the rate of reaction by logger pro. Using the data points the slope can be calculated, and this will give the initial rate of reaction. d. We need to measure the pressure which is dependent on the amount of O produced during the reaction. Groups will be responsible for collecting measurements of pressure dependent on partial rate, different temperatures as well as the presence of KI. e. Each group of two will be responsible for completing 3 trials for their assigned control(Rate, Temperature, and KI) This way all data can be obtained much faster. 3. Determine the activation energy for the catalase-catalysed decomposition of hydrogen peroxide. a. To determine the activation energy, the relationship between reaction rate and concentration of hydrogen peroxide can be determined by Rate= [ H 2 O 2] [ catalase ] k x y From this we need the rate constant, k, as well as the values of x and y which are the orders of reactions. b. We can assume that the concentrations of hydrogen peroxide and catalase remain unchanged, thus are independent. The initial rate would also be dependent. Temperature is also independent. c. We can determine the reaction rate using Arrhenius’ equation. Also, the initial rate We can measure the initial rate right after the reaction begins using the data collected. d. Questions d/e are described above. 4. Determine the activation energy for the KI catalysed decomposition of hydrogen peroxide. a. Procedure for part 4 is identical to the procedure for part 3 except for the substitution of KI as a catalyst instead of catalase

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b. The addition of KI into the solution of hydrogen peroxide will provide an alternate path for the reaction. Thus the formation of oxygen is accelerated. The concentrations for the reactants and of the catalyst are independent. c. Initial rates can be determined by taking the slope of the data collected by logger pro. We can speculate that the slopes of the graphs will change with the addition of the catalyst.
• Fall '14
• Pell, Wendy

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