Investigating Factors That Affect the Rate of Reaction of the Decomposition of Hydrogen Peroxide

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Investigating Factors that Affect the Rate of Reaction of the Decomposition of Hydrogen Peroxide
Emilio Lanza

Introduction-
In this experiment, the rate of reaction, calculated in kPa sec-1, of the decomposition of hydrogen peroxide will be investigated to see how the change in concentration of hydrogen peroxide and the change in temperature affect the rate of reaction. The data will be collected by measuring the gas pressure. The product of Hydrogen Peroxide is oxygen in a gas state thus it is mandatory to use the gas pressure sensor. By calculating the difference of the gas pressure divided by the amount of time from the raw data collection it is able to find the rate of reaction of the decomposition of hydrogen peroxide. * Control Variable- 1mL of yeast (catalyst) is being used in every trial. The volume of H2O2 is always 4 mL, even though the concentration changes and the sizes and type of test tube was the same because it can change the pressure. * Independent Variable- Concentration of H2O2 (M) and the temperature (°C) * Dependent Variable- The rate of reaction of the decomposition of hydrogen peroxide → rate of reaction = ∆ Pressure (kPa)Time (sec) . * Research Question- it is needed to calculate the rate of reaction (kPa sec-1) of the decomposition of H2O2 to understand how different factors such as the change in concentration and the change in temperature of H2O2 affect the rate of reaction.

Materials and Method-

Materials:
* 0.5 M Yeast solution (the catalyst) - 15 mL
* 45 mL of 3 % H2O2 solution
* A thermometer
* A computer with LoggerPro Program.
* A Vernier computer interface
* A Vernier Gas Pressure Sensor
* A 1 liter beaker
* A match to light up the bunsen burner
* A tripod
* Two 10 mL test tubes
* Two 10 mL pipette
* Distilled water - 15 mL
* A matt/cover that is fire resistant
* 700 mL of room temperature water from a sink
* A one-hole rubber stopper with stem
* Two test tube holders
* Two 10 mL graduated cylinders
* A bunsen burner
* Two solid rubber stopper
* Plastic tubing containing two Luer-lock connectors
* A one-hole rubber stopper with stem
* A test tube rack

Procedure:
Part 1 of the experiment: Decomposing 3 % of H2O2 solution with 0.5 Yeast at about 30°C 1. Take the 1-liter beaker and add 700 mL of room temperature water. Take the tripod, place a matt/cover that is fire resistant on top of the tripod and onto the matt/cover place the 1-liter beaker that has been filled up with 700 mL of room temperature water from a sink. 2. First hook the rubber tube from the Bunsen burner to a gas source, then take a match and turn on the gas source. Once the gas is on light the match and then light the bunsen burner. (MAKE SURE TO NOT BURN YOURSELF)!! 3. Place the lit bunsen burner underneath the tripod so it can begin to heat the 1 liter beaker with the 700 mL of room temperature water from the sink. 4. Insert a thermometer into the 1 liter beaker that is being heated and adjust the flame of the bunsen burner so it will heat the water to a temperature of about 30°C. 5. Take the 10 mL pipette and the 10 mL-graduated cylinder use the pipette and transfer 4 mL of H2O2 and using a 10 mL pipette transfer 4 mL of H2O2 from a container into the 10 mL graduated cylinder. 6. Take a 10 mL test tube and add fill 4 mL of H2O2 from the 10 mL graduated cylinder into the 10 mL test tube. Once that is done, take a rubber stopper and seal the 10 mL test tube containing the H2O2. Use the test tube holder to hold the test tube into the 1 liter beaker the is being heated to a temperature of about 30°C. Make sure that the majority of the test tube is submerged in water. 7. Using the other 10 mL pipette, transfer 1 mL of 0.5 M Yeast into the other 10 mL graduated cylinder. From this graduated cylinder, transfer the 0.5 M Yeast to a new 10 mL test tube; seal the test...
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