Decomposition Reaction Of H2o2 Lab Solution

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Chemistry
Lab Report

NAME: Serina Alashi

DATE:

TITLE: Decomposition reaction: hydrogen peroxide (H2O2) decomposed into hydrogen and oxygen ( H2 and O2)

RESEARCH
QUESTION: How will changing the concentration of hydrogen peroxide affect the rate of reaction, that is represented by the increase in pressure over time?

Introduction: Hydrogen peroxide is a chemical compound of hydrogen and oxygen. It is a very strong oxidant but weak in water solution. Hydrogen peroxide decomposes into water and oxygen when heated above about 80°C and also decomposes in the presence of a catalyst. A catalyst is a substance that increases the rate of a chemical reaction but is not changed by the reaction. The catalyst in this case would be breaking hydrogen
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Set time to 300 seconds.
Step 4: Immediately cap the graduated cylinder with the gas pressure sensor to record initial rate
Step 5: After the initial rate has been calculated, add 10 micro-liters of catalyst using a micropipette into the hydrogen peroxide
Step 6: Measure the pressure build up of the catalyst with the hydrogen peroxide, again using the gas pressure sensor
Step 7: Constantly stir the hydrogen peroxide with the magnetic stirrer to release oxygen gas trapped inside the solution
Step 8: Add 10, 20, 30, and 40 ml of distilled water into the test tubes
Step 9: Draw 1 mL of solution from the graduated cylinder with a micropipette and transfer it to test tube B and mix thoroughly. (The solution that originally had a volume of 10 ml now has a volume of 1 mL in test tube B. The solution, therefore, has been diluted by a factor of 10.)
Step 10: Move 1 mL of the solution from test tube B to test tube C using the technique described previously and thoroughly mix the contents of test tube C. (The solution in test tube C has been diluted by a factor of 100.)
Step 11: Repeat the same techniques from step 9 and 10 but by performing it for the other test
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The linear graph shows the relationship between the rate of reaction and the hydrogen peroxide concentration. However, there is no evidence to conclude that the correlations are always proportional. The uncertainty of the gas pressure was kPa + 0.01.While observing the data for 10 mL and 20 mL H2O, seems to be overlapping, rather than seeing an obvious increase between the two. On the contrary, this could be due to the fact that the volumes were different as well as the hydrogen peroxide concentrations. On the other hand, the steeper the slope, the faster the rate of reaction. Similarly, the more gradual the slope is, the slower the rate of reaction. The graph seems to be increasing very slowly. As observed in the graph, the control, which only contained H2O2 has a more steeper slope than the trials with H2O in it. Looking at the graph, the greater the volume, the slower the rate of reaction. For example the trial with 10 mL H2O2 + 40 mL H2O had a slower reaction rate than the trial with 10 mL H2O2 + 10 mL H2O. Looking at the slopes of the lines, the trial with 20 mL H2O and 10 mL H2O2 has the fastest reaction time because its slope is 1.0251. The second data with the fastest reaction time was the control (H2O2) with a slope of 0.9149. The third data with the next fastest reaction time was 20mL H2O with 10 mL

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