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How the rate of the decomposition of Hydrogen Peroxide is affected by the concentration of Hydrogen Peroxide.

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Introduction

Scott Bissett 10B 15/2/03 Factors Affecting the Rate of the Decomposition of Hydrogen Peroxide Aim: To see how the rate of the decomposition of Hydrogen Peroxide is affected by the concentration of Hydrogen Peroxide. Prediction: I know that Hydrogen Peroxide is unstable and gradually breaks down into water and oxygen over time. The equation for this reaction is 2H2O2* (aq) 2H2O (l) + O2 (g). I think that the higher the concentration, the faster the rate of reaction will be. I think this because the higher the concentration, the more atoms there are, then there are more chickens and therefore there are more collisions as a direct result of the concentration. This is based on the Collision theory, which states that if there are more atoms, there are more collisions, therefore it is more likely to reach the activation energy level required to have a reaction. This likelihood is improved by the fact that there are catalysts (Manganese (IV) Oxide) involved in the equation. Catalysts lower the activation energy requirement, thus increasing the chance of a reaction. My preliminary results show me that the higher the volume of Hydrogen Peroxide, the faster the rate is. Also that the higher the amount of catalyst, the faster the reaction. The lower the particle area the faster the reaction. The higher the temperature the faster the reaction. Also the more concentration, the faster the reaction. ...read more.

Middle

20.5 25 26 23.8 210 21.5 26.5 27 25 225 22.5 27.5 28.5 26.2 240 23 29 29.5 27.2 255 24 30 30.5 28.2 270 25 31 31.5 29.2 285 25.5 32.5 33.5 30.5 300 26 33 34.5 31.2 Concentration of Hydrogen Peroxide: 0.67M Time (sec) Volume of Oxygen (cm3) 1 2 3 Average 0 0 0 0 0 15 2 3 2.5 2.5 30 4 4.5 4 4.2 45 6 6.5 6 6.2 60 8 8 7.5 7.8 75 9.5 9 9 9.2 90 11 10.5 10.5 10.7 105 12.5 11.5 11.5 11.8 120 13.5 13 13 13.2 135 15 14 14 14.3 150 16 15 15 15.3 165 17 16 16 16.3 180 18 17 17 17.3 195 19.5 18 18 18.5 210 20.5 19 19 19.5 225 21.5 19.5 19.5 20.2 240 22.5 20 20.5 21 255 23 21 21 21.7 270 24 22 22 22.7 285 25 22.5 23 23.5 300 26 23 23.5 24.2 Concentration of Hydrogen Peroxide: 0.5M Time (sec) Volume of Oxygen (cm3) 1 2 3 Average 0 0 0 0 0 15 2 1.5 1.5 1.7 30 3 3 3 3 45 4 4 4 4 60 5 5.5 5.5 5.3 75 5.5 6.5 6.5 6.2 90 6.5 7.5 7.5 7.2 105 7 8.5 8.5 8 120 8 9.5 9.5 9 135 8 10 10.5 9.5 150 9 11 11 10.3 165 9.5 11.5 12 11 180 10 12.5 13 11.8 195 10.5 13 13.5 12.3 210 11 14 14.5 ...read more.

Conclusion

This agrees with my prediction quite closely, as I said that the less H2O2, the slower the rate of reaction, and so the less 02 produced. Another thing that I can tell from looking at my graph is that as the lines are pretty straight, that the reaction is directly proportional to the amount of times that passed. There is however one anomaly that occurs in the line of concentration of Hydrogen Peroxide: 0.83M. I think that there are several possible reasons for this. It could be human error, or that I may have had some imperfections on my equipment, or slightly inaccurate solutions. Evaluation: If I were to do the experiment again, I would repeat the experiment more often, and then remove the top and bottom 15% so as to remove all anomaly results. Then I would be able to produce a graph without kinks in, or so I believe. I do however think that my results were accurate enough, as except for the odd one or two strange results, they kept in a straight line. As with most experiments, I am sure that they could be more accurate. There are several reasons for this. I could have read my instruments wrongly. I may have had some imperfections on my equipment, or slightly inaccurate solutions. To further this work, I could experiment with the amount of Manganese (IV) Oxide in the solution and see how that affects the experiment. Other experiments that I could try are by changing the temperature, or the brightness of light, or something else entirely. ...read more.

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