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Investigation of the effect of the concentration of hydrogen peroxide on the rate of reaction of its decomposition in the presence of Manganese (IV) Oxide catalyst

Extracts from this document...

Introduction

Plan Investigation of the effect of the concentration of hydrogen peroxide on the rate of reaction of its decomposition in the presence of Manganese (IV) Oxide catalyst What is the reaction? Hydrogen Peroxide decomposes in the presence of manganese (IV) oxide to produce water and oxygen, as shown below. Mn (IV) oxide 2H2O2(l) 2H2O(l)+O2(g) Hypothesis. I predict that the rate of reaction will increase as the concentration of the Hydrogen Peroxide increases. Procedure. For this experiment it was essential that the affecting factors of the experiment were kept constant. The reason for this is that as I was measuring the rate of the reactions the results could be easily changed by even a slight fluctuation in temperature, thus everything was kept constant except the concentration of the Hydrogen Peroxide. The way I kept the temperature constant in the experiment was by carrying out all the experiments in the same double period. This way the temperature could not be changed by the temperature at that time of day because the trial was carried out in a relatively short time. The other main constant to be kept was the volume of the Manganese Oxide and Hydrogen Peroxide. This was done by only accepting measurements for the Magnesium to within 0.01 of a gram. This ensured accuracy and reliable readings. With the Hydrogen Peroxide I measured the water and the Hydrogen Peroxide in different cylinders in order to ensure that if I added too much of one substance I did not have to throw the whole batch away. ...read more.

Middle

Investigation of the effect of the concentration of hydrogen peroxide on the rate of reaction of its decomposition in the presence of Manganese (IV) Oxide catalyst What is the reaction? Hydrogen Peroxide decomposes in the presence of manganese (IV) oxide to produce water and oxygen, as shown below. Mn (IV) oxide 2H2O2(l) 2H2O(l)+O2(g) Hypothesis. Having already tested this theorem I predict that the rate of reaction will increase as the concentration of the Hydrogen Peroxide increases. Procedure. For this experiment it was essential that the affecting factors of the experiment were kept constant. The reason for this is that as I was measuring the rate of the reactions the results could be easily changed by even a slight fluctuation in temperature, thus everything was kept constant except the concentration of the Hydrogen Peroxide. The way I kept the temperature constant in the experiment was by carrying out all the experiments in the same double period. This way the temperature could not be changed by the temperature at that time of day because the trial was carried out in the same double period. The other main constant to be kept was the volume of the Manganese Oxide and Hydrogen Peroxide. This was done by only accepting measurements for the Magnesium to within 0.01 of a gram, this accuracy proved problems in the first planning experiment and affected the readings so therefore in the coursework it was made sure that this hitch was changed to ensure that the optimum data were collected. This ensured accuracy and reliable readings. ...read more.

Conclusion

If it was not then I repeated the experiment again to get better results. * Also due to the fact that I was by myself I was often in a hurry and as a result of this I often spilt the apparatus as I was in such a rush to do everything in time. Due to this I had to start three experiments again. Modifications: * One modifications I could possibly make is that I would do it in a pair As having done a trial experiment there was nothing really that I could obtain better by using a different method therefore the only modification would be to do it in a pair, as it would be easier to obtain the data and carry out the experiment. * Another is that I would measure the weight of the piece of paper after the experiment to make sure all the Manganese Oxide had been deposited. If it had not I would repeat the experiment. Conclusion: Having studied my results and reading over my recordings the experiment has led me to believe that my hypothesis was correct. As the higher the concentration of the Hydrogen Peroxide, the quicker the reaction rate was. For instance a concentration of 1M produced 51ml and 38ml of Oxygen in 10secs, whereas a concentration of 0.4M only produced 10ml and 14ml. This clearly shows that the higher the concentration of the Hydrogen Peroxide the higher the reaction rate. ?? ?? ?? ?? Gcse Chemistry Coursework 2002-05-03 Leonard Percival Gcse Chemistry Coursework 2002-05-03 Leonard Percival ...read more.

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