• Join over 1.2 million students every month
  • Accelerate your learning by 29%
  • Unlimited access from just £6.99 per month
Page
  1. 1
    1
  2. 2
    2
  3. 3
    3
  4. 4
    4
  5. 5
    5
  6. 6
    6
  7. 7
    7
  8. 8
    8
  9. 9
    9
  10. 10
    10
  11. 11
    11
  12. 12
    12
  13. 13
    13
  14. 14
    14
  15. 15
    15
  16. 16
    16
  17. 17
    17
  18. 18
    18
  19. 19
    19
  20. 20
    20
  21. 21
    21
  22. 22
    22
  23. 23
    23
  24. 24
    24
  25. 25
    25
  26. 26
    26
  27. 27
    27
  28. 28
    28

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.

The above preview is unformatted text

This student written piece of work is one of many that can be found in our GCSE Patterns of Behaviour section.

Found what you're looking for?

  • Start learning 29% faster today
  • 150,000+ documents available
  • Just £6.99 a month

Not the one? Search for your essay title...
  • Join over 1.2 million students every month
  • Accelerate your learning by 29%
  • Unlimited access from just £6.99 per month

See related essaysSee related essays

Related GCSE Patterns of Behaviour essays

  1. The Decomposition of H2O2 using Catalase, in yeast as a catalyst.

    In other words there were the most amount of successful collisions at 40?C of all the temperatures in my range. Theoretically, the rate of reaction should have been highest at 70?, and it would have been if this were not a reaction that involved enzymes.

  2. Rates of Reaction experiments

    and the acid for reactions to take place therefore increasing rate of reaction. The rate simply depends on how fast and often particles collide with each other. The increase in surface area also results an increase in the rate of reaction.

  1. Decomposition of Hydrogen Peroxide Investigation.

    Contaminated clothes should be removed and then soaked. If a large area has been affected or blistering appears, seek medical attention. * Cases of spillage- make sure you are wearing eye protection and gloves. The area should be covered with a mineral absorbent and cleared up into a bucket.

  2. Investigation of a Factor Affecting the Rate of Hydrogen Peroxide Decomposition

    It was also very difficult to transfer the catalyst from the watch glass to the solution in the conical flask.

  1. Studying the rate of reaction of the catalyst decomposition of hydrogen peroxide.

    A clamp stand will be used to support the burette so that it so it not fall down. We will use a bung to make sure that no gas escapes from the conical flask. We will use scales so that we can weigh the amount of catalyst used in each of the experiment.

  2. The Effect of Catalase in the Breakdown of Hydrogen Peroxide

    can be changed in such a way that it may seem odd if when written next to the other results. Another factor affecting the use of a stop watch is the questioning if the watch actually works properly. By avoiding finding the answer when it's too later (during the reactions),

  1. Measuring the Decomposition of Hydrogen Peroxide Using Manganese (IV) Oxide Catalyst.

    However, Hydrogen Peroxide decomposes very slowly without a catalyst. A catalyst is a substance that speeds up a reaction without being used itself. This is because Hydrogen Peroxide can't get over one barrier - activation energy. The catalyst for Hydrogen Peroxide Decomposition is Manganese (IV) Oxide.

  2. The effect of changing the concentration of the Enzyme catalyst on the Rate of ...

    If you increase the concentration the molecules will be closer together therefore colliding with each other more often. This will mean an increase in the rate of reaction. A catalyst speeds up the rate of reaction, but does not get used up.

  • Over 160,000 pieces
    of student written work
  • Annotated by
    experienced teachers
  • Ideas and feedback to
    improve your own work