• 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

To investigate different masses of catalysts with Hydrogen Peroxide to see if the rate of reaction changes

Extracts from this document...

Introduction

Index Title Page No. Introduction 2 Hypothesis 2 Scientific Background 2 - 5 Preliminary Work: Apparatus 5 Method 5 - 6 Results 6 - 7 Fair Testing 7 Obtaining Evidence: Safety 8 Results 8 Analysing Information 8 - 10 Evaluating Information 10 Bibliography 10 Ravi Aggarwal GCSE Chemistry Coursework Aim: To investigate different masses of catalysts with Hydrogen Peroxide to see if the rate of reaction changes Introduction In this investigation I will firstly be finding out which catalyst out of the three available breaks down hydrogen peroxide the quickest. Then with the catalyst that works fastest I will use it to see if a change in volume of the catalyst which change the rate of hydrogen peroxide breaking down. The equation for the decomposition of hydrogen peroxide is: 2H2O2 (aq) 2H2O (l) + O2 (g) (It is worth noting that the compounds used are catalyst and therefore they are not used up, nor do they play and part in the equation. They simply act to speed up the natural process of hydrogen peroxide decomposition.) The catalysts being used in this investigation are: Copper (II) Oxide CuO Iron (III) Oxide Fe2O3 Manganese (IV) ...read more.

Middle

As soon as it is all in, put the rubber bung on the flask and start the stop clock. * Every five seconds, check how many cm3 Oxygen has entered the gas syringe and record it on a chart up to sixty seconds. * Repeat this experiment again so you can create an average out of the two sets of results. * Then repeat the experiment with 0.30g of Iron Oxide and 0.30g of Manganese Oxide doing each experiment twice. Results The results to the preliminary work were as follows: Time (secs) Manganese Oxide (cm3) Iron Oxide (cm3) Copper Oxide (cm3) 0 0.0 0.0 0.0 5 9.0 3.0 1.0 10 15.0 4.0 1.0 15 20.0 4.5 1.0 20 25.0 5.0 1.0 25 30.0 5.0 1.0 30 34.0 5.0 1.0 35 39.0 5.0 1.5 40 43.0 5.5 1.5 45 46.0 5.5 1.5 50 50.0 6.0 2.0 55 54.0 6.0 2.0 60 56.0 6.0 2.5 Rate of Reaction 1.7cm3/s 0.6cm3/s 0.25cm3/s After the preliminary work we decided that we should do the second part of the investigation with Manganese Oxide. We decided to change the mass of the Manganese Oxide in 0.05g steps starting at 0.05g and ending at 0.30g. ...read more.

Conclusion

One improvement we could have made was that we could have some sort of electrical device which would measure the amount of Oxygen given off and display it every five seconds digitally. Another problem we were having is that it was difficult to get exactly the right mass of Manganese Oxide every time. Another thing is that sometimes it would take quite a lot of time to pour the Hydrogen Peroxide into the conical flask and then by the time we put the bung on, the reaction had started and we would loose some Oxygen through the top. This is important because the results at the beginning are the most important to work out the rate of reaction. All together our results were very successful but we did have on anomalous result with 0.25g of Manganese Oxide, which was slower than the 0.20g result. The reasons for this I have already discussed above. We could have got better results by repeating the experiments maybe a few more times so we could get lots of results and then get a better average from those results. This would give us more accurate results and maybe not have the anomalous result. We could also have extended the preliminary work by trying out more catalysts to see if we could have got a better one than Manganese Oxide. ...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. Investigation of the effect of the concentration of hydrogen peroxide on the rate of ...

    This lowered my results and thus affected the average. Modifications & Improvements: * In the real coursework I will use a more accurate method of measuring the amount of Manganese Oxide added to the Hydrogen Peroxide. The way I will do this is by weighing the paper after the Manganese

  2. Factors Affecting the Rate of Catalytic Decomposition of Hydrogen Peroxide.

    would affect rate of reaction * The hydrogen peroxide could have already partially decomposed, which would mean that some of the contents would just be water - hence there would be less collisions between hydrogen peroxide particles and manganese dioxide particles, and rate of reaction might decrease but when it

  1. To Investigate the Effect of Manganese IV Oxide on the rate of decomposition of ...

    * Temperature of hydrogen peroxide. * Temperature of catalyst. Results Table to show the rate of decomposition of hydrogen peroxide adding different amounts of Manganese Oxide AMOUNT OF Mn0 ADDED ( g ) TIME TAKEN (secs)

  2. How does the activation enthalpy and the rate of the iodine-clock reaction vary with ...

    given temperature, EA is the activation enthalpy of the reaction, and R is the ideal gas constant. A is known as the 'pre-exponential factor', and it is a quantitative representation of the orientation of the particles when they collide. It is no good if the particles do not collide at

  1. To investigate the effect of varying the masses of white sugar and yeast and ...

    The only risk involved was the high temperatures reached by the thermostatic bath. Contact with the water in the bath was avoided since water was only 3/4th the height of the measuring cylinder. Conclusion: The null hypothesis stated that the rate of rising of dough would be independent of the

  2. Find out how the rate of hydrolysis of an organic halogen compound depends on ...

    have energies above 50kJ mol-1. This means that twice as many molecules have enough energy to react - so the reaction goes twice as fast. Figure 18 (IX) Catalyst What is a catalyst? A catalyst is a substance, which alters the rate of reaction and you can always get them back to the end.

  1. An investigation to see the difference in the rate of reaction when catalyse is ...

    Volumes of H2O2. - if you have a large volume of H2O2 and you mix it with catalase then the break down rate will be faster than a small volume. This is because if there is a larger volume then there are more H2O2 molecules around and available for the catalase to breakdown.

  2. Magnesium Oxide

    If I was to use glass the chanced of and injury would be high. Another advantage for safety with the crucible is that we won't be able to see the light produced from the creation which means there would be no risk of your eyes being damaged.

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