• Join over 1.2 million students every month
  • Accelerate your learning by 29%
  • Unlimited access from just £6.99 per month

I am going to investigate one factor, which affects the rate of decomposition of hydrogen peroxide H2O2 (aq).

Extracts from this document...


GCSE Science - Sc1 Coursework - Experimental and Investigative Science Plan I am going to investigate one factor, which affects the rate of decomposition of hydrogen peroxide H2O2 (aq). We know that when a certain solid is added to a solution of hydrogen peroxide in water, it makes the hydrogen peroxide break down into water and oxygen gas much faster then it would on its own. We also know that the following decomposition takes place: Hydrogen peroxide water + oxygen 2H2O (aq) 2H2O (l) + O2 (g) so this can help me in making a prediction. To make the test a fair one I would only be able to change one thing at a time so therefore the factors, which I could investigate, are: 1) The amount (mass) of catalyst e.g. 0.1g, 0.2g, 0.3g etc 2) Temperature 3) Different catalysts e.g. copper oxide, zinc, iron oxide. 4) State of division of the catalyst (powder, small, medium, large lumps). 5) Rate of swirling e.g. slow, medium, fast. 6) Change the volume of the H2O2 (aq). ...read more.


I then placed the syringe in the clamp and put the delivery tube going into a bung in the syringe (see diagram below): I then very quickly put the manganese oxide into the boiling tube filled with 20cm� of hydrogen peroxide and put the bung into the boiling tube (see above diagram). I then timed every 10 seconds with a stopwatch and at every 10th second I measured the amount of oxygen that had gone into the syringe. I noted the results down on paper using a pen. I was going to repeat the experiment in order to get averages and make my results more reliable, but I ran out of time. To make the experiment fair I only changed one factor. I also made sure I only started timing once the test tube was attached to the syringe. There were no gaps for oxygen to seep in, making the test a fair one. Results Amount of oxygen in syringe with ...g of catalyst (cm�) Time (secs) 0.1 0.2 0.3 0.4 0.5 0.6 10 12 14 15 34 50 60 20 22 22 44 63 87 97 30 31 31 65 ...read more.


Several times I did not push the syringe back into the original place, so I had to re-weigh and perform the experiment for that particular mass of catalyst. This took up some time. I may have been slightly inaccurate in measuring the amount of oxygen collected in the syringe. This is because you have to look at the stopwatch as well as the measurements on the syringe, which can be hard. Therefore I could have made my results inaccurate by only a couple of cm�. To improve the experiment I could repeat the experiment three times and work out an average for each amount of catalyst. This would make my results more reliable. I could also do the experiment with other people so that one can time, one person could read and another could write down the results. This would make my results more reliable. It would also be a good idea to use a syringe that can hold more than 100cm� because I could see how long it took to actually stop decomposing, improving my results. To further my work I could repeat the same experiment using different catalysts such as copper oxide or iron oxide and see if they worked better at decomposing the hydrogen peroxide quicker. 1 ...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. Investigate the factors, which affect the rate of decomposition of Hydrogen Peroxide.

    aiming to get from my main investigation and to identify any problems I might encounter, I needed to perform the experiment as described above. This would act as a 'trial run'. I set the equipment up as shown below: I carried out the experiment as explained in the plan above, except that I only used Manganese Oxide as the catalyst.

  2. Investigation of the effect of the concentration of hydrogen peroxide on the rate of ...

    experiments would accelerate very quickly so it was hard to read off the value in time. By this method I had plenty of time to put the bung on and take the reading easily. Also I found that if I used 20secs as my reading the gas syringe would fill up too much and fall off on the higher concentrations.

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

    There are several defects with the method. Firstly, it is quite difficult to obtain an initial rate as that would require multiple readings taken for various volumes given off which is reasonably accurate as it is based on human judgement - human error is very possible. Also, there was a limited range due to the size of

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

    Therefore; the steeper the gradient, the slower the rate of the reaction. Based on my gradient, I have taken into account aspects that could have assisted me before I began the experiment. This was firstly; the Lock and Key Principle, which explained how the enzyme-substrate complex was formed.

  1. Investigation into the decomposition of hydrogen peroxide.

    I followed the method written above. Time (seconds) Amount of yeast (cm3) Oxygen produced (cm3) 30 10 50 30 5 46 30 1 28 My results seem reliable as, they fit my prediction and there seem to be no anomalies or extreme pieces of data.

  2. To investigate different masses of catalysts with Hydrogen Peroxide to see if the rate ...

    There is a minimum amount of energy which colliding particles need in order to react with each other. If the colliding particles have less that this minimum energy, then they just bounce off each other and no reaction occurs.

  1. Investigate a factor that influences the rate of decomposition of Hydrogen Peroxide (solution) H2O2 ...

    * Surface area. This would be mostly used for solids, because increasing the surface area of a solid would mean breaking it into smaller pieces. I would not consider this for this investigation because it would be harder to concoct. However, the factor I have chosen to look at is temperature and how it affects the rate of reaction.

  2. To investigate a factor that affects the rate of reaction and why?

    However most reactions take place at a steady rate. During a reaction, reactants are being used up and products are being produced. So the amount of reactants fall and the amount of products rise. The reaction rate tells us how fast a reaction is happening.

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