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

To find how the rate of reaction/rate of decomposition is affected by the concentration of hydrogen peroxide. Liver will be used as a source of catalase, used as a catalyst.

Extracts from this document...


BIOLOGY INVESTIGATION PLAN- INVESTIGATING THE DECOMPOSITION OF HYDROGEN PEROXIDE Aim: To find how the rate of reaction/rate of decomposition is affected by the concentration of hydrogen peroxide. Liver will be used as a source of catalase, used as a catalyst. Diagram: Hypothesis: Hydrogen is a colourless substance that is sometimes used to bleach hair. It is harmful to humans. Some cells in the body can break down harmful substances such as hydrogen peroxide into non-toxic chemicals such as water and oxygen. The equation for this is: 2H2O2(aq)-->2H2O(l)+O2(g) One of the organs that can break hydrogen peroxide down into water and oxygen is the liver, which contains catalase. Catalase is an enzyme that acts as a catalyst. This can help to decompose Hydrogen Peroxide quickly. A catalyst is a substance that speeds reactions. The concentration of hydrogen peroxide is given as the volume of oxygen that can be obtained from one volume of the solution. For example, 10cm3 of 1 Volume hydrogen peroxide produces 10 cm3 oxygen when it decomposes. 5 Volume hydrogen peroxide will make 5 times this amount. I predict that the rate of reaction will be faster when the concentration of hydrogen peroxide is higher. ...read more.


39 40 42 44 43 45 10 8 11 14 18 20 23 24 26 29 31 34 38 40 44 48 52 57 60 63 66 70 75 81 84 91 95 96 97 100 100 10 7 11 14 17 18 21 22 24 29 30 33 36 37 42 45 50 56 62 62 63 64 65 67 68 71 72 76 80 87 98 12.5 2 4 7 8 10 11 14 14 15 16 16 18 22 24 25 28 34 34 39 46 48 54 55 58 60 68 75 80 86 92 12.5 5 7 10 14 15 20 27 32 37 40 42 43 45 47 50 52 54 51 65 68 72 79 85 89 90 100 100 100 100 100 15 9 13 16 20 23 25 28 32 34 37 41 44 48 49 55 59 64 67 78 89 94 96 98 99 100 100 100 100 100 100 15 5 9 14 17 21 24 27 29 31 33 35 39 41 43 45 48 52 55 62 68 71 76 81 88 90 97 100 100 100 100 20 4 7 10 15 18 25 29 33 36 40 43 45 47 51 53 57 66 ...read more.


I would expect this to make the rate of reaction faster as there would be more catalyst readily available to speed up the reaction. -The size of liver used will affect the results, for example, if the size of one piece of liver was larger than another piece of liver used with the same strength and amount of hydrogen peroxide, the hydrogen peroxide containing the larger piece of liver will have a faster rate of reaction as it will contain more catalase. -Any error in measurement throughout the experiments in my investigation will affect the results in this investigation, for instance if the hydrogen peroxide was measured incorrectly, different results will be found which could possibly be anomalous. Most of these factors affecting my results are out of my control, such as whether the gas syringe is broken or the size and surface area of the liver (because it is almost impossible to weigh such a small piece of liver). The pieces of liver I used were only approximately the size of a grain of rice, although some were inevitable larger or smaller. Errors in my measurement, however, can be controlled and so I was very careful whilst measuring everything out and timing my experiments. Rebecca Allot 11Y Page 1 03/05/2007 ...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. Factors Affecting the Rate of Catalytic Decomposition of Hydrogen Peroxide.

    Volume of H202 As volume of the H2O2 increases, the total number of H2O2 particles also increases. The frequency of collisions between the H2O2 particles and the catalyst (Mn02 particles) therefore increases, as there are more H2O2 particles for the catalyst to collide with, and there will initially be more reactants for the catalyst to adsorb onto.

  2. The effect of aspirin on the action of bovine liver catalase

    Results of Pilot Table 1. Finding appropriate concentrations of liver and hydrogen peroxide Volume of liver solution (ml) Concentration of liver solution (%of original solution) Volume of hydrogen peroxide solution (ml) Concentration of Hydrogen peroxide (mol/dm� ) Volume of water (ml)

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

    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. This was done by using two smaller cylinders to measure the liquid

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

    Concentration of H2O2 If the concentration of H2O2 is increased, there are more particles in a given volume. This means that more collisions take place. Concentration can be changed by adding water or more H2O2 to the solution. Amount of yeast If the amount of yeast is increased, this means

  1. Investigate the factors, which affect the rate of decomposition of Hydrogen Peroxide.

    The following diagram explains how this happens: The major difference with an enzyme catalyst is the way that it is affected by temperature. All enzymes are proteins and like all proteins, they break down at high temperatures. Because the enzyme has broken down, its active site is changed.

  2. Effect Of Substrate Concentration On The Activity Of Catalase

    Also, the same volume of water will be added to the beaker each time a new test is to be done, so as not have any differences in how long the water maintains its heat for. 3. It must be ensured that when taking readings off the measuring cylinders and

  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. Investigating the rate of a reaction

    At intervals of 20, 40, 60, 80, 100, 120 seconds, which can be seen from the stopwatch, note down the amount of carbon dioxide released from the reading on the gas syringe in cm3. Note the result down in the table of results.

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