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

Investigation of a Factor Affecting the Rate of Hydrogen Peroxide Decomposition

Extracts from this document...


SACE Stage 2 Chemistry Design Practical: Reaction Rates Investigation of a Factor Affecting the Rate of Hydrogen Peroxide Decomposition. 1. Design Aim: To determine how the rate of decomposition of hydrogen peroxide will change with a change in concentration of hydrogen peroxide. Hypothesis: If the concentration is increased then the rate of decomposition should increase. This is because an increase in the concentration will cause more frequent collisions. An increase in collision frequency will result in more frequent formation of products. As when the concentration of hydrogen peroxide increases there will be more hydrogen peroxide molecules in the same amount of volume causing a higher frequency of collision leading to a faster rate of reaction. Variables: Independent: Concentration of hydrogen peroxide Dependant: The time taken to form a certain amount of products. Controlled: � Amount of catalyst if this is changed the rate of the reaction will change as well. � Amount of hydrogen peroxide as it is the concentration that is changing not the amount of hydrogen peroxide. � Temperature as a change in the temperature will change the rate of the reaction. � Environmental surroundings kept constant otherwise external changes may alter the results. ...read more.


All of this should be done in as short a time as possible to prevent inaccuracies in the readings. 9. Stop the timing when 40 mL of gas has been collected. Record the time that this takes. 10. Repeat Steps 2-8 using 2mL more of hydrogen peroxide and 2mL less of distilled water each time until the mixture is completely hydrogen peroxide. Make sure that the temperature and the amount of the catalyst remain the same throughout the experiment. 2. Presentation: Results: Table 1: Time taken for 40mL of gas to be collected when changing the concentration of hydrogen peroxide. H2O2 (mL �0.05mL) H2O (mL �0.05mL) Time (s �0.5s) 1/Time (s-1 �0.5s) 2 8 84.80 0.01179 4 6 46.27 0.02161 6 4 37.37 0.02676 8 2 24.38 0.04101 10 0 24.19 0.04134 3. Conclusion and Evaluation: Discussion: The first graph has a fairly high R2 value of 0.9537. However, a couple of he points on the graph are a fair way out from the line of best fit suggesting some random error in these points. Random error in these points could have been caused by human error. The second graph suggests a large systematic error. Because although the points are fairly close to the line, suggesting they are reasonably precise, the graph does not pass through the origin like it should suggesting a systematic error. ...read more.


This was because some of the manganese oxide would stay on the watch glass and due to its shape it made it difficult to make sure that all of it has gone into the mixture. Because the amount of catalyst was very small loosing some of it could have made a very large difference to the results obtained. This problem could have been fixed by using a funnel to convert all of the catalyst from the measuring apparatus to the hydrogen peroxide. Another problem was with the time delay of putting the stopper into the top of the flask after the catalyst had been added. This time delay meant that some of the gas might have been able to escape thus changing the results. The time delay between this could have been minimised by using a conical flask that had a hole in the side of it that could be covered so that the stopper could already be in and then the catalyst could be put in and the hole covered immediately after. This process would be a lot less difficult as it is a lot easier to place the cover over the hole than it is to put on the stopper whilst making sure that the tube does not come out of the inverted measuring cylinder. SACE Stage 2 Chemistry Design Practical Jess Goodchild ...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.

    This would result in an increase in rate of reaction. Concentration of Hydrogen Peroxide (H202) As concentration increases, there are more H202 particles contained in the solution per unit volume. As there are more H202 particles, the probability of a collision between H202 particles would increase, and so in theory, there should be more collisions.

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

    An enzyme becomes denatured around 45?C, so it is around here that I expected the reaction to slow down. This prediction was incorrect. It wasn't until around 60?C that the enzyme became denatured. I know this because it is here that the top of the graph goes flat.

  1. Factors Affecting Enzyme Activity

    Below is the method I would use if I were to investigate the affects of temperature on enzyme activity. Method for temperature investigation From my own scientific knowledge I know that catalase is commonly found in human livers and that human body temperature is approximately 37.5�C therefore I predict that

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

    0.2g of Manganese Oxide was then measured out onto a piece of paper and weighed to ensure accuracy. The Manganese Oxide was then placed into the conical flask, which was then immediately sealed with the bung, and the stopwatch was started.

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

    Thus, a faster rate of the reaction, which is the reason that the rate increases when there is a lower volume of water. The graph shows an increase in the volume of oxygen as the average initial reading of experiments conducted also increased.

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

    and it had a lot more molecules for the catalyst to collide causing the reaction to happen quicker, and the 0% was just distilled water there was nothing for the catalyst to react with so no collisions occurred. Conclusion: I saw a pattern from my results which was the more concentrated the hydrogen peroxide, the quicker the rate of reaction.

  1. The Decomposition of Hydrogen peroxide - investigation in to the effect of concentration ...

    Hydrogen peroxide (H2O2) decomposes naturally at a very slow rate (weeks), this is due to its instability so reacts with the air slowly. H2O2 H2O + O2 2H2O2(l) 2H2O(l) + O2(g) I think that as the concentration of hydrogen peroxide to water is increased the rate of reaction will increase

  2. Investigation into the decomposition of hydrogen peroxide.

    tube holder * Metal clamp stand * Stopclock * Yeast (containing catalase) * Hydrogen Peroxide * Bung Fair Test In order to obtain reliable results, I will need to make sure that each of the tests I carry out will be equal and fair.

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