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

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

Extracts from this document...

Introduction

Investigate a factor that influences the rate of decomposition of Hydrogen Peroxide (solution) H2O2 (aq) PLANNING Hypothesis The higher the temperature, the faster the rate of decomposition of hydrogen peroxide (H2O2). Before I can look at factors that will affect the rate of decomposition of Hydrogen Peroxide (H2O2), I have to consider that on its own hydrogen peroxide' will not decompose to produce oxygen and water as a result at room temperature. Hydrogen peroxide --> oxygen + water 2H2O2 (aq) O2 (g) 2H2O2 (l) This equation shows the decomposition of hydrogen peroxide. From doing my experiment I will be testing to see if either oxygen or water was present at the end. This will help me see if I concocted the experiment correctly. In order to speed up the reaction so that it is fast enough for me to be able to measure the rate of decomposition at room temperature in a given time, a catalyst will be added. This catalyst is called Manganese(IV) oxide. This catalyst is a substance which will speed up the decomposition of H2O2. However, the catalyst itself does not take part in the reaction, and is not used up; therefore after the reaction has taken place the same amount of catalyst that was added will remain. The catalyst works by providing a convenient surface for the reaction to occur. This then means that the particles collide more frequently with each other and so more collisions results in more bonds breaking which leads to a reaction between particles. ...read more.

Middle

5 20 25 0.5 33 5 40 25 0.5 43 5 Not completed 25 0.5 53 5 91 From this second set of preliminary experiments I found out the right amounts that I wanted to use, which are now stated in the method that I used. List of apparatus I am going to use * 250cm� of Hydrogen peroxide * 5g of Manganese(IV) oxide * 5 boiling tubes + rack * 5 weighing boats * Gas syringe + clamp and stand * Bunsen burner * Thermometer * Stopwatch Method * I am going to first set up my gas syringe by clamping it, because it will be a lot easier to place the bung on after adding the manganese(IV) oxide. * I am then going to measure out 25cm� of hydrogen peroxide into 5 boiling tubes each, and set them in a rack. * I will then measure out 0.5g of manganese(IV) oxide into five weighing boats, one to add to each test tube of solution. * I will then light my Bunsen burner and collect a stopwatch. * I will then take a thermometer and record the room temperature of the solution. I will add in the manganese (IV) oxide and place the bung from the gas syringe on and start the stop watch. Whilst this is going on I will shake the contents of the boiling tube, as the reaction will only occur on the surface. This would produce unreliable results, as not a lot of gas may be given off and so the catalyst needs to work with all the hydrogen peroxide, for this to work fairly. ...read more.

Conclusion

For example, after heating it to 25�c, it rose up to 27�c, and this is why my temperatures do not match exactly but are close. This also shows that my fair testing did not come into practice too well. As to have made it fairer I should have done both sets of experiments on the same day. The largest error made was between the last two plots on the graph. At 42�c 50cm� of gas was collected, whereas on the second day at 39�c 55�c of gas was collected. Again this is due to the faults I stated about that could not be avoided. The graph that shows the average set of results shows that the plots lie directly on the curve of best fit. This shows that despite the minor errors made between the two experiments, the average shows a reliable set of results, which erases all the anomalous results shown before. Taking into consideration that the method did produce a reliable set of averaged out results, to make this experiment more reliable in the future I can: * Do all sets of experiments on the same day, to improve my chances of gaining fairer results * The time between adding in the manganese(IV) oxide and placing the bung on top could be reduced by having both sets of apparatus closer together. * I could have done more temperatures, some higher than the one I stopped at and maybe even some lower to get more sets of results. This may prevent anomalous results happening and give a more precise average. Also this could support my scientific background to larger extent. Nana Agyeman. 11V Ms Yates ...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.

    Temperature: This will be kept at room temperature (approximately 20 �) where possible, though it is difficult to keep this always constant as the reaction is exothermic, so heat will be given off during the experiment, especially as higher concentrations are used when the reaction becomes more vigorous.

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

    Concentration of Hydrogen Peroxide Displacement of air Volume of Oxygen produced In 10secs (1) Displacement of air Volume of Oxygen produced In 1'secs (2) 1M 3 53 3 42 0.9M 4 45 3 35 0.8M 3 44 3 28 0.7M 3 29 3 22 0.6M 2 23 2 18 0.5M

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

    results down and watch the timer and prepare to take the next reading. From this point onwards, I took a reading every 15 seconds, which was more efficient and practical. Pre-test 2 * 0.1g yeast used * 5cm3 H2O2 * This experiment was carried out at 66?C.

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

    The amount of gas that I was collecting was also consistently 50cm3. All these factors needed to be kept constant because otherwise they would affect the experiment and it wouldn't be a fair test, which is essential to produce reliable results.

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

    the dangerous nature of many of the compounds involved in this experiment, it is important that safety goggles or safety glasses are worn during all tests.

  2. To find out the effect of varying concentration of potassium iodide in a I2 ...

    Thus half-life of the substance depends upon the concentration: Volume of KI/dm3 Time/s Moles/mol Concentration in 145cm3 solution/ mol dm-3 Rate/mol dm-3 s-1 0.025 51.06 0.0025 0.01724 0.000337642 0.020 60.03 0.0020 0.01379 0.000229718 0.015 74.00 0.0015 0.01034 0.00013973 0.010 87.63 0.0010 0.00689 7.8626E-05 0.005 110.26 0.0005 0.00345 3.12897E-05 When a Rate/Concentration graph is plotted, a straight line is obtained.

  1. To determine the rate law for a chemical reaction among hydrogen peroxide, iodide and ...

    reaction with respect to each reactant and the rate law of the reaction, which of the form: Rate = k [H2O2]x[I-]y[H+]z By knowing the reaction times (?t) and the concentrations of H2O2 of two sepatate reaction mixtures (mixtures A & B), the reaction order of H2O2, x, can be calculated.

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

    It shows that there are more molecules than 50%. Because there are more molecules the reaction will happen quickest at this concentration. Preliminary Work: Before we done our original experiment we had to do another experiment. This gave us some idea of what our results were going to be like.

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