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

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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.

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