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To investigate different masses of catalysts with Hydrogen Peroxide to see if the rate of reaction changes

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Introduction

Index Title Page No. Introduction 2 Hypothesis 2 Scientific Background 2 - 5 Preliminary Work: Apparatus 5 Method 5 - 6 Results 6 - 7 Fair Testing 7 Obtaining Evidence: Safety 8 Results 8 Analysing Information 8 - 10 Evaluating Information 10 Bibliography 10 Ravi Aggarwal GCSE Chemistry Coursework Aim: To investigate different masses of catalysts with Hydrogen Peroxide to see if the rate of reaction changes Introduction In this investigation I will firstly be finding out which catalyst out of the three available breaks down hydrogen peroxide the quickest. Then with the catalyst that works fastest I will use it to see if a change in volume of the catalyst which change the rate of hydrogen peroxide breaking down. The equation for the decomposition of hydrogen peroxide is: 2H2O2 (aq) 2H2O (l) + O2 (g) (It is worth noting that the compounds used are catalyst and therefore they are not used up, nor do they play and part in the equation. They simply act to speed up the natural process of hydrogen peroxide decomposition.) The catalysts being used in this investigation are: Copper (II) Oxide CuO Iron (III) Oxide Fe2O3 Manganese (IV) ...read more.

Middle

As soon as it is all in, put the rubber bung on the flask and start the stop clock. * Every five seconds, check how many cm3 Oxygen has entered the gas syringe and record it on a chart up to sixty seconds. * Repeat this experiment again so you can create an average out of the two sets of results. * Then repeat the experiment with 0.30g of Iron Oxide and 0.30g of Manganese Oxide doing each experiment twice. Results The results to the preliminary work were as follows: Time (secs) Manganese Oxide (cm3) Iron Oxide (cm3) Copper Oxide (cm3) 0 0.0 0.0 0.0 5 9.0 3.0 1.0 10 15.0 4.0 1.0 15 20.0 4.5 1.0 20 25.0 5.0 1.0 25 30.0 5.0 1.0 30 34.0 5.0 1.0 35 39.0 5.0 1.5 40 43.0 5.5 1.5 45 46.0 5.5 1.5 50 50.0 6.0 2.0 55 54.0 6.0 2.0 60 56.0 6.0 2.5 Rate of Reaction 1.7cm3/s 0.6cm3/s 0.25cm3/s After the preliminary work we decided that we should do the second part of the investigation with Manganese Oxide. We decided to change the mass of the Manganese Oxide in 0.05g steps starting at 0.05g and ending at 0.30g. ...read more.

Conclusion

One improvement we could have made was that we could have some sort of electrical device which would measure the amount of Oxygen given off and display it every five seconds digitally. Another problem we were having is that it was difficult to get exactly the right mass of Manganese Oxide every time. Another thing is that sometimes it would take quite a lot of time to pour the Hydrogen Peroxide into the conical flask and then by the time we put the bung on, the reaction had started and we would loose some Oxygen through the top. This is important because the results at the beginning are the most important to work out the rate of reaction. All together our results were very successful but we did have on anomalous result with 0.25g of Manganese Oxide, which was slower than the 0.20g result. The reasons for this I have already discussed above. We could have got better results by repeating the experiments maybe a few more times so we could get lots of results and then get a better average from those results. This would give us more accurate results and maybe not have the anomalous result. We could also have extended the preliminary work by trying out more catalysts to see if we could have got a better one than Manganese Oxide. ...read more.

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