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An experiment investigating the factors which alter the rate of the catalysed decomposition of Hydrogen Peroxide.

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Introduction

Jessica Hartley Centre no: 64335 Candidate no: 6107 An experiment investigating the factors which alter the rate of the catalysed decomposition of Hydrogen Peroxide. Aim To investigate one factor that alters the rate of the catalyzed decomposition of Hydrogen Peroxide. Introduction Particles can only react if they collide with enough energy to break existing bonds which will allow for the reaction to take place. This theory is called The Collision Theory. There are four factors affecting the rate of a chemical reaction. These are: Temperature:- Increasing the temperature will cause the particles to move faster, with more energy. They will therefore collide more often and with greater energy. These two things mean there are more successful collisions per second and therefore a faster rate of reaction. Concentration:- Increasing the concentration of a reactant simply means there are more particles which may collide and so react. More collisions means a faster reaction. Surface area:- Using powdered reactants instead of a lump means the surface area is greater, which means a greater area of reactant is exposed and so available for collision. More collisions means a faster reaction. Catalysts:- Use of catalysts means that particles having only minimal, energy may react. If s of catalysts work because one of the reactants is fixed to the surface. This makes the chance of a reaction more likely. ...read more.

Middle

8 0.24 25 41 38 10 10 0.24 25 39 56 8 12 0.24 25 36 75 6 14 0.24 25 35 129 Fair test I've decided I shall keep the same concentrations of the solutions. If I used a lower concentration i.e. 4ml of solution and 16ml of distilled water the reaction would have been too slow to measure accurately. If I had used 20ml of water the reaction wouldn't have taken place at all because a compound is needed to react with a catalyst. I've also decided to keep the collection of 100ml of oxygen because if it was smaller it may not be as accurate. For my next investigation I shall use a smaller amount of Manganese (IV) Oxide which has been advised. This is because the reaction is happening too quickly Apparatus * 25ml Measuring Cylinder * 100ml Measuring Cylinder * A Conical Flask * A Delivery Tube with Bung * A Water basin * Top Pan Balance * Plastic Dish * A Stop Clock * Hydrogen Peroxide Solution * Distilled water * Manganese (IV) Oxide Method In this investigation I shall make three sets of 8 different concentrations of the hydrogen peroxide solution by adding different amounts of water which all equal 20ml. To this I shall add equal amounts of Manganese (IV) oxide (roughly 0.2 grams), this shall make it a fair test. ...read more.

Conclusion

Hydrogen Peroxide Solution (ml) Distilled Water (ml) Manganese (IV) Oxide (g) Temperature before (�C) Temperature after (�C) Time taken to obtain 100cm� of Oxygen (s) 20 0 0.20 23 45 19 18 2 0.20 22 44 21 16 4 0.20 23 42 28 14 6 0.20 21 39 32 12 8 0.20 22 37 40 10 10 0.20 22 35 57 8 12 0.20 23 32 71 6 14 0.20 20 29 147 Average results (figure 1) Hydrogen Peroxide Solution (ml) Distilled Water (ml) Manganese (IV) Oxide (g) Temperature before (�C) Temperature after (�C) Time taken to obtain 100cm� of Oxygen (s) 20 0 0.20 23 46 17 18 2 0.20 22 44 21 16 4 0.20 23 41 25 14 6 0.20 22 39 27 12 8 0.20 21 37 33 10 10 0.20 21 36 49 8 12 0.20 22 33 64 6 14 0.20 20 28 120 Conclusion The evidence suggests that the more manganese (IV) oxide added the quicker the reaction becomes. This is because there is a greater surface area. Also the less Hydrogen peroxide used the slower the reaction becomes. The time taken for the first two reactions is slower than the third set of results this is because the catalyst speeds up the reaction time. Overall I think this experiment went very well but it probably could have been done fairer and more accurately. ...read more.

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