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Chemistry Investigation catalysts.

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Introduction

Chemistry Investigation catalysts Aim Prediction I predict the higher the amount of catalyst used the higher the rate of reaction (ROR). This is because a catalyst speeds up a reaction; so the higher the amount of catalyst used the higher the ROR. The ROR can be measured by the amount of oxygen given off by the reaction. My preliminary work also points out that the higher the amount of catalyst used the more vigorous the reaction, I think this is because. The hydrogen peroxide is slowly breaking down, the catalyst works like an enzyme, it speeds a reaction up without taking part in it. I predict that this reaction will be sped up by the catalyst: 2H202 --> 2H2O+O2 The reaction I predict will take place: 2H202 --> 2H2O+O2 MaO2 A Catalyst is a substance that alters the rate of a chemical reaction without itself undergoing any chemical change. If a reaction has more catalyst present, the catalyst (Manganese Oxide), stands more chance of colliding with a hydrogen peroxide particle, thus creating a greater reaction rate. If there is less catalyst then, the catalyst will take longer to collide with the same amount of hydrogen peroxide and make it react. The diagram bellow illustrates this: Manganese oxide (the catalyst) Hydrogen peroxide My preliminary work seems to agree with this conclusion so far: In my preliminary work I tried different amounts off catalyst with a 50% hydrogen peroxide solution and this is what I found: Amount of Catalyst used (g) ...read more.

Middle

I will take readings every 10 seconds of the amount of water displaced from the burette. so I can see how the ROR changes throughout the reaction. I will repeat each test twice. Results: Table recording the amount of gas (oxygen) given off from the reaction at different time intervals: 1st Set of Results: Time(secs)/ Mass (g) 0.02g 0.04g 0.06g 0.08g 0.10g 10 0.5 2 1 5.6 12 20 4.5 8 9 19 30 30 7.0 13.5 15 27.4 45 40 9.5 17 19 34.4 - 50 11.5 21 23 40 - 1:00 13.0 23 27 44.7 - 1:10 15.0 25.5 30 49 - 1:20 16.5 28 33 - - 1:30 17.5 30 35.5 - - 1:40 19 32 38 - - 1:50 20 34 40 - - 2:00 21.5 36 42 - - 2:10 23 38 45 - - 2:20 24 39.8 46 - - 2:30 25.3 41.5 49 - - 2:40 26 33.2 - - - 2:50 27.5 45 - - - 3:00 28.5 47 - - - 2nd Set; Repeats Time(secs)/ Mass (g) 0.02g 0.04g 0.06g 0.08g 0.10g 10 0.5 2 1.5 4 11 20 5 11 10 17 28 30 7.5 15.5 16 25.5 44 40 8.5 20.2 19.5 32.5 - 50 12.5 23.5 23.5 38 - 1:00 13.5 26.5 27 44.5 - 1:10 15.5 29.3 30.5 47 - 1:20 17 31.5 34 - - 1:30 18 33.8 36.5 - - 1:40 19 36 39 - - 1:50 20.5 38 41 - - ...read more.

Conclusion

I could have made a timing error, or a reading error when noting down results. I could have made my results more accurate in a number of ways; I could have used more precise measuring equipment; for example a weighing scales that measures up to 0.000g, this would increase the accuracy of my results greatly. I could do more repeats, as this would make my results more accurate, if I took the average of all sets of results. Although my evidence/ results are not perfect, they are still satisfactory to support my conclusion. I set out to see how the amount of catalyst used affects the reaction, and my results show a trend. What makes me more convinced that I can support my results is that my prediction is similar to what actually happened. My results contain a few anomalies but they are still sufficient to support my conclusion. My results are not accurate enough to say; for example that it takes 32 seconds for the reaction to complete if 0.01g of catalyst is used. I now know the affect that the amount of catalyst (manganese oxide) used has on the reaction rate off hydrogen; I could keep this variable the same and alter the strength of the hydrogen peroxide solution. I would still use the same equipment set up as before, but would use the concentration of hydrogen peroxide as my variable, instead of manganese oxide. I would use these concentrations of hydrogen peroxide: 20% 40% 60% 80% 100%, the hydrogen peroxide would be diluted with water. GCSE Catalyst Investigation Page 1 ...read more.

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