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Rates Investigation Report.

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Rates Investigation Report. Hydrogen Peroxide,H2O2, decomposes into water and oxygen: 2H2O2 2H2O + O2 The reaction can be catalysed by Manganese Oxide and by the enzyme catalyst, found in yeast. Our task was to investigate the factors, which affect the rate of decomposition of Hydrogen Peroxide. Introduction The factors, which we were allowed to investigate, which could have affected the rate of the reaction were: Temperature and concentration. The factor, which I chose to investigate, was the affect of concentration on the reaction rate. Prediction I predict that the higher the concentration of Hydrogen Peroxide the quicker the reaction rate will be. I have predicted this because the higher the concentration of Hydrogen Peroxide the more it reacts. This is because there are more particles in the same solution, therefore they move more often within a certain time. This what I predict my results graph will look like: Method Apparatus: Ice Cream Tub Conical Flask 100ml Measuring Cylinder Delivery Tube Clamp Stand Clamp Yeast 2 Placed Scales 20ml Measuring Cylinder Hydrogen Peroxide Water Stop Clock What we measured to record our results was how long it took for 20ml3 of oxygen to be produced. ...read more.


Here are our results: H2O2. (ml3) H2O (ml3) Time (sec) 10 10 29 2 18 261 Once we had checked that our highest and lowest concentrations were okay to use we were able to begin our full Preliminary Experiment here are our results: H2O2. (ml3) H2O (ml3) Time (sec) Average Time (Sec) Rate of Reaction (mm3/s) 10 10 29 31 30 0.6 8 12 19 34 27 0.7 6 14 37 40 39 0.5 4 16 102 96 99 0.2 2 18 277 261 269 0.07 After recording our preliminary results we found a problem with our method. The problem was that as the yeast has shell around it we were only getting half of the catalyst really. To solve this problem we decided to add 5ml of water to the yeast this would liquidize the yeast and therefore releasing the full power of the catalyst. Results These were our results using liquidized yeast as the catalyst: H2O2. ...read more.


My results and graphs have proved my prediction to be correct. Scientific reasons for why this happens are that as you increase the concentration of Hydrogen Peroxide the amount of Hydrogen Peroxide particles increase and therefore they move around more often during a certain time and collide more often with each other. At first I thought we may have had an anomalous result when the 2vol concentration of Hydrogen Peroxide took so long to produce 20ml3 of oxygen but as this result repeated itself through our experiments I think that it must be correct. Evaluation I am glad that we did our preliminary work otherwise we would not have been able pick up on an error in our method that error was that we had not liquidized the yeast to use its full affect as the catalyst. Further ways to back up our results would be to check our results with another groups just to clarify that our results are along the right lines, although I believe that our evidence is of a high quality anyway. ...read more.

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