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Investigating the Speed of the Reaction of a Catalytic Decomposition of Hydrogen Peroxide

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Introduction

MARCUS HESSENBERG INVESTIGATING THE SPEED OF THE REACTION OF A CATALYTIC DECOMPOSITION OF HYDROGEN PEROXIDE For our experiment, we shall be investigating the catalytic decomposition of Hydrogen Peroxide. To do this, we shall use manganese dioxide as a catalyst. The Equation for this experiment is as so: 2H2O2 (aq) -----> 2H2O + O2 We shall be finding out how the concentration of the Hydrogen Peroxide affects the rate of the reaction. Reactions occur at different speeds, from a few seconds, to millions of years. Chemists have a theory to why this happens. Collision Theory Chemists believe that chemical reactions take place when the reactant's particles collide and so produce the product. This is called the collision theory. Not all collisions that take place though cause a reaction, to cause a reaction they must have enough Activation Energy. This breaks the bonds. There are four ways of increasing the rate of a reaction: Increase the concentration Increasing the concentration in soluble reactants means that as there is less space between the particles, there are more collisions, and because there are more collisions, there are more successful collisions i.e. ...read more.

Middle

When the cross was invisible through the reactants we stopped the timer. The results were as follows: H2O (ml) Acid (ml) Thiosulphate (ml) Time (s) Rate 0 20 20 71 1/71 5 15 20 85 1/85 10 10 20 100 1/100 15 5 20 120 1/120 As shown in this experiment, as the concentration was diluted, the rate decreased. I believe a similar occurrence will happen in our experiment. Strategy The reaction produces oxygen. We can use this to our advantage either in two ways. A) We could find out how much of this gas is produced in a certain amount of time, or B) Find out how long it takes for a certain amount of gas to be collected. Apparatus 2 Measuring Cylinders - To measure the chemicals, Chronicle Flask - For the reactants to be contained and mixed, Water bath - To contain water so as the oxygen can reach the top of the delivery tube, Stop watch - To time the experiment, Set up the apparatus as shown below: >Oxygen Delivery Chronicle Flask Tube Hydrogen Peroxide ManganeseOxide Water Method 1. Place Safety Glasses and Laboratory Coats on 2. ...read more.

Conclusion

Justification The reason for this is because when a concentration is high, the particles have less space between them, so they collide more often, meaning that more are successful. The reason why the rate always slowed down towards the end was because, as the reaction went on, fewer particles were there to collide as many have already reacted. This means that more space was between the particles and so collisions were not as common. This is as predicted in the prediction. Problems Errors Reliability To make sure if our results are reliable, we can re-do the experiment to double check our results but we did not have enough time to do this. There are many ways we could improve our experiment. We could have used an electric water bath that kept the temperature at a constant temperature for example. We could use a computer to measure the amount of oxygen left at the start to make it more accurate than our sight allowed. We could also have extended the amount of results to see if the rate slowed down. Further Work If we had more time, there would have been alot more useful information that we could have gained. We could use other concentrations of Hydrogen Peroxide to test if this affected the rate even further or we could use other acids completely. ...read more.

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