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Rate of catalase activity.

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Enzymes such as catalyse are protein molecules, which are found in living cells. They are used to speed up specific reactions in the cells. They are all very specific as each enzyme just performs one particular reaction. Catalyse is an enzyme found in food such as potato and liver. It is used for removing Hydrogen Peroxide from the cells. Catalyse reacts to decomposition Hydrogen Peroxide into water and oxygen. It is able to speed up the decomposition of Hydrogen Peroxide because it reacts with the Hydrogen Peroxide molecule. This type of reaction where a molecule is broken down into smaller pieces is called an anabolic reaction. I will be investigating how temperature effects the rate of catalyse activity. To do this I will be adding liver (Catalyse) to hydrogen peroxide at different temperatures and measuring the oxygen given off against the time. I believe that the longer the liver is left in the hydrogen peroxide solution the greater the reaction and the more oxygen will be released. I think at first the reaction will be rapid but as time goes on the reaction will slow down. ...read more.


This will all make the results more accurate and make the investigation better and more reliable. While carrying out this experiment I had to make sure it was a fair test to help me do this I made sure I kept to the following precautions: always use 2M hydrogen peroxide. Always use 50ml hydrogen peroxide. Make sure that no air gets into the measuring cylinder until the experiment has started. Keep the surface area of the liver the same. Keep the weight of the liver the same. While carrying out this investigation I had to follow these safety rules. Always wear safety goggles to protect the eyes from the hydrogen peroxide. Keep all apparatus away from the edge of the desk to prevent breakages. Temperature 200C Time Amount of o2 produced 30 seconds 32.8ml 1:00 minute 37.2ml 1:30 minutes 43.1ml 2:00 minutes 50ml 2:30 minutes 60ml 3:00 minutes 70.1ml Temperature 300C Time Amount of o2 produced 30 seconds 32.6ml 1:00 minute 56.2ml 1:30 minutes 72.8ml 2:00 minutes 100+ml 2:30 minutes 100+ml 3:00 minutes 100+ml Temperature 400C Time Amount of o2 produced 30 seconds 72ml 1:00 minute 100+ml 1:30 minutes 100+ml 2:00 minutes 100+ml 2:30 minutes 100+ml 3:00 minutes 100+ml Temperature 500C Time Amount of o2 produced ...read more.


From looking at the tables and my graphs I have confirmed my predictions. As the time increases so does the amount of oxygen as there is longer for the reaction to take place. This is fairly obvious but the second part of my prediction is also backed up, that as time goes on the reaction will lessen because the hydrogen peroxide will be used up. This means the reaction slows up and it releases less oxygen. This is shown in my graph as the first 30 seconds are much steeper that the next as the reaction becomes less rapid. I believe the experiment went well and the results are reliable as it supports my original idea of what would happen. I think my experiment has some limitations as I do not know what would happen to the reaction after three minutes. I believe that my experiment could be improved, to do this I would repeat the experiments and take averages to make it even more accurate. I would also do it for longer and try to do it until the reaction stops and the hydrogen peroxide becomes totally used up. I think this would show that the reaction slows down and then would eventually stop when the hydrogen peroxide is completely used up. ...read more.

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