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I shall be investigating what affects the decomposition of Hydrogen Peroxide. I will accomplish this by setting up an experiment with a hypothesis, diagrams and a complete write up.

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I shall be investigating what affects the decomposition of Hydrogen Peroxide. I will accomplish this by setting up an experiment with a hypothesis, diagrams and a complete write up. Hydrogen Peroxide is a colourless, viscous and unstable liquid with strong oxidising properties. It is a chemical compound of Hydrogen and Oxygen with the chemical formula H202. Pure, anhydrous Hydrogen Peroxide is a colourless, syrupy liquid with a relative density of 1.44. It blisters the skin and has a metallic taste. The liquid solidifies at -0.41�C (31.4�F). Concentrated solutions are unstable, and the pure liquid may explode violently if heated to a temperature above 100�C (302.4�F). It is soluble in water. To slow the decomposition of the peroxide into water and oxygen, organic substances such as acetanilide are added to the solutions, and they are kept in dark bottles at a low temperature. Hydrogen Peroxide is manufactured in large amounts by the electrolysis of aqueous solutions of sulphuric acid or of potassium bisulphate or ammonium bisulphate. In this investigation I am exploring what affects the decomposition of Hydrogen Peroxide and the variables are what affect the reaction. There are five types of variables, these are: - 1) Categorical - these variables are things such as colour and shape of object used to carry out experiment. As I am investigating what affects the decomposition of Hydrogen Peroxide, this type of variable does not alter the investigation, as it shall be kept as a constant. ...read more.


The main risk, which scientists carrying out this experiment would experience, is the corrosiveness and harmfulness of the Hydrogen Peroxide. It blisters the skin and can be poisonous. This hazard can be overcome by handling the compound with care, wearing protection i.e. gloves and eye protection e.g. goggles. Another risk is the hazard glass can pose when not handled and used correctly. The gas syringe can pop out causing a danger to the scientist conducting the experiment. This minor hazard can be overcome by handling all glassware with care and full attention. Due to the experiment only taking a short duration of time to complete, most variables are ineffective. Categorical, Continuous and discrete variables will all be at a constant throughout the practical ensuring a fair test. The Independent and Dependant variables shall be calculated, controlled and recorded by the scientists performing the experiment, this shall also ensure a fair test. To ensure fair testing measuring cylinders and spatulas are used to make sure that the exact same amount of each substance is used for each experiment. Whether it be just one scientist conducting the experiment, or three, the same set of eyes and actions shall carry out the same job in each experiment to ensure fair testing. Conclusion * From my research I have discovered the formula: - Rate of Reaction = volume of oxygen given off Time taken to complete Experiment This formula enables me to calculate the rate of reaction for each concentration: - 20% = 377.5 � 240 = 1.57 cm�/s 16% = 200 � ...read more.


The abnormal amount of Oxygen given off was due to the freshness of the Hydrogen Peroxide as it had just been made up by one of the laboratory technicians at school, therefore making it more reactive as it had not had anytime to decompose itself in anyway. I will modify and expand the original experiment in a number of ways. Firstly I must decide what I'm going to investigate. I am going to investigate how temperature affects the decomposition of Hydrogen Peroxide. Method to investigate how temperature affects the decomposition of Hydrogen Peroxide: - 1. Pour 10ml Hydrogen Peroxide into a test tube. 2. Place the test tube into a water bath at a certain temperature and begin the stopwatch. 3. After 3 minutes in the water bath, withdraw the test tube and re-measure the Hydrogen Peroxide left. Record the amount left in the test tube. 4. Carry out the experiment for temperature ranging from 10�C to 90�C. Don't range the temperatures near the boiling and freezing points of water (100�C and 0�C), as the state of the Hydrogen Peroxide will affect the rate of reaction. 5. After recording the set of results, place them onto a table and graph from analysis and observation. Enabling an investigation into how temperature affects the decomposition of Hydrogen Peroxide. * Encarta Encyclopaedia 1998 Version CD - ROM. * Britannia Encyclopaedia 2002 Version CD - ROM. * Multimedia Science Software * SEC Science Books * CGC Chemistry GCSE Revision Book. Coursework Factors Affecting The Decomposition September / October Of Hydrogen Peroxide 2002 Chemistry 1 David Clark Mr Edwards room 20 ...read more.

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