Review of two experiment the first on the reaction between a gummy bear and molten potassium and the second is Oxidation of glycerine by potassium permanganate

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When combining one gummy bear, which is composed mostly of sucrose with molten potassium chloride, a violent reaction occurs. A surprising amount of energy us released by the reactant, and in process, the atom and molecule rapidly rearrange to form 3 products(CO2/H2O and KCl). This reaction is said to be products favor. A favoured product reaction is where almost all of the reactants, react to form products. In this case its sucrose and potassium chlorate react completely to form carbon dioxide, water and potassium chloride. This reaction is exothermic, releasing energy in the form of heat and light (we can see flame a bright light during the experiment). The energy released is also equal to the calorific content of the Gummy- Bear. This reaction shows the conversion of a form of energy to different forms such as thermal/heat energy and light energy. The potassium is acting like an enzyme in the reaction.

It is basically like cellular respiration, it demonstrates the conversion of chemical bonds. For example, energy in food like glucose is transformed into a specific form of energy that our body can use. It is the same process for this gummy bear and molten potassium chlorate reaction. Since, sucrose contains glucose, a gummy bear is used. Bonds of glucose have a lot of energy in them and these bonds are converted into different forms of energy. During the reaction, we can see the substance coming out of the test tube. Carbon dioxide and water are ejecting from the tube. The same occurs with cellular respiration and our bodies. The molten Potassium Chlorate oxidising properties are well shown. Sucrose is oxidized into Carbon, carbon dioxide and water. This reaction is exothermic, releasing energy, as said before in the form of light and heat. The total energy released in this reaction is equal to the calorific content of the Gummy bear.

C12H22O11(s)+ 8 KClO3(l) + HEAT ----> 12 CO2(g) + 11 H2O(g) + 8 KCl(s)Experiment 2: Oxidation of glycerine by potassium permanganatePotassium permanganate is a very powerful oxidising agent and when combined with glycerine, an easily oxidized substance, the properties of both are very well shown and a reaction occurs. When a few drops of glycerine are placed in a pile of potassium permanganate, a redox type reaction occurs. This reaction is exothermic (releasing energy). With the glycerine boiling giving off smoke and eventually producing flame that spreads around the pile of potassium permanganate. All the glycerine is going to be consumed by the permanganate. Also in the reaction, both kinds of energy are produced. Light and thermal energy. After all the reactants of this reaction have reached the necessary activation energy, the pile of Potassium permanganate combusts into a very hot flame which is usually exceeding 1000 degrees Celsius. Potassium permanganate oxidizes glycerine in a spontaneous reaction that generates a lot of energy in the forms of heat and light. It is said that items of food contain considerable energy. With appropriate conditions, this energy is released much more rapidly than in our body. That is why this reaction appears so violent to our eyes. The energy is released very rapidly. The two reaction are really similar one to the other.

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