Objective: To investigates the enzymatic effect of various materials in the hydrogen peroxide solution. Apparatus & Equipment: Beaker Test tubes Either: water bath (95oC) or Bunsen burner Materials: Fresh Liver Potato cubes Manganese dioxide Hydrogen peroxide** Wood splints **Caution: Hydrogen peroxide is formed continuously as a by-product of chemical reactions in living cells; it is a very toxic (poisonous) substance. [Note: using boiling tubes may provide
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For many years Hydrogen peroxide was widely used for disinfecting‚ sterilization and its antiseptic properties‚ it is cheap and easily available OTC at any drug store or grocery store. “This readily available oxidant is rapidly converted to the highly reactive hydroxyl radical that damages an array of cellular components” (Atiyeh‚ Dibo‚ and Hayek‚ 2009). “The Medicines and Healthcare Products Regulatory Agency (MHRA‚ 2014). Have issued a warning regarding its use in surgery and in deep and large
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Decomposition Of Hydrogen Peroxide By The Enzyme Catalase Which Is Found In The Liver" Introduction: Enzymes are biological catalysts. They speed up the chemical reactions which go on inside living things. Without them the reactions would be so slow that life would grind to a halt. Enzymes work by when a substrate molecule bumps into a molecule of the right enzyme‚ it fits into a depression on the surface of the enzyme molecule. This depression is called the active site. The reaction then takes
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speed up reactions. They have an area with a very particular shape called the ‘active site’. When the right molecule comes along (substrate molecule) it will fit perfectly into the active site and there will be a reaction. After the reaction the products then leave the active site. This process is often referred to as the lock and key theory as only one enzyme can carry out one type of reaction. The catalase enzyme speeds up the breakdown of hydrogen peroxide into oxygen and water. The hydrogen peroxide
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Chemical Kinetics of Hydrogen Peroxide Decomposition Purpose The purpose of this experiment was to determine the rate equation for the catalyzed decomposition of hydrogen peroxide H2O2. Procedure The procedure for this lab can be found on pages 36 - 40 in “General Chemistry CHE111L Laboratory Manual Spring 2014.” Data Tables Carbon copies of data tables and the graph have been attached to the back of this lab report. Calculations 30 mL of
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Kinetics of the Decomposition of Hydrogen Peroxide Lab Introduction: In this week’s lab experiment‚ the rate of decomposition of hydrogen peroxide forming oxygen gas will be observed and studied. Since the rate of a chemical reaction is dependent on two things; the concentrations of the reactants and the temperature at which the process is performed‚ the rate can be measured at which a reactant disappears or at which a product appears. When measuring the rate‚ the rate law will be applied. The
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because it can cause hazard for the humans and possibly to the environment‚ the hydrogen peroxide is now as an alternative to replace formalin for a common treatment for parasites (Pedersen and Flemming‚ 2010). Graslund et al‚ 1 (2003) showed that the hydrogen peroxide acts as chemical that served several purposes such as to eliminate bacteria‚ parasite and also algae in shrimp farming. However‚ the hydrogen peroxide still can be hazardous for the health of farmers (Boyd‚ 1999) and also affect
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the rate of Hydrogen Peroxide degradation using Catalase Introduction An enzyme is a globular protein which functions as a catalyst that speeds up the rate of a reaction without being consumed in the reaction. An enzyme-catalyzed reaction occurs when a substance called the substrate binds onto the active site of the enzyme. This joining allows for a reduction in the activation energy and the reduction in activation energy helps the reaction to occur at a quicker rate. Enzyme reaction can be affected
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of hydrogen peroxide with a fixed mass of catalyst. A catalyst is a substance‚ which alters the speed‚ or rate of a chemical reaction but is chemically unchanged at the end of the reaction. The two factors that we can change are the temperature and the concentration. We chose to vary the concentration of hydrogen peroxide. The catalyst to speed up the reaction without affecting the result will be manganese oxide. Prediction: I predict that the higher the concentration of hydrogen peroxide‚ the
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Study of the first element – Hydrogen. Answer the following questions:- 1. Give a reason why hydrogen can be placed in group 1[IA] and group 17[vIIA] of the periodic table. 2. What similarities does it show with group 1[IA] and group 17[VIIA]. With special reference to valency electrons and ion formaton and examples. 3. How does hydrogen occur in the free and combined state? 4. Which metals react with cold‚steam and boiling water to form their respected oxides and hydroxides ? Give examples and
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