Effects of Different Concentration of Catalyse on Hydrogen Peroxide Aim: In this investigation I will try to find how long it takes for the filter paper disc to rise up whilst varying the amounts of concentration of catalyse. Prediction: I predict that the lower the concentration of catalyse the longer it will take for the filter paper disc to rise to the surface of the tube. Equipment: 1. Hydrogen peroxide in a container 2. Flat bottom tube 3. Tweezers 4. Filter paper
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about the kinetics of reactions I decided to do an investigation in this area. I was initially introduced to this particular reaction1 in EP6.4 and then in AA2.1. I was interested in using this reaction as a means of potentially supporting and quantifying some of the theories that I have studied along with also perhaps extending on them. Aim: Using a clock reaction I shall: Investigate the effect of concentration for each reactant and use the results to find the rate equation for this particular
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the increase of hydrogen peroxide; as the amount of substrate increases‚ the more oxygen is produced from the enzymatic reaction of hydrogen peroxide. For example‚ when five drops of hydrogen peroxide was added‚ it can be seen that 16.2mL of oxygen collected in the gas syringe‚ whilst when 15 drops were added‚ 96.4mL of oxygen was indicated‚ strongly supporting the original hypothesis‚ which was that as more hydrogen peroxide was added to the yeast‚ the higher the rate of reaction. Graph 5 further
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affecting the catalytic decomposition of Hydrogen peroxide Please refer to the additional files for tables/graphs. Aim- The purpose of this investigation is to investigate how certain factors affect the catalytic decomposition of Hydrogen peroxide. I will investigate the effect of altering the mass of catalyst used on the rate of the decomposition of Hydrogen peroxide. Introduction- The decomposition of Hydrogen peroxide is a process by which Hydrogen peroxide decomposes into water and Oxygen. It
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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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D-block ions and the kinetics of reactions iodine clock reaction: By Stephen Parsons 6K2 Centre number: 61813 Candidate number: 8270 Table of Contents My aim and my reaction: 3 Rate of reaction: 4 Activation enthalpy: 5 Collision theory: 6 The effect of temperature on reaction rate: 7 The effect of concentration on reaction rate: 7 The effect of a catalyst on reaction rate: 8 D-block elements: 9 The effect of extra kinetic energy (from stirring etc.): 10 Where do we use D-block ion catalysts
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Abstract The decomposition of hydrogen peroxide (H2O2) in a whole and diced wedges by with The enzyme catalase was observed. The catalase was able to break down the hydrogen peroxide In the diced banana wedge better than the whole banana because after the banana was diced that Increases the surface area allowing the breakdown to flow. The effects of temperature on enzyme In a liver sample were observed under iced‚ boiling‚ 37 degrees‚ and room temperature Conditions. The enzymes became completely
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Summary This experiment will measure the rate of oxidation of iodide ions by persulphate ions to derive the rate law for the reaction. Starch will be added to the reaction to facilitate the measure of time during the reaction. The reactant solutions will contain (NH4)2SO4 and KI‚ represented as: (NH4)2S2O8 + 2KI -> I2 + (NH4)2SO4 + K2SO4 This can be simplified to: S2O82- + 2I- -> I2 + 2SO42- These equations can only be carried out and be visible after the iodine has completely
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goggles and an apron or lab coat to protect our eyes and clothes. As we are using enzymes and Hydrogen Peroxide we need to be extra careful‚ ensuring they don’t come into contact with our eyes‚ skin or clothes. Catalyse is an enzyme found in all living cells. It makes Hydrogen Peroxide decompose into water and Oxygen. We will be measuring the amount of Oxygen released from the Hydrogen Peroxide. In order to do this we will use a measuring cylinder. This piece of apparatus measures the
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Hulsey Fire Tech 107 15 November 2015 Hydrogen Peroxide According to Lee Lerner‚ (2008)‚ “Hydrogen Peroxide is most widely found in homes in brown bottles containing three percent solutions (3% hydrogen peroxide and 97% water).” Lee Lerner (2008) writes “Hydrogen Peroxide is a colorless liquid that mixes with water and is widely used as a disinfectant and bleaching agent.” Hydrogen Peroxide is used in many different ways and has different hazards. “Hydrogen peroxide is a strong oxidizing agent used in
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