Title : Properties of hydrocarbon Objective : 1) To study the properties of hydrocarbons. 2) To determine the unknown samples. Results : Part A : Combustion Compounds Observations Hexane There was orange flame and burned mildly during the burning process. No soots and smoke were produced. C6H14 + 19/2 O2 6CO2 + 7H2O Cyclohexene Orange flame burned vigorously. A small amount of black soot and smoke were produced during the burning process.
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Permanganate Process (McBride Method) Optical Method of Analysis: Use of Beer’s Law on KMnO_4 Solution Abstract Potassium permanganate (KMnO_4) is commonly used as an oxidizing agent and in this experiment‚ it is used as both the titrant and indicator. A standard of potassium permanganate solution was prepared and computed to be 0.02235 M and was used to titrate a sulfuric acid solution wherein the sample salt was dissolved. The solution was heated to 90°C then titrated until a light pink colored
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Preparation of the Complex A sample of copper sulfate pentahydrate (6.285g) was weighed out. The copper sulfate pentahydrate was dissolved in water (11.99mL) in a 250mL beaker. The solution was heated on a hot plate to 90 degrees Celsius. A sample of potassium oxalate monohydrate (10.006g) was dissolved in water (50.0mL).
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A theoretical mass of 1140 mg and an experimental mass of 263 mg resulted in a 23.1% yield. This low percent yield is most likely due to error in the experiment. The potassium permanganate test was positive for the presence of a double bond in the product as brown precipitate formed along with the discoloration of the solution. An IR spectroscopy of the product was also performed. Results of the IR absorptions of this experiment
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The amount of hydrogen peroxide was recorded after the reaction for the certain time given has taken place. We used sulfuric acid to stop the reaction with the catalase from occurring. This process is known as denaturing (Campbell 152). The potassium permanganate in this experiment was used as hydrogen peroxide indicator. It determined the amount of hydrogen peroxide remaining after the reaction occurred. Based on our experiment we observed that the time does play a crucial role on the catalase reaction
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solution. The area in which light is absorbed can provide information about the molecule‚ such as the concentration‚ by identifying the most preferentially absorbed wavelength.1 Food coloring and potassium permanganate: This method was used with red‚ blue‚ and purple food colorings and potassium permanganate. Wavelength measures energy in nanometers‚ from the top of one peak to the top of another peak‚ of a wave. Each wavelength
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The Effect of pH on the Rate of Enzyme Catalysis of Catalase Objectives: The objective of this lab was to develop a protocol to investigate the effect of an environmental variable on the catalytic function of an enzyme. More specifically‚ the objective was to perform an experiment in order to test the effect of pH on the function of the enzyme catalase. Introduction: Enzymes are proteins that act as catalysts for reactions. This simply means that enzymes lower the activation energy required
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Kinetics of the Harcourt-Essen Reaction Name: Manpreet Kaur Candidate Number: 7123 AS and A2 Aims: AS AIMS: 1. Investigate the effect of temperature on the rate of reaction. For this aim 3 sets of results will be obtained by timing how long it takes for the colour change to occur in different temperatures determined by the use of an electric water bath. With these results‚ the effect of temperature on the rate of reaction will be investigated. 2
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Introduction In this Lab the students dealt with Osmosis‚ movement of water molecule or solvent from a high concentration to a low concentration‚ through selective permeability‚ a protective barrier that provide some particle the ’direct ’ passage in and out of the plasma membrane ( Lacerda L.2011) Allowing some molecules enter and exit the cell membrane‚ to create a balance in concentration inside and outside of the cell‚ by doing so the cell often become hypotonic‚ where the concentration
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60). Label the remaining beaker “control”. 2. With the “control” beaker pour 10 mL’s of H2O2‚ add 10 mL’s of distilled water (in place of the catalase). Finally add the 10 mL’s of sulfuric acid. 3. Suck up 10 mL’s of potassium permanganate in the pipet. Add potassium permanganate one drop at a time to the beaker. After each drop‚ stir the mixture. Continue to add KMnO4 to the mixture turns brown and stays brown. 4. Invert the pipet and record the amount of KMnO4 left in the pipet. Subtract the
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