added bromine to alkenes. This caused an electrophilic halogenation reaction. If the bromine reacted with the alkene the bromine would discolor from orange and turn clear. Experiment Part A) Solubility of Alkanes: 1 mL of nine solvents (water‚ methanol‚ n-butanol‚ ethylene‚ glycol‚ acetone‚ hexane‚ toluene‚ ethyl acetate‚ and dichloromethane.) was added to nine sample vials. Each vial then had 0.5 mL of the alkane decalin added to each one. The mixtures were stirred to determine if the materials
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OBJECTIVE The purpose of this experiment is to analyze mixtures of compounds prior to‚ during and after a separation scheme. This experiment also allows monitoring reactions of organic molecules‚ and determines the identity of a mixture of compounds. STRUCTURES AND PHYSICAL PROPERTIES OF REACTANTS [1] SOLVENTS | a. Hexane1Molecular Molarity: 86.18 g/molBoiling Point: 69 ºCMelting Point: -95ºCDensity: 0.659 g/mL at 25ºCWater Solubility: Insoluble in waterColor/Texture: Colorless/LiquidHazardous
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HKCEE Chemistry 2007 Paper 1 Section A 1. A is a compound formed from oxygen and magnesium‚ while B is a compound formed from oxygen and fluorine. a) Draw the electronic diagram of A‚ showing electrons in he outermost shells only. (1) b) Draw the electronic diagram of B‚ showing electrons in the outermost shells only. (1) c) Compare the melting points of A and B. Explains your answer. Melting point of A is higher than that of B. Ions of A are linked by strong ionic bonds /
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Conditions section. Glass backed TLC plates will be created with the following three spots: Ketone Standard/Co-Spot/Crude Reaction Mixture. Prepare the TLC plate while the reaction is being set up. To the initial solution of 4-tert-butylcyclohexane in methanol‚ before adding the reducing solution‚ insert a TLC capillary. Use this sample as your ketone standard. Do NOT stop the reaction before checking the progress by TLC. If the reaction is not complete‚ add another portion of the reducing solution.
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nitration of Acetanilide i.e. how hydrogen on a carbon chain is replaced with a nitro group. Reagents and Chemicals: • Acetanilide (5g) • Glacial acetic acid (5mL) • Concentrated sulphuric acid (10mL &1.5mL) • Concentrated Nitric acid (2.0mL) • Methanol (30-50mL) Modification to experimental procedure: The experimental procedure was conducted as per instructions from the chemistry 220 manual. We were told to add 5grams of Acetanilide but due to time constraints I had added 5.05grams. Whilst preparing
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selected for sample preparation. Extract preparation: The extracts of Callistemon citrinus was prepared by grinding the sample into fine powder. Methanol was used as solvent for preparation of extracts. 20 grams of sample was dissolved in 200ml of methanol. After proper mixing‚ they were kept in
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8/21/2009 |Secondary 2 | Shela Septania Usadi | [pic] Table of Contents Part 1: Abstract 1 Part 2: Introduction 1 Fire 1 Color Of Fire 2 Colored Flame 2 Part 3: A Simple Experiment‚ Green Flames 5 The Materials 5 The Method 5 A Higher Explanation 5 Part 4: Multicolored Fire 6 The Materials 6 The Method 6 Part 5: Uses Of Colored Fire 7 Part 6: Effects
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Vol. 1 ACETIC ACID 115 ACETIC ACID 1. Introduction Acetic acid [64-19-7]‚ CH3COOH‚ is a corrosive organic acid having a sharp odor‚ burning taste‚ and pernicious blistering properties. It is found in ocean water‚ oilfield brines‚ rain‚ and at trace concentrations in many plant and animal liquids. It is central to all biological energy pathways. Fermentation of fruit and vegetable juices yields 2–12% acetic acid solutions‚ usually called vinegar (qv). Any sugar-containing sap or juice can
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ABSTRACT: LCZ696 (sacubitril/valsartan‚ EntrestoTM) is a novel therapy proposed for heart failure treatment. It was recently approved by the FDA in order to decrease the mortality rate and hospitalization for patients with chronic heart failure. So this study is considered as the first report to investigate the fluorimetric behavior of sacubitril in addition to pursuing all the different conditions which may affect its fluorescence. Numerous conditions were studied such as studying the effects of
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difference results from internet and mine. The results for Hexane for example was much quicker than I expected‚ I found that it boiling point was 60C but in my experiment it was 30 C it’s the double of what it should be. Most of the sample like methanol and ethanol was pretty clos to the result that I found on internet. The trial that I did was Butanol again with the hot plates and it took of course much longer to boil and it started to boil before 105 °C like at 103 °C and I didn’t expect that
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