Exp 23 B Synthesis of t-Pentyl Chloride 11-8-12 Purpose: The sysnthesis of t-Pentyl Chloride from alcohol. Procedure: Preparation of t-Pentyl Chloride. In a 125-mL separatory funnel‚ place 10.0 mL of t-pentyl alcohol (2-methyl-2-butanol‚ MW _ 88.2‚ d _ 0.805 g/mL) and 25 mL of concentrated hydrochloric acid (d _ 1.18 g/mL). Do not stopper the funnel. Gently swirl the mixture in the separatory funnel for about 1 minute. After this period of swirling‚ stopper the separatory funnel and
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Valenzuela City Science High School A Marcelo st.Dalandanan‚ Valenzuela City The Feasibility of Ripe Aratiles (Muntingia calabura) as a Source of Bioethanol Table of Contents Abstract ...........................................................................................................................2 Introduction……………………………………………………………………….……………..3 Background of the Study......…………………………………………………………………………….…..3 Significance of the Study .............................................
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oil refining process begins with treating the fractions into mixtures by various methods such as reforming‚ cracking‚ alkylation‚ isomerisation and polymerisation. These new substances are then separated using fractional distillation or solvent extraction. Fractional distillation of petroleum is the process of separating the oil into different materials. Separation by
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145 (2003) 122-128. [7]Bouker M‚ Harmin A. Effect of Climate conditions on the performance of a simple basin solar still : A comparative study. Desalination 137 (2001) 15-22. [8]G.N. Tiwari‚ S.A. Lawrence‚ Thermal Evaluation of High temperature distillation under an active mode of operation‚ Desalination‚ 85 (1992) 135-145. [9]Singh H N‚ G N Tiwari. Monthly performance of passive and active solar stills for different climate conditions‚ Desalination‚ 168 (2004) 145-150. [10]Manmook Rustum‚ Omar Badran
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plus 3 drops of concentrated sulfuric acid). A strong exothermic reaction occurs. Once the reaction mixture is cooled in the fume cupboard (after about 10mins-15mins)‚ the process of isolating the ester by solvent extraction and purifying it by distillation began. The first step of purifying the ester was to add 100mL of water to the reaction mixture and transfer it to a 250mL separating funnel. A further 50mL of water was used to make sure all of the reaction mixture had been transferred to the
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catalyzing agent. The crude ester produced in lab was isopentyl acetate‚ because first‚ the product smelled of bananas and second‚ the IR spectrum for the product shows that the product is isopentyl acetate. As for the purity of the product‚ the distillation of the crude ester showed that its boiling point was supposed to be 130°C - 140°C and the boiling points of the impurities that could have been in the crude ester have lower boiling points. Therefore‚ since the crude product had a boiling point
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The five common methods that can be used to separate various types of mixtures are filtration‚ fractional distillation‚ evaporation‚ sublimation‚ and chromatography. Evaporation is the changing of a liquid into a gas often under the influence of heat. A mixture of a solid and liquid can be separated by evaporation. Filtration is a technique that uses a porous barrier
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Introduction: The purpose of this experiment is to derive Isopentyl acetate (banana oil) from the reaction of an alcohol and a carboxylic acid in a process called Fischer esterification (Fischer-Speier esterification). The name‚ banana oil‚ is due to banana odour released by formation of Isopentyl acetate. The alcohol and the carboxylic acid used in this experiment are Isopentyl alcohol and Glacial Acetic Acid. Both the overall reaction of Fischer esterification and the specific Fischer esterification
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Preparation of Synthetic Banana Oil Eric Nelson Chem. 253-1: Deepali Rathore Lab 1: Preparation of Synthetic Banana Oil 9-24-10 Purpose To create Isopentyl acetate with no more than 10% isopentyl alcohol and no more than 2% acidic acid in its composition. Theory Esters are a chemical functional group that usually forms by loosing a hydroxyl group and having it replaced with an alkoxy group with the loss of hydrogen. Esters are most commonly produced by taking a carboxylic acid‚ and
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phosphoric acid to become 4-methylcyclohexene. This demonstrates the loss of an alcohol group by protonation‚ the loss of a proton from the cyclohexane to form an alkene through elimination. This also demonstrates Le Chatelier’s principle‚ by using distillation to remove the product as it is formed the equilibrium of the reaction will constantly be in favor of the product. Reaction: Side Reaction: Due to a 1‚3-hydride shift dehydration of 4-methycyclohexanol will produce a small amount of 1-methylcyclohexene
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