Using ethanol as an alternate fuel‚ or fuel extender includes a heterogenous agglomeration of advantages and disadvantages. On cars: ethanol is preferable to lead as an octane booster. A 10% addition of ethanol to petrol is more effective than lead at boosting octane rating (+2.5) and making car run smoother. It’s cheaper than lead‚ and ethanol-blended fuels leave no gummy deposits‚ thus keeps engine clean. Although a minimal 10% ethanol blend should be compatible with internal combustion engines
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Heat of Mixing: Ethanol and Water Abstract The temperature change when known amounts of water and ethanol were mixed was determined to see the enthalpy change in an isothermal and isobaric environment. Agreeable data was found compared to similar experiments. As the mole fraction increased of the solution so did the enthalpy until a certain limit of about 0.32. Since water’s structure and unique properties affect many aspects of a solution‚ the solutions enthalpy’s decreased at a certain time
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the mass and the given percent mass of ethanol‚ we found the density of pure ethanol for each known concentration of alcohol‚ and averaged the three calculated densities to give us a density of pure ethanol (0.8391 g/mL) that we could use to calculate the concentration of the unknown solution. We used this to calculate the volume of ethanol in the unknown test tube (7.918 mL)‚ and used the calculated density of ethanol to convert volume ethanol to mass ethanol in the unknown test tube (6.644 g). Since
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Distillation of an Ethanol- water Mixture Abstract The purpose of this experiment is to understand the process of distilling a solution. Thesolution of 50/50 ethanol-water was used in the experiment. Using fractional distillationapparatus ethanol-water mixture was separated. The fractional use of copper sponge wasused in distillation process which created the heat exchange area between the vapor of ethanol and liquid water. The fractional distillation process yield 9.5 ml of ethanol incollecting flask
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a tabular form which showed how the data presented. Physical Properties Table 1: Differences of BIT and Commercial Ethanol in Density and Smoke Emission Properties BIT (MEAN) Ethanol (MEAN) Density 300 kg/m^3 354.64 kg/m^3 Smoke Emission Clear Clear In table 1‚ the researchers compared the physical properties such as the density and smoke emission of BIT and commercial ethanol. The density of BIT which was the 300 kg/m^3 was obtained by using the formula of mass over
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BIOFERTILIZER: The pathophysiology of the Tuberculin reaction is explained thus: M. Tuberculi are engulfed by macrophages after being identified as foreign‚ but due to a self- preserving mechanism peculiar to TB it is able to block the fusion of the phagosome within which it is existing with the lysosome which would destroy it. So it can continue existing and replicating within the immune cell designed to destroy it. After several weeks‚ the immune system somehow [ mechanism as yet unexplained]
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the M button. 3. The method was then saved based on sample name and the FILE menu was clicked. The method is then saved as on a created new folder. 4. Calibration must be done using BaSO4 for solid sample or solvent for liquid (50%ethanol and 50% DI water / 70% ethanol and 30% in DI water) containing the analyte (five concentration of analyte plus bank i.e without sample) as standard calibration. 5. The BaSO4 for solid or solvent for liquid cell was placed at sample holder. The BASELINE icon
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95% ethanol and 1.5 mL of 2 M sodium hydroxide solution to the flask 5)Stir with magnetic stirrer for 15 minutes or longer if precipitate still forming (if cloudy after 15 mina heat mixture on a asteam bath or in boiling water for 10 mins then cool to room temp) When precipitate is complete cool flask in ice-water bath for 10 mins MEANWHILE--- A)place 4 mL of 4 acetic acid in 95% ethanl in a test tube B)Repeat this procedure with 2mL of 4% acetic acid in 95 % ethanol (v/v)
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organic solvents The emulsion test is a method to determine the presence of lipids using wet chemistry. The procedure is for the sample to be suspended in ethanol‚ allowing lipids present to dissolve (lipids are soluble in alcohols). The liquid (alcohol with dissolved fat) is then decanted into water. Since lipids do not dissolve in water‚ when the ethanol is diluted‚ it
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alkenes (C2H4) * Functional group = highly reactive double C=C bond * Readily transformed into many useful compounds ( polyethylene) through addition reactions * Examples: ethylene oxide (CH2)2O -> sterilizer Ethanol (C3COOH) -> solvent Polyethylene (CH2)n -> plastic 1D – identify that ethylene serves as a monomer from which polymers are made * Individual monomers of ethene join by covalent bonds to form long chain polymers 1E
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