define , destructive distillation?
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Destructive Distillation means driving off (and collecting) gas from some matter by heating it in the absence of air. This is the process called 'coking' when referring to the transformation of bituminous coal into coke (at 1,000 C).\n\nExamples of substances that are commonly destructive distilled to extract chemicals and other materials include:\n\n    * Wood\n    * Soft coal\n\nExamples of substances extracted include:\n\n    * Acetic acid\n    * Methyl or wood alcohol\n    * Coal gas\n    * Tar
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Denatured alcohol is ethanol with added adulterants that make it useless for consumption as an intoxicating beverage by rendering it toxic or extremely distasteful to drink, but still useful for industrial processes or as a household chemical. This is done in order to make it exempt from taxes that apply to potable alcohol.\n\nEthanol, also known as ethyl alcohol or grain alcohol, is a flammable, colorless chemical compound, one of the alcohols that is most often found in alcoholic beverages. In common parlance, it is often referred to simply as alcohol. Its molecular formula is C2H6O, variously represented as EtOH, C2H5OH or as its empirical formula C2H6O.\n\nIsopropyl alcohol or isopropanol is a common name for propan-2-ol, a colorless, flammable chemical compound with a strong odor. It has the chemical formula CH3CHOHCH3, and is the simplest example of a secondary alcohol, where the alcohol carbon is attached to two other carbons. It is an isomer of propan-1-ol.
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LIQUID-VAPOR EQUILIBRIUM IN BINARY SYSTEMS\nApparatus\nBoiling apparatus with heating mantle and variac (S), 1/100o thermometer (S),\nrefractometer (L), glass beads or boiling chips (S), weighing bottles (D), small\nstoppered vials (D), 250 ml n-hexane (S) and 250 ml absolute ethanol (S).\nOther binary systems which may be investigated are (1) cyclohexane (S)-\nethanol (S); (2) ethyl acetate (S)-ethanol (S); (3) Methanol (S)-ethyl acetate (S);\n(4) isopropanol (S)-n-hexane (S); (5) isopropanol (S)-cyclohexane (S); (6)\nisopropanol (S)-ethylacetate (S); (7) Acetone (S)-cyclohexane (S); (8) Acetone\n(S)- hexane (S); and (9) cyclohexane (S)-2-propanol (S), (10) 1 Propanol-water.\nCONSULT YOUR LAB INSTRUCTOR TO FIND OUT WHICH SYSTEM YOU\nARE TO INVESTIGATE.\nCAUTION: The ORGANIC LIQUIDS are TOXIC and FLAMMABLE! Use all\nnecessary precautions to avoid accidents!\nCAUTION: DISPOSE OF THESE ORGANIC LIQUIDS by placing in the\nWaste Containers provided. DO NOT POUR DOWN THE DRAIN!\n\nAssemble the apparatus with care; consult instructor if you are at\nall doubtful how to put the pieces together. A 3-way stopcock (shown in Figure\n2) is provided as a means of withdrawing samples of distillate and residue at the\nappropriate time. Best procedure is to withdraw distillate first, then the residue.\n\nProcedure\nClean the apparatus by rinsing with a few milliliters of pure n-hexane. Make sure\nvials are clean and DRY and have labels for marking. Add glass beads to flask\n(carefully).\nThere are three particularly important requirements in this experiment.\n• Make sure that the condensed distillate and the liquid residue samples are\ncollected under equilibrium conditions\n• Read the equilibrium temperature accurately\n• Analyze the compositions accurately\nPlace the thermometer in a position near the top and center of the three legs of\nthe first insert as seen in Figure 3. The hole in the second insert should be\nplaced pointed towards the condenser\nPlace 50 ml n-hexane in a flask. Adjust the variac (not more than 100 -110 volts)\nso that liquid boils "reversibly" (very moderate boiling with only very tiny bubbles\nformed) and so that distillate comes over at a rate which will fill the sample tube\nonce every two or three minutes.\nDraw off the first fraction (containing impurities) which comes over and discard\n(use waste container). When a constant boiling mixture is obtained, record the\nboiling point and withdraw samples from distillate and residue into marked vials.\nAdd 1 ml ethanol to the distillate in the flask, obtain equilibrium-boiling, record the\nboiling point, and again withdraw samples of distillate and residue for analysis.\nBoiling points and refractive indices of the distillate and residue are then\ndetermined after successive additions of 0.2, 0.5, 1, 2, 5 and 5 ml of ethanol. The\nrefractive indices are used to obtain the mole fractions of ethanol in these\nsolutions.\nClean the apparatus by rinsing with a few milliliters of ethanol, and repeat the\nprocess starting with 50 ml of ethanol in the flask. Now, however, boiling points\nare to be determined after successive additions of 0.5, 1, 2, 5, 15 and 20 ml of nhexane\nto the flask.\nIn order to construct a plot of refractive index versus mole percent ethanol, the\nrefractive indices are determined for the pure hexane and ethanol and for a\nseries of solutions containing accurately known weights of hexane and ethanol.\nMixtures about 5 ml in volume containing approximately 1 volume of ethanol to 1,\n3, and 6 volumes of hexane are convenient. To obtain a decent standardization\ncurve of refractive index versus mole fraction, a series of 6 to 8 solutions\ncontaining accurately known weights of n-hexane and ethanol must be prepared\nand their refractive indices measured. Only a few milliliters of each of these\nsolutions are required, so do not waste chemicals when preparing them. The\nrequired data for the vapor pressures of the organic liquids are availab
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Distillation. Put sugar water in a crucible or beaker and heat over a burner. When all the water has evaporated, the sugar will be left. If you are actually going to carry out this experiment, be careful to not burn the sugar after the water has evaporated, unless you don't mind throwing out the beaker or doing some serious scrubbing.
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a simple distillation unit can be made using a bucket or nother resevior and placing plastic or plexiglass slightly above it at an angle that will direct the water that condensates on the glass into another container. this however will only remove the minerals. the water changes to a gas and then condense on the glass into a liquid again, the minerals do not
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I'm going to assume you mean water distillation.  Water distillation is done by evaporating water (one change of state: evaporation), and then cooling that water vapor (another change of state) and collecting the liquid water.
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Sloppily-produced moonshine can be contaminated with toxins, mainly from materials used in construction of the still. Despite the well-known hazards, it is claimed that stills constructed using car radiators for a condenser are still used. The lead used in soldering these radiators ends up in the moonshine, and in some cases, glycol products from antifreeze used in the radiator can appear as well. Both are poisonous.\n\nOccasionally moonshine is deliberately mixed with industrial alcohol-containing products, including methanol and denatured alcohol. Results are toxic, with methanol easily capable of causing blindness and death.\n\nMethanol and other toxic alcohols can occur naturally in distilled spirits and are called fusel oils. The methanol is concentrated in the first few percent of condensate produced in a batch. The fusel oils are mostly found at the end of a batch or run. Ordinarily these portions are discarded, though if ingested alone or included with the rest of the distilled product it may cause toxic effects. Like commercial beer, wine, and liquor, properly produced moonshine contains small amounts of methanol at levels that are not toxic. A common way to determine the "quality control" of a batch of moonshine was to see if the moonshiner would dare to drink it.\n\nIn addition, moonshine that is over 100 proof (i.e. 50%) is very flammable and easily ignitable. This is especially true during the distilling process in which oxidized vaporized alcohol can accumulate in the air if there is not enough ventilation.
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http://en.wikipedia.org/wiki/Sugaring_(epilation)\n\nTry this.\n\nOuch
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-making liquor.  \n-When painting, you are basically doing a distillation of polymers in solvent while it dries.  The same with stain/polyurethane.\n-Drinking water obtained from the oceans must be distilled to get rid of the salt and minerals.\n-Often decontamination of drinking water will cause a city to issue a boil order, which means clean water must be distilled in your home.
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bleach, otherwise just mountain dew
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Ethanol is classified as a depressant.
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Dilution (with liquid)\nOxidation (heat)\nAggregation (mixing different ingredients)\nFrustration (when it comes out burnt)
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rubbing alcohol will desolve most adheisives
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Well, when I was an organic chemist, I mostly mixed and poured.  So, what you do is, take something that's kinda like what you're making, add something that's very reactive (so toxic and/or explosive), mix, and heat.  Wash out the impurities, then either crystallize or distill-crystallization-kinda fun, distilling-monumentally boring(although those explode sometimes too).  Then analyze by NMR, TLC, HPLC,GC and IR.  Some people just do the analysis.\nThat's about it.  It was kinda fun, but it got old, and it was dangerous.  And scale varies depending on where you work.
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Distillation Fatty acids and fatty alchols for the Cosmetic industry
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Multiple Effect Distillation (MED) is the most efficient common way using 2-4 kWh/kL
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That's called earthshine. Moonshine is homemade liquor.