i want modelling and simulation code for the separation of the acetic acid from water by using pervaporation .
300439
This question is miscategorized.\n\nSpecial Education refers to the education and parenting of children with special needs.
80429
The CRC Handbook of Chemistry and Physics has all kinds of good information like that (although it is pricey).\n\nOr, search the web for the specific liquid of interest.
696809
PVOH \nYou need to register at 1st site below to gain access but not at any of the others...;\nhttp://www.omnexus.com/login.aspx?url=/resources/innovation/news.aspx%3Fid%3D4489&rfr=http%3A//www.omnexus.com/resources/innovation/index.aspx%3FReturnUrl%3D%252fresources%252finnovation%252fnews.aspx%253fid%253d4489%234489\nhttp://www.ctp-plasro.co.uk/PDF/PVOH%20articles(new).pdf\nhttp://www.amcuk.ltd.uk/water_soluble_film.htm\nPOLYMERS\nhttp://www.e-polymers.org/index.cfm\nhttp://scifun.chem.wisc.edu/chemweek/polymers/polymers.html\nhttp://www.cem.msu.edu/~reusch/VirtualText/polymers.htm
498348
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
1077305
Refer to IUPAC's web site iupac.chemsoc.org or search on Google.
445522
Acetic acid (HC2H3O2, or CH3COOH). Vinegar.
386757
I think there is a program called Acid. Find out about it here: http://www.acidplanet.com/tools/default.asp?p=acid\nIt should be available at your local electronic store. Maybe.
757850
use multiple effect evaporator.\nhttp://www.answers.com/topic/sugar
1118753
Take 2 hard glass boiling tubes.In one of the tubes put small pieces of wood, and some water in the other tube.Heat the first tube with burner.First heat gently and then strong heating.Through a delivery tube collect all the gases produced in the first tube under water in the second tube.By means of another delivery tube the gases over water in the second tube is taken out. This gas is simply called wood gas.Though we call it wood gas it is not a simple gas but a mixture of many.You will see  drops of black liquid at the bottom of the second tube .This black liquid is called tar.Usually methanol and acetic acid is produced which mix with water in the second tube.Residue left in the first tube is charcoal.\n\n\nBoiling point of methanol is abt 65 degree celcius and boiling point of acetic acid is 118 degree celcius. Acetic acid is a high boiling liquid then methanol. On the other hand, water has a boiling point of 100 degree celcius.Now apply fractional distillation to separate the three. For fractional distillation visit:\nhttp://en.wikipedia.org/wiki/Fractional_distillation
1043394
Of course you must specify whether you want the thermodynamic properties of water (or chewing gum?).  Good luck.
548580
Have a look at the Flavour and Extract Manufacturers Association, web page.\n\nhttp://www.femaflavor.org/index.html
245409
You could contact your local EPA office.
936366
Right here : http://www.cement-process.com/simulator.htm\nor\ntry the TMT Kiln Simulator from http://www.udgroup.com/industries/lime_x.html
774136
http://www.fike.com/products_overview_products.html\nhttp://www.ansul.com\n\nIf I knew even more specifics about the application, I could make a recommendation.  (Tank Farm?  Holding area?  Process Area?  Tanker Filling Station?)
925700
Try www.acdlabs.com\n\nAlso check out JMol.
727216
use beers law to figure out the concentration and then take that to mole ratio
203010
Simulation software is available for many types of engineering.  \n\nASPEN and HYSIM are good for chemical processes.\n\nFEA (Finite Elemental Analysis) is used to simulate effects on objects by breaking down the problem into small simple blocks.  \n\nCatia and Unigraphics are programs that are used to model 3D parts and objects which can be used to create assemblies and evaluate them with additional add-on software.\n\nI'm sure thats only a small sample of what's available.. truth is, there are many simulations and with advancements today, it is very difficult to find any one simulation that is general enough to cover all applications.