Why would yeast not produce ethyl alcohol in a maltose medium?
109626
the production of alcohol is an anoxic reaction, if oxygen is present alcohol isn't produced. This is usually achieved by putting the fermentation mixture in a sealed flask with a water stopper in the top, this allows the escape of CO2 produced in the fermentation but doesn't allow O2 in the air to dissolve in the water
47084
The yeast would pretty much eat the sugar until they died from the high concentration of alcohol surrounding them. Tha alcohol is their waste product.
813208
Isopropyl alcohol does not occur naturally.\nIt is produced from propene by indirect hydration in a\ncomplex process known as "strong-acid process", or by\ndirect catalytic reduction of acetone.
930110
Well, for starters, Temp is important for the catalytic effect, a low temp will slow the reaction, while too high a temp will kill the yeast.  Sugar is the food source for the yeast, so if there is not enough, the yeast wont divide as much.  Water is important of course to provide a comfortable anaerobic environment. Hope that helps you some.
768548
Anaerobic respiration occurs without oxygen.  In yeast, it produces carbon dioxide and alcohol, in humans, it produces lactic acid and carbon dioxide.
222646
because yeast is heavier than beer and lighter than water.
16727
Ethanol is ethyl alcohol, the pharmacologically active part of beer.  It depends on the "proof" of the alcohol.  Pure alcohol is generally not "edible" (or drinkable) because ethanol forms an azeotrope (a mixture that cannot be separated by distillation) when it is ~95% ethanol and 5% water.  The azeotrope is broken by chemicals that are bad for humans, like benzene.
964456
d, because the Krebs cycle is the next step in energy generation (when oxygen is present). (a) is incorrect, because lactic acid fermentation occurs when there is no oxygen. (b) is incorrect, because alcoholic fermentation is also anaerobic, and occurs mainly in yeast. (c) is incorrect, because photosynthesis does not require oxygen to occur.
780804
Yeast can grow on all sorts of agar plates.  They don't need fancy cell culture conditions like mammallian cell lines do.\n\nhttp://www.midsci.com/docs/qbio/ChapterPDF/EU_04.pdf#search='media%20for%20yeast%20growth'  those guys sell some yeast growth media.  \n\nA kind I've used before is SAB (per liter: 40g glucose/10g peptone/5g agar).\n\nI would go with agar plates instead of liquid culture because it will be easier to insure uniform exposure.  The yeast should also remain viable for longer on plates than in liquid culture. \n\nThis sounds like a clever idea for an experiment, good luck.
282426
If we're talking about bacteria, this sounds like the lac operon.  The absence of lactose causes a repressor protein to halt production of beta-galactosidase.  When lactose is present, the machinery to produce beta-galactosidase is released from repression.  This makes sense, since the presence of lactose dictates the need for catabolic enzymes to metabolize the lactose.\n\nSearch for information on the lac operon for plenty of information, it's a very well-elucidated mechanism.
715535
Yeast is an organism that metabolizes sugar much the same way you do and produces carbon dioxide.  This carbon dioxide forms bubbles in liquids or dough.  A yeast colony will typically deplete its growth medium of oxygen, (as in the case of bread making or beer making) and use an organic terminal electron acceptor producing alcohol.
139601
This is an esterification, \nButanoic Acid (CH3CH2CH2CO2H)+ ethanol (HO-CH2CH3), in basic media, yields ethyl butyrate. \n\nCH3CH2CH2CO2H + HO-CH2CH3 --> CH3CH2CH2COO-CH2CH3
741444
Fermentation is the process sugar is converted to alcohol by yeast.    Root beer is non-alcoholic, so there is no fermentation happening.
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
285773
A still works by taking advantage of the different boiling points for various liquids. For instance, alcohol boils at a lower temperature than water; therefore, you can heat a mixture of alcohol and water and the alcohol will tend to boil first. If you then condense the alcohol vapors, you have made a separation.\n\nThis is an over simplification because even with the alcohol as it vaporizes, some of the water also vaporizes. To make a purer product, you must repeat the process many times. A special column called a fractional distillation column permits you to make a nearly perfect separation
861968
most likely a starch molcule, which is just a simple polymer of glucose, if the enzymes from the yeast extract were intact.
1144782
You can't have a metal alkoxide. Well, you can, but you can't. \n\nEthanol is an alcohol, and has CH3CH2OH. If a reactive metal such as cesium is mixed with it, the hydroxide ion breaks to form hydrogen gas.\n\n2CH3CH2OH (l) + Cs (s)  --> CH3CH2O- (aq) + Cs+ (aq) + H2 (g)\n\nAlkoxide is the conjugate base of the alcohol, hence CH3CH2O-