Beside the bromine test what are the other test for alkanes?
81025
alkaline potassium permanganate test
1172979
Lead II Nitride\n\nCa(BrO2)2
23146
If you know the compounds you tested you could always try a MSDS (Material saftey data sheet). This will tell you the lethal dose of the chemicals but you must be more specific than oil and grease. There are many different forms of petroleum and hydrocarbons.
319095
An alcohol could give a positive iodoform test after it has been oxidised to a methyl ketone. This of course implies that the OH group is on the 2nd carbon atom. I trust that you can work out the rest for yourself.
398750
If it is a 2 panel, 3 panel, 5 panel or 10 panel urine test then no they are not testing for alcohol.  If they swab your cheek, yes...this is called an Alco test.  If they do a blood test the answer is also yes.\n\nhttp://www.onsitedrugtesting.com/drugtest/multidrug.htm\n\nHope this helps!
205915
By methods I presume you mean analytical tools, by which these are: electrophoresis, spectrophotometers, chromatography, gas photometers...i cant think of anymore
718831
Try chemdex.\n\nhttp://www.chemdex.org/
912496
Actually, the Baeyer's reagent is alkaline KMNO4 . Firstly,\nreact the unsaturated hydrocarbon with alkaline KMnO4. Then, decolourization of KMNO4 occurs , this shows that the hydrocarbon is unsaturated. \n             This is given by alkenes and alkynes.\nTHe basis of this test is the strong oxidising action of KMNO4 in alkaline medium .
140226
ethanol and oil\nwater and chloroform
858619
The easiest way to approach problems like these, my friend, is to look at your alkyl halide first and then look at your nucleophile or base.\n\nT-butyl bromide is a tertiary halide.  Tertiary halides undergo E1 and SN1 reactions because of their ability to form a stable carbocation intermediate.  If you recall, tertiary carbocations are more stable than primary and secondary.\n\nYour -OCH3 is a strong base known as methoxide, the conjugate base of methanol.  Strong bases favor elimination reactions and thus the elimination product is your answer.
1127301
I leave the H's:\nC-C-C-C-O butanol-2\nC-C-CO-C  butanol-2\nC-O-C-C-C propyloxy methane\nnot shown: isopropyloxy methane\nC-C-O-C-C ethoxy ethane
100081
Litmus tests for acidity are probably the most well-known, but there are lots and lots of them. The Encyclopaedia Britannica article below is pretty thorough.\n\nGood luck.
198798
Liebermann-Burchard test\nA colourimetric test for unsaturated sterols, notably cholesterol; a blue-green colour develops when such substances are added to acetic anhydride and sulfuric acid in chloroform.\n\nFor the Liebermann-Burchard test for cholesterol, students put 10 drops of the above solutions of cholesterol, coconut oil, or lard in separate dry test tubes and add 3 drops of acetic anhydride and one drop of concentrated sulfuric acid. Formation of a green or green-blue color after a few minutes is positive. Ideally, the cholesterol solution gives a nice reaction, the coconut oil should show no significant color change, and the lard gives a weak reaction. The results for this test have been variable over the past few years. For example, coconut oil sometimes gives a green color, and unsaturated oils invariably do, whereas lard often gives a brown color.  I think the variabilities have been due to using old solutions; they should be made fresh with reasonably fresh samples, which is fairly inconvenient.
1015522
Primarily volatility.  The shorter the alkane chain, the more volatile the compound.  Think of it as a distillation of a very complex mixture.  Isomerization of alkanes with similar volatilities is why petroleum "fractions" like gasoline will contain many different compounds.
931837
20) B.  CH4\n24) C.  nonpolar with difference between 0 and 1.7\n25) B. pentane (more carbons to branch)\n27) C. H and Br\n28) C. 5 pairs - 3 between carbons and one on each end between carbon and hydrogen\n29) B. nylon
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
798103
It means that there are no reducing groups in the compund which you are testing. Precisely speaking there are no compounds which have aldehydic group in them. This test is mostly used to check for the presence of reducing sugars especially the Glucose content in urine. The glucose is one example of reducing sugar.