what is the chemical formula for gasoline?
466572
--------------------------------------------------------------------------------\n\nFirst, gasoline is not a simple chemical compound like water or ethanol. It is a mixture of hundreds of different compounds. The reason for this is that gasoline is made from crude oil. Crude oil, or petroleum, is made up of thousands of different compounds, and the exact compounds present and their relative amounts differ depending on where the petroleum is produced. (For example, oil produced in West Texas differs remarkably from oil produced in the Middle East.) After the oil is produced (or taken out of the ground via oil wells), it is shipped to an oil refinery, where it is separated into different products, including gasoline, jet fuel, and diesel fuel, among others. \n\n\nThe separation of the oil takes place in a process called distillation. (Note that there are other processes which occur in a refinery as well, but the simplification to consider just distillation is not too far off.) In distillation, the oil is heated until it starts to boil. Some of the thousands of chemical compounds that make up the oil start to boil at low temperatures, and some do not boil until the petroleum has been heated up to higher temperatures. The different products (such as gasoline) that come out of a refinery are defined by their boiling temperatures during distillation. The lightest compounds (those that boil at the lowest temperature) become aviation gasoline, the next lightest become automotive gasoline, the next lightest become lightweight solvents and so on. In order of increasing boiling point, some other categories of refinery products are jet fuel, kerosene, diesel fuel, lubricants, greases, and asphalt. Gasoline is typically made from the fraction of the crude oil that boils at temperatures between about 50 degrees Celsius and 200 degrees Celsius. \n\n\nSo, we can't say for sure exactly what compounds are present in gasoline, but we can define gasoline to some extent. First, it is made up almost entirely of hydrocarbons, which are molecules made up of carbon and hydrogen. (Some of the compounds present in gasoline also contain small amounts of other elements, including sulfur, nitrogen, oxygen, and some trace metals.) Next, those hydrocarbons which make up most of gasoline boil at temperatures between about 50 and 200 degrees Celsius (120 to 400 degrees Fahrenheit). This means that these compounds are mostly those hydrocarbons that have between 6 and 12 carbon atoms in each molecule. A good average is probably octane, which has eight carbon atoms and 18 hydrogen atoms and is written C8H18. \n\n\nsource:http://www.madsci.org/posts/archives/apr2001/987004809.Ch.r.html
842808
1) determine the mass of carbon, hydrogen and oxygen.\ncarbon: 9.847 g x (12 / 44) = 2.686 g\nhydrogen: 5.038 g x (2 / 18) = 0.560 g\noxygen: 4.146 - 2.686 - .560 = 0.900 g\n\n2) convert to moles.\ncarbon: 2.686 / 12 = 0.224 mol\nhydrogen: 0.560 / 1 = 0.560 mol\noxygen: 0.900 / 16 = 0.056 mol\n\n3) divide each molar amount by the lowest value\ncarbon: 0.224 / 0.056 = 4\nhydrogen: 0.560 / 0.056 = 10\noxygen: 0.056 / 0.056 = 1\n\nThe empirical formula of the substance is (C4H10O)n\nThe atomic masses add up to 74, which is also the molar mass of the compound. Therefore n=1 and we find C4H10O
796215
1) determine the mass of carbon, hydrogen and oxygen.\ncarbon: 9.270 g x (12 / 44) = 2.528 g\nhydrogen: 3.795 g x (2 / 18) = 0.422 g\noxygen: 3.797 - 2.528 - .422 = 0.850 g\n\n2) convert to moles.\ncarbon: 2.528 / 12 = 0.211 mol\nhydrogen: 0.422 / 1 = 0.422 mol\noxygen: 0.850 / 16 = 0.0531 mol\n\n3) divide each molar amount by the lowest value to obtain small integers\ncarbon: 0.211 / 0.0531 = 4\nhydrogen: 0.422  / 0.0531 = 8\noxygen: 0.0531 / 0.0531 = 1\n\nThe empirical formula of the substance is (C4H8O)n\nThe atomic masses add up to 72.1, which is also the molar mass of the compound. Therefore n=1 and we find C4H8O
41866
there are many chemicals formulas for pterolium, not just one. Petrolium is a mix of ALCANS like butene, propane, izobutane, etc and mercaptans (combinations of Sulf, wich give petrolium the specific smell)
851916
C:H = 85.63:14.37 (mass ratio)\n= 85.63/12.01:14.37/1.008 (molar ratio)\n= 7.13:14.26\n= 1:2\nSo the empirical formula is CH2 and its empirical molecular weight ≈ 14.03\n\nP1V1/T1 = P2V2/T2\n0.980 * 1/(273.2 + 51.5) = 1.V2/273.2 (at STP of 1 atm and 0°C)\nSo V2 = 0.980 * 273.2/324.7\n= 0.825 L\nThus 3.09 g occupies 0.824 L\nSo 3.09 * 22.4/0.825 g occupies 22.4 L at STP\nie 1 g mole = 83.9\nThus MW of this gas is 83.9\nSo number of empirical units = 83.9/14.03 ≈ 6\nSo the molecular formula is C6H12
46188
the formula is CH3CH2OH,the structural formula for ethyl alcohol. The molecular formula is C2H5OH\n\nOh sorry!the answer should be: CnH2n+1OH(general formula)
272349
Ca(s) + 2HCl(aq)-->CaCl2 + H2(g)\n\nor...\n\nCalcium Chloride and Hydrogen Gas... you know... the stuff that fuels rockets! :)
518977
85% Ethanol; OK, stay with me now.........\n\n15% of a gallon = gasoline.  1 gallon = 4 quarts\n\n15% of 4 quarts = .6 quarts = 1 pint, 6 tablespoons, 1 teaspoon\n\nSo, you would need to mix 1 pint, 6 tablespoons and 1 teaspoon of gasoline with every 3.4 quarts of ethanol
130217
Because gasoline is a solvent.\n\nChemistry.\n \n solvent- a) A substance in which another substance is dissolved, forming a solution. \nb) A substance, usually a liquid, capable of dissolving another substance.
384774
CH3CH2OH\n\nC ~ 12\nO ~ 16\nH ~ 1\n\n2*C + 1*O + 6 * H = 2*12 + 1*16 + 6*1 = 46 g/mol
373250
C3H7NO2 \n\nwww.chemfinder.com is a useful resource.  \n\nI hope this helps :)
965162
Pentane is a Highly Flammable Liquid which may form Explosive Mixtures with air.  It chemically combines with the oxygen in the atmosphere to give carbon dioxide and water:\n\nC5H12 (l) + 8O2 (g) --> 5CO2 (g) + 6H2O (g)
893330
look at this:\n\nhttp://en.wikipedia.org/wiki/Gasoline
199454
Gas is octane  is nontane m=9 n=21\nIt may not be so pure.
697475
1) determine the mass of carbon, hydrogen and oxygen.\ncarbon: 7.849 g x (12 / 44) = 2.141 g\nhydrogen: 3.213 g x (2 / 18) = 0.357 g\noxygen: 3.215 - 2.141 - .357 = 0.717 g\n\n2) convert to moles.\ncarbon: 2.141 / 12 = 0.178 mol\nhydrogen: 0.357 / 1 = 0.357 mol\noxygen: 0.717 / 16 = 0.0448 mol\n\n3) divide each molar amount by the lowest value to obtain small integers\ncarbon: 0.178 / 0.0448 = 4\nhydrogen: 0.357  / 0.0448 = 8\noxygen: 0.0448 / 0.0448 = 1\n\nThe empirical formula of the substance is (C4H8O)n\nThe atomic masses add up to 72, which is also the molar mass of the compound. Therefore n=1 and we find C4H8O
821017
(CH3)2 N2H2+2N2O4-->3N2+4H2O+2CO2
444491
http://www.faqs.org/faqs/autos/gasoline-faq/part2/preamble.html\n\nhttp://www.atsdr.cdc.gov/toxprofiles/tp72-c3.pdf\n\nhttp://www.elmhurst.edu/~chm/vchembook/514gasoline.html