what is the difference between butadiene and benzene?
955929
butadiene is a straight chain with two double bonds while benzene is a ring structure with three alternate double bonds
809812
1.aliphatic(straight chain)\n2.aromatic(contains benzene ring)\n3.alicyclic(closed chain)
730330
Different chemical composition, one has a reaction the other doesn't..☺
430202
They have the same number of electrons and protons *relative to each other*.  \n\nFor example: carbon has 6 protons in it's nucleus, and therefore has 6 electrons to be neutral.  It's atomic number also happens to be 6 :-)
181496
Even though water is polar and benzene is nonpolar, a very small amount of each will stay suspended in the other. Dry benzene is simply benzene with all traces of water removed.
141403
Ethanol = -1277.1 kJ/mol\n\nButanol = -2078 kJ/mol
1090773
pH can be calculated for substance which can disassociates into ions(mainly H+ and OH-). Butane is a pure covalent compound and it cannot be ionised. \nFor properties please visit: http://en.wikipedia.org/wiki/Butane
947454
2,3 - butadione, or better say buta-2,3-dione
993231
Okay, first picture a benzene ring - six carbons, flat topology thanks to its aromaticity.  By definition, the benzene carbon with the carboxylic acid group attached is carbon #1.  So, you have two cases here, both with a ring substituent "para" (or directly opposite) the carboxylic acid.  Everybody on the same page?\n\nNow, acidity is defined, in simple terms, as the willingness of a molecule to give up a proton, aka an H+ ion.  The more easily it will part with that H+, the more acidic a compound is.  So, the question, really, is what makes a proton stay stuck to an acid?\n\nA carboxylic acid anion (COO-) has a large electron density delocalized between its two oxygen atoms.  A hydrogen ion will tend to stay stuck to this negatively charged group to balance out it's negative charge.  In layman's terms, a carboxylic acid is more comfortable with a positively charged bit hanging around to make all those nonbonding electrons on the oxygens less unwieldy.  \n\nWith your two compounds, the difference between them is the substituent in the 4 position.  Remember that an aromatic system like this has a flat electron cloud above and below the ring, and this electron cloud will interact directly with any ring substituents.  \n\nThe methoxy group is an electron donor.  It is not, overall, very electronegative, so it will tend to "push" its electron density into the benzene ring, and that will tend to prevent the  carboxylate group from sharing its negative charge density with the aromatic system.  With the negative charge localized to the carboxylate, it will be difficult for the hydrogen ion to dissociate, and 4-methoxybenzoic acid will be very weak.  \n\nFluorine, on the other hand, is an excellent  electron sink; it is one of the most electronegative substituents you can put on a benzene ring.  It will tend to draw electron density towards itself, allowing the carboxylate to push some of its negative charge into the aromatic ring.  The negative charge, then, will be more delocalized, making it easier for the acidic proton to dissociate from the carboxylate group.  4-fluorobenzoic acid will, therefore, be a stronger acid than 4-methoxybenzoic acid.\n\nDoes that make sense?  I hope this helps.
756535
chemical properties of benzene\nElectrophilic aromatic substitution is a general method of derivatizing benzene. Benzene is sufficiently nucleophilic that it undergoes substitution by acylium ions or alkyl carbocations to afford give substituted derivatives. \n\nThe Friedel-Crafts acylation is a specific example of electrophilic aromatic substitution. The reaction involves the acylation of benzene (or many other aromatic rings) with an acyl chloride using a strong Lewis acid catalyst such as aluminium chloride.. \n\nLike the Friedel-Crafts acylation, the Friedel-Crafts alkylation involves the alkylation of benzene (and many other aromatic rings) usng an alkyl halide in the presence of a strong Lewis acid catalyst. \n\nsulfonation. \nNitration: Benzene undergoes nitration with nitronioum ions (NO2+) as the electrophile. Thus, warming benzene with a combination of concentrated sulphuric and nitric acid gives nitrobenzene. \nHydrogenation: Benzene and derivatives convert to cyclohexane and derivatives when treated with hydrogen at high hydrogen pressures. \nBenzene is an excellent ligand in the organometallic chemistry of low-valent metals. Important examples include the sandwich and half-sandwich complexes respectively Cr(C6H6)2 and [RuCl2(C6H6)]2
927086
The boiling point of Benzene is 80.1 degrees C
771996
because they are two totally different chemicals
718672
There are essentially three types of hydrocarbons:\n\naromatic hydrocarbons, which have at least one aromatic ring \nsaturated hydrocarbons, also known as alkanes, which don't have any double, triple or aromatic bonds \nunsaturated hydrocarbons, which have one or more double or triple bonds between carbon atoms, are divided into: \nalkenes \nalkynes \nSorry I only found 3
863885
Aromatic hydrocarbons have a high electron density due to the pi cloud of electrons which exist.  They hence undergo electrophilic substitution, that is they are attacked by an electrophile.\n\nAn electrophile is an electron-loving particle, such as the positive ions and other alkyl groups (CH3, C2H5).
322532
No, water (H2O) and Gasoline [mostly Octane] (C8H18) are quite different on a molecular level,\nFor one, water has no carbon, and Octane has no Oxygen.
445656
I think it's 'gammexane' instead. It's also referred to as BHC (benzene hexachloride)\n\nEDIT: Referring to Supertramp_82's answer, hexachlorocyclohexane (HCH) as C6H6Cl6, gammexane and benzene hexachloride (BHC) are the same. Crude BHC or gammexane is a chlorinated hydrocarbon which exists in at least 5 isomeric forms - it doesn't matter which one you write, it's still the same compound.
870109
Benzene forms when ascorbic acid, the vitamin C added to many beverages, reacts with either sodium benzoate or potassium benzoate, two common preservatives that companies add to their products to prevent bacterial growth.\n\nUnfortunately I don't know about the pH but it must be very near 7 (just below) because ascorbic acid is a very weak acid and hardly ionsises to form H+.