can ne one tell me the boiling pt of benzene???
927086
The boiling point of Benzene is 80.1 degrees C
718187
The formula for the increase in the boiling point caused by the addition of a solute is:\n\n delta-T = i * K * m\n\nwhere \n\ndelta-T is the change in boiling point temperature\n\ni is the so-called van 't Hoff factor, which is accounts for the possible dissociation of the solute.  For solutes that don't dissociate, like sugar, i = 1.\n\nK is a constant (the "molal boiling point elevation constant) that depends only on the identity of the solvent, and for water is equal to 0.52°C·kg/mol = 0.52°C/molal \n\nm is the concentration of solute in moles/kg solvent (concentration in molal)\n\n\nRearranging and plugging in your numbers:\n\n  m = (104 - 100 C)/(0.52 C/molal)*1 = 4 C/0.52 C/molal\n  m = 7.692 molal
1049433
http://genchem.chem.wisc.edu/sstutorial/FunChem.htm
946245
Here you are (nice circles and atoms and stuff):\n\nhttp://www.uwgb.edu/dutchs/PETROLGY/ScaleAtomsCsRn.HTM
782646
Titanium melting point = 1675 C, boiling point = 3260C, so at NPT it is a metal, and will be insoluble in anything other than dilute acid (CRC, physical constants of inorganic compounds).
519677
Simple\nFirst Benzene is reacted with AlCl3 and chloroethane, performing the Friedel Crafts reaction.\nThen secondly, now youll be having a compound toluene (methyl benzene). Now start oxidsing it with say Potassium dichromate (any oxidising agent),toluene is oxidised to Benzyl alcohol (Ph-CH2OH), which is further oxidised to benzaldehyde(Ph-CHO), which can be further oxidised to Ph-COOH)----- Ph stands for phenyl group\n\nPlease make it the best answer
978594
Acetone       2.13kJ/kg K or  0.51  btu/lb F\nWater, fresh 4.19kJ/kg K or  1.0   btu/lb F\n\nsee also http://www.engineeringtoolbox.com/specific-heat-fluids-d_151.html
363084
Actually the answer is Tungsten.  Rhenium is close, boiling at 5627c (9,668.93 degrees Fahrenheit), but the king of boiling points is still Tungsten at 5660c (10,220 degrees Fahrenheit)\n\nThere could be others, but many elements don't really stick around long enough for us to test their boiling point.
783365
Use the gibbs free energy equation G=H-TS.  If you yous the boiling point as T, the system is at equilibrium at that point and G=0.  Dont forget to change T into Kalvin.
512153
The mean van der Waals diameter of water has been reported as identical with that of isoelectronic neon (2.82 Å) [112]. Molecular model values and intermediate peak radial distribution data indicates however that it is somewhat greater (~3.2Å). The molecule is clearly not spherical, however, with about a ±5% variation in van der Waals diameter dependent on the axis chosen; approximately tetrahedrally placed slight indentations being apparent opposite the (putative) electron pairs.
242072
Mol of benzene is 6.50 g/(78 g/mol) = 0.083 mol. Consequently, a solution of 6.50g of benzene is 160g of CHCl3 is 0.083 mol/0.160 kg or 0.520 molal. The freezing point lowering is thus ΔT = Kfpm, or ΔT = (4.60 °C/m)(0.520 m) = 2.43 °C, and the freezing point is -63.5 °C - 2.43 °C = -65.9 °C.\n\nI'm sure this helps,\nUltimeaciax
1187079
Boiling point depends on the strength of the intermolecular forces. Following is the list of them all with their strength and when they occur. \nnetwork covalent (strongest) with only diamond or SiO2\nIonic (ionic compound, 2nd strongest) like Na-Cl etc. Gets stronger with smaller sizes. \nHydrogen bonding (N, O, F with H) 3 rd strongest. \nDipole dipole (when there is a polar molecule) 4 th strongest, gets stronger with more polarity. \nLondon dispersion weakest. Stronger with more mass. \n\na NH3of the first two. Because NH3 has hydrogen bonding (only if you have N, O, or F with hydrogen) while PH3 has regular dipole dipole (based on polarity), which is weaker than NH3. \nNow in this one its c because if you draw their Lewis diagrams out c molecule has on O----H bond while d doesn't. That hydrogen bond is strong enough to make c stronger. As other than that they only have London dispersion force, (which are found in non polar molecules, and they get stronger as atomic mass gets higher). \ne and f both have the London dispersion force that I talked about earlier cause they both are non polar. So f has greater mass so f has higher boiling point. \ng because HCl has polarity (dipole dipole forces) which are stronger than F2 which is non polar and has London dispersion forces (they are the weakest).
644051
See if this article has a diagram\n\nhttp://jchemed.chem.wisc.edu/Journal/Issues/1999/Apr/abs542.html
39906
Liquid nitrgen absorbs heat as it boils away. Its boiling temperature at normal atmospheric pressure is about -270 deg F. Almost all mechanical refrigeration uses a boiling substance (refrigerant) to absorb heat. \n\nREK Mechanical engineer
539607
This is a 2 part question.  You have to figure the amount of heat to raise the temp of the ethanol then find out how much heat to boil.\n\nHeat energy = mass x change in temp x specific heat  \nHeat energy = mass x heat of vaporization\n\nHeat energy = 21 x (76.29-11) x 2.44\nHeat energy = 21 x 38.56\n\nFind those two values and then add them together.
598319
http://www.sbuniv.edu/~ggray/CHE3345/chp14.html\nhttp://web.odu.edu/sci/tisenhou/chem321/chap12/index.htm\n\nbest luck
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.