wat is the boiling point of ether???
963281
Ether boils at 34.6 deg C\n\nGeneral\nSynonyms: ether, ethyl ether, ethoxyethane, 1,1'-oxybis ethane, diethyl oxide, aether, ethyl oxide, aether, anesthetic ether, rcra waste number U117, solvent ether \nMolecular formula: C4H10O \nCAS No: 60-29-7 \nEC No: 200-467-2 \nAnnex I Index No: 603-022-00-4 \n\nPhysical data\nAppearance: colourless liquid \nMelting point: -116 C \nBoiling point: 34.6 C \nSpecific gravity: 0.71 \nVapour pressure: 400 mm Hg at 18 C \nFlash point: -40 C \nExplosion limits: 1.7% - 48% \nAutoignition temperature: 170 C \nWater solubility: 6.9% (20 C)
744693
Any time you dissolve something in water, the boiling point of the water increases just a little bit.  The actual boiling point depends on the concentration of the substance you dissolve.  You can calculate the actual boiling point if you know the molality of ions produced from the baking soda.  If you do a web search for "boiling point elevation" you find more specific information.
807315
Methanal is a gas (boiling point -21°C), and ethanal has a boiling point of +21°C. That means that ethanal boils at close to room temperature.\n\nThe other aldehydes and the ketones are liquids, with boiling points rising as the molecules get bigger.\n\nThe size of the boiling point is governed by the strengths of the intermolecular forces.\n\nThe aldehyde (with dipole-dipole attractions as well as dispersion forces) has a boiling point higher than the similarly sized alkane which only has dispersion forces. However, the aldehyde's boiling point isn't as high as the alcohol's. In the alcohol, there is hydrogen bonding as well as the other two kinds of intermolecular attraction:\n\nmolecule      type      boiling point (°C)\nCH3CH2CH3alkane       -42\nCH3CHO           aldehyde+21\nCH3CH2OHalcohol        +78
760384
Everything has a melting point and a boiling point.  In the case of water, the melting point is 0 C and the boiling point is 100 C.  In argon, as you have pointed out, the melting point is much, much lower, whereas for something like iron, it is 1535 C.  Neither of these temperatures occur normally on Earth's surface.  That's why you don't see puddles of argon lying around on the street, or clouds of iron vapor floating in the air:)
131196
The melting point is 1068 kelvin and 795 celsius. The boiling point is 3633 kelvin and 3360 celsius.
857462
log10(P) = A − (B / (T + C))\n    P = vapor pressure (bar)\n    T = temperature (K)\n\nAntoine Equation Parameters\nTo get the References, go to the website below, search by compound name using Phase Change checkmarked, hyperlink to complete journal reference\n\nEthane: (two sets for two temperature ranges)\nTemperature (K) 91.33 - 144.13\nA  4.50706\nB  791.300\nC  -6.422\nReference: Carruth and Kobayashi, 1973\n\nTemperature (K) 135.74 - 199.91\nA  3.93835\nB  659.739\nC  -16.719\nReference: Loomis and Walters, 1926\n\n\nEthylene:\n\nTemperature (K) 149.37 - 188.57\nA  3.87261\nB  584.146\nC  -18.307\nReference: Michels and Wassenaar, 1950
929951
Because you have to know which is the top and which is the bottom layer. \n\nFor example, if you're using diethyl ether to extract something from water, the density of water is 1.00g/mL and of ether 0.71g/mL. So if you shake up a mixture of water and ether, the water will settle to the bottom and the ether will collect on top. You open a stopcock ("faucet") on the bottom of your vessel and let the water drain out and stop before the ether goes. \n\nIf you're using chloroform to extract from waster, the density of chloroform, is 1.48. So after shaking, it's the chloroform that winds up on the bottom.\n\nThe other solvent should not be too close to 1.00g/mL, because you'll get a liquid mush that doesn't separate into layers.
998521
that is wrong!!!!\nthe values should have been the other way round!\nnow look:since ethane is a parafin we cannot discuss its prop\ncome to acetone. the central carbon is double bonded to an oxygen atom\nnow when an electrophile comes to this oxygen the bond attains polar character wth the oxygen having partial negative charge(grearter electronegativity), and the carbon having partial positive charge\nnow obviously the electrophile will go towards this oxygen atom, showin its basic character\nlook at the other way(the one described above)\nwhen the oxygen atom reduces the electron cloud density, the carbon atom is more strogly attached to the hydrogens which means that it cannot be released easily which once agains shows its basic character\nhence the values should have been the othr way round
859471
1) determine the mass of carbon, hydrogen and oxygen.\ncarbon: 9.630 g x (12 / 44) = 2.626 g\nhydrogen: 4.928 g x (2 / 18) = 0.548 g\noxygen: 4.055 - 2.626 - .548 = 0.881 g\n\n2) convert to moles.\ncarbon: 2.626 / 12 = 0.219 mol\nhydrogen: 0.548 / 1 = 0.548 mol\noxygen: 0.881 / 16 = 0.0551 mol\n\n3) divide each molar amount by the lowest value to obtain small integers\ncarbon: 0.219 / 0.0551 = 4\nhydrogen: 0.548  / 0.0551 = 10\noxygen: 0.0551 / 0.0551 = 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
209192
Boiling Point: \n204C (399F) \nMelting Point: \n100C (212F) \n\nCHECK IT OUT BUT I THINK ITS CORRECT
822453
The boiling point series for short alcohols is dominated by hydrogen bonding.  That's where the H on the hydroxyl group (OH)  on one molecule is attracted to the O on a nearby molecule.\nEven tough "normal alcohol" (I imagine you mean n-butanol from the context of your question) is just as heavy, it will have a higher boiling point because its structure makes hydrogen bonding easier.  It is basically alike to a bunch of strings with the magnets on their ends with nothing to impede the other strings from glomming on.\nTert-butanol, on the other hand, is like a bunch of knotted strings with magnets at the base of the knot.  The hydroxyl group on these molecules are not all that available for their neighboring molecules to find and be attracted to.  This is called "steric hinderance" and is more a physical and spatial consideration than a chemical phenomenon.
172281
The first answer is correct. Here is a page to help you figure out the altitude. You punch in the elevation and it will tell you the boiling point.
941271
KCl will have higher boiling point because its bond is polar.This can arise the posiibility of dipole-dipole interaction.Main factor which is determines boiling point is intermolecular forces.
969783
1) determine the mass of carbon, hydrogen and oxygen.\ncarbon: 6.406 g x (12 / 44) = 1.747 g\nhydrogen: 5.244 g x (2 / 18) = 0.583 g\noxygen: 4.664 - 1.747 - .583 = 2.334 g\n\n2) convert to moles.\ncarbon: 1.747 / 12 = 0.146 mol\nhydrogen: 0.583 / 1 = 0.583 mol\noxygen: 2.334 / 16 = 0.146 mol\n\n3) divide each molar amount by the lowest value\ncarbon: 0.146 / 0.146 = 1\nhydrogen: 0.583 / 0.146 = 4\noxygen: 0.146 / 0.146 = 1\n\nWe have now arrived at the answer: the empirical formula of the substance is CH4O.\nThe atomic masses add up to 32, which is also the molar mass of the compound.
501588
Ether, or diethyl ether as it is more correctly called is made by combining ethanol molecules with each other on a catalyst so that ether and water is formed as the product. 2Ethanol + heat + catalyst = 1 diethyl ether + 1 H2O
975732
Substance: Water\nLatent Heat Melting J/g:  335\nMelting Temp°C: 0\nLatent Heat Boiling J/g:  2272\nBoiling Temp °C: 100 \nHeat of vaporization (kJ/mol): 40.65
123942
The normal boiling point is, of course 100 degrees Celcius at standard pressure at sea level (760 torr). \n\nHowever, boiling point depends on several factors:\n\n1. What is the pressure? At higher altitudes, water boils at lower temperatures.\n\n2. Is it pure water, or water containing dissolved materials and other impurities? For example, dissolved salt can raise the boiling temperature by a few degrees.  \n\n3. Water can be superheated, in a microwave, and be above its normal boiling point without boiling. People have been scalded by this.