Heat of combustion of ethanol and butanol?
141403
Ethanol = -1277.1 kJ/mol\n\nButanol = -2078 kJ/mol
491547
Ethanol has a low flash point (-5 C), which is the temperature at which enough vapors in the air can be present to create an explosive atmosphere; a spark or flame can cause an explosion.  It also does burn with a weakly colored flame, making it hard to see.  \nAlso - high-strength ethanol that you can by is called denatured alcohol - there are many kinds, but they are all poisoned with something - methanol, isopropanol, toluene etc. which render it undrinkable.  Don't do it.\nPunch in "MSDS" and "ethanol" into yahoo and pull up a material safety data sheet.
1174414
The engines are designed to run on gasoline which burns a little differently and much dirtier than ethanol. ETOH burns to only CO2 and H2O, very clean. Ethanol can be made easily from any organic material. Corn stalks, wood, petroleum, potatoes, sugar, whatever you have mostly. Crack the large molecles to 2 carbons with an OH attachesd and you have ethanol. Fermentations with yeast are usually the easiest way.
496070
I would like to say yes but at this point I would have to say no. I worked at an ethanol pilot plant and anyone in the industry can tell you to break down starch in the corn you need what they call a jet cooker. This uses high pressure steam at appx 400-600F. There is no way in hell solar panels could heat water to this temperature effeciently and consistently. Plus a lot of ethanol plants run 24 hours a day and that right there pretty much shoots that plan in the ass. A good thought though. Ethanol will become more effecient once the enzyme industry catches up and can CHEAPLY use switchgrass as a fuel source.
226004
Exothermic\n\nSugar(with yeast)--->\nalcohol+carbondioxyde+heat
123146
the density of ethanol in liquid state is: 0.789 g/cm3\nim ta winnar! lol
984026
You need to find the heats of formation of each species (will come from a standard table) and use this equation to get the heat of reaction:\n\n(delta)H = sum of heat of formation of products - sum of heat of formation of reactants\n\nEach heat of formation will be multiplied by its stoichiometric ratio, and the physical state will be important (especially that of water, as the heat of formation of steam is higher than that of liquid water).  You will not find a heat of formation for oxygen gas, because by definition there is no heat of formation for an element.
324369
A thermometer is the most common method...\n\nUsually weather thermometres use alcohol rather than mercury as it is cheaper, less hazardous than mercury, and you are unlikely to measure close to or above 75 degrees celcius (which is the boiling point of ethanol).\nA thermometer works by filling a tube with the alcohol, as the temperature increases then the alcohol expands, thereby increasing in volume and rising up the tube. When the temperature decreases then the ethanol contracts and takes less space, thereby moving down the tube.\nIf you were to heat an alcohol thermometer in a fire it will burst as the ethanol expands so much as to destroy the tube.\n\nSome thermometers have small parts in them that are pushed up the tube and when the temperature drops the parts are stuck ther until you shake them... this hepls measure a maximum temperature.\n\n\n\nThere are also electronic methods, however these are often dependant on the humidity (moisture in the air) as a conductor... you may see such instruments in a sauna close to the roof.\nOther electronic thermometers are dependant on metal strips that change shape due to heat, allowing small changes in temperature to be measured. Your toaster will use something similar as a thermostat.\n\nI dont know much about the electronic types...
195015
1. No it's the methanol is a highly explosif gas.  It absorbs heat very quickly which is what makes the flame change color\n2. the whoosh sound is created by the oxygen trying to get in and the methanol trying to get out very quickly from a very small hole\n3.The jug is extremly hot because the methanol would explode if it was in contact with oxygene.  Since inside the jug, there is practicly no oxygene, it holds heat.  This is why the jug gets hot because inside it is holding heat in.\n4.  If we didnt wait for the methanol to vaporise, it would create an explosion and you would prolly die.  \n5. For a fire (explosion) to happen, you need 3 elements, heat, a burner and a burning (soryy i dunno if those are the rigth terms, i learned them in french)  The thing getting burned is always the oxygen (alone or with an organic material such as wood or paper)  Without oxygene the metanol wouldnt explode\n6.  I'm not too sure about this one, but it's probably with the moleculs.  Water is H2O and carbone dioxide is CO2.  Methanol must be a mix of those two moleculs.  Did the teahcer give you the molecular equation?\n7.  The water comes from the reaction.  You have to look at you molecular equation ( each prodoct at the beiginning and at the end)  Water is H2O  so it means that the reaction seperated moleculs from the methanol and those moleculs got paired up with some others that creat H2O. Basiclly a reaction is just moleculs getting broken and reformed with other moleculs.  Im not sure but i would guess in the methanol's moleculs, there is hydrogen (highly explosif, what creates the burning) and that hydrogen moleculs would form water with the oxygen that is burnign
423892
I'm sure that's what you're supposed to determine in the lab you're working on. Good luck.\n\nI've been able to find a value for the heat capacity of n-hexadecanol (cetyl alcohol) in my copy of _Lange's Handbook of Chemistry, 13th Edition_.  When you've come up with your value from the experiment, post it here and I'll check to see if you're close.
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
991603
one is propanol..the other that u can derive is 2-methyl ethanol...i thinks that's the iupac name..not sure about the commercial name
293861
The combustion of glucose is as follows:\n\nC6H12O6 + 6O2 --> 6CO2 + 6H2O\n\nSo, the mole ratio is 1 mol glucose per 6 mols O2.
75087
without knowing the specifics of your problem, the formula I think you're asking for is deltaH=H(products)-H(reactants). You get the H values for your products and reactants from tables, multiply them by their coefficients, add all the reactants and all the products, the subtract reactants from products.\n\nThe only other enthalpy equation I can think of is \nH=E+PV where E=energy, P=pressure, and V=volume.
1128825
rubbing alcohol - isopropyl alcohol, 2-propanol\nCH3CHOHCH3
776867
There are several possibilities.\n\nThe TEOS solubility in water is negligible.  It is not much better in methanol, but it does adhere to the ethyl group of ethanol to some degree.\n\nThe boil point of ethanol is 78.4 degrees C, which is higher than the boiling point of methanol (at 64.7 degrees).  This might be a factor.\n\nThe last has to do with the physical size and role of the alcohol as a catalyst.  Methanol is smaller and may not have the correct geometry.\n\nI totally agree with the suggestion to experiment, using the same molar quantities for methanol and ethanol.  You might also want to try n-propyl alcohol to give additional data.\n\nBy the way, chemistry being what it is, you might try searching for additional answers using an alternate name for the TEOS.  It is also called Tetraethoxysilane.
761721
Take the 125g ethanol (E), C2H6O, and multiply by 1 molE/46gE.\nThe gE cancel, leaving moles E. For the CO2 part, multiply by 2 mol CO2/1 molE. That comes from the balanced equation. The molE cancel, leaving molCO2. Next multiply by 44gCO2/1mol CO2. The molCO2 cancel, leaving gCO2. That's the first part of the problem. Next, go back to the beginning where you got molE. Multiply by 3molH2O/1molE. This also comes from the balanced equation.The molE cancel, leaving molH2O. Multiply by 18gH2O/1molH2O. The molH2O cancel, leaving the gH2O, which is the second part of the problem. At. wts. C=12, H=1, O=16, C2H6O=46