What is the conclusion for water boiling?
97620
the conclusion is that when you heat water it will boil.\nif you donot stop it will ecoporate
666167
Good question.  I have noticed it but have never put a lot of thought into the phenomenon.  Now that you have mentioned it, I too would like to find out why.\n\nIt is not the actual boiling of the water; it occurs just prior to boiling.  I wonder if the molecules at the hottest point (just above the bottom of the pot) have gained enough energy and begin to expand into small bubbles of steam but as they rise, they loose energy to the molecules higher up and in so doing, they implode.  The resulting sound is what is heard.\n\nOr there could be some kind of resonance as many areas suddenly turn to vapour IN THE water.  Just a few thoughts.
786932
Boiling point is the temperature at which the vapor pressure of a liquid is equal to the atmospheric pressure.  Raising the temperature of a liquid increases the vapor pressure.  The higher the vapor pressure of a liquid already is, the lower the temperature required for it to boil.  Oxygen has a lower boiling point than hydrogen because it has a higher vapor pressure.  The reason for this is because there are less intermolecular forces holding oxygen together than there are intermolecular forces holding together hydrogen chloride.  In oxygen, there are weak London forces and nonpolar-covalent bonds.  In hydrogen chloride, there are London forces AND a polar-covalent bond.
860853
It justs super heats the steam defined as the heating of a fluid after reaching its boiling point. If you have more doubt on this feel free to mail me. But if the questions are seriously done.
579734
Water always evaporates. Higher temperatures will increase the evaporation rate, but water always evaporates. It has no relation with the boiling point; evaporation is a different phenomenon.\n\nExtracted from wikipedia:\n"It is a misconception that at 1 atm, water vapor only exists at 100 °C. Water molecules are in a constant state of evaporation and condensation flux near the surface of liquid water. "
496451
The correct answer is B, leave water on the bench at room temp and watch it evaporate. Boiling is the temperature at which the vapour pressure equals the atmospheric pressure.
551765
MILK BOILS OVER BE CAUSE WHEN IT APPROACHES THE BOILING POINT, IT FORMS A FILM WHICH DOES NOT LET STEAM ESCAPE. THE STEAM WILL FIND ITS OWN WAY.
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.
195177
It  isn't boiling.\n\nIt steams because it is well above the temperature of the surrounding air.\n\nWhen the air heated by the hot water in the teacup rises, and reaches the cooler room of the air, the moisture condenses.\n\nBoiling is 212 F. Room temperature might be 70 F.
780627
WATER BOIL AT:  27*C at 26.739 (pressure(torr)  thru 30*C at 31.824\n pressure(torr)
48785
Boiling Point: 444.6 °C (717.75 K, 832.28 °F)
149000
maybe like salt crystals diluted in water and then when you paint on paper with that water and let the water evaporate, the salt crystals are left behind on water. you can see it. just an idea? \nlike when water evaporates, all teh minerals in water are  left behind. so when you boil water and hold the lid above the steam, the droplets that form on the lid is pure H2O, because all teh minerals are left behind in the pot.
427695
To "boil" something means to heat it to its boiling point and (I guess ) watch bubbles form and pop.  "Boiling point" means the temperature at which a substance turns from liquid to gas (this temperature will depend on the air pressure or pressure of another gas on the liquid: no pressure means no liquid phase).\n\nWe're used to thinking of water doing this as it turns from liquid to gas, but any liquid turning into a gas at the right temp will do it. So start with liquid nitrogen, heat it, watch bubbles form.  The liquid is nitrogen in liquid phase; the bubbles are nitrogen in gas phase.  It's still just nitrogen (N2, two atoms of nitrogen stuck together to make a single molecule).  The N2 bubbles burst and the nitrogen floats away, that's all.  By the way, this happens at -170 degrees or so, as I recall, so don't touch it....hard to think of this as "boiling" temperature, but there it is......
383320
the idea isn't that water can't heat up when it boils at low pressure, but that it doesn't have to. no matter what temperature something is, its molecules are moving somewhat, and some of them escape as a gas. also, any gas always is condensing into a liquid or solid. when pressure and tempurature are constant, these processes reach equilibrium where they cancel each other out. at high temperature, more gasses escape, and at low pressure, less gases return to liquid. so at somewhat low temperature and relativly lower pressure, even though few gases relatively escape, even fewer return to liquid, so the net effect is that the liquid evaporates at low temperature. if the temperature were raised, it would boil even faster.
700946
Interesting question.  I would guess not for long, for the following reason.\n\nThe vapor pressure of liquid water at 32 F or 0 C is 0.08854 psia.  In theory, reducing the pressure above the liquid below this value will cause the water to boil.  However, the escaping steam has a much higher enthalpy than the liquid water.  It draws this heat from the liquid water surrounding the steam bubble as it is formed, thereby cooling the liquid in the process.  Since the liquid is already at the freezing point, the liquid will have to go thru a phase change to ice to supply the heat.  The heat of fusion is much less than the heat of vaporization, so before long you would have a block of ice.\n\nIf you heat the liquid container to match the heat lost in steam, you could keep a boil going, but could not use temperature as a guide since the freeze-up is isothermal.
776438
Dont know if this is relevant to your question, but I know water can boil at this temp range if pressure is reduced enough.
168436
Water boils at 212 F.  The hotter the water, the less energy is needed to achieve this temp.  Of course pressure counts too.  Higher altitudes require different amounts of energy.  I think this is Doyles law.  Chem 101 would be a good class to learn this type of thing.  Also the purity of the water makes a difference.  The less pure the water (minreals, other impurities with lessen the amount of energy needed to achieve boiling temp.