How can water be liquid state at 212 degrees F,  and also be steam at same temperature. How can this be?
363447
this re minds me of a kind of heat called latent heat.this is the heat a subtance requires to change it state without changing it temperature,so water changes from liquid to steam at the same temperatutre if it assumes it latent heat of vapourization.thus water could be liquid at 100*c and also steam at the same temperature.
412906
To turn liquid water into steam the weak bonds between the molecules have to be broken and the molecules accelerated enough to leave the water surface and become vapour. This requires energy supplied by heating. \n\nNow add salt.\n\nThe salt consists of NaCl crystals. In water these dissolve into Na+ and Cl- ions. These ions will become surrounded by water molecules that are attracted to them, forming large clumps of molecules. To break these bonds requires more energy than in the case where the salt was absent.\n\nWe have to supply this extra energy and the result is boiling at a higher temperature.
27210
im not sure of the exact curve.  but i know you have take in account the heat of fusion (the energy it takes to convert ice to liquid water, where the temperature stays the same, 0 degrees celsius, even though energy is being added)  and the heat of vaporization (the energy it takes to convert liquid water into steam, where the temperature remains the same, 100 degrees celsius, even though energy is being added)
294759
211 would be the hottest as water boils at 212 degrees.
403230
It takes quite a lot of energy for water to change phase.  Steam actually contains much more energy than does boiling water, therefore it burns far worse when it comes in contact with human skin.\n\nSee the link below.  You can actually do the math to confirm this -- it takes 100 cal/gm to heat water from 0 to 100 degrees C, but 539 cal/gm to change that water into steam.  So ten grams of water at 0 degrees C absorbs 1000 calories to boil but nearly 6400 calories to turn completely into steam.\n\nThat's a lot of heat.\n\nIn rebuttal to some of the other answers, burns are caused (I believe) by heat convection -- that is, the hot substance in direct contact with the skin, transferring its heat to the skin cells and damaging or destroying them.  Water is more likely to stay in contact with the skin than steam is, because steam is a gas that rises away from the skin.  This is why some people seem to erroneously believe that steam doesn't burn.\n\nHowever if skin comes into continuous contact with steam, it will burn, and quite badly.
264462
Because steam is hotter than boiling water.
620300
Anything can exist in two phases at its freezing point or its boiling point or at its sublimation point.\nWater, however, is special beacuse it can exist in not just two but in three phases. This happens at a temperature called, "Triple Point of Water". This happens when the curve denoting the solid state of water, in the PV diagram, intersects the curve denoting liquid state of water in the PV diagram.
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
870952
To answer this Question you need to use the Conservation of Energy Law.   This takes its simplest form in the idea that:\n\nHeat Lost by the Steam    =   Heat Gained by the cold water\n\nYou will need to say:\nLet L be the unknown Quantity and form an Equation:\n\nHeat Lost by the Steam:\nThe steam (one assumes at 100Celsius) condenses to water at 100Celsius.  In doing this it gives up its Latent Heat of Vaporization (mL)   The water it forms is then cooled to the final temperature giving up this Internal Energy to the System.  The Internal Energy(Heat) gained is given by m.s.dT where dT is the change in temperature.\nNote that we have two  Energies to Add Together here.\n\n\nHeat Gained by the cold water:\nThe Internal Energy(Heat) gained is given by m.s.dt where dt is the change in temperature.\nBoth the cold water and the Calorimeter are heated from their starting temperature(15C) to the final temperature(70.6C)\nNote that we have two  Energies to Add Together here.\n\nNow write down the equation:\nHeat Lost by the Steam (steam + hot water)     =   Heat Gained by the cold water (cold water + calorimeter)\n              \nm1.L + m1.s.dT  =  m2.s2.dt + m3.s3.dt\nAnd solve for the Unknown L
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.
1040977
It is done with steam. Just simple steam that you might get from a tea kettle. It doesn't have to be under pressure or any hotter than 212 deg F.
247914
since the steam is coming from the inside of the water,\nI beleive it is an endothermic.  Endothermic means the \nheat comes from inside the object, and exothermic means\nfrom outside sources.  I think steam is a product of heat and water, but mainly water because the heated object is the water.  The heating element is being produced oustide the water, but the water itself is what is producing the steam.  (if you see above, "water" is stacked on top 3X)
282772
Like all elements, its physical state depends on temperature and pressure. It is a liquid at room temperature, but can be frozen and evaporated at extreems.\n\nIt freezes at -38.83 °C, -37.89 °F\nIt boils at 356.73 °C, 674.11 °F
227906
Put water under a vacuum. It will boil at room temperature. \n\nOr do you just want to create the illusion of steam? You could put dry ice in water. Then it will be could and appear to be steaming and boiling. And many people will think it is steaming.
1163335
Wrong. There is the critical temperature/pressure up to which gas and liquid behave differently. Above these conditions, there cannot exist a liquid phase. Rather than speaking about gaseous phase, this state is called fluid. This state is also called supra-critical.\n\nBasically what happens is that the attractive forces in the liquid diminish as the critical point is approached, until the liquid behaves just like the vapour. The evaporation heat becomes zero.
461446
I found that cold water (38 degrees Fahrenheit) froze faster than hot water out of the tap (125 degrees F). I chose these two temperatures because (1) they were pretty much what the average amateur ice-cube maker would have readily available and (2) I couldn't find a mercury thermometer that went higher than 125 degrees.\n\nJearl, who is not afflicted with penny-pinching editors like some of the rest of us, was able to get his mitts on a thermocouple that could measure as high as the boiling point, 212 degrees F. He found that water heated to, say, 195 degrees would freeze three to ten minutes faster than water at 140-175 degrees. (There were differences depending on how much water was used, where the thermocouple was placed, and so on.) \n\nJearl suggested that the most likely explanation for this was evaporation: when water cools down from near boiling to the freezing point, as much as 16 percent evaporates away, compared to 7 percent for water at 160 degrees. The smaller the amount of water, of course, the faster it freezes. \n\nIn addition, the water vapor carries away a certain amount of heat. To test this theory, Jearl covered his lab beaker with Saran Wrap to prevent water vapor from escaping. The freezing rate difference was greatly diminished. Conceivably convection (motion within the water) also plays a role.\n\nFascinating as all this no doubt is, all it basically proves is that very hot water freezes more slowly than very VERY hot water. The ordinary fumbler in the fridge, on the other hand, is dealing with temps more like the ones I was measuring, in which case cold freezes faster than hot. I rest my case.
109177
i believe its because the boiling point of water is only 212 at normal atmospheric pressure, so if the pressure is changed the boiling point does too.