Does water escape a solution when the temperature is close to 100 degrees Celsius?
In: Chemistry
To warm water, you must put energy into it. Similarly, when water is at 100°C, you must put more energy into it for it to turn into a gas. Water vapor and water can both exist at the same temperature (boiling point) but energy must be either put into or taken out of the water/vapor in order to transform it to the other.
Boiling happens when the amount of pressure in the water is greater than the forces keeping it together (atmospheric pressure). So at sea level and standard pressure the boiling point is 100 C or 212F. The forces are in favor of the atmosphering pressure holds it together normally.
At temperatures above those values the water has greater pressure inside it and it boils by overcoming air pressure.
However, under lower pressure the water will boil at lower temperatures.
Here is something interesting
[https://www.youtube.com/watch?v=glLPMXq6yc0](https://www.youtube.com/watch?v=glLPMXq6yc0)
At 100 deg C there is so much energy in the water that the molecules separate and go from liquid to gas.
At zero deg C there is so little energy in the water that the molecules slow down and get close together, so close they can’t slide across each other, and this is ice.
Water is not a solution. It can be a solute, with other molecules dissolved in it.
The three classical states of matter – solid, liquid, gas – are determined by two classes of forces:
* the force(s) pushing the molecules apart
* the force(s) holding them together
When the latter is *much* stronger, the molecules can barely move at all, producing a solid.
When the latter is *a little* stronger, the molecules can slip and slide over each other and rearrange, but usually still stick together, producing a liquid.
When the latter *is sufficiently weaker*, the molecules freely separate, forming a gas. (The fourth state of matter, plasma, has an ambiguous distinction from gas that depends who you ask.)
Not all substances display all three states. “Dry ice” (CO2), for instance, sublimes directly from a solid to a gas, skipping the liquid state.
The boiling, freezing, etc. temperature of water or any other substance are not static because boiling, freezing, etc. also depends on pressure. Furthermore, impurities in water have their own boiling or freezing temperatures which will affect the water+impurities as a single whole.
Water is also known to *evaporate* when under boiling temperature. This is, effectively, the boiling only of the very surface-most molecules of water, which immediately escape and become vapor in the air while the rest of the water stays the same temperature or even cools down. Evaporation cannot occur if the air is too humid to accept any more vapor particles. There is actually a very, very thin layer between the liquid and the air where water vapor is just sitting there (the Knudsen layer).
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