Water evaporates at room temperature, and shows that when you wash your hands they dry after that as you wash and spread clothes to dry. Certainly the temperature will not reach 100 degrees Celsius, the question arises is there a convincing scientific explanation?
It's simple. Water molecules move at different speeds. The velocity distribution of molecules depends on temperature. This distribution is called the Maxwell Distribution (https://en.wikipedia.org/wiki/Maxwell%E2%80%93Boltzmann_distribution). At any temperature, there are molecules whose velocity is so great that they evaporate. When a liquid boils, all molecules have this velocity
Because of the vapur pressure difference of water in its liquid form and that in the air.
No problem, thank you for presenting a great discussion point!
The air circulation is the effective factor in this process since it is saturated with water through moving which dehydrates the hands or the clothes
Water evaporation starts at 4 ° C, so it evaporates at room temperature. Because evaporation differs from boiling.
This is very important fact. Thank you for your contribution Dr Ali Alhayany .
Why the atmosphere is humid it means there is presence of moisture and relative humidity is high. Hence clothes or anything will not dry.
The humidity is related with the amount of water vapours present per unit amount of the dry air. Now with increase in the humidity means that we are moving towards saturation or intake ability of molecules decreases and at saturation no more water vapours can enter. So,
Flux(N) is directly dependent on {(Ps-P),driving force}
where Ps is the vapour pressure of water at the surface and P is the partial pressure of water in the air flowing over the surface
N= kg*(Ps-P) where kg is the gas phase local mass transfer coefficient
N=kg*Ps*{1-(P/Ps)}
N=kg*Ps*(1-Relative humidity)
It implies that with increase in relative humidity rate of evaporation decreases and vice-versa
I appreciate your valuable contribution. Many thanks Ali Nasr .
The boiling point of water is 100 deg C at 1 atm. This is the temperature that liquid is in equilibrium with its gas phase. And you are right that below this temperature (at 1 atm) water should not vaporize. Imagine a close system at 1 atm and 25 degree with a SINGLE water component, you will see that water never vaporize. The water vaporization from our daily observations is an open system of water-air. If you close this system of mixture, the vaporization stops (macroscopically) at the equilibrium partial vapor pressure.
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