Why does steam form when you shower?
The water doesn't reach 100°C. Am I making a mistake? Or is the water not a gas at all, but rather just tiny droplets like clouds?
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What you see is air-condensed water, i.e. smallest water droplets (also fog or steam).
This arises because the shower water is significantly warmer than the other air in the bathroom. Part of the water dissolves in the (warm) air in the shower cabin and thus increases its humidity. The air rises, mixes with the other air.
This increases the relative humidity. At some point the dew point is reached. The air is maximally saturated and, upon further cooling, the water dissolved in the air falls out of the air as just these tiny water droplets (condensed).
Not necessarily, but you want to go out to the right end. It would be better to say here that simply the steam pressure of water increases with the temperature.
It is true that shower water is not always warmer than the air in the bathroom. But then there is no condensation.
Of course, I could have tried the term steam pressure. Would have been more professional, but perhaps exceeds the understanding of the FS.
I therefore referred to the absolute because it is invariant to the temperature.
Of course, the condensation and evaporation can best be described with the relative humidity.
However, as the temperature changes here, I felt the indication with absolute humidity as more direct.
No thing, I also understood your comment as a corresponding supplement/clearance.
Then I have to add something:
It is rather untypical to refer to the absolute humidity, since usually only the relative humidity is known (because it is easier to measure). Whether condensation takes place or does not therefore primarily depend on the relative humidity and temperature in the state 1 and the temperature in the state 2, since it results from whether the dew point is below or not. In this connection, reference is also made to the h-x diagram or moiller diagram. There is often also a scale of absolute humidity, which is very useful in the case of condensation in order to determine the amount of condensate.
Sure is more complicated but sounds in your answer as if evaporation in itself could only take place if the water is warmer than the air, which is not the case.
Likewise, of course, the condensation does not necessarily have to take place, just how much the absolute humidity is raised by evaporation.
With my comment only wanted to prevent a misunderstanding.
Water also evaporates at -150°. This is how freeze drying works. The question of whether you see the steam is a question of the temperature difference between the steam and the environment.
Water vapor always from small droplets. The question is when they are big enough to see them.
Each liquid has a so-called vapor pressure even at temperatures below boiling point. The water is much lower at 20° C. than for example cleaning alcohol – which evaporates faster. At 40° C., the water also rises.
It is always a very small proportion of water in the atmosphere, gaseous or liquid. Therefore there is climate, clouds, rain, snow.
Humidity says how much % of the physically possible air has already taken up – nothing evaporates only at 100%. Therefore, in summer water already evaporates from puddles and not only at 100°C. Or forms at night.
When the temperature rises – or the pressure drops, the steam pressure rises at some point over ambient pressure and the liquid begins to boil. A rule of thumb: the steam pressure doubles all 12 °C. At higher pressure water cooks later. Like in pressure cookers. At less pressure earlier, as in the high mountains.
The fog you see is just air that is cooled and then oversaturated. The LF rises to over 100% and forms the finest droplets.
This is what the steam pressure curve looks like. Note the intersection at 100° C. and 1000 hPa (1 bar).
The question was 5 years ago.
Water needed at normal pressure was 100 degrees Celsius for cooking, but can also pass into the gaseous state at much lower temperatures. Although the water cannot boil due to the impregnation pressure, it can evaporate according to its equilibrium pressure until the water content in the surrounding air corresponds to the pressure which allows water to boil at the respective temperature. Only when the partial pressure of the water in the air corresponds to the steam pressure in equilibrium does this stop.
Now you smell hot. The air around dicjbeewärmt and water evaporates (the steam pressure is high), then this feucjtwsrme air mixes with older air, the steam pressure that the air can hold decreases faster than the air volume rises through mixing. Voila, fog.
100 degrees Celsius is just the boiling point, so the point begins to boil from the water. Evaporating/evaporating, it basically does from the point where it becomes liquid.
Water Evaporates even at lower temperatures than 100 degrees
The water is warmer than the ambient temperature – then steam is created!
Exhaled or sweated outside in winter?