To answer the above two questions more meaningfully, we need to consider condensation in more detail.
1. In liquid water, the water molecules are closely packed and kept together by the intramolecular forces of attraction. To become a gas molecule, the water molecule must overcome the attraction force and break away via the liquid-gas interface. Apparently, only the most energetic molecules can achieve that.
2. The number of such energetic molecules leaving the liquid phase per unit time grows exponentially with increasing temperature. It approximately doubles per each ten degrees of temperature increase.
3. On the other hand, those molecules that are in the gas (water vapor) can occasionally enter the liquid phase. To do so, the molecule does not need to be particularly energetic (because the molecules of gas are free to move). Therefore, the number of vapor molecules entering the liquid phase per unit time depends mostly on how many of them are around.
4. So, in equilibrium, the energetic molecules leave the liquid phase for gas and some gas molecules return to the liquid. The situation is like in a closed bottle with water. We do not see either evaporation or condensation (which are macroscopic processes).
5. Now imagine that the temperature decreases. The number of energetic molecules leaving the liquid phase abruptly diminishes. If there are enough vapor molecules around, they will continue to enter the liquid phase. We will see condensation (formation of droplets). This happens when you bring a cold bottle to a warm room. You can see mist on the bottle immediately.
6. If there are not enough vapor molecules around, nothing will happen. Upon the decrease of temperature, evaporation will continue at a slower rate, but no condensation will occur. You will need to decrease the temperature even further for the condensation to start.
7. For condensation to happen, you need to decrease the temperature to a point when the number of energetic water molecules leaving the liquid phase per unit time becomes less than the number of vapor molecules that enter the liquid phase. The first number depends on the air temperature, the second number depends on relative humidity (how “dry” is the air compared to the saturated equilibrium). Relative humidity is the ratio of the number of vapor molecules to the maximum equilibrium number of vapor molecules that can be present in a given volume at a given temperature.
8. So, to answer the first question above, the height at which condensation will occur will depend on the relative humidity of air at the surface. If the relative humidity is close to 100% (the air bears as much water vapor as possible at a given temperature), then as soon as the moist air rises just a little bit and cools, condensation will occur. Below are two pictures of how condensation happens just immediately over the forest, the first photo was shared by our colleague and friend Phil Shearman (hi, Phil!) and shows condensation above the virgin forests of Papua New Guinea, another is from the Prisursky Nature Reserve in Russia.

This is how PNG forest works.

And this is his Russian brother.
For a typical 80% humidity at the surface, the height at which condensation occurs will range from about 0.5 km to about 1 km depending on how fast the temperature declines with height in the ascending air. Below is Fig. 1B from Makarieva et al. 2013 JAS, where this height is shown as dependent on surface temperature and the vertical lapse rate, see the lowest three lines, green triangles are for 5 K/km, blue circles are for 6.5 K/km and red squares are for 9.8 K/km (it is the lowest line). All heights are below 1 km.





Dear Anastassia, many thanks for clear explanation. I like it.
I have a comment to the point 7: condensation is catalysed by volatile organic matter ( VOC - isoprene, monoterpene etc.) produced by the forest. Can we imagine the VOC like “tiny hooks” or continuation of forest stand up to atmosphere which keep the humidity produced by transpiration trees?
Best regards
Jan
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