Question

explain why more water evaporates when the water is kept at 80

Answer 1

Answer:

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Explanation:

Water Evaporation

Evaporation of water requires a large quantity of energy, most of which comes from the Sun. The heat required to vaporize water is 540MJkg−1 at 373K (101kPa) and increases to 2.26MJkg−1 at 273K.

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Answer 2

Answer:

Water does not “evaporate” at 100°C, it “boils”. Water can evaporate at any temperature, the rate of evaporation depending on the temperature and the humidity in air.

Boiling is when evaporation is super fast, and ALL the water has to becomes gaseous. Evaporation happens when there is still liquid water, and a small part of it randomly gathers enough energy to becomes gaseous.

Think of water as a mass of molecules constantly bumping into each other. Statistically, some of the water molecules will be hit more and gather more energy, which will allow them to break free of the mass and go in the air. When it is 100°C, virtually all the water molecule have enough energy to break free, hence the boiling. At lower temperature, you will only have a few molecules at the surface that can evaporate due to this random accumulation of hits between molecules (you can see it as 100°C very locally, at the scale of one molecule).

It is the same mechanism at work when you sweat. If humidity in the air is low (hence there is still room for more water vapor in the air at that temperature and pressure), the water in your sweat will tend to evaporate, stealing some of your heat in the process of breaking free. That cools you down, which is the main purpose of sweating. Now if you go in the rainforest (or in the UK), with 100% humidity, it does not have to be that warm for you to overheat because the air is already saturated in water and your sweat cannot evaporate anymore. As a result, you can't dissipate your heat and you feel terrible

Explanation: