# How to accurately explain evaporative cooling?

I am trying to clearly express in one or two sentences how increased evapotranspiration could cool a region. The audience is educated but non-scientific.

Is it accurate to say that the water vapor has removed latent heat? Is there a more clear explanation?

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## 3 Answers

One or two sentences?

Heat is transferred to water, which therefore evaporizes, taking away the heat with it.

Latent heat is the amount of heat necessary to trigger a phase transition in a substance, and is not spent to increase or decrease the substance's temperature. So it is incorrect to say tha the water has removed the latent heate. I'd rather say that water removed a heat quantity equal to its latent heat.

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Yours is quite clear, but are my statements accurate? – Abe Nov 3 '12 at 12:45

A volume of water contains a gigantic number of molecules, each with different speeds. The ones with faster speeds are the ones that escape the surface boundary forces to evaporate into the air. Thus the remaining ensemble of water molecules has a lower average speed of movement = lower "temperature".

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One may wonder when does evaporative cooling occur? To describe the liquid gas interface for say a substance X, we must use the concept of vapour pressure. Every Liquid at a given pressure and temperature has a definite value for its vapour pressure. If the partial pressure,(pressured exerted by the gas molecules only of X) is less than the vapour pressure of the liquid at that temperature then the liquid has a tendency to evaporate.

Why is some particular molecules chosen to escape the Liquid? The molecules of the substance X have a tendency to attract each other, To separate them one needs to provide energy to fuel their separation. Evaporation happens at the surface, Molecules tend to experience an average attractive force at the surface pulling not allowing them to escape.

Since the liquid is at a certain temperature, some molecules move faster than the others. If a particular molecule at the surface has a large enough Kinetic energy that it can overcome the attractive barrier allowing it to escape. Since only the fastest of the molecules escape the, liquid will consequently find itself with molecules of lower average energy, thus an overall decrease in its temperature. This will continue until the vapour pressure of the liquid is equal to the partial pressure of vapour outside.

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