1. The problem statement, all variables and given/known data Imagine a wet thermometer whose bulb is covered with a wet wick at 1 atm. Temperature of the water happens to drop during the process of evaporation. 2. Relevant equations N/A 3. The attempt at a solution Does evaporation lower the temperature of water just by removing high-kinetic-energy molecules and lowers it's temperature, just so there can be a driving force for heat transfer? So basically heat from the air is supplied to the water resulting in lowering it's temperature by some small amount? Somewhere I read that temeprature difference between wet and dry thermometer goes up to 10°C, or more. It's sorta shocking to me, does that mean that water and air at differ by that large amount in a real environment? So they are basically never in a thermal equilibrium until all water evaporates? Wow... I'm not really interested in math behind it, i just dont get what's going on in molecular, practical level.