Why does water evaporate even below its boiling point?

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Water evaporates below its boiling point primarily because some molecules at the surface possess enough energy to escape into the air. This occurs due to the movement of water particles, where not all bonds are strong enough to keep every molecule contained. While convection currents can enhance evaporation by increasing surface area and facilitating the movement of warmer molecules, the key factor is the varying speeds of individual molecules. The hotter molecules can break free, leaving behind cooler ones. Thus, evaporation is a result of molecular dynamics rather than solely temperature or convection.
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why does water evaporate even below its boiling point? is it because the bonds between particles aren't strong (while particles in water moves) thus some escape periodically or does it have something to do with convection currents?
 
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Convection may speed up the evaporation process by, e.g., increasing the surface area but the main effect is that some of the water molecules near the surface are moving at speeds sufficient to let them "escape." In effect, they are the hotter molecules and leave the cooler ones behind.
 
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