Increasing the temperature increases the vaporization rate of a liquid because the excess energy is used to break covalent bonds

True or False?

False

Explanation:

False. The molecules of liquid are hold in the liquid state due to intermolecular forces or Van de Waals forces, without affecting the molecule itself and its atomic bonds (covalent bonds). When the temperature increases the kinetic energy of the molecules is higher, therefore they have more possibilities to escape from the attractive intermolecular forces and go to the gas state.

Note however that this is caused because the intermolecular forces are really weak compared to covalent bonds, therefore is easier to break the first one first and go to the gas state before any covalent bond breaks (if it happens).

A temperature increase can increase vaporisation rate if any reaction is triggered that decomposes the liquid into more volatile compounds, but nevertheless, this effect is generally insignificant compared with the effect that temperature has in vaporisation due to Van der Waals forces.