What does an increase in temperature do to the vapor pressure of a liquid?

An increase in temperature leads to an increase in the vapor pressure of a liquid. This relationship is due to the fact that as temperature rises, the kinetic energy of the liquid's molecules also increases. When molecules have higher kinetic energy, a greater proportion of them can overcome the intermolecular forces holding them in the liquid state. As a result, more molecules can escape into the vapor phase, effectively increasing the vapor pressure.

This phenomenon can be understood through the concept of dynamic equilibrium between the liquid and gas phases of a substance. At any given temperature, there is a point at which the rate of evaporation of molecules from the liquid phase equals the rate of condensation of gas molecules back into the liquid. When temperature rises, the rate of evaporation increases, shifting the equilibrium and increasing the vapor pressure until a new equilibrium is established.

In summary, increasing the temperature causes an increase in the vapor pressure of a liquid by providing more energy for molecules to escape into the vapor phase.