Which statement about vapor pressure is accurate regarding temperature and kinetic energy?

Vapor pressure is a measure of the pressure exerted by a vapor in equilibrium with its liquid or solid form at a given temperature. The relationship between vapor pressure, temperature, and kinetic energy is pivotal to understanding how substances transition between states of matter.

As temperature increases, the average kinetic energy of the molecules in a substance also increases. When the kinetic energy is high enough, more molecules can escape from the liquid phase into the vapor phase, which directly results in an increase in vapor pressure. This is because a greater number of molecules possess sufficient energy to overcome intermolecular forces in the liquid and enter the gas phase.

Therefore, the statement that vapor pressure is directly related to kinetic energy is accurate. As the kinetic energy increases due to higher temperatures, more molecules escape into the vapor phase, raising the vapor pressure. This understanding aligns with the fundamental principles of thermodynamics and kinetic molecular theory, highlighting the direct correlation between increased molecular motion and the ability to vaporize, which manifests as higher vapor pressure.

In summary, the correct option underscores the critical link between kinetic energy and the vapor pressure of a substance, establishing that as kinetic energy increases, vapor pressure will also rise, affirming the validity of the statement.