How does the vapor pressure of a liquid relate to its rate of evaporation?

The correct choice highlights a fundamental principle in physical chemistry regarding the behavior of liquids and their transitions to gas. Vapor pressure is defined as the pressure exerted by a vapor in equilibrium with its liquid at a given temperature. A higher vapor pressure indicates that a larger number of molecules are escaping from the liquid into the vapor phase.

When a liquid has a greater vapor pressure, it means that the molecules are more energetic and have the tendency to escape into the atmosphere more readily. Consequently, this increased activity leads to a faster rate of evaporation. As molecules leave the liquid surface and enter the gas phase, the evaporation rate rises in tandem with the vapor pressure.

In contrast, the other options do not correctly describe the relationship between vapor pressure and evaporation. For example, stating that higher vapor pressure slows down evaporation contradicts the fundamental concept that increased vapor pressure correlates with increased molecular movement and evaporation rates. Similarly, suggesting that no relationship exists overlooks the intimate connection between vapor pressure and the dynamics of evaporation, and implying that lower vapor pressure increases evaporation fails to recognize that a lower vapor pressure would actually indicate reduced molecular activity and, thus, a slower rate of evaporation.