# Question #cc2fd

Vapor pressure is the equilibrium state change of a $L r i g h t \le f t h a r p \infty n s G$, where the pressure is the pressure of vapor that has vaporized out of the liquid. The liquid's boiling point is when ${P}_{v} = {P}_{a}$.
The more volatile a liquid, the higher its vapor pressure. Generally, as temperature increases, ${P}_{v}$ also does. At a molecular level, this is because the liquid particles' average kinetic energy increases enough to break free of the intermolecular forces within the liquid.
When a liquid has a low ${P}_{v}$, it vaporizes less readily and thus tends to not vaporize (think honey, or something, compared to an organic solvent). More simply, the pressure of the vapor of the liquid (within a closed system) isn't high and thus there aren't many gas particles that have "evaporated" from the liquid.