How does vapor pressure vary with temperature

Vapor pressure increases as temperature rises. When a liquid is heated, its molecules gain more kinetic energy and move faster. As a result, more molecules escape from the liquid surface into the vapor phase. 

This increases the number of vapor molecules colliding with the container walls, which raises the vapor pressure. The relationship between vapor pressure and temperature is exponential, not linear. Even a small increase in temperature can cause a significant rise in vapor pressure. This happens because molecular motion and evaporation rates grow rapidly with heat. 

At a certain temperature called the boiling point, the vapor pressure equals the surrounding atmospheric pressure, and the liquid starts to boil. Each liquid has a unique vapor pressure curve, depending on molecular structure and intermolecular forces. 

Substances with weak intermolecular forces (like acetone) show high vapor pressures at lower temperatures, while those with strong forces (like water) need more heat to reach the same vapor pressure. In short, as temperature goes up, vapor pressure rises rapidly because more molecules can overcome intermolecular attractions and enter the vapor phase.