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Vapor pressure is defined as the pressure exerted by the vapor molecules above a liquid when the liquid and vapor are in equilibrium. In other words, it is the pressure at which the rate of evaporation equals the rate of condensation.

Temperature plays a crucial role in influencing vapor pressure. As the temperature of a liquid increases, the kinetic energy of the molecules in the liquid also increases. This causes a greater number of liquid molecules to transition into the vapor phase, resulting in more molecules escaping the liquid surface and moving into the surrounding space.

As the temperature increases, the evaporation rate of molecules from the liquid's surface also increases. This is because, with higher kinetic energy, a larger number of molecules have sufficient energy to overcome the intermolecular forces that hold them in the liquid phase. As a result, they can escape the surface and transition into the vapor phase.

When the temperature rises, the equilibrium between the liquid and vapor phases shifts to accommodate the increased number of vapor molecules. Eventually, the rate of condensation also increases to match the increased evaporation rate, thus maintaining equilibrium. However, this new equilibrium state results in a higher vapor pressure since more molecules are now present in the vapor phase above the liquid surface. In conclusion, the vapor pressure of a liquid increases as temperature increases because higher temperatures give the liquid molecules greater kinetic energy, allowing more of them to escape the liquid surface and enter the vapor phase. This results in a higher vapor pressure when equilibrium is reached between evaporation and condensation rates at higher temperatures.