Partial pressure and vapor pressure are both commonly used scientific terms to refer to the amount of pressure exerted by a pressure component. The two look similar, though, but they still have their differences in their identity and effects. Foremost, talking about pressure, this can be defined as the amount of force per unit area on an object. It can also be defined as the force applied to particles colliding with each other.
The unit can be Newton per meter square or Pascal. Kinetic theory of gasses and the gas equations are used in the case of colliding particles to measure pressure. Vapor pressure is used in liquid and solid phases on their condensed state in equilibrium, while partial pressure is used in a gaseous phase in a non-reactive gas mixture. Raoult's law gives a good explanation of the vapor pressure, while Dalton's law gives a good explanation of the partial pressure.