Within a gas phase that is in contact with a liquid phase, molecules are moving randomly. These molecules are constantly entering into collisions with each other and with the liquid phase. The rate at which this occurs depends on the number of collisions which occur and this rate is to the partial pressure of the vapor.

Directly Proportional

Explanation:

The partial pressure is defined as the pressure exerted by an individual gas that are present in a mixture as if it were alone in that particular system.

The kinetic molecular theory of gases is explained as the state of matter that is composed of tiny particles in constant motion even though there are distance between the colliding particles.They posses low density and Because of their nature gases can expansion and contraction of gas can be influenced under some condition.Unlike other fluid like liquids, the volume that gas usually occupied is empty space.

The gas particles are always in constant motion, and all the particles of the individual gases move and collide with one another and with the walls of the container they occupied. The magnitude of the gas pressure is been determined by the force with which they collide with one another.

Therefore,The rate at which collision occurs depends on the number of collisions which occur and this rate is directly proportional to the partial pressure of the vapor

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