What is the difference between vapor pressure and partial pressure?

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VAPOR PRESSURE PARTIAL PRESSURE
1. The vapor pressure is defined as the pressure that is exerted by the vapors of solid and liquid in their condensed phase when they are in the equilibrium. 1. The partial pressure is defined as the pressure that is exerted by the components in a gas mixture in an unreactive phase.
2.This can be explain by Raoult's Law 2.This can be explain by Dalton's Law.
3. The vapor pressure is applicable only for the solid and liquid phases. 3. The partial pressure is applicable only for the gaseous phase.
4. The vapor pressure does not depends on the surface area or the system's volume. 4. The partial pressure can be calculated by using the same volume of gases.
5. The vapor pressure can be calculated using the solute's mole fraction. 5. The partial pressure can be calculated using gas's mole fraction.

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VAPOR PRESSURE	PARTIAL PRESSURE
1. The vapor pressure is defined as the pressure that is exerted by the vapors of solid and liquid in their condensed phase when they are in the equilibrium.	1. The partial pressure is defined as the pressure that is exerted by the components in a gas mixture in an unreactive phase.
2.This can be explain by Raoult's Law	2.This can be explain by Dalton's Law.
3. The vapor pressure is applicable only for the solid and liquid phases.	3. The partial pressure is applicable only for the gaseous phase.
4. The vapor pressure does not depends on the surface area or the system's volume.	4. The partial pressure can be calculated by using the same volume of gases.
5. The vapor pressure can be calculated using the solute's mole fraction.	5. The partial pressure can be calculated using gas's mole fraction.