What is the difference between partial vapour pressure and vapour pressure of the components?

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Solution

In a solution the two terms mean the same, the total vapour pressure of a solution will be the sum of the vapour pressures of all the components of the system multiplied by their respective mole fractions.

partial vapour pressure = vapour pressure x mole fraction.

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Q. The ratio of partial pressure of gaseous component to the total vapour pressure of the mixture is equal

The mole fraction of component A in vapour phase is $x_{1}$ and mole fraction of component A in liquid mixture is $x_{2} (P_{A}^{0}$ = vapour pressure of pure A; $P_{B}^{0}$ = vapour pressure of pure B). What is the total pressure?

What will be the vapour pressure of pure components A and B respectively if vapour pressure of mixture of these two liquids is given by Pt=100+250Xb torr

Q. Assertion :At equilibrium, vapour phase will be always rich in component which is more volatile Reason: The composition of vapour phase in equilibrium with the solution is determined by the partial pressure of the components.

Q. Mole fraction of component

A

in the vapour phase is

X_{1}

and mole fraction of component

A

in liquid mixture is

X_{2} (P_{A}^{o} =

vapour pressure of pure

A; P_{B}^{o} =

vapour pressure of pure B) then total vapour pressure of the liquid mixture is:

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What is the difference between partial vapour pressure and vapour pressure of the components?

In a solution the two terms mean the same, the total vapour pressure of a solution will be the sum of the vapour pressures of all the components of the system multiplied by their respective mole fractions. partial vapour pressure = vapour pressure x mole fraction.

In a solution the two terms mean the same, the total vapour pressure of a solution will be the sum of the vapour pressures of all the components of the system multiplied by their respective mole fractions.

partial vapour pressure = vapour pressure x mole fraction.