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Mole fraction of A vapours above ideal s...

Mole fraction of A vapours above ideal solution in mixture of A and B will be: `("Given" X_(A) = 0.4, P_(A)^(o) = 100mm, P_(B)^(o) = 200 mm)`

A

0.4

B

0.8

C

0.25

D

None of these

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The correct Answer is:
C
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Mole fraction of vapour of A above solution in mixture of A and B(X_(A) = 0.4) will be (P_(A)^(@) = 100mm, P_(B)^(@) = 200 mm) :

The vapour pressure of a liquid solution containing A and B is 99 torr. Calculate mole % of B in vapour phase. (Given : P_(A^(@)) = 100 torr , P_(B^(@)) = 80 torr)

Two liquids A and B are mixed to form an ideal solution. The totol vapour pressure of the solution is 800 mm Hg. Now the mole fractions of liquid A and B are interchanged and the total vapour pressure becomes 600 mm of Hg. Calculate the vapour pressure of A and B in pure form. (Given : p_(A)^(@)-p_(B)^(@)=100 )

P_(A)=(235y -125xy)mm of HgP_(A) is partial pressure of A,x is mole fraction of B in liquid phase in the mixture of two liquids A and B and y is the mole fraction of A in vapour phase, then P_(B)^(@) in mm of Hg is:

Total vapour pressure of mixture of 1 mole of volatile component A (P_(A)^(@)=100 mm Hg) and 3 mole of volatile component B (P_(B)^(@)=80 mm Hg) is 90 mm Hg . For such case :

The total pressure exerted in ideal binary solution is given by P=P_(A)^(@)X_(A)+P_(B)^(@)X_(B) where P_(A)^(@)&P_(B)^(@) are the respective vapour pressure of pure components and X_(A)&X_(B) are their mole fraction in liquid phase. And composition of the vapour phase is determined with the help of Datton's law partial pressure: Y_(A)=(P_(A)^(@)X_(A))/(P) If total pressure exerted in an ideal binary solution is given by P=(5400)/(60+30Y_(A))mm of Hg. If the value of Y_(A)=0.4 then the value of X_(B) is:

The total pressure exerted in ideal binary solution is given by P=P_(A)^(@)X_(A)+P_(B)^(@)X_(B) where P_(A)^(@)&P_(B)^(@) are the respective vapour pressure of pure components and X_(A)&X_(B) are their mole fraction in liquid phase. And composition of the vapour phase is determined with the help of Datton's law partial pressure: Y_(A)=(P_(A)^(@)X_(A))/(P) If total pressure exerted in an ideal binary solution is given by P=(5400)/(60+30Y_(A))mm of Hg. The value of P_(A)^(@) is:

The total pressure exerted in ideal binary solution is given by P=P_(A)^(@)X_(A)+P_(B)^(@)X_(B) where P_(A)^(@)&P_(B)^(@) are the respective vapour pressure of pure components and X_(A)&X_(B) are their mole fraction in liquid phase. And composition of the vapour phase is determined with the help of Datton's law partial pressure: Y_(A)=(P_(A)^(@)X_(A))/(P) If total pressure exerted in an ideal binary solution is given by P=(5400)/(60+30Y_(A))mm of Hg. The more volatile liquid is:

Mole fraction of component A in vapour phase is chi_(1) and that of component A in liquid mixture is chi_2 , then ( p_(A)^@ )= vapour pressure of pure A, p_(B)^@ = vapour pressure of pure B), the total vapour pressure of liquid mixture is

Mole fraction of component A in vapour phase is chi_(1) and that of component A in liquid mixture is chi_2 , then ( p_(A)^@ )= vapour pressure of pure A, p_(B)^@ = vapour pressure of pure B), the total vapour pressure of liquid mixture is

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