Home
Class 12
CHEMISTRY
The vapour pressure of pure benzene at ...

The vapour pressure of pure benzene at `88^(@)C` is `957 mm` and that of toluene at the same temperature is `379.5 mm`. The composition of benzene-toluene mixture boiling at `88^(@)C` will be

A

`chi_("benzene")=0.66 , chi_("toluene") = 0.34`

B

`chi_("benzene")=0.34, chi_("toluene") = 0.66`

C

`chi_("benzene")= chi_("toluene") = 0.5`

D

`chi_("benzene")=0.75, chi_("toluene") = 0.25`

Text Solution

Verified by Experts

The correct Answer is:
a
`p = p_("benzene").^(@)chi_("benzene")+ p_("toluence").^(@)chi_("toluence")`
760= 957
Promotional Banner

Similar Questions

Explore conceptually related problems

The vapour pressure of pure benzene is 639.7 mm Hg and the vapour pressure of solution of a solute in benzene at the temperature is 631.9 mm Hg . Calculate the molality of the solution.

The vapour pressure of pure benzene at 50^(@) is 268 mm of Hg . How many moles of non-volatile solute per mole of benzene are required to prepare a solution of benzene having a vapour pressure of 16.0 mm of Hg at 50^(@)C ?

The osmotic pressure of urea solution at 10^(@)C is 200 mm .becomes 105.3 mm when it is diluted and temperature raised to 25^(@)C . The extent of dilution is

Benzene and toluene form nearly ideal solutions. At 20^(@)C , the vapour pressure of benzene is 75 torr and that of toluene is 22 torr. The partial vapour pressure of benzene at 20^(@)C for a solution containing 78 g of benzene and 46 g of toluene in torr is

The vapour pressure of pure benzene C_(6)H_(6) at 50^(@)C is 268 "torr" . How many moles of non-volatile solute per mole of benzene is required to prepare a solution of benzene having a vapour pressure of 167 "torr" at 50^(@)C ?

The vapour pressure of pure benzene C_(6)H_(6) at 50^(@)C is 268 "torr" . How many moles of non-volatile solute per mole of benzene is required to prepare a solution of benzene having a vapour pressure of 167 "torr" at 50^(@)C ?

At 25^(@)C , the vapour pressure of pure water is 25.0 mm Hg . And that of an aqueous dilute solution of urea is 20 mm Hg . Calculate the molality of the solution.

At a certain temperature, the vapour pressure of pure ether is 640 mm and that of pure acetone is 280 mm . Calculate the mole fraction of each component in the vapour state if the mole fraction of ether in the solution is 0.50.

At 40^(@)C the vapour pressure of pure liquids, benzene and toluene, are 160 mm Hg and 60 mm Hg respectively. At the same temperature, the vapour pressure of an equimolar solution of the liquids, assuming the ideal solution will be: