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An ideal solution contains two volatile compounds A and B. The relation between mole fraction of A in vapour phase $(y)$ and mole fraction in liquid phase $(x)$ is given by $3 y - 2 x = x y .$ Then,

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Important Questions on Solutions

HARD

Chemistry>Physical Chemistry>Solutions>Raoult's Law

The plot of total vapour pressure as a function of mole fraction of the components of an ideal solution formed by mixing liquids

X

and

Y

MEDIUM

Chemistry>Physical Chemistry>Solutions>Raoult's Law

A solution contains

5

moles of

X

and

5

moles of

Y

, and has a normal boiling point of

90 ° C

. The vapor pressure of pure

X

300 mm Hg

. What is the vapor pressure of pure

Y

at this temperature?

HARD

Chemistry>Physical Chemistry>Solutions>Raoult's Law

Benzene and toluene form an ideal solution over the entire range of composition. The vapour pressure of pure benzene and toluene at $T (K)$ are $50 mmHg$ and $40 mmHg$ , respectively. What is the mole fraction of toluene in vapour phase when $117 g$ of benzene is mixed with $46 g$ of toluene?

(Molar mass of benzene and toluene are $78$ and $92 g {mol}^{- 1}$ , respectively)

HARD

Chemistry>Physical Chemistry>Solutions>Raoult's Law

Liquids

A

and

B

form an ideal solution in the entire composition range. At

350 K,

the vapour pressure of pure A and pure B are

7 \times 10^{3} Pa

and

12 \times 10^{3} Pa

, respectively. The composition of the vapour in equilibrium with a solution containing 40 mole percent of A at this temperature is:

MEDIUM

Chemistry>Physical Chemistry>Solutions>Raoult's Law

Liquid

M

and liquid

N

form an ideal solution. The vapour pressures of pure liquids

M

and

N

are

450

and

700 m m H g,

respectively, at the same temperature. Then correct statements is:
(

x_{M} = M o l e f r a c t i o n o f {' M}^{'} i n s o l u t i o n;

x_{N} = M o l e f r a c t i o n o f {' N}^{'} i n s o l u t i o n;

y_{M} = M o l e f r a c t i o n o f {' M}^{'} i n v a p o u r p h a s e;

y_{N} = M o l e f r a c t i o n o f {' N}^{'} i n v a p o u r p h a s e;

)

EASY

Chemistry>Physical Chemistry>Solutions>Raoult's Law

On mixing

20 mL

of acetone with

60 mL

of chloroform, the total volume of the solution is

MEDIUM

Chemistry>Physical Chemistry>Solutions>Raoult's Law

How many grams of glucose are required to prepare an aqueous solution of glucose having a vapor pressure of

23.324 mm Hg

25 ° C

100 g

of water? The vapour pressure of pure water at

25 ° C

23.8 mm Hg .

MEDIUM

Chemistry>Physical Chemistry>Solutions>Raoult's Law

A mixture of toluene and benzene boils at

100^{o} C

. Assuming ideal behaviour, the mole fraction of toluene in the mixture is closest to [Vapour pressures of pure toluene and pure benzene at

100^{o} C

are

0.742

and

1.800

bar respectively. 1 atm

= 1.013

bar]

EASY

Chemistry>Physical Chemistry>Solutions>Raoult's Law

9 gram anhydrous oxalic acid (mol. Wt. = 90) was dissolved in 9.9 moles of water. If vapour pressure of pure water is

P_{1}^{o}

the vapour pressure of solution is

MEDIUM

Chemistry>Physical Chemistry>Solutions>Raoult's Law

An open beaker of water in equilibrium with water vapour is in a sealed container. When a few grams of glucose are added to the beaker of water, the rate at which water molecules :

EASY

Chemistry>Physical Chemistry>Solutions>Raoult's Law

The vapour pressure of pure liquids

A

and

B

are

450

and

700 mm

Hg

350 K

respectively. If the total vapour pressure of the mixture is

600 mm

Hg,

the composition of the mixture in the solution is

MEDIUM

Chemistry>Physical Chemistry>Solutions>Raoult's Law

A solution at

20^{o} C

is composed of 1.5 mol of benzene and 3.5 mol of toluene. If the vapour pressure of pure benzene and pure toluene at this temperature are 74.7 torr and 22.3 torr respectively, then the total vapour pressure of the solution and the benzene mole fraction in equilibrium with it will be, respectively:

EASY

Chemistry>Physical Chemistry>Solutions>Raoult's Law

The correct option for the value of vapour pressure of a solution at $45 º C$ with benzene to octane in molar ratio $3 : 2$ is:

[At $45 ° C$ vapour pressure of benzene is $280 mm Hg$ and that of octane is $420 mm Hg .$ Assume Ideal gas]

EASY

Chemistry>Physical Chemistry>Solutions>Raoult's Law

A mixture of toluene and benzene forms a nearly ideal solution. Assume

P_{B} °

and

P_{T} °

to be the vapor pressures of pure benzene and toluene, respectively. The slope of the line obtained by plotting the total vapor pressure to the mole fraction of benzene is:

HARD

Chemistry>Physical Chemistry>Solutions>Raoult's Law

Liquids A and B form ideal solution over the entire range of composition. At temperature

T

, equimolar binary solution of liquids A and B has vapour pressure

45 T o r r

. At the same temperature, a new solution of A and B having mole fractions

x_{A} and x_{B}

, respectively, has vapour pressure of

22.5 T o r r

. The value of

\frac{x_{A}}{x_{B}}

, in the new solution is ____.

(Given that the vapour pressure of pure liquid A is

20 Torr

at temperature

T

)

MEDIUM

Chemistry>Physical Chemistry>Solutions>Raoult's Law

300 K

, the vapour pressure of a solution containing

1

mole of

n

-hexane and

3

moles of

n

-heptane is

550 mm

Hg

. At the same temperature, if one more mole of

n

-heptane is added to this solution, the vapour pressure of the solution increases by

10 mm

Hg

. What is the vapour pressure in

mmHg

n

- heptane in its pure state______?

MEDIUM

Chemistry>Physical Chemistry>Solutions>Raoult's Law

A solution is prepared by mixing

8.5

g of

{CH}_{2} {Cl}_{2}

and

11.95 g

{CHCl}_{3}

. If vapour pressure of

{CH}_{2} {Cl}_{2}

and

{CHCl}_{3}

298

K are

415

and

200

mm Hg respectively, the mole fraction of

{CHCl}_{3}

in vapour form is:

(M o l a r m a s s o f Cl = 35.5 g m o l^{- 1})

MEDIUM

Chemistry>Physical Chemistry>Solutions>Raoult's Law

38.4 g

of unknown substance (molar mass

384 g {mol}^{- 1}

) and

116 g

of acetone is used to prepare a solution at

313 K

. If vapour pressure of pure acetone (molar mass

58 g {mol}^{- 1}

) is

0.842

atmosphere, what is the vapour pressure of solution ?

MEDIUM

Chemistry>Physical Chemistry>Solutions>Raoult's Law

The vapour pressures of pure liquids

A

and

B

are

400

and

600 mm Hg

respectively at

298 K .

On mixing the two liquids, the sum of their volumes is equal to the volume of the final mixture. The mole fraction of liquid

B

0.5

in the mixture. The vapour pressure of the final solution, the mole fractions of components

A

and

B

in the vapour phase, respectively are

HARD

Chemistry>Physical Chemistry>Solutions>Raoult's Law

Which of the following statements about the composition of the vapour over an ideal 1 : 1 molar mixture of benzene and toluene is correct? Assume that the temperature is constant at

25^{o} C

. (Given vapour pressure data at

25^{o} C

, benzene = 12.8 kPa, toluene = 3.85 kPa)

An ideal solution contains two volatile compounds A and B. The relation between mole fraction of A in vapour phase y and mole fraction in liquid phase x is given by 3y-2x=xy. Then,

Important Questions on Solutions

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An ideal solution contains two volatile compounds A and B. The relation between mole fraction of A in vapour phase $(y)$ and mole fraction in liquid phase $(x)$ is given by $3 y - 2 x = x y .$ Then,