If P^@ and P are the vapour pressure of ...

If `P^@` and P are the vapour pressure of the pure solvent and solution and `n_1` and `n_2` are the moles of solute and solvent respectively in the solution, then the correct relation between P and `P^@` is

`P^@=P[(n_1)/(n_1+n_2)]`

`P^@=P[(N_2)/(N_1+N_2)]`

`P=P^@[(n_1)/(n_1+n_2)]`

Text Solution

Verified by Experts

Topper's Solved these Questions

SOLUTIONS
MODERN PUBLICATION|Exercise EXERCISE|635 Videos
SOLID STATE
MODERN PUBLICATION|Exercise EXERCISE|525 Videos
STRUCTURE OF ATOM
MODERN PUBLICATION|Exercise EXERCISE|102 Videos

Similar Questions

Explore conceptually related problems

Why the vapour pressure of a solution of glucose in water is lower than of pure water

Why is the vapour pressure of a solvent lowered on the addition of non-volatile solute into it ?

Why the vapour pressure of saline solutions is lower than that of pure water ?

P_A and P_B are the vapour pressure of pure liquid components A and B respectively of an ideal binary solution. If X_A represent the mole fraction of component A, then the total pressure of the solution will be

The vapour pressure of the solvent decreased by 10 mm of Hg when a non volatile solute was added to the solvent. The mole fraction of the solute in the solution is 0.2. What should be the fraction of the solvent if a decrease in vapour pressure of 20 mm of Hg is desired:

A aqueous solution contains 10 moles of sucrose in 1 kg of solvent. calculate the molality of solution.

What is meant by lowering of vapour pressure? How does the relative lowering of vapour pressure depend on the number of moles of solute in a solution?

True or false Colligative properties depend only upon the moles of solute and are independent of the nature of solute and solvent.

Benzene and toluene form nearly ideal solution. At a certain temperature the vapour pressure of pure benzene and toluene are 150 and 50 torr. respectively. Calculate the vapour pressure of solution containing equal weights of benzene and toluene at this temperature .

The vapour pressure of pure liquid A at 310^@C is 0.158bar. The vapour pressure of this liquid in solution with liquid B is 0.095 bar. Calculate the mole fraction of A in the solution if the mixture obeys Raoult's law.

MODERN PUBLICATION-SOLUTIONS -EXERCISE

What is the mole fraction of solute in 2.5m aqueous solution .
Text Solution
|
A solution containing 2.44 g of solute dissolved in 75 g of water boil...
Text Solution
|
If P^@ and P are the vapour pressure of the pure solvent and solution ...
Text Solution
|
The equation that represents van't Hoff factor general solution equati...
Text Solution
|
Which of the following 0.1 M aqueous solution is liekly to have the hi...
Text Solution
|
5.0 g of sodlium hydroxide (molar mass 40g mol^-1) is dissolved in lit...
Text Solution
|
Which law states the relation between solubility of gas in liquid at c...
Text Solution
|
Calculate the molality of a solution that contains 51.2 g of napthalen...
Text Solution
|
31 gm of ethylene glycol (C2H6O2) is mixed with 500 gm of solvent. (K...
Text Solution
|
Which of the following is not a colligative property?t
Text Solution
|
What is Van't Hoff factor ?
Text Solution
|
Osmotic pressure of the solution can be increase by
Text Solution
|
The elevation in boiling point of a solution 13.44 g of CuCl2 in 1 kg...
Text Solution
|
When 20 g of napthoic acid (C11H8O2) is dissolved in 50 g of benzene(K...
Text Solution
|
The Henry's law constant for the solubility of N2 gas in water at 298K...
Text Solution
|
Dissolving 120g of urea (mol.wt 60) in 1000g of water gave a solution ...
Text Solution
|
The freezing point of a solution containing 0.1g of K3[Fe(CN)6] in 100...
Text Solution
|
For a dilute solution containing 2.5 g of a non volatile non electroly...
Text Solution
|
Colligative properties of a solution are
Text Solution
|
The solution showing positive deviations
Text Solution
|