Home
Class 12
CHEMISTRY
Assertion (A): Henry's law and Raoult's ...

Assertion (A): Henry's law and Raoult's law are not independent, i.e., one can be derived from the other.
Reason (R ): The partial pressure is directly proportional to the mole fraction of the concerned species for ideal solutions.

A

If both `(A)` and `(R )` are correct, and `(R )` is the correct explanation of `(A)`.

B

If both `(A)` and `(R )` are correct, but `(R )` is not the correct explanation of `(A)`.

C

If `(A)` is correct, but `(R )` is incorrect.

D

If `(A)` is correct, but `(R )` is correct.

Text Solution

Verified by Experts

The correct Answer is:
B

Henry's law is for solute while Raoult's law is for solvent, both are dependent to each other.
Promotional Banner

Similar Questions

Explore conceptually related problems

If Raoult's law is obeyed, the vapour pressure of the solvent in a solution is directly proportional to

If Raoult's law is obeyed, the vapour pressure of the solvent in a solution is directly proportional to

Solution of two volatile liquids x and y obey Raoult's law. At a certain temperature it is found that when the total pressure above a given solution is 400 mm of Hg , the mole fraction of x in the vapour is 0.45 and in the liquid is 0.65 . What are the vapour pressures of two pure liquids at the given temperature?

When a solution of CHCl_(3) and acetone is formed, the solution is non-ideal with ………deviation from Raoult's law. The vapour pressure of such a solution will be ………….than the corresponding ideal solution.

What are non-ideal solutions ? Mention the reason for the negative deviation from the Raoult's law.

(a) The vapour pressures of benzene and toluene at 293 Kare 75 mm Hg and 22 mm Hg respectively. 23.4 g of benzene and 64.4 g of toluene are mixed. If the two form an ideal solution, calculate the mole fraction of benzene in the vapour phase assuming that the vapour pressures are in equilibrium with the liquid mixture at this temperature. (b) What is meant by +ve and -ve deviations from Raoult's law and how is the sign of H solution related to +ve and -ve deviations from Raoult's law ?

For a solution of acetone in chloroform, Henry's law constant is 150 torr at a temperature of 300 K. (a) Calculate the vapour pressure of acetone when the mole fraction is 0.12. (b) Assuming that Henry's law is applicable over sufficient range of composition to make the calculation valid, calculate the composition at which Henry's law pressure of chloroform is equal to Henry's law pressure of acetone at 300 K. (Henry's law constant for chloroform is 175 torr.)

The vapour pressure of a pure liquid A is 40 mm Hg at 310 K . The vapour pressure of this liquid in a solution with liquid B is 32 mm Hg . The mole fraction of A in the solution, if it obeys Raoult's law, is:

The vapour pressure of pure components A and B are 200 torr and 100 torr respectively. Assuming a solution of these components obeys Raoult's law, the mole fraction of component. A in vapour phase in equilibrium with a solution containing equimoles of A and B is :

The vapour pressure of methyl alcohol at 298 K is 0.158 bar. The vapour pressure of this liquid in solution with liquid B is 0.095 bar. Calculate the mole fraction of methyl alcohol in the solution if the mixture obeys Raoult's law.