Vapour pressure of a solution is different from that of pure solvent. Name the law which helps us to determine partial vapour pressure of a volatile component.
State the above law.

In the depression of freezing point experiment it is found that (i) The vapour pressure of the solution is less than that of pure solvent (ii) The vapour pressure of the solution is more than that of pure solvent (iii) Only solute molecules solidify at the freezing point (iv) Only solvent molecules solidify at the freezing point

Assertion : At equilibrium, vapour phase will be always rich in component which is more volatile. Reason : The composition of vapour phase in equilibrium with the solution is determined by the partial pressures of the components. 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 both (A) and (R) are incorrect.

Partial pressure of a vessel containing Cl_2 , CO_2 and CO is the sum of the partial pressure of Cl_2 , O_2 and CO . State the law.

State Dalton's law of partial pressures.

Vapour pressure of pure water at 298 K is 23.8mmHg. 50g of urea is dissolved in 850g of water. Calculate the vapour pressure of water for this solution and its relative lowering.

An aqueous solution is 1 molal in KI. Which change will cause the vapour pressure of the solution to increase

Which one of the statements given below concerning properties of solutions, describes a colligative effect? a)Boiling point of pure water decreases by the addition of ethanol b)Vapour pressure of pure water decreases by the addition of nitric acid c)Vapour pressure of pure benzene decreases by the addition of naphthalene d)Boiling point of pure benzene increases by the addition of toluene

The total vapour pressure of a 4 mole % solution of NH_(3) in water at 293k is 50.0 torr, the vapour pressure of pure water is 17.0 torr at this temperature. Applying Henry's and Raoult's laws, calculate the total vapour pressure for a 5 mole% solution

100 g of liquid A (molar mass 140g"mol"^(-1) ) was dissolved in 1000 g of liquid B (molar mass 180 g"mol"^(-1) ) . The vapour pressure of pure liquid B was found to be 500 torr. What will be the vapour pressure of pure liquid A and its vapour pressure in the solution respectively if the total vapour pressure of the solution is 475 torr?

100 g of liquid 'A' (molar mass '140 g/ mol' ) was dissolved in 1000 g of liquid 'B'. (molar mass 180 g/mol The vapour pressure of pure liquid B was found to be 500 torr. Calculate the vapour pressure of pure liquid A and its vapour pressure in the solution, if the total vapour pressure of the solution is 475 torr.