In a mixture of closely related liquids (such as benzene and toluence), the Roult's law states that the ratio P_(A) is proportional to the mole fraction of A in the liquid, P_(A)x_(A) . Mixtures that obey the law throughout the composition ranges from pure A to pure B are called ideal solutions . In ideal solution the solute also obeys Roult's law . Then the total pressure is given by P_("total")=P_(A)^(0)x_(A)+P_(B)^(0)x_(B) Each of the following solution obeys Raoult's law except
State and explain Raoult's law ?
The vapour pressure of a pure liquid A is 40 mm of Hg at 310K. The vapour pressure of its liquid in a solution with liquid B is 32 mm of Hg. Mole fraction of A in the solution, if it obeys Raoult's law is :
A solution that obeys Raoult's law is called
Assertion:Ideal solutions follow Raoult's law. Reason: DeltaH and DeltaV of ideal solutions are zero
NARENDRA AWASTHI-DILUTE SOLUTION-Level 3 - Match The Column
