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 frac

Question

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 is 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

Canvas Classes · Accepted Answer

Strategy:
 Use Raoult's Law to find the total pressure () and then apply Dalton's Law () to find the vapour phase mole fractions.

Step 1: Identify the solution type
"Sum of volumes... equal to... final mixture" , indicating an ideal solution.

Step 2: Calculate Total Vapour Pressure ()
.

Step 3: Calculate vapour phase composition
- 
-

More questions from Solutions