These questions please...
Dear student,
1) Mixture of acetone and chloroform shows negative deviation from Raoult's law.
On mixing the the components, weak hydrogen bonding will arise in the molecules of the two components present in the solution. As a result, they will have lesser tendency to escape out of the liquid mixture than when they were present alone in their respective containers.this will decrease the vapour pressure of each component in the solution and also that of the solution as a whole.
2)Given : Liquid X = 28% by mass of solution (molecular mass of X = 140 g)
Total vapour pressure of liquid (P) = 160 mm of Hg (at 30o C)
Vapour pressure of water (PB) = 150 mm of Hg (at 30o C)
To find : Vapour pressure of liquid X
3) Osmotic pressure (π) = CRT
π = (0.1 M)(0.0821 L atm K-1 mol-1)(288 K)
π = 2.36 atm
4) Osmotic pressure (π) = CRT
π = (0.1 M)(0.0821 L atm K-1 mol-1)(300 K)
π = 2.463 atm
1) Mixture of acetone and chloroform shows negative deviation from Raoult's law.
On mixing the the components, weak hydrogen bonding will arise in the molecules of the two components present in the solution. As a result, they will have lesser tendency to escape out of the liquid mixture than when they were present alone in their respective containers.this will decrease the vapour pressure of each component in the solution and also that of the solution as a whole.
2)Given : Liquid X = 28% by mass of solution (molecular mass of X = 140 g)
Total vapour pressure of liquid (P) = 160 mm of Hg (at 30o C)
Vapour pressure of water (PB) = 150 mm of Hg (at 30o C)
To find : Vapour pressure of liquid X
For total miscible liquids,
Ptotal = Mol. fraction of A × pA0 + Mol. fraction of B × pB0
No. of moles of A = 28/140
Liquid B is water. its mass is (100−28), i.e., 72.
No. of moles of B = 72/18
Total number of moles = 0.2 + 4.0 = 4.2
Given, Ptotal = 160 mm
pB0 = 150 mm
So 160 = 0.2/4.2 × pB0 + 4.0/4.2 × 150
pA0 = 17.15×4.2/0.2 = 360.15 mm
3) Osmotic pressure (π) = CRT
π = (0.1 M)(0.0821 L atm K-1 mol-1)(288 K)
π = 2.36 atm
4) Osmotic pressure (π) = CRT
π = (0.1 M)(0.0821 L atm K-1 mol-1)(300 K)
π = 2.463 atm