Raoult's Law
Trending Questions
What is the formula of brine?
- 0.35
- 0.035
- 0.65
- 0.965
Assume that at the given constant temperature of solution, vapour pressure of phenol (A) in pure state is more than that of aniline (B) in pure state.
- 4.13 m
- 2.57 m
- 3.85 m
- 5.46 m
The vapour pressure will be lowest for
0.1 M sugar solution
0.1 M KCl solution
0.1 M Cu(NO3)2 solution
0.1 M AgNO3 solution
- 500 mm Hg; 0.4, 0.6
- 500 mm Hg; 0.5, 0.5
- 450 mm Hg; 0.5, 0.5
- 450 mm Hg; 0.4, 0.6
Vaour pressure of pure B, (p∘B)=150 mm Hg
2 mol of liquid 'A' and 3 mol of liquid 'B' are mixed to form an ideal solution. The vapour pressure of solution will be :
- 130 mm Hg
- 140 mm Hg
- 135 mm Hg
- 145mm Hg
- Mole fraction of component 2 in vapour phase is 0.3
- Mole fraction of component 2 in vapour phase is 0.7
- Mole fraction of component 1 in liquid phase is 0.4
- Mole fraction of component 1 in liquid phase is 0.6
The vapour pressure of pure benzene and toluene are 160 and 60 torr respectively. The molefraction of toluene in vapour phase in contact with equimolar solution of benzene and toluene is
0.50
0.6
0.27
0.73
What is p∘toluene(25∘C)?
- 30 mm Hg
- 100 mm Hg
- 22 mm Hg
- 40 mm Hg
The condition of Efflorescence
Vapour pressure of hydrated crystal < atmospheric vapour pressure
Vapour pressure of hydrated crystal ≤ atmospheric vapour pressure
Vapour pressure of hydrated crystal = atmospheric vapour pressure
Vapour pressure of hydrated crystal > atmospheric vapour pressure
- 50
- 25
- 37.5
- 53.5
For a solution of volatile liquids the partial vapour pressure of each component in solution is directly proportional to
Molarity
Mole fraction
Molality
Normality
A liquid mixture is composed of 1 mol of A and 3 mol of B.
If the pressure over the mixture at room temperature is reduced. At what pressure does the first vapour form?
What will be the mole fraction of component A in vapour phase (yA) if the total pressure (PT) of the solution is 500 mm Hg?
Equal volumes of 0.1M urea and 0.1M glucose are mixed. The mixture will have:
Same osmotic pressure
Lower osmotic pressure
Higher osmotic pressure
Cannot be predicted
An aqueous solution of sucrose (C12H22O11) containing 34.2 g/L of sucrose has an osmotic pressure of 2.38 atm at 17° C. For an aqueous solution of glucose (C6H12O6) to be isotonic with this solution, it's concentration (in g/L) should be:
- 34.2 g/L
17.1 g/L
18.0 g/L
36.0 g/L
- 50
- 25
- 37.5
- 53.5
KBr is 80% dissociated in solution. The freezing point of 0.5 molal solution is:
273 K
277 K
271.326 K
269 K
12 g of urea is dissolved in 1 litre of water and 68.4 g of sucrose is dissolved in 1 litre of water.The lowering of vapour pressure of the first case is:
Equal to second
Greater than second
Less than Second
Double that of second.
The pressure under which liquid and vapour can coexist at equilibrium is called the
- Limiting vapour pressure
- Real vapour pressure
- Normal vapour pressure
- Saturated vapour pressure
What is the mole fraction of liquid benzene in the solution?
- 0.25
- 0.75
- 0.50
- 0.90
Here,
p∘A= vapour pressure of pure A
p∘B= vapour pressure of pure B
- p∘B×x1x2
- p∘A×x1x2
- p∘B×x2x1
- p∘A×x2x1
- carbon tetrachloride + methanol
- carbon disulphide + acetone
- benzene + toluene
- phenol + aniline
The vapour pressure of pure benzene and toluene are 160 and 60 torr respectively. The molefraction of toluene in vapour phase in contact with equimolar solution of benzene and toluene is
0.50
0.6
0.27
0.73