NEET Exam  >  NEET Notes  >  Chemistry Class 12  >  Raoult's Law

Raoult's Law | Chemistry Class 12 - NEET PDF Download

Who discovered Raoult's Law?

  • Raoult’s law has been named after François-Marie Raoult, a French chemist who while experimenting found out that when substances were mixed in a solution, the vapour pressure of the solution decreased simultaneously. 
  • Raoult’s law was established in 1887  and is also considered the law of thermodynamics.

What is Raoult’s Law?

Raoult’s law states that:

For a solution of volatile liquids, the partial vapour pressure of each component of the solution

is directly proportional to its mole fraction present in solution.

Mathematical representation of Raoult’s law:

Let's understand this by looking at the example below

Ideal Solution of Two Volatile LiquidsIdeal Solution of Two Volatile Liquids

Let two volatile liquids A and B dissolve each other to form an ideal solution. Then the vapours above the solution will contain the vapours of A and B. Applying Dalton’s law of partial pressure the total vapour pressure of the solution will be 

Psolution = PA + PB

Where,
 PA and PB are the partial vapour pressures of A and B.

PA = PºA XA

PB = PºB XB

Where:

  • PºA and PºB are vapour pressures of pure A and B  respectively
  • xA and xB are mole fractions of A and B in a liquid solution respectively

Hence, 𝑃 (Solution) 𝑜𝑟 Ps =   PA0 XA + PB0 XB

Also, Ps = P0A(1-XB) + P0BXB

⇒ Ps = P0A+(P0B - P0A)XB

This equation is of the form y = mx + c. The value of m (slope) may be (+ve) or (–ve) depending upon whether P0B > P0A (m = + ve) or P0B < P0A (m = –ve).

Hence a plot of a graph of Ps versus XB will be a straight line with an intercept on the y-axis equal to pA and a slope equal to (P0B - P0A)

Plot of Vapour Pressure and Mole Fraction Plot of Vapour Pressure and Mole Fraction 

The total Pressure of a Solution will be:

  • P (Solution) = PA + PB = xAP0+ xBP0B
    Raoult`s Law | Chemistry Class 12 - NEET

Question for Raoult's Law
Try yourself:“Total pressure of gas mixture is the sum of individual pressures”. Which law is reflected in this statement?
View Solution

Finding Vapour Composition

  • Vapour composition means to find out the mole fraction of A and B in vapour i.e yA and yB. 
  • Dalton’s law of particle pressure is used to calculate the vapour composition, as we know, Partial pressure = mole fraction × total pressure
    ⇒ pA= yA × pS
    or yA =𝑃A/𝑃𝑆
    Similarly for B
    ⇒ yB = 𝑃A/𝑃𝑆

where yA and yB are mole fractions of ‘A’ and ‘B’ in the vapour phase and yA +  yB = 1

SPECIAL NOTE: 
xA and xB are mole fraction of ‘A’ and ‘B’ in the solution phase and xA +  xB =1

yA and yB are mole fraction of ‘A’ and ‘B’ in the vapour phase and yA +  yB =1

Raoult's Law as a special case of Henry's law

  • At a given temperature liquids vaporize. At equilibrium, the pressure exerted by the vapour of the liquid over the liquid phase is referred to as vapour pressure.
  • According to Raoult’s law, the vapour pressure of a volatile component in a given solution can be defined by pi = pi˚xi
  • In an answer of a gas in a fluid one of the segments is volatile to the point that it exists as a gas and solvency is given by Henry's law which expresses that p = KH x
  • Comparing both the equations we get that partial pressure of the volatile component or gas is directly proportional to its mole fraction in solution. The proportionality constant KH differs from pi˚
  • Therefore, Raoult's law turns into a unique instance of Henry’s law in which KH get to be equivalent to pi˚

Question for Raoult's Law
Try yourself:
According to Raoult's law, the partial vapour pressure of each component in a solution is directly proportional to its _____.
View Solution

Limitations of Raoult’s Law

There are a few limitations to Raoult’s law:

  1. Raoult’s law is apt for describing ideal solutions. However, ideal solutions are hard to find and they are rare. Different chemical components have to be chemically identical equally.
  2. Since many of the liquids that are in the mixture do not have the same uniformity in terms of attractive forces, these type of solutions tends to deviate away from the law.

There is either a negative or a positive deviation: 

  • Negative deviation happens when the vapour pressure is lower than what Raoult's law predicts. For instance, this occurs in a mix of chloroform and acetone or in a solution of water and hydrochloric acid.
  • On the other hand, positive deviation occurs when the attraction among similar molecules is stronger, surpassing the attraction between dissimilar molecules. In such cases, both components of the mixture can easily evaporate from the solution. An example of positive deviation is seen in mixtures like benzene and methanol or ethanol and chloroform.

Positive and Negative DeviationPositive and Negative Deviation

Solved Examples

Example 1. The vapour pressure of ethanol and methanol are 44.5 mm and 88.7 mm Hg respectively. An ideal solution is formed at the same temperature by mixing 60 g of ethanol with 40g of methanol. Calculate the total vapour pressure of the solution.
Solution. 
Number of moles of ethanol = 60/40 = 1.5
Number of moles of methanol = 40/32 = 1.25
X= 1.25/1.25 + 1.3 = 0.4545 and XB = 1 – 0.4545 = 0.545
Let A = CH3OH, B = C2H5OH
Total pressure of the solution
PT = XAP0A + XBP0B
= 0.4545 × 88.7 + 0.545 × 44.5 = 40.31 + 24.27
= 64.58 mm Hg

Example 2. The composition of vapour over a binary ideal solution is determined by the composition of the liquid. If XA and YA are the mole fraction of A in the liquid and vapour, respectively find the value of XA for which YA − Xhas a minimum. What is the value of the pressure at this composition?
Solution. 
Raoult`s Law | Chemistry Class 12 - NEET
Subtracting xA from both sides, we get
Raoult`s Law | Chemistry Class 12 - NEET
Now differentiating w.r.t. xA, we get
Raoult`s Law | Chemistry Class 12 - NEET
The value of xA at which yA − xA has a minimum value can be obtained by putting the above derivative equal to zero. Thus we have
Raoult`s Law | Chemistry Class 12 - NEET
Solving for xA, we get 

Raoult`s Law | Chemistry Class 12 - NEET 
hence
Raoult`s Law | Chemistry Class 12 - NEET

Example 3. A very small amount of non-volatile solute (that does not dissociate) is dissolved in 56.8 cm3 of benzene (density 0.889 g cm-3). At room temperature, the vapour pressure of this solution is 99.88 mm Hg while that of benzene is 100mm Hg. Find the molality of this solution. If the freezing temperature of this solution is 0.73 degrees lower than that of benzene. What is the value of the molal freezing point depression constant of benzene?
Solution.
Raoult`s Law | Chemistry Class 12 - NEET
Raoult`s Law | Chemistry Class 12 - NEET
Raoult`s Law | Chemistry Class 12 - NEET
Raoult`s Law | Chemistry Class 12 - NEET
Raoult`s Law | Chemistry Class 12 - NEET
Also,
ΔTf = Kf × molality f
∴ 0.73 = K × 0.1452
fK = 5.028 K. molality

Example 4. What is the composition of the vapour which is in equilibrium at 30°C with a benzene-toluene solution with a mole fraction of benzene of 0.400? 
(PoB = 119 torr and PTo = 37.0 torr)
Solution.
The Total pressure of the solution is given by
PT = XB P0B + XTP0T
= 0.4 × 119 + 0.6 × 37
= 47.6 + 22.2
= 69.8 torr
Applying Dalton’s law for mole fraction in the vapour phase.
YB = PB/PT = 47.6/62.4
= 0.763
YT = 1– 0.763
= 0.237

The document Raoult's Law | Chemistry Class 12 - NEET is a part of the NEET Course Chemistry Class 12.
All you need of NEET at this link: NEET
150 videos|378 docs|213 tests

FAQs on Raoult's Law - Chemistry Class 12 - NEET

1. Who discovered Raoult's Law?
Ans. François-Marie Raoult, a French chemist, discovered Raoult's Law.
2. What is Raoult’s Law?
Ans. Raoult's Law states that the partial vapor pressure of each component in an ideal mixture of liquids is directly proportional to its mole fraction in the solution.
3. How can we find vapor composition using Raoult's Law?
Ans. To find the vapor composition using Raoult's Law, we need to know the mole fraction of each component in the liquid mixture. Multiply the mole fraction of each component by its vapor pressure at that temperature to find the partial vapor pressure. The ratio of partial vapor pressure of each component to the total vapor pressure gives the vapor composition.
4. How is Raoult's Law related to Henry's Law?
Ans. Raoult's Law can be considered a special case of Henry's Law. Henry's Law relates the solubility of a gas in a liquid to its partial pressure. When the solute is a volatile liquid, Henry's Law can be used to describe the behavior of the solute in the vapor phase, which is similar to Raoult's Law.
5. What are the limitations of Raoult’s Law?
Ans. Raoult's Law assumes ideal behavior of the components, which may not be true for non-ideal solutions. It also assumes that the components do not interact with each other or with the container, which may not be the case in reality. Raoult's Law is most accurate for solutions of volatile components at low to moderate concentrations.
150 videos|378 docs|213 tests
Download as PDF
Explore Courses for NEET exam

How to Prepare for NEET

Read our guide to prepare for NEET which is created by Toppers & the best Teachers
Signup for Free!
Signup to see your scores go up within 7 days! Learn & Practice with 1000+ FREE Notes, Videos & Tests.
10M+ students study on EduRev
Download the FREE EduRev App
Track your progress, build streaks, highlight & save important lessons and more!
Related Searches

Semester Notes

,

Viva Questions

,

video lectures

,

shortcuts and tricks

,

Previous Year Questions with Solutions

,

pdf

,

Free

,

Raoult's Law | Chemistry Class 12 - NEET

,

past year papers

,

Important questions

,

Exam

,

Extra Questions

,

Raoult's Law | Chemistry Class 12 - NEET

,

Raoult's Law | Chemistry Class 12 - NEET

,

Objective type Questions

,

practice quizzes

,

Summary

,

study material

,

mock tests for examination

,

MCQs

,

Sample Paper

,

ppt

;