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 Which of the following solutions shows negative deviation from Raoult’s law?
  • a)
    Acetone and chloroform
  • b)
    Acetone and carbon disulphide
  • c)
    Ethyl alcohol and cyclohexane
  • d)
    Benzene and toluene
Correct answer is option 'A'. Can you explain this answer?
Verified Answer
Which of the following solutions shows negative deviation from Raoult&...
On mixing acetone and chloroform, hydrogen bond is formed between them. Due to this vapour pressure of the solution formed by them decreases. Hence solution shows negative deviation from Raoult’s law.

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Which of the following solutions shows negative deviation from Raoult&...
Solution:

Negative deviation from Raoult’s law occurs when the intermolecular forces between the components of the solution are stronger than the forces between the molecules of the pure components. This results in the vapor pressure of the solution being less than what is predicted by Raoult’s law.

Out of the given options, the solution of acetone and chloroform shows negative deviation from Raoult’s law.

Explanation:

Acetone and chloroform are two liquids that have different molecular structures and intermolecular forces. Acetone is a polar molecule with a carbonyl group that can form hydrogen bonds, whereas chloroform is a nonpolar molecule that has a dipole moment but cannot form hydrogen bonds. When these two liquids are mixed together, the polar and nonpolar molecules form weak intermolecular forces, resulting in a negative deviation from Raoult’s law.

The deviation from Raoult’s law can be explained by the fact that the intermolecular forces between acetone and chloroform molecules are weaker than the intermolecular forces between the molecules of the pure components. Thus, the vapor pressure of the solution will be lower than expected based on Raoult’s law.

Therefore, the correct option is A) Acetone and chloroform.
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Community Answer
Which of the following solutions shows negative deviation from Raoult&...
A solution of CHCL3 AND CH3COCH3 shows (-ve) deviation from Raoult's law》》molecules of pure chloroform and those of pure acetone cannot form H- bonds among themselves. however in a solution of chloroform and acetic anhydride, the hydrogen of CHCL3 is attacked by the O2 of acetic anhydride and thereby leads to the formation of H-bonds between the molecules of CHCL3 and (CH3)2CO molecules, which lower their tendency to escape from the solute. As a result ,the partial vapour pressure of CHCL3 and acetic anhydride and total vapor pressure of the solution becomes less than expected from Raoult's law.the strong forces of attraction between the molecules CHCL3 AND acetic anhydride leads to the lowering of potential energy of the system, which is accompanied with the evolution of heat..Hence,del H solution is negatives for the solution.
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Which of the following solutions shows negative deviation from Raoult’s law?a)Acetone and chloroformb)Acetone and carbon disulphidec)Ethyl alcohol and cyclohexaned)Benzene and tolueneCorrect answer is option 'A'. Can you explain this answer?
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Which of the following solutions shows negative deviation from Raoult’s law?a)Acetone and chloroformb)Acetone and carbon disulphidec)Ethyl alcohol and cyclohexaned)Benzene and tolueneCorrect answer is option 'A'. Can you explain this answer? for Class 12 2024 is part of Class 12 preparation. The Question and answers have been prepared according to the Class 12 exam syllabus. Information about Which of the following solutions shows negative deviation from Raoult’s law?a)Acetone and chloroformb)Acetone and carbon disulphidec)Ethyl alcohol and cyclohexaned)Benzene and tolueneCorrect answer is option 'A'. Can you explain this answer? covers all topics & solutions for Class 12 2024 Exam. Find important definitions, questions, meanings, examples, exercises and tests below for Which of the following solutions shows negative deviation from Raoult’s law?a)Acetone and chloroformb)Acetone and carbon disulphidec)Ethyl alcohol and cyclohexaned)Benzene and tolueneCorrect answer is option 'A'. Can you explain this answer?.
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