Question:
Ethanol + Water shows:
Ethanol + Water shows:
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Weak interactions = Happy to leave (Vaporize) = Positive Pressure Deviation.
Updated On: May 5, 2026
- Negative deviation from Raoult's law
- Zero deviation (ideal)
- Positive deviation from Raoult's law
- Azeotrope from start
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The Correct Option is C
Solution and Explanation
Step 1: Concept
Raoult's Law describes ideal solutions where interactions between different molecules ($A-B$) are identical to interactions between similar molecules ($A-A$ or $B-B$).
Step 2: Meaning
Positive deviation occurs when the $A-B$ attractive forces are weaker than the original $A-A$ and $B-B$ forces, causing more molecules to escape into the vapor phase.
Step 3: Analysis
In a mixture of ethanol and water, the molecules interfere with each other's hydrogen bonding networks. The resulting total vapor pressure of the solution is higher than predicted by Raoult's law.
Step 4: Conclusion
Since the unlike-molecule interactions are weaker than the like-molecule interactions, the system exhibits positive deviation. Final Answer: (C)
Raoult's Law describes ideal solutions where interactions between different molecules ($A-B$) are identical to interactions between similar molecules ($A-A$ or $B-B$).
Step 2: Meaning
Positive deviation occurs when the $A-B$ attractive forces are weaker than the original $A-A$ and $B-B$ forces, causing more molecules to escape into the vapor phase.
Step 3: Analysis
In a mixture of ethanol and water, the molecules interfere with each other's hydrogen bonding networks. The resulting total vapor pressure of the solution is higher than predicted by Raoult's law.
Step 4: Conclusion
Since the unlike-molecule interactions are weaker than the like-molecule interactions, the system exhibits positive deviation. Final Answer: (C)
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