Question:
Two statements are given below:
Statement - I: Liquids A and B form a non-ideal solution with positive deviation. The interactions between A and B are weaker than A-A and B-B interactions.
Statement - II: For an ideal solution, \( \Delta H_{\text{mix}} = 0 \), \( \Delta V_{\text{mix}} = 0 \).
The correct answer is
Two statements are given below:
Statement - I: Liquids A and B form a non-ideal solution with positive deviation. The interactions between A and B are weaker than A-A and B-B interactions.
Statement - II: For an ideal solution, \( \Delta H_{\text{mix}} = 0 \), \( \Delta V_{\text{mix}} = 0 \).
The correct answer is
Statement - I: Liquids A and B form a non-ideal solution with positive deviation. The interactions between A and B are weaker than A-A and B-B interactions.
Statement - II: For an ideal solution, \( \Delta H_{\text{mix}} = 0 \), \( \Delta V_{\text{mix}} = 0 \).
The correct answer is
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For non-ideal solutions with positive deviation, A and B have weaker interactions than A-A and B-B, resulting in a positive heat of mixing.
Updated On: Mar 13, 2025
- Both Statements - I and Statement - II are correct
- Both Statements - I and Statement - II are not correct
- Statement - I is correct but Statement - II is not correct
- Statement - I is not correct but Statement - II is correct
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The Correct Option is A
Solution and Explanation
- Statement - I is correct because when A and B form a non-ideal solution with positive deviation, it implies that the interactions between A and B are weaker than the A-A and B-B interactions.
- Statement - II is also correct for an ideal solution where both enthalpy and volume changes are zero.
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