Question

Assertion (A): The boiling point of ethanol is higher than that of methoxymethane. 
Reason (R): There is intramolecular hydrogen bonding in ethanol. 

• A. Both Assertion (A) and Reason (R) are true and Reason (R) is the correct explanation of the Assertion (A).
• B. Both Assertion (A) and Reason (R) are true, but Reason (R) is not the correct explanation of the Assertion (A).
• C. Assertion (A) is true, but Reason (R) is false.
• D. Assertion (A) is false, but Reason (R) is true.

Hint:

Hydrogen bonding increases the boiling point of compounds as it requires more energy to break these bonds.

Answer 1

The Correct Option is C

Ethanol vs. Methoxymethane Boiling Point Analysis

Step 1: Comprehending Boiling Point Differences. Ethanol exhibits a higher boiling point than methoxymethane. This is attributable to intermolecular hydrogen bonding present in ethanol molecules, which necessitates greater energy input to overcome these intermolecular forces.

Step 2: Elucidating the Cause of Boiling Point Variance. The higher boiling point of ethanol, relative to methoxymethane, stems from its capacity for intermolecular hydrogen bonding, a characteristic absent in methoxymethane.

Step 3: Final Determination. Given that both the Assertion (A) and the Reason (R) are factually correct, and that Reason (R) accurately provides the rationale for Assertion (A), option (A) is the designated correct response.