The molecular mass of butanol, C4H,OH, is 74.14; that of ethylene glycol, CH2(OH)CH,OH, is 62.08, yet their boiling points are 117.2 °C and 174 °C, respectively. Explain the reason for the difference. The two hydroxyl groups in ethylene glycol provide more locations for the formation of hydrogen bonds. The existence of more hydrogen bonds considerably decreases the boiling point The two hydroxyl groups in ethylene glycol provide less locations for the formation of hydrogen bonds. The existence of less hydrogen bonds considerably increases the boiling point The two hydroxyl groups in ethylene glycol provide more locations for the formation of hydrogen bonds. The existence of more hydrogen bonds considerably increases the boiling point
The molecular mass of butanol, C4H,OH, is 74.14; that of ethylene glycol, CH2(OH)CH,OH, is 62.08, yet their boiling points are 117.2 °C and 174 °C, respectively. Explain the reason for the difference. The two hydroxyl groups in ethylene glycol provide more locations for the formation of hydrogen bonds. The existence of more hydrogen bonds considerably decreases the boiling point The two hydroxyl groups in ethylene glycol provide less locations for the formation of hydrogen bonds. The existence of less hydrogen bonds considerably increases the boiling point The two hydroxyl groups in ethylene glycol provide more locations for the formation of hydrogen bonds. The existence of more hydrogen bonds considerably increases the boiling point
Introductory Chemistry: A Foundation
9th Edition
ISBN:9781337399425
Author:Steven S. Zumdahl, Donald J. DeCoste
Publisher:Steven S. Zumdahl, Donald J. DeCoste
Chapter15: Solutions
Section: Chapter Questions
Problem 20CR
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