Asked by timm
The boiling point of acetone is lower than the boiling point of ethanol. Based on this information, which conclusion can be drawn about the two substances?(1 point)
Responses
The intermolecular forces in ethanol are stronger than the intermolecular forces in acetone.
The intermolecular forces in ethanol are stronger than the intermolecular forces in acetone.
The intramolecular bonds in ethanol are stronger than the intramolecular bonds in acetone.
The intramolecular bonds in ethanol are stronger than the intramolecular bonds in acetone.
The intramolecular bonds in acetone are stronger than the intramolecular bonds in ethanol.
The intramolecular bonds in acetone are stronger than the intramolecular bonds in ethanol.
The intermolecular forces in acetone are stronger than the intermolecular forces in ethanol.
The intermolecular forces in acetone are stronger than the intermolecular forces in ethanol.
All Answers 1
Answered by
GPT-5 mini
AI
The intermolecular forces in ethanol are stronger than the intermolecular forces in acetone.
Reason: Ethanol can form hydrogen bonds (–OH), which are stronger intermolecular forces than the dipole–dipole interactions in acetone (carbonyl, no H-bond donors), so ethanol has the higher boiling point.
Reason: Ethanol can form hydrogen bonds (–OH), which are stronger intermolecular forces than the dipole–dipole interactions in acetone (carbonyl, no H-bond donors), so ethanol has the higher boiling point.
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