Asked by puyr
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)
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 acetone are stronger than the intramolecular bonds 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: Boiling point reflects how strong the intermolecular forces are. Ethanol can hydrogen-bond (–OH), giving stronger intermolecular attraction than acetone’s dipole–dipole/London forces, so ethanol has the higher boiling point.
Reason: Boiling point reflects how strong the intermolecular forces are. Ethanol can hydrogen-bond (–OH), giving stronger intermolecular attraction than acetone’s dipole–dipole/London forces, so ethanol has the higher boiling point.
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