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How do we compare the degree of intermolecular force that operates in ethanol, to that which operates in glycerol, #"HOH"_2"CCH(OH)CH"_2"OH"#?

Answer 1

Clearly, glycerol, has a higher intermolecular force. There are several metrics we could use to determine this.

Compare the boiling point of ethyl alcohol, #H_3C-CH_2OH#, #"b.p" = 78 ""^@C# to that of glycerol, #"b.p" = 290 ""^@C#. Glycerol also has a much higher melting point (which I've forgotten!), and is much more syrupy and viscous.

Given all of these facts, it seems reasonable to conclude that the intermolecular force acting in glycerol should be significantly larger than that acting in ethyl alcohol, with the tendency of glycerol to form hydrogen bonds acting as the decisive factor.

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Answer 2

Ellie Andrews

The intermolecular forces in glycerol are stronger than those in ethanol due to the presence of three hydroxyl groups in glycerol, leading to more hydrogen bonding opportunities compared to ethanol's single hydroxyl group.

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Answer from HIX Tutor

When evaluating a one-sided limit, you need to be careful when a quantity is approaching zero since its sign is different depending on which way it is approaching zero from. Let us look at some examples.