Explain why propanol has a higher boiling point than that of the hydrocarbon,butane?
(N/A) Propanol $(CH_3CH_2CH_2OH)$ undergoes intermolecular hydrogen bonding due to the presence of the polar $-OH$ group.
On the other hand,butane $(C_4H_{10})$ is a non-polar hydrocarbon and only exhibits weak van der Waals forces.
Because of the strong intermolecular hydrogen bonds in propanol,extra energy is required to overcome these forces during the phase transition.
Therefore,propanol has a significantly higher boiling point than butane.
On the other hand,butane $(C_4H_{10})$ is a non-polar hydrocarbon and only exhibits weak van der Waals forces.
Because of the strong intermolecular hydrogen bonds in propanol,extra energy is required to overcome these forces during the phase transition.
Therefore,propanol has a significantly higher boiling point than butane.
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