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Question

(A) $I$. $C_2H_5OH$: Exhibits strong intermolecular hydrogen bonding,which leads to the highest boiling point.$II$. $C_2H_5Cl$: Exhibits dipole-dipole

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$(III) < (IV) < (II) < (I)$

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(A) $I$. $C_2H_5OH$: Exhibits strong intermolecular hydrogen bonding,which leads to the highest boiling point.$II$. $C_2H_5Cl$: Exhibits dipole-dipole interactions. It is more polar than the ether $(IV)$,resulting in a higher boiling point.$III$. $C_2H_5CH_3$ (Propane): Only weak London dispersion forces exist,leading to the lowest boiling point.$IV$. $C_2H_5OCH_3$ (Methoxyethane): Exhibits weaker dipole-dipole interactions compared to $C_2H_5Cl$.Therefore,the increasing order of boiling points is: $(III) < (IV) < (II) < (I)$.

The increasing order of the boiling points for the following compounds is
$C_2H_5OH$ $(I)$,$C_2H_5Cl$ $(II)$,$C_2H_5CH_3$ $(III)$,$C_2H_5OCH_3$ $(IV)$

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The increasing order of the boiling points for the following compounds is$C_2H_5OH$ $(I)$,$C_2H_5Cl$ $(II)$,$C_2H_5CH_3$ $(III)$,$C_2H_5OCH_3$ $(IV)$