Which of the following is correct?

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(D) Let us analyze each option:$A$: $n$-pentane is a non-polar alkane,while diethyl ether is polar due to the $C-O-C$ bond. Thus,diethyl ether has a h

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Resonance energy $\Rightarrow$ phenyl cation $>$ cyclohexadienyl cation

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(D) Let us analyze each option:$A$: $n$-pentane is a non-polar alkane,while diethyl ether is polar due to the $C-O-C$ bond. Thus,diethyl ether has a higher boiling point than $n$-pentane. This statement is incorrect.$B$: Solubility in water depends on the extent of hydrogen bonding and the hydrophobic alkyl chain. $n$-butyl alcohol has a straight chain,while isobutyl alcohol is branched. Branching reduces the surface area,making the hydrophobic part less effective,thus increasing solubility. Therefore,isobutyl alcohol is more soluble than $n$-butyl alcohol. This statement is incorrect.$C$: $o$-nitrophenol exhibits intramolecular hydrogen bonding,which reduces intermolecular forces,leading to a lower boiling point. $p$-nitrophenol exhibits intermolecular hydrogen bonding,leading to higher boiling points due to association. Thus,$p$-nitrophenol $>$ $o$-nitrophenol. This statement is incorrect.$D$: The phenyl cation is an aromatic species ($H$ückel's rule: $6\pi$ electrons),which is significantly stabilized by resonance. The cyclohexadienyl cation is a non-aromatic conjugated system. Aromatic systems have much higher resonance energy than non-aromatic conjugated systems. Therefore,the resonance energy of the phenyl cation is greater than that of the cyclohexadienyl cation. This statement is correct.

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