From the series, #"butane"#; #"methylbutane"#; #"neopentane"#; #"pentane"#, why does pentane have the highest boiling point?

Answer 1

Why? Because pentane is the most volatile of the given hydrocarbons.

Take into consideration the straight chain alkanes' typical boiling points:

#"n-butane"# #1# #""^@C#;
#"n-pentane"# #35# #""^@C#;
#"n-hexane"# #68# #""^@C#;
#"n-heptane"# #98# #""^@C#;
#"n-nonane"# #151# #""^@C#.
The longer the alkyl chain, the greater the opportunity for Van der Waals interactions between chains. Thus as the chain length increases, the boiling point increases. When crude oil is distilled, they use a fractionating tower that may be many meters high. At appropriate heights in the tower they collect off the fractions that boil between #40-60# #""^@C#, the pentanes, and the isomeric hexanes at #60-80# #""^@C# etc.
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Answer 2

Pentane has the highest boiling point because it has the strongest intermolecular forces due to its longer carbon chain, resulting in greater surface area for van der Waals interactions.

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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.

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.

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.

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.

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