Why does C4H10 have a higher boiling point than CH4?

C4H10 molecule is bigger than CH4, as a result the dispersion forces are more effective because of the bigger surface of butane. Therefore the butane molecules are held together stronger than the methane molecules, and their boiling point is higher. The boiling point of alkanes increases with the number of carbon atoms, that is the larger the number of carbon atoms, the higher the boiling point.

Also, the dispersion forces are more effective at straight chain alkanes, rather than at branched alkanes because the contact surface is bigger in straight chain alkanes.

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RE:

Why does C4H10 have a higher boiling point than CH4?

In terms of bonding and intermolecular forces?

C4h10 Boiling Point

mostly it's because it is a heavier molecule and requires more energy to free itself from the liquid state

and

the intermolecular forces are greater because the heavier molecules have a higher gravitational attraction to each other

It has more bonds, and each bond requires more energy input to break it. Breaking bonds is what allows it to evaporate or boil.

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