Why is the melting point of #"isobutane"# LESS than that of #"n-butane"#?
Because the degree of intermolecular force is LESS in isobutane than in butane........
Long chain alkanes can interact chain to chain by (fairly weak) intermolecular dispersion forces; the longer the chain, the greater the intermolecular force and the higher the melting and boiling points. The corresponding boiling points also demonstrate the degree of intermolecular force.
I'm not sure, but you should know what the typical melting and boiling points of butane and isobutane are.
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The melting point of isobutane is lower than that of n-butane because isobutane has a more branched structure, which reduces the strength of intermolecular forces, leading to weaker van der Waals interactions.
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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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