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Answered 2011-12-30 18:02:24

The geometric structure of butane allows closer packing between molecules than can be achieved with 2-methylpropane, increasing the total van der Waal's forces in the butane solid and raising its melting point compared with that of 2-methylpropane.

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Why butane has higher melting point than 2-methylpropane?

Both are isomers. As branching increases (as in 2-methylpropane) the intermolecular force of attraction decreases, and hence melting point decreases.


What is the melting and boiling point of butane?

n-butane : Melting point −138.4 °C (135.4 K), boiling at −0.5 °C (272.6 K)iso-butane (methylpropane): Melting point -159.6 °C, (114 K) , boiling at -11.7 °C, (261 K)


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The melting and boiling points are different. Butane has a melting point of 135.4K and 2-methylpropane [isobutane] has a melting point of 114K. The boiling point of Butane is 272.6K and isobutane @ 261K. It has to do with there structures. J



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