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The melting point of ethane and methane is almost the same.

Ethane - mp = -183 oC

Methane - mp = -182 oC

However, the boiling point of ethane is higher at -88.6 oC compared to methane at -162 oC.

Generally, the larger the molecule the higher the boiling point. This trend can be seen in the hydrocarbon series.

Methane (molar mass, Mr = 16) bp = -162 oC

Ethane (Mr = 30) bp = -88.6 oC

Propane (Mr = 44) bp = -42.2 oC

Butane (58) bp = -0.5 oC

Pentane (72) bp = 36.3 oC

and so on.

The trend is that boiling points increase as size of molecule increases. The intermolecular bonds are stronger as the larger molecules can form temporary electrostatic interaction areas. These intermolecular forces are called van der Waal forces or dispersion forces.

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