Chemistry 20?

Both ethanol and methane are molecular compounds. When each compound boils, heat is absorbed to break the intermolecular forces.

The intermolecular forces between methanol molecules are hydrogen bonds as shown in the figure below. Ethane are non-polar compound and thus the intermolecular forces between methane molecules are London dispersion forces. Between molecules in similar sizes, hydrogen bonds are stronger than London dispersion forces. Therefore, more heat is needed to break the hydrogen bonds between methanol molecules, and thus methanol has a higher boiling point.

Jay was misleading.

The O-H bond in methane is a covalent bond,  Ut is strong, but is nt hydrogen bonding.  H from one molecule of methanol is attracted to an O of a different methanol molecule.  This is done over and over with many molecules.  This makes it harder for a methanol molecule t break away == boil.   Ethane has NO oxygen so this kind of attractin does not ocur.  Single molecules of ethane can easily break away fro the other molecules (boiling)  ===  

The reason that the boiling point of methanol is much higher than ethane is because of the Hydrogen bonding of the O and the H in the methanol molecule. Ethane is just a series of neutral carbon bonds to Hydrogen, therefore requiring much less energy to liberate in breaking their bonds (turning them to liquid). :)