The boiling point of methanol CH3OH is approximately 64.7C 148.5F , while the boiling point of ethanol CH3CH2OH is around 78.4C 173.1F . Ethanol has a higher boiling point compared to methanol.The key factor contributing to the difference in their boiling points is the strength of the intermolecular forces between the molecules. Both methanol and ethanol exhibit hydrogen bonding due to the presence of the hydroxyl group -OH in their structures. Hydrogen bonding is a strong type of dipole-dipole interaction that occurs between a hydrogen atom bonded to a highly electronegative atom such as oxygen and a lone pair of electrons on another electronegative atom.In the case of methanol and ethanol, the difference in boiling points can be attributed to the size and molecular weight of the molecules. Ethanol has a larger molecular size and higher molecular weight than methanol due to the presence of an additional CH2 group. This results in stronger London dispersion forces a type of van der Waals force between ethanol molecules compared to methanol molecules. London dispersion forces are weak intermolecular forces that arise from temporary fluctuations in electron distribution, leading to the formation of temporary dipoles.The combination of hydrogen bonding and stronger London dispersion forces in ethanol leads to a higher boiling point compared to methanol.