@broken_glassware Which data are you using? If the units are in kilojoules per mole . . . . convert to kilojoules per kilorgram (or per liter) and you’ll see that methanol has higher heat of evaporation per unit mass/volume.
@Rowan I think it’s due to intermolecular forces being stronger with methanol. Here is an explanation that I like. Maybe someone can correct if this seems off:
“The dominant intermolecular force in both cases is the hydrogen bonding through the OH group, this is taken to be of similar strength for both ethanol and methanol as it is localised to the hydroxyl. Methanol, being the smaller molecule, therefore has a larger proportion of its mass (over 50%) in the hydroxyl group and is more polar. Therefore it experiences stronger overall intermolecular electrostatic forces as a function of its mass.”
-https://www.quora.com/What-has-a-higher-IMF-methanol-or-ethanol
However a carbon-carbon bond seems relatively strong to me. I’m calling for a real chemist!