Intermolecular forces

Dipole-induced dipole interaction occurs between a polar and a non-polar species.
HCl is polar ($\mu \ne 0$) and He is non-polar ($\mu = 0$).

Vaporisation separates the molecules from one another; the covalent bonds within each molecule are not broken.
In methanol, hydrogen is bonded to the highly electronegative oxygen atom, so the molecules are associated through intermolecular hydrogen bonds (O–H···O).
Hydrogen bonding is much stronger than the ordinary dipole–dipole and London dispersion forces that are also present.
This is why methanol has a much higher boiling point than compounds of similar molar mass that cannot form hydrogen bonds.
Hence the dominant force to be overcome is hydrogen bonding.