(Solved): How does water (H2O) compare to methane (CH4) ? They have similar molecular masses, but because H2O ...

How does water $$(\mathrm{H}2\mathrm{O})$$ compare to methane $$(\mathrm{CH}4)$$ ? They have similar molecular masses, but because $$\mathrm{H}2\mathrm{O}$$ has a much higher boiling point due to hydrogen bonding. Because water has a heavier molecular mass it has a higher boiling point. They have similar molecular masses, but methane is more volatile and so has a higher boiling point. Water has a higher boiling point because the van de Waals forces in methane push the molecules apart. The low dielectric constant of methane compared to water raises its boiling point.