The boiling point of methane (CH₄) is significantly lower than that of water (H₂O).
Methane has a boiling point of approximately -161.5°C (-258.7°F), while water has a boiling point of 100°C (212°F) at standard atmospheric pressure. The main reason for this difference is the nature of the intermolecular forces present in the two substances.
Water exhibits hydrogen bonding due to the polarity of its molecules, which leads to a relatively high boiling point. In contrast, methane is a nonpolar molecule and primarily experiences weaker London dispersion forces. As a result, it requires much less energy (in the form of heat) to break the intermolecular forces in methane, leading to its much lower boiling point.
In summary, methane's boiling point is much lower than that of water due to differences in molecular structure and the types of intermolecular forces at play.