Boiling point

Figure 1. Water has a boiling point of 100oC at sea level pressure conditions.[1]

Boiling point is the temperature that a liquid will change phase into a gas. Boiling occurs when the vapor pressure of a liquid is equal to the atmospheric pressure of the gas outside of it. Because of this, as the outside pressure changes so does the boiling point of the liquid. Therefore there is a set pressure known as a standard atmosphere (atm) which determines what is called the normal boiling point of a liquid. For example, water's normal boiling point is 100oC, which occurs when the atmospheric pressure is exactly 1 atm. If the atmospheric pressure is less than 1 atm, the boiling point of the liquid will decrease, as is the case at higher altitudes on Earth. And if the atmospheric pressure is greater than 1 atm, such as in a pressure cooker, the boiling point will begin to increase drastically.[2]

If a liquid is undergoing a phase change, its temperature will not increase until it is done.[3] This is known as latent heat, and is common among all phase changes.

Another factor that determines the boiling point is molecular bonds, structure and composition. If the intermolecular forces in a liquid are relatively strong, the boiling point will be relatively high, and if the forces are relatively weak the boiling point will be relatively low.[2] For example, Ammonia has a very low boiling point, at -35.5oC, while mercury has a boiling point of 356.9oC.[4]


  1. Wikimedia Commons [Online], Available:
  2. 2.0 2.1 Purdue Chemistry, Boiling [Online], Available:
  3. Hyperphysics, Boiling point [Online], Available;
  4. Engineering toolbox, Boiling Points of some common Fluids and Gases [Online], Available:

Authors and Editors

Jordan Hanania, Kailyn Stenhouse, Jason Donev
Last updated: September 18, 2015
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