Boiling Point
| Formula / Notation | P_vapour = P_external (at T_b) |
|---|---|
| Also Known As | Boiling temperature, vaporisation point, normal boiling point (at 1 atm) |
What is Boiling Point?
The boiling point of a liquid is the temperature at which its vapour pressure equals the atmospheric pressure, causing the liquid to vaporise throughout its volume. The normal boiling point is measured at 1 atm (101.325 kPa). Boiling point depends on the strength of intermolecular forces and applied pressure; substances with stronger intermolecular forces have higher boiling points.
Formula & Notation
Other Names / Synonyms: Boiling temperature, vaporisation point, normal boiling point (at 1 atm)
Properties & Characteristics
Uses & Applications
Safety Information
Always consult the SDS/MSDS before handling any chemical. This information is for educational purposes only.
Key Facts
Frequently Asked Questions
The boiling point of a liquid is the temperature at which its vapour pressure equals the atmospheric pressure, causing the liquid to vaporise throughout its volume. The normal boiling point is measured at 1 atm (101.325 kPa). Boiling point depends on the strength of intermolecular forces and applied pressure; substances with stronger intermolecular forces have higher boiling points.
Boiling points are used to characterise and identify substances, design separation processes (fractional distillation), set process temperatures in chemical engineering, and determine the boiling points of mixtures using Raoult's law. They are key data in thermodynamic databases.
Boiling liquids pose serious burn hazards from hot vapour and splashing. Superheating (heating liquid above its boiling point without nucleation) can cause explosive bumping; add boiling chips to prevent this. Always use heat-resistant glassware rated for the temperature involved.
The formula or notation for Boiling Point is: P_vapour = P_external (at T_b)