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Intensive and extensive properties

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Intensive and extensive properties

Physical properties of materials and systems are often described as intensive and extensive properties. This classification relates to the dependency of the properties upon the size or extent of the system or object in question.

The distinction is based on the concept that smaller, non-interacting identical subdivisions of the system may be identified so that the property of interest does or does not change when the system is divided or combined.

An intensive property is a bulk property, meaning that it is a physical property of a system that does not depend on the system size or the amount of material in the system. Examples of intensive properties include temperature, refractive index, density, and hardness of an object. When a diamond is cut, the pieces maintain their intrinsic hardness (until their size reaches a few atoms thick).

By contrast, an extensive property is additive for independent, non-interacting subsystems.[1] The property is proportional to the amount of material in the system. For example, both the mass and the volume of a diamond are directly proportional to the amount that is left after cutting it from the raw mineral. Mass and volume are extensive properties, but hardness is intensive.

The ratio of two extensive properties of the same object or system is scale-invariant, and is therefore an intensive property. For example, the ratio of the extensive properties mass and volume, the density, is an intensive property.

This terminology of intensive and extensive properties was introduced by Richard C. Tolman in 1917.[2]


  • Intensive properties 1
    • Combined intensive properties 1.1
    • Examples 1.2
  • Extensive properties 2
    • Combined extensive properties 2.1
    • Examples 2.2
  • Related extensive and intensive properties 3
  • Generality of classification 4
  • References 5

Intensive properties

An intensive property is a physical quantity whose value does not depend on the amount of the substance for which it is measured. For example, the temperature of a system in thermal equilibrium is the same as the temperature of any part of it. If the system is divided the temperature of each subsystem is identical. The same applies to the density of a homogeneous system; if the system is divided in half, the mass and the volume change in the identical ratio and the density remains unchanged. Additionally, the boiling point of a substance is another example of an intensive property. For example, the boiling point for water is 100 °C at a pressure of one atmosphere, which remains true regardless of quantity.

According to the state postulate, a sufficiently simple thermodynamic system requires only two independent intensive variables to fully specify the system's entire state. Other intensive properties are derived from the two known values.

Some intensive properties, such as viscosity, are empirical macroscopic quantities and are not relevant to extremely small systems.

Combined intensive properties

There are four properties in any thermodynamic system, two are intensive and two are extensive.

If the set of parameters, \{a_i\}, are intensive properties and another set, \{A_j\}, are extensive properties, then the function F(\{a_i\},\{A_j\}) is an intensive property if for all \alpha,

F(\{a_i\},\{\alpha A_j\}) = F(\{a_i\},\{A_j\}).\,

It follows, for example, that the ratio of two extensive properties is an intensive property - density (intensive) is equal to mass (extensive) divided by volume (extensive).


Examples of intensive properties include:

Extensive properties

The IUPAC Green Book defines an extensive property as a physical quantity that is the sum of the properties of separate non-interacting subsystems that compose the entire system.[1] The value of such an additive property is proportional to the size of the system it describes, or to the quantity of matter in the system. Taking on the example of melting ice, the amount of heat required to melt ice is an extensive property. The amount of heat required to melt one ice cube would be much less than the amount of heat required to melt an iceberg, so it is dependent on the quantity.

Extensive properties are the counterparts of intensive properties, which are intrinsic to a particular subsystem. Dividing one type of extensive property by a different type of extensive property generally gives an intensive value—for example: mass (extensive) divided by volume (extensive) gives density (intensive).

Combined extensive properties

If a set of parameters \{a_i\} are intensive properties and another set \{A_j\} are extensive properties, then the function F(\{a_i\},\{A_j\}) is an extensive property if for all \alpha,

F(\{a_i\},\{\alpha A_j\})=\alpha F(\{a_i\},\{A_j\}).\,

Thus, extensive properties are homogeneous functions (of degree 1) with respect to \{A_j\}. It follows from Euler's homogeneous function theorem that

F(\{a_i\},\{A_j\})=\sum_j A_j \left(\frac{\partial F}{\partial A_j}\right),

where the partial derivative is taken with all parameters constant except A_j. The converse is also true: any function that obeys the above relationship is extensive.


Examples of extensive properties include:

Related extensive and intensive properties

Although not true for all physical properties, some properties have corresponding extensive and intensive analogs, many of which are thermodynamic properties. Examples of such extensive thermodynamic properties, that are dependent on the size of the thermodynamic system in question, include volume, internal energy, enthalpy, entropy, Gibbs free energy, Helmholtz free energy, and heat capacity (in the sense of thermal mass). The symbols of these extensive thermodynamic properties shown here are capital letters.

For homogeneous substances, these extensive thermodynamic properties each have corresponding intensive thermodynamic properties, which are expressed on a per mass or volume basis. The name is usually prefixed with the adjective specific to indicate that they are bulk properties, valid at any location (smaller subdivision) in a thermodynamic system. They may be dependent on other conditions at any point, such as temperature, pressure, and material composition, but are not considered dependent on the size of a thermodynamic system or on the amount of material in the system.

Specific volume is volume per mass—the reciprocal of density, which equals mass per volume.

Corresponding extensive and intensive thermodynamic properties
Symbol SI units Intensive
Symbol SI units
m3 or L*
Specific volume***
m3/kg or L*/kg
Internal energy
Specific internal energy
Specific entropy
Specific enthalpy
Gibbs free energy
Specific Gibbs free energy
Heat capacity
at constant volume
Specific heat capacity
at constant volume
Heat capacity
at constant pressure
Specific heat capacity
at constant pressure
* L = liter, J = joule
** specific properties, expressed on a per mass basis
*** Specific volume is the reciprocal of density.

If a molecular weight can be assigned for the substance, or the amount of substance (in moles) can be determined, then each of these thermodynamic properties may be expressed on a molar basis, and their name may be qualified with the adjective molar, yielding terms such as molar volume, molar internal energy, molar enthalpy, molar entropy. Standards for the symbols of molar quantities do not exist. A well known molar volume is that of an ideal gas at standard conditions for temperature and pressure, with the value 22.41liters/mol. Molar Gibbs free energy is commonly referred to as chemical potential, symbolized by μ, particularly when discussing a partial molar Gibbs free energy μi for a component i in a mixture.

Generality of classification

The general validity of the division of physical properties into extensive and intensive kinds has been addressed in the course of science.[3] Redlich noted that physical properties and especially thermodynamic properties are most conveniently defined as either intensive or extensive,[2] however, these two categories are not all-inclusive and some well-defined physical properties conform to neither definition. Redlich also provides examples of mathematical functions that alter the strict additivity relationship for extensive system, such as the square or square root of volume, which occur in some contexts, altbeit rarely used.[2]

Other systems, for which standard definitions do not provide a simple answer, are systems in which the subsystems interact when combined. Redlich pointed out that the assignment of some properties as intensive or extensive may depend on the way subsystems are arranged. For example, if two identical galvanic cells are connected in parallel, the voltage of the system is equal to the voltage of each cell, while the electric charge transferred (or the electric current) is extensive. However if the same cells are connected in series, the charge becomes intensive and the voltage extensive.[2] The IUPAC definitions do not consider such cases.[1]


  1. ^ a b c IUPAC Green Book Quantities, Units and Symbols in Physical Chemistry (3rd edn. 2007), page 6 (page 20 of 250 in PDF file)
  2. ^ a b c d O. Redlich, Journal of chemical education, 47, 154-156 (1970)
  3. ^ Hatsopoulos G.N. and Keenan J.H. Principles of general thermodynamics, John Wiley and Sons 1965 p.19-20
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