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The chemical potential of a species in a mixture is defined as ... [13] Therefore, the total chemical potential can be split into internal chemical potential and ...
The relative activity of a species i, denoted a i, is defined [4] [5] as: = where μ i is the (molar) chemical potential of the species i under the conditions of interest, μ o i is the (molar) chemical potential of that species under some defined set of standard conditions, R is the gas constant, T is the thermodynamic temperature and e is the exponential constant.
In thermodynamics, an activity coefficient is a factor used to account for deviation of a mixture of chemical substances from ideal behaviour. [1] In an ideal mixture, the microscopic interactions between each pair of chemical species are the same (or macroscopically equivalent, the enthalpy change of solution and volume variation in mixing is zero) and, as a result, properties of the mixtures ...
As originally formulated by Benjamin Widom in 1963, [1] the approach can be summarized by the equation: = = where is called the insertion parameter, is the number density of species , is the activity of species , is the Boltzmann constant, and is temperature, and is the interaction energy of an inserted particle with all other particles in the system.
Molar Gibbs free energy is commonly referred to as chemical potential, symbolized by , particularly when discussing a partial molar Gibbs free energy for a component in a mixture. For the characterization of substances or reactions, tables usually report the molar properties referred to a standard state .
where μ is the chemical potential, μ 0 is the standard value of the chemical potential. The expression = is the so-called activity. It measures the "effective concentration" of a species in a non-ideal mixture.
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