Mass diffusivity
Diffusivity or diffusion coefficient is a proportionality constant between the molar flux due to molecular diffusion and the gradient in the concentration of the species (or the driving force for diffusion). Diffusivity is encountered in Fick's law and numerous other equations of physical chemistry.
The diffusivity is generally prescribed for a given pair of species and pairwise for a multi-species system. The higher the diffusivity (of one substance with respect to another), the faster they diffuse into each other. Typically, a compound's diffusion coefficient is ~10,000× as great in air as in water. Carbon dioxide in air has a diffusion coefficient of 16 mm2/s, and in water its diffusion coefficient is 0.0016 mm2/s.[1][2]
Diffusivity has an SI unit of m2/s (length2 / time). In CGS units it is given in cm2/s.
Temperature dependence of the diffusion coefficient
Solids
The diffusion coefficient in solids at different temperatures is generally found to be well predicted by the Arrhenius equation:
where
- D is the diffusion coefficient (m2/s),
- D0 is the maximal diffusion coefficient (at infinite temperature; m2/s),
- EA is the activation energy for diffusion in dimensions of (J/atom),
- T is the absolute temperature (K),
- k is the Boltzmann constant.
Liquids
An approximate dependence of the diffusion coefficient on temperature in liquids can often be found using Stokes–Einstein equation, which predicts that
where
- D is the diffusion coefficient,
- T1 and T2 are the corresponding absolute temperatures,
- μ is the dynamic viscosity of the solvent.
Gases
The dependence of the diffusion coefficient on temperature for gases can be expressed using Chapman–Enskog theory (predictions accurate on average to about 8%):[3]
where
- D is the diffusion coefficient (cm2/s),[3][4]
- 1 and 2 index the two kinds of molecules present in the gaseous mixture,
- T is the absolute temperature (K),
- M is the molar mass (g/mol),
- p is the pressure (atm),
- is the average collision diameter (the values are tabulated[5]) (Å),
- Ω is a temperature-dependent collision integral (the values are tabulated[5] but usually of order 1) (dimensionless).
Pressure dependence of the diffusion coefficient
For self-diffusion in gases at two different pressures (but the same temperature), the following empirical equation has been suggested:[3]
where
- D is the diffusion coefficient,
- ρ is the gas mass density,
- P1 and P2 are the corresponding pressures.
Effective diffusivity in porous media
The effective diffusion coefficient describes diffusion through the pore space of porous media.[6] It is macroscopic in nature, because it is not individual pores but the entire pore space that needs to be considered. The effective diffusion coefficient for transport through the pores, De, is estimated as follows:
where
- D is the diffusion coefficient in gas or liquid filling the pores,
- εt is the porosity available for the transport (dimensionless),
- δ is the constrictivity (dimensionless),
- τ is the tortuosity (dimensionless).
The transport-available porosity equals the total porosity less the pores which, due to their size, are not accessible to the diffusing particles, and less dead-end and blind pores (i.e., pores without being connected to the rest of the pore system). The constrictivity describes the slowing down of diffusion by increasing the viscosity in narrow pores as a result of greater proximity to the average pore wall. It is a function of pore diameter and the size of the diffusing particles.
Example values
Gases at 1 atm., solutes in liquid at infinite dilution. Legend: (s) – solid; (l) – liquid; (g) – gas; (dis) – dissolved.
| Species pair (solute – solvent) | Temperature (°C) | D (cm2/s) | Reference |
|---|---|---|---|
| Water (g) – air (g) | 25 | 0.282 | [3] |
| Oxygen (g) – air (g) | 25 | 0.176 | [3] |
| Species pair (solute – solvent) | Temperature (°C) | D (cm2/s) | Reference |
|---|---|---|---|
| Acetone (dis) – water (l) | 25 | 1.16×10−5 | [3] |
| Air (dis) – water (l) | 25 | 2.00×10−5 | [3] |
| Ammonia (dis) – water (l) | 25 | 1.64×10−5 | [3] |
| Argon (dis) – water (l) | 25 | 2.00×10−5 | [3] |
| Benzene (dis) – water (l) | 25 | 1.02×10−5 | [3] |
| Bromine (dis) – water (l) | 25 | 1.18×10−5 | [3] |
| Carbon monoxide (dis) – water (l) | 25 | 2.03×10−5 | [3] |
| Carbon dioxide (dis) – water (l) | 25 | 1.92×10−5 | [3] |
| Chlorine (dis) – water (l) | 25 | 1.25×10−5 | [3] |
| Ethane (dis) – water (l) | 25 | 1.20×10−5 | [3] |
| Ethanol (dis) – water (l) | 25 | 0.84×10−5 | [3] |
| Ethylene (dis) – water (l) | 25 | 1.87×10−5 | [3] |
| Helium (dis) – water (l) | 25 | 6.28×10−5 | [3] |
| Hydrogen (dis) – water (l) | 25 | 4.50×10−5 | [3] |
| Hydrogen sulfide (dis) – water (l) | 25 | 1.41×10−5 | [3] |
| Methane (dis) – water (l) | 25 | 1.49×10−5 | [3] |
| Methanol (dis) – water (l) | 25 | 0.84×10−5 | [3] |
| Nitrogen (dis) – water (l) | 25 | 1.88×10−5 | [3] |
| Nitric oxide (dis) – water (l) | 25 | 2.60×10−5 | [3] |
| Oxygen (dis) – water (l) | 25 | 2.10×10−5 | [3] |
| Propane (dis) – water (l) | 25 | 0.97×10−5 | [3] |
| Water (l) – acetone (l) | 25 | 4.56×10−5 | [3] |
| Water (l) – ethyl alcohol (l) | 25 | 1.24×10−5 | [3] |
| Water (l) – ethyl acetate (l) | 25 | 3.20×10−5 | [3] |
| Species pair (solute – solvent) | Temperature (°C) | D (cm2/s) | Reference |
|---|---|---|---|
| Hydrogen – iron (s) | 10 | 1.66×10−9 | [3] |
| Hydrogen – iron (s) | 100 | 124×10−9 | [3] |
| Aluminium – copper (s) | 20 | 1.3×10−30 | [3] |
See also
References
- ↑ CRC Press Online: CRC Handbook of Chemistry and Physics, Section 6, 91st Edition
- ↑ Diffusion
- 1 2 3 4 5 6 7 8 9 10 11 12 13 14 15 16 17 18 19 20 21 22 23 24 25 26 27 28 29 30 31 32 Cussler, E. L. (1997). Diffusion: Mass Transfer in Fluid Systems (2nd ed.). New York: Cambridge University Press. ISBN 0-521-45078-0.
- ↑ Welty, James R.; Wicks, Charles E.; Wilson, Robert E.; Rorrer, Gregory (2001). Fundamentals of Momentum, Heat, and Mass Transfer. Wiley. ISBN 978-0-470-12868-8.
- 1 2 Hirschfelder, J.; Curtiss, C. F.; Bird, R. B. (1954). Molecular Theory of Gases and Liquids. New York: Wiley. ISBN 0-471-40065-3.
- ↑ Grathwohl, P. (1998). Diffusion in natural porous media: Contaminant transport, sorption / desorption and dissolution kinetics. Kluwer Academic. ISBN 0-7923-8102-5.