Dielectric gas


Dielectric gas

A dielectric gas, or insulating gas, is a dielectric material in gaseous state. Its main purpose is to prevent or rapidly quench electric discharges. Dielectric gases are used as electrical insulators in high voltage applications, e.g. transformers, circuit breakers (namely sulfur hexafluoride circuit breakers), switchgear (namely high voltage switchgear), radar waveguides,

A good dielectric gas should have high dielectric strength, high thermal stability and chemical inertness against the construction materials used, non-flammability and low toxicity, low boiling point, good heat transfer properties, and low cost.[1]

The most common dielectric gas is air, due to its ubiquity and low cost. Another commonly used gas is a dry nitrogen.

In special cases, e.g., high voltage switches, gases with good dielectric properties and very high breakdown voltages are needed. Highly electronegative elements, e.g., halogens, are favored as they rapidly recombine with the ions present in the discharge channel. The halogen gases are highly corrosive. Other compounds, which dissociate only in the discharge pathway, are therefore preferred; sulfur hexafluoride, organofluorides (especially perfluorocarbons) and chlorofluorocarbons are the most common.

The breakdown voltage of gases is roughly proportional to their density. Breakdown voltages also increase with the gas pressure; many gases however have limited upper pressure due to their liquefaction.

The decomposition products of halogenated compounds are highly corrosive, the occurrence of corona discharge should therefore be prevented.[2]

Build-up of moisture can degrade dielectric properties of the gas. Moisture analysis is used for early detection of this.

Dielectric gases can also serve as coolants.

Vacuum is an alternative for gas in some applications.

Mixtures of gases can be used where appropriate. Addition of sulfur hexafluoride can dramatically improve the dielectric properties of poorer insulators, e.g. helium or nitrogen.[3] Multicomponent gas mixtures can offer superior dielectric properties; the optimum mixtures combine the electron attaching gases (sulfur hexafluoride, octafluorocyclobutane) with molecules capable of thermalizing (slowing down) accelerated electrons (e.g. tetrafluoromethane, fluoroform. The insulator properties of the gas are controlled by the combination of electron attachment, electron scattering, and electron ionization.[4]

Atmospheric pressure significantly influences the insulation properties of air. High-voltage applications, e.g. xenon flash lamps, can experience electrical breakdowns at high altitudes.

Relative spark breakdown voltages of insulating gases at 1 atm
Gas Formula Breakdown voltage relative to air Molecular weight (g/mol) Density* (g/l) ODP GWP Properties
Sulfur hexafluoride SF6 3.0 146.06 6.164 22800 The most popular insulating gas. It is dense and rich in fluorine, which is a good discharge quencher. Good cooling properties. Excellent arc quenching. Corrosive decomposition products. Its price increased and supply got limited, as many manufacturing plants switched to production of more profitable perfluorocarbons. The most potent known greenhouse gas with extremely long atmospheric lifetime. Although most of the decomposition products tend to quickly re-form SF6, arcing or corona can produce disulfur decafluoride (S2F10), a highly toxic gas, with toxicity similar to phosgene. Sulfur hexafluoride in an electric arc may also react with other materials and produce toxic compounds, e.g. beryllium fluoride from beryllium oxide ceramics. Frequently used in mixtures with e.g. nitrogen or air.
Nitrogen N2 1.15 28 1.251 Often used at high pressure. Does not facilitate combustion. Can be used with 10–20% of SF6 as a lower-cost alternative to SF6. Can be used standalone or in combination with CO2.
Air 29/mixture 1 1.2 Breakdown voltage 30 kV/cm at 1 atm. Very well-researched. When subjected to an electrical discharge, forms corrosive nitrogen oxides and other compounds, especially in presence of water. Corrosive decomposition products. Can facilitate combustion, especially when compressed.
Ammonia NH3 1 17.031 0.86
Carbon dioxide CO2 0.95 44.01 1.977 1
Hydrogen sulfide H2S 0.9 34.082 1.363
Oxygen O2 0.85 32.0 1.429 Very effectively facilitates combustion.
Chlorine Cl2 0.85 70.9 3.2
Hydrogen H2 0.65 2.016 0.09 Low breakdown voltage but high thermal capacity and very low viscosity. Used for cooling of e.g. hydrogen-cooled turbogenerators. Handling and safety problems. Very fast deexcitation, can be used in high repetition rate spark gaps and fast thyratrons.
Sulfur dioxide SO2 0.30 64.07 2.551
1,2-Dichlorotetrafluoroethane (R-114) CF2ClCF2Cl 3.2 170.92 1.455  ? Saturated pressure at 23 °C is about 2 atm, yielding breakdown voltage 5.6 times higher than nitrogen at 1 atm. Corrosive decomposition products.
Dichlorodifluoromethane (R-12) CF2Cl2 2.9 120.91 6 1 8100 Vapor pressure 90 psi (6.1 atm) at 23 °C, yielding breakdown voltage 17 times higher than air at 1 atm. Yet higher breakdown voltages can be achieved by increasing pressure by adding nitrogen. Corrosive decomposition products.
1,1,1,3,3,3-Hexafluoropropane (R-236fa) CF3CH2CF3 152.05 6300 Corrosive decomposition products.
Carbon tetrafluoride (R-14) CF4 1.01[1] 88.0 3.72 6500 Poor insulator when used alone. In mixture with SF6 somewhat decrases sulfur hexafluoride's dielectric properties, but significantly lowers the mixture's boiling point and prevents condensation at extremely low temperatures. Lowers the cost, toxicity and corrosiveness of pure SF6.[5]
Hexafluoroethane (R-116) C2F6 2.02[1] 138 5.734 9200
Perfluoropropane (R-218) C3F8 2.2[1] 188 8.17  ?
Octafluorocyclobutane (R-C318) C4F8 3.6[1] 200 7.33  ? Possible alternative of SF6.
Perfluorobutane (R-3-1-10) C4F10 2.6[1] 238 11.21  ?
30% SF6/70% air 2.0[1]

* the density is approximate; it is normally specified at atmospheric pressure, the temperature may vary, though it is mostly 0 °C.

References

  1. ^ a b c d e f g M S Naidu; NAIDU M S (22 November 1999). High Voltage Engineering. McGraw-Hill Professional. pp. 35–. ISBN 9780071361088. http://books.google.com/books?id=RF-MvfqYMagC&pg=PA35. Retrieved 17 April 2011. 
  2. ^ About HV Devices-04
  3. ^ Paul G. Slade (2008). The vacuum interrupter: theory, design, and application. CRC Press. pp. 433–. ISBN 9780849390913. http://books.google.com/books?id=uJT4mENgMbQC&pg=PA433. Retrieved 17 April 2011. 
  4. ^ Ramapriya Parthasarathy Use of Rydberg Atoms as a Microscale Laboratory to Probe Low-Energy Electron-Molecule Interactions
  5. ^ Loucas G. Christophorou; James K. Olthoff (1 January 1998). Gaseous Dielectrics VIII. Springer. pp. 45–. ISBN 9780306460562. http://books.google.com/books?id=1fgjnGtAdSkC&pg=PA45. Retrieved 17 April 2011. 

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