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Claus process

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Claus process

Piles of sulfur produced in Alberta by the Claus process awaiting shipment at docks in Vancouver, Canada.

The Claus process is the most significant gas desulfurizing process, recovering elemental sulfur from gaseous hydrogen sulfide. First patented in 1883 by the chemist Carl Friedrich Claus, the Claus process has become the industry standard. C. F. Claus was born in Kassel in the German State of Hessen in 1827, and studied chemistry in Marburg before he emigrated to England in 1852. Claus died in London in the year 1900.[1]

The multi-step Claus process recovers sulfur from the gaseous hydrogen sulfide found in raw natural gas and from the by-product gases containing hydrogen sulfide derived from refining crude oil and other industrial processes. The by-product gases mainly originate from physical and chemical gas treatment units (Selexol, Rectisol, Purisol and amine scrubbers) in refineries, natural gas processing plants and gasification or synthesis gas plants. These by-product gases may also contain hydrogen cyanide, hydrocarbons, sulfur dioxide or ammonia.

Gases with an H2S content of over 25% are suitable for the recovery of sulfur in straight-through Claus plants while alternate configurations such as a split-flow set up or feed and air preheating can be used to process leaner feeds.[2]

Hydrogen sulfide produced, for example, in the hydro-desulfurization of refinery naphthas and other petroleum oils, is converted to sulfur in Claus plants.[3] The overall main reaction equation is:

2 H2S + O2 → 2 S + 2 H2O

The vast majority of the 64,000,000 metric tons of sulfur produced worldwide in 2005 was byproduct sulfur from refineries and other hydrocarbon processing plants.[4][5][6] Sulfur is used for manufacturing sulfuric acid, medicine, cosmetics, fertilizers and rubber products. Elemental sulfur is used as fertilizer and pesticide.


  • History 1
  • Process description 2
    • Thermal step 2.1
      • Side reactions 2.1.1
      • Detailed chemical kinetic modeling 2.1.2
    • Catalytic step 2.2
    • Sub dew point Claus process 2.3
  • Process performance 3
  • See also 4
  • References 5


The process was invented by Carl Friedrich Claus, a chemist working in England. A British patent was issued to him in 1883. The process was later significantly modified by a German company called IG Farben[7]

Process description

A schematic process flow diagram of a basic 2+1-reactor (converter) SuperClaus unit is shown below:

Schematic flow diagram of a straight-through, 3 reactor (converter), Claus sulfur recovery unit.

The Claus technology can be divided into two process steps, thermal and catalytic.

Thermal step

In the thermal step, hydrogen sulfide-laden gas reacts in a substoichiometric combustion at temperatures above 850 °C [8] such that elemental sulfur precipitates in the downstream process gas cooler.

The H2S content and the concentration of other combustible components (hydrocarbons or ammonia) determine the location where the feed gas is burned. Claus gases (acid gas) with no further combustible contents apart from H2S are burned in lances surrounding a central muffle by the following chemical reaction:

2 H2S + 3 O2 → 2 SO2 + 2 H2O       (ΔH = -4147.2 kJ mol−1)

This is a strongly exothermic free-flame total oxidation of hydrogen sulfide generating sulfur dioxide that reacts away in subsequent reactions. The most important one is the Claus reaction:

2 H2S + SO2 → 3 S + 2 H2O

The overall equation is:[6]

10 H2S + 5 O2 → 2 H2S + SO2 + 7/2 S2 + 8 H2O

This equation shows that in the thermal step alone two-thirds of the hydrogen sulfide can be converted to sulfur.

Gases containing ammonia, such as the gas from the refinery's sour water stripper (SWS), or hydrocarbons are converted in the burner muffle. Sufficient air is injected into the muffle for the complete combustion of all hydrocarbons and ammonia. The air to the acid gas ratio is controlled such that in total 1/3 of all hydrogen sulfide (H2S) is converted to SO2. This ensures a stoichiometric reaction for the Claus reaction in the second catalytic step (see next section below).

The separation of the combustion processes ensures an accurate dosage of the required air volume needed as a function of the feed gas composition. To reduce the process gas volume or obtain higher combustion temperatures, the air requirement can also be covered by injecting pure oxygen. Several technologies utilizing high-level and low-level oxygen enrichment are available in industry, which requires the use of a special burner in the reaction furnace for this process option.

Usually, 60 to 70% of the total amount of elemental sulfur produced in the process are obtained in the thermal process step.

The main portion of the hot gas from the combustion chamber flows through the tube of the process gas cooler and is cooled down such that the sulfur formed in the reaction step condenses. The heat given off by the process gas and the condensation heat evolved are utilized to produce medium or low-pressure steam. The condensed sulfur is removed at the liquid outlet section of the process gas cooler.

The sulfur forms in the thermal phase as highly reactive S2 diradicals which combine exclusively to the S8 allotrope:

4 S2 → S8

Side reactions

Other chemical processes taking place in the thermal step of the Claus reaction are:[6]

2 H2S → S2 + 2 H2        (ΔH > 0)
CH4 + 2 H2O → CO2 + 4 H2
H2S + CO2 → S=C=O + H2O
CH4 + 2 S2 → S=C=S + 2 H2S

Detailed chemical kinetic modeling

Recent efforts to develop complex chemical kinetic models for the thermal reactions of Hydrogen sulfide under conditions of the Claus process furnace can now be found. The models consist of hundreds of elementary reactions including kinetic coefficients and thermochemical data. Such efforts can be found in the following references:

a. I.A. Gargurevich, Hydrogen Sulfide Combustion: Relevant Issues under Claus Furnace Conditions,Ind Eng Chem Res, 44 (2005), pp. 7706–7729 (
b.Selim, H. M. M. E. (2012). Characteristics and chemical kinetics of hydrogen sulfide combustion in thermal Claus reactor (Doctoral dissertation, UNIVERSITY OF MARYLAND, COLLEGE PARK).(
c. Manenti, F., Papasidero, D., & Ranzi, E. (2013). Revised Kinetic Scheme for Thermal Furnace of Sulfur Recovery Units. Chemical Engineering Transactions, 32, 2013, 1185-1290.(

The most significant effort is in the development of sound chemistry (elementary reactions) for the mechanism since it must explain formation of intermediate chemical species and final products. Development of the kinetic coefficients involves experimental data, computational chemistry (e.g., reaction activation energy via Quantum Chemistry) as well as estimation methods such as kinetic theory, transition state theory. Reactions can involve chemical activation and methods are available to treat such reactions. A simple presentation of such methods can be found in:

Gargurevich, Ivan A., Reaction Kinetics & Chemical Reaction Models, 2001.

Bimolecular chemical activation, an important reaction in combustion for example, can be explained by the illustration below (from Gargurevich (2001) referenced above):

Bimolecular Chemical Activation Diagram

In the case of a bimolecular activation reaction is meant that as the result of a bimolecular reaction (addition of free radical to a double bonded species for example) an intermediate A* is formed possessing excess energy over the ground state that can more easily lead to some final product by decomposition or,

R + R' < = = > Activated Molecule (A*) < = = > Products

A nice introduction to Computational Chemistry is given by David C. Young in his book "Computational Chemistry: A Practical Guide for Applying Techniques to Real World Problems (Wiley, 2001)", and his website It is not the intention here to present a discussion on such complex subject. Computational Chemistry methods can be used to estimate thermochemical properties of molecules such as Heat of Formation as well. However, Semi-empirical methods such as group additive are described by S. W. Benson in his book "Thermochemical Kinetics ".

The overall process of constructing such Detailed Chemical Kinetic Models is illustrated by Swihart, Mark, T, "Constructing Reaction Mechanisms", in Modeling of Chemical Reactions, vol. 42, Chapter 5, p. 187, W. R. Carr Editor., 2007 ( Comprehensive Chemical Kinetics Series (N. J. B. Green Series Editor, by Elsevier, a copy of the volume is found at (

The diagram below depicts the major steps in constructing complex or detailed chemical kinetic reaction models. It is self-explanatory and depicts quite well the major steps in building a detailed chemical kinetic model starting with the assembly of the elementary chemical reactions, followed by estimating chemical kinetic parameters and thermochemical parameters. The validation of the reaction model must be conducted with an appropriate experimental apparatus. Eventually, the development and design of a pilot/commercial size reactor must be considered including simulation by CFD including chemical reactions. The scale up parameters for the reactor must also be determined.

Stepwise Procedure To Develop Detailed Reaction Mechanisms

Two other excellent references for detailed chemical kinetic modeling are [9] and [10]

As an illustration of such modeling, a reduced mechanism for the oxidation of Hydrogen Sulfide can be constructed as below (

        Elementary Reaction     A       n  E/RT    
  1. H2S+M = S+H2+M — 1.60E+24 2.61 44800
  2. H2S+H = SH+H2 - 1.20E+07 2.1 350
  3. H2S+0 = SH+OH 7.50E+07 1.75 1460
  4. H2S+OH= SH+H20 2.70E+12 0 0
  5. H2S+S= 2SH 8.30E+13 0 3700
  6. H2S+S = HS2+H 2.03E+13 0 3723.84
  7. S+H2= SH+H 1.40E+14 0 9700
  8. SH+0 = H+SO 1.00E+14 0 0
  9. SH+OH = S+H20 1.00E+13 0 0
  10. SH+02= HS0+0 1.90E+13 0 9000
  11. S+OH = H+SO 4.00E+13 0 0
  12. S+02= SO+0 5.20E+06 1.81 -600
  13. SH+S = S2+H 1.00E+13 0 0
  14. S2+11+14 = HS2+M 1.00E+16 0 0
  15. S2+0= SO+S 1.00E+13 0 0
  16. SO+OH = S02+H 1.08E+17 -1.35 0
  17. SO+02= S02+0 7.60E+03 2.37 1500
  18. 2S0= S02+S 2.03E+12 0 2000
  19. HS0+02= S02+0H 1.00E+12 0 5000
  20. 2SH = S2+112 1.00E+12 0 0
  21. S2+M = 2S+M 4.80E+13 0 38800
  22. HS2+H = S2+H2 1.20E+07 21 352.42
  23. HS2+0= S2+OH 7.50E+07 1.8 1460
  24. HS2+OH = S2+H20 2.70E+12 0 0
  25. H52+5= S2+SH 8.30E+13 0 3700
  26. SO+O(+M) = S02(+M) 3.20E+13 0 0
  27. SO+M = S+O+M 4.00E+14 0 54000
  28. SO+H+M = HSO+M 5.00E+15 0 0
  29. HSO+H = SH+OH 4.90E+19 -1.86 785
  30. HSO+H = S+H20 1.60E+09 1.37 -170
  31. HSO+H = H2S+0 1.10E+06 1.03 5230
  32. HSO+H = SO+H2 1.00E+13 0 0
  33. HSO+O = S02+H 4.50E+14 -0.4 0
  34. HS0+0 = OH+SO 1.40E+13 0.15 150
  35. HSO+OH = SO+H20 1.70E+09 1.03 235
  36. S+OH = SH+O 6.30E+11 0.5 4030.55
  37. SH+02= SO+0H 1.00E+12 503 248

The mechanism with chemical kinetic data and thermodynamic properties is an input to software (as a batch file ) to simulate a plug flow reactor, or CSTR for example satisfying heat, component and mass balances. Note that at the high temperature typical of a Claus furnace, the mechanism involves a radical chain reaction mechanism for the decomposition and oxidation of Hydrogen sulfide.

Catalytic step

The Claus reaction continues in the catalytic step with activated aluminum(III) or titanium(IV) oxide, and serves to boost the sulfur yield. More hydrogen sulfide (H2S) reacts with the SO2 formed during combustion in the reaction furnace in the Claus reaction, and results in gaseous, elemental sulfur.

2 H2S + SO2 → 3 S + 2 H2O      (ΔH = -1165.6 kJ mol−1)

This sulfur can be S6, S7, S8 or S9.

A recent mechanism for the formation of sulfur on a catalyst surface is given in a recent publication by T.K. Khanmamedox and R.H. Welland titled "How Sulphur Really Forms on The Catalyst Surface ", Sulphur, 345, March–April 2013, p62. Their conclusion is as follows: "A mechanism path for catalytic oxidation of Hydrogen Sulfide has been discussed. The mechanism involves S(6) and S(8) that desorb form the catalyst's active sites with simultaneous formation of stable cyclic elemental sulfur. Kinetic models that identify the main peculiarities of catalytic oxidation in the Claus reaction and the oxidation of Hydrogen Sulfide with Oxygen have been suggested."

The catalytic recovery of sulfur consists of three substeps: heating, catalytic reaction and cooling plus condensation. These three steps are normally repeated a maximum of three times. Where an incineration or tail-gas treatment unit (TGTU) is added downstream of the Claus plant, only two catalytic stages are usually installed.

The first process step in the catalytic stage is the gas heating process. It is necessary to prevent sulfur condensation in the catalyst bed, which can lead to catalyst fouling. The required bed operating temperature in the individual catalytic stages is achieved by heating the process gas in a reheater until the desired operating bed temperature is reached.

Several methods of reheating are used in industry:

  • Hot-gas bypass: which involves mixing the two process gas streams from the process gas cooler (cold gas) and the bypass (hot gas) from the first pass of the waste-heat boiler.
  • Indirect steam reheaters: the gas can also be heated with high-pressure steam in a heat exchanger.
  • Gas/gas exchangers: whereby the cooled gas from the process gas cooler is indirectly heated from the hot gas coming out of an upstream catalytic reactor in a gas-to-gas exchanger.
  • Direct-fired heaters: fired reheaters utilizing acid gas or fuel gas, which is burned substoichiometrically to avoid oxygen breakthrough which can damage Claus catalyst.

The typically recommended operating temperature of the first catalyst stage is 315 °C to 330 °C (bottom bed temperature). The high temperature in the first stage also helps to hydrolyze COS and CS2, which is formed in the furnace and would not otherwise be converted in the modified Claus process.

The catalytic conversion is maximized at lower temperatures, but care must be taken to ensure that each bed is operated above the dew point of sulfur. The operating temperatures of the subsequent catalytic stages are typically 240 °C for the second stage and 200 °C for the third stage (bottom bed temperatures).

In the sulfur condenser, the process gas coming from the catalytic reactor is cooled to between 150 and 130 °C. The condensation heat is used to generate steam at the shell side of the condenser.

Before storage, liquid sulfur streams from the process gas cooler, the sulfur condensers and from the final sulfur separator are routed to the degassing unit, where the gases (primarily H2S) dissolved in the sulfur are removed.

The tail gas from the Claus process still containing combustible components and sulfur compounds (H2S, H2 and CO) is either burned in an incineration unit or further desulfurized in a downstream tail gas treatment unit.

Sub dew point Claus process

The conventional Claus process described above is limited in its conversion due to the reaction equilibrium being reached. Like all exothermic reactions, greater conversion can be achieved at lower temperatures, however as mentioned the Claus reactor must be operated above the sulfur dew point (120–150 °C) to avoid liquid sulfur physically deactivating the catalyst. To overcome this problem, the sub dew point Claus process operates with reactors in parallel. When one reactor has become saturated with adsorbed sulfur, the process flow is diverted to the standby reactor. The reactor is then regenerated by sending process gas that has been heated to 300–350 °C to vaporize the sulfur. This stream is sent to a condenser to recover the sulfur.

Process performance

Using two catalytic stages, the process will typically yield over 97% of the sulfur in the input stream. Over 2.6 tons of steam will be generated for each ton of sulfur yield.

The physical properties of elemental sulfur obtained in the Claus process can differ from that obtained by other processes.[6] Sulfur is usually transported as a liquid (melting point 115 °C). In ordinary sulfur viscosity can increase rapidly at temperatures in excess of 160 °C due to the formation of polymeric sulfur chains but not so in Claus-sulfur. Another anomaly is found in the solubility of residual H2S in liquid sulfur as a function of temperature. Ordinarily the solubility of a gas decreases with increasing temperature but now it is the opposite. This means that toxic and explosive H2S gas can build up in the headspace of any cooling liquid sulfur reservoir. The explanation for this anomaly is the endothermic reaction of sulfur with H2S to polysulfane.

See also


  1. ^ Ralf Steudel, Lorraine West, Vita of Carl Friedrich Claus - inventor of the Claus process for production of sulfur from hydrogen sulfide, online document of 2015 on the platform
  2. ^ Gas Processors Association Data Book, 10th Edition, Volume II, Section 22
  3. ^ Gary, J.H. and Handwerk, G.E. (1984). Petroleum Refining Technology and Economics (2nd ed.). Marcel Dekker, Inc.  
  4. ^ Sulfur production report by the United States Geological Survey
  5. ^ Discussion of recovered byproduct sulfur
  6. ^ a b c d Der Claus-Prozess. Reich an Jahren und bedeutender denn je, Bernhard Schreiner, Chemie in Unserer Zeit 2008, Vol. 42, Issue 6, Pages 378-392.
  7. ^ Bibliographic Citation Sulfur Recovery Technology, B.G. Goar, American Institute of Chemical Engineers Spring National Meeting, New Orleans, Louisiana, April 6, 1986
  8. ^ Or between 950 and 1200 °C and even hotter near the flame, as stated in Der Claus-Prozess. Reich an Jahren und bedeutender denn je, Bernhard Schreiner, Chemie in Unserer Zeit 2008, Vol. 42, Issue 6, Pages 378-392.
  9. ^ Battin-Leclerc, Frederique et al., Cleaner Combustion: Developing Detailed Chemical Kinetic Models, 2013, Springer
  10. ^ Gargurevich, Ivan A., Combustion Models and he Prediction of Polycyclic Aromatic Hydrocarbons (PAH) in laminar flames of simple hydrocarbons: Methane, Methyl Chloride, and 1,1 Dichloroethane, Doctoral Dissertation, University of California at Los Angeles (UCLA),1997 (
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