International Journal of Electrochemistry

International Journal of Electrochemistry / 2016 / Article

Research Article | Open Access

Volume 2016 |Article ID 7628761 | 5 pages | https://doi.org/10.1155/2016/7628761

A Method for the Simultaneous Cleansing of H2S and SO2

Academic Editor: Abel C. Chialvo
Received04 Sep 2015
Revised19 Nov 2015
Accepted13 Dec 2015
Published17 Jan 2016

Abstract

A method for the simultaneous electrochemical purification of hydrogen sulfide and sulfur dioxide from sea water or industrial wastes is proposed. Fundamentally the method is based on the electrochemical affinity of the pair H2S and SO2. The reactions (oxidation of H2S and reduction of SO2) proceed on а proper catalyst in a flow reactor, without an external power by electrochemical means. The partial curves of oxidation of H2S and reduction of SO2 have been studied electrochemically on different catalysts. Following the additive principle the rate of the process has been found by intersection of the curves. The overall process rate has been studied in a flow type reactor. Similar values of the process rate have been found and these prove the electrochemical mechanism of the reactions. As a result the electrochemical method at adequate conditions is developed. The process is able to completely convert the initial reagents (concentrations ), which is difficult given the chemical kinetics.

1. Introduction

A number of past methods for the removal of sulfur-containing compounds from gas and water streams have been investigated by different researchers. These methods generally separate the sulfur compounds from the gas stream by an absorption stage. The so-called Claus process is the most widely utilized [1] and follows the general reaction: The Claus process proceeds at temperatures above 1300°C; however, by utilizing different catalysts, this can be reduced to 250–850°C [25]. The purification of SO2 is currently a standalone process. There are different methods for extraction of sulfur dioxide, like neutralization methods, conversion of SO2 into CaSO4 [6], and liquefaction of SO2 by adsorption in sulfate solution [7]. All these methods are based on the oxidation of SO2. Previous research by Petrov on the electrochemical oxidation reduction processes for SO2 and H2S cleansing by their oxidation with oxygen contained in the air labeled ELCOX as innovative process for SO2 cleansing in waste gases [8].

The present work is aimed at the opportunity of simultaneously cleansing the hydrogen sulfide and sulfur dioxide from industrial wastes and natural (Black Sea) H2S containing waters. It is well known that Black Sea deep waters contain an enormous amount of hydrogen sulfide (as hydrosulfides and sulfide ions) estimated as 4600 Tg, that is, 4.6 billion tons [9]. There are efforts to attack the problem by various methods: low temperature adsorption of hydrogen sulfide from sea waters followed by thermal decomposition [10, 11], electrolysis leading to hydrogen and sulfur production [12], or burning the hydrogen sulfide itself in electric power stations, as proposed by [13]. All these methods encounter the problem of low H2S concentrations ( 8–10 mg·L−1) which do not allow for the application of feasible technologies [14].

In this work we review the simultaneous reduction of SO2 and oxidation of hydrogen sulfide. Various kinds of electrode materials were utilized in the past for the reduction of SO2, namely, mercury, gold, platinum, bismuth, copper, iron phthalocyanine on graphite, and uranium iron alloys. Previous studies do not fully explain the electrochemical process in the reduction of sulfur dioxide [15]. Various electrochemical methods to convert hydrogen sulfide to its elements, at different concentrations, have been studied [16]. Different catalysts for the oxidation of hydrogen sulfide were used previously like ferric, cobalt, graphite, platinum, manganese cations, cobalt and carbon compounds, and perovskites or cobalt phthalocyanine [1719]. The anodic process of sulfide oxidation can be carried out leading to different final products (elemental sulfur, polysulfides, or sulfates), depending on the reaction conditions: temperature, concentrations, catalysts, and so forth.

The aim of the proposed method is to simultaneously purify both reagents (SO2 and H2S) at room temperatures. Fundamentally the method is based on the electrochemical affinities of both compounds. The thermodynamic potentials of the pair H2S and SO2 for oxidation and reduction areOverall reaction isFrom the theory for concurrent redox (corrosion) reactions it follows that these electrochemical reactions can occur due to the potential difference of  V as indicated for reactions (1) and (2) on dispersed microgalvanic elements [20, 21]. Based on this the reactions may proceed on the right catalyst in a flow reactor, without an external power source by electrochemical means. The reaction rate may be determined by studying the partial electrochemical reactions of H2S oxidation and SO2 reduction, in accordance with the so-called additive principle [2022].

An advantage of these electrochemical reactions is that they are able to completely convert the initial reagents (concentrations ) [23], which is difficult given the chemical kinetics [24]. An application has been filed for a patent entitled “the electrochemical method for separation of sulfur dioxide and hydrogen sulfide from fluids” [25].

The electrochemical realization of the process is possible due to the launching of novel microgalvanic cells. To illustrate the main idea a physical model of the process with a porous catalytic electrode is schematically shown in Figure 1. The model is similar to our previously published work [26]. The structure of the catalytic mass is composed of teflonized carbon black/charcoal with a deposited catalyst . Teflon is needed as a binding and hydrophobic agent because some of the reagents are in a gaseous form (e.g., 14% of H2S in Black Sea waters exist as diluted gas). The catalytic particles are in direct electronic contact through a teflonized carbon network . Ion contact is achieved through the solution (electrolyte)—. These conditions are sufficient for the realization of a galvanic element between the pair SO2-H2S. Depending on the pH of electrolyte the final products can be sulfur, polysulfides, or sulfates.

2. Materials and Methods

Sodium sulfide (Na2S·9H2O, Sigma-Aldrich 98.0%), Sodium sulfite (Na2SO3, Sigma-Aldrich), and Sodium Chloride (NaCl, Sigma-Aldrich) were for realizing of electrolyte. Deionized water was used. The Vulcan XC-72 carbon black (particle size ~50 nm) and acetylene blacks were from Cabot Corporation. The CoPc (cobalt phthalocyanine) was prepared by pyrolysis [18].

The total amount of sulfide and sulfite ions was determined iodometrically with starch as the indicator [27]. Sulfides were separately determined photometrically with N,N-dimethyl-n-phenylenediamine in the presence of Fe(III) and the formation of methylene blue [2830]. This method allows for a doubled increase in the sensitivity of determination. The presence of thiosulfates, sulfites, and sulfates was also qualitatively checked. Thiosulfates form an unstable purple complex with Fe(III). The opalescence of the solution after the addition of barium cations shows the presence of sulfite and sulfate. The dissolution of the deposit in concentrated hydrochloric acid proves the presence of a sulfite, whereas the barium sulfate remains nondissolved [31].

We utilized a three-electrode cell to complete the electrochemical tests. For SO2 reduction we used sulphurous acid H2SO3 (10 g·L−1). The H2S concentration in the electrolyte has been varied in the range 100–20 000 mg·L−1 introduced as NaHS. This range has been selected having in mind that the electrochemical process is very slow (practically does not occur) at lower concentrations, especially at the naturally encountered concentration of about 8 mg·L−1 [9], and higher concentrations were studied in previous investigations [14]. A supporting electrolyte of 18 g·L−1 NaCl (similar to the concentration in Black Sea waters) is added to the electrolyte, as well as 1 M NaOH in some cases.

The cell volume is 150 mL. The electrolyte was stirred continuously with a magnetic stirrer. A Solartron 1286 Electrochemical Interface is used for the electrochemical measurements. A reference hydrogen electrode by “Gaskatel Gmbh”, Germany, is applied. The counter electrode is Pt-foil. A minimum of four measurements were made for each result to achieve better reproducibility. Arithmetic averages are presented in the graphs.

An overall reaction rate for the simultaneous oxidation of hydrogen sulfide and reduction of sulfur dioxide without external power is studied in a flow type chemical reactor. The catalyst is placed in the reactor.

All the electrodes studied are of the immersed type and have a geometrical area of 1 cm2 or 10 cm2. The electrodes are prepared from a mixture of the catalysts and teflonized carbon black (Vulcan XC-72 + 35% Teflon)—TV35—as a binder. The mixture is pressed onto both sides of a stainless steel current collector at and  atm.

3. Results and Discussion

3.1. Electrode Properties and Optimization

The immersed type electrodes for the oxidation of H2S and reduction of SO2 were previously optimized with respect to the catalyst used, the electrode thickness, and the mass ratio between catalysts and binder by varying one parameter at a time and keeping the others constant [31, 32]. Different catalysts have been studied: (DG + 20% CoPc) + 35% teflonized Vulcan XC-72 (DGCPV); (DG + 20% CoPc) + 35% teflonized Acetylene Black (DCPAB); La1.3Sr0.7NiO4 + 35% teflonized Vulcan XC-72 (LSNV); Bulk Graphite; (DG + 20% CoPc) + 35% teflonized Vulcan XC-72 + 6% Pt., [31]. (DG + 20% CoPc) is active carbon type DG on which cobalt phthalocyanine is deposited [18].

The electrochemical characteristics of the best optimized electrodes for H2S oxidation ((a) DG + 20% CoPc compare 35% teflonized Vulcan XC-72,DGCPV, ratio 30 : 70; the quantity is 60 mg/cm2; (b) La1.3Sr0.7NiO4 + 35% teflonized Vulcan XC-72, LSNV) are shown in Figure 2. It is seen that both electrodes provide fairly similar electrochemical behaviour.

The polarization curves of sulfur dioxide reduction are shown in Figure 3. It can be seen that the substrate used (a) does not have a catalytic effect. The good initial results with electrodes containing DG + 20% CoPc + 6% Pt (d) have not been confirmed by long-term tests due to platinum poisoning. The curves (b) and (c), respectively, DG + 20% CoPc and Perovskite are similar.

The influence of the electrolyte (with or without NaOH and NaCl) on SO2 reduction is shown in Figure 4. The figure shows that the absence of NaCl (curve (b)) leads to a conductivity reduction, while NaOH absence leads to a decrease in pH and change in process kinetics, yielding sulfur.

3.2. Electrochemical Mechanism

The electrochemical mechanism was studied by juxtaposition of the partial curves of oxidation of hydrogen sulfide (Figure 2(a)) and the reduction of SO2 (Figure 3(b)) as presented in Figure 5. From the intersection of the curves we can determine the mixed potential and current density, which are  mV and  mA/cm2. The overall reaction rate can be estimated using Faraday’s equation:The agreement between the mixed potential (in a solution containing hydrogen sulfide and sulfur dioxide  mV and the potential calculated from the intersection of the partial curves  mV) is very good, since the deviations for porous electrodes of around  mV are acceptable [33]. This agreement is an indication of the electrochemical mechanism of the process. In order to indubitably prove the electrochemical mechanism we have to measure the overall reaction rate.

3.3. Estimation of the Overall Reaction Rate in a Flow Type Reactor

The overall reaction rate has been estimated in a flow type reactor with a solution (electrolyte) H2SO3 + 18 g·L−1 NaCl + 1 M NaOH + Na2S·9H2O. The electrolyte was circulated all the time. The amount of catalytic mass in the reactor is equal to the catalytic amount in 10 cm2 immersed electrodes (420 mg 35% teflonized Vulcan XC-72 + 18 mg DG (Standard Degussa carbon black) with 20% CoPc). The inlet and outlet concentrations were found analytically. Unfortunately we do not have a method for instant analysis of the solution in order to find the momentary reaction rate. The overall rate of the oxidation reduction process was estimated analytically after one hour of operation. The whole electrolyte volume of circulating electrolyte is  mL. It can be converted into (electrochemical rate) with the aid of (5). The number of exchanged electrons, following reactions (2) and (3), is for H2S oxidation and for SO2 reduction. All data are shown in Table 1.


ReagentInitial amount ()Final amount ()
per hour 
()
= /
(mA)
= /10
mA·cm−2

, mg·L−15737.7521.25
(gEqv) 3.56·10−3 2.23·10−3 1.33·10−335.643.56
, mg·L−14016.523.5
Ns2− (gEqv) 23.5·10−3 9.7·10−3 13.8·10−337.03.7

From the good agreement between the analytical and electrochemical results as shown in Table 1, we can conclude that the electrochemical rather than chemical conversion of hydrogen sulfide and sulfur dioxide is preferable.

4. Conclusion

The set-up used to accomplish the process discussed can be a continuously stirred tank reactor containing the sea water and the catalyst and bubbles by the stack gases containing sulfur dioxide. The process could be carried out either in acid or alkaline media.

Based on the data in Table 1 we can suppose that the conversion of 18 g hydrogen sulfide per hour into environmentally friendly products like sulfate, sulfur, and polysulfides will require about 460 g of catalyst.

Based on these results we have developed a method for purification of both contaminants at normal atmospheric conditions by electrochemical means. The optimum conditions and suitable catalytic mass have been determined. The realized process completely converts H2S and SO2 into environmentally friendly products (sulfur, polysulfides, etc.). A medium size coal thermal power station of 630 MW releases about 20 metric tons of sulfur dioxide daily which requires 2 mln m3 (two million cubic meters per hour) of sea water.

One cubic meter of sea water (8 mg·L−1; 8 g·m−3) cleans three cubic meters of SO2 containing gases ( = 0.1% vol.; ~2.85 g·m−3).

It seems more realistic to convert reasonable amounts of hydrogen sulfide to produce sulfur and polysulfide as commercial products, thus reducing small amounts of sulfur dioxide, and to remove the rest by traditional methods, like treatment with lime or limestone.

Conflict of Interests

The authors declare that there is no conflict of interests regarding the publication of this paper.

Acknowledgments

This work was supported by the project Hydrogen Production from Black Sea Water by Sulfide-Driven Fuel Cell HYSULFCEL (http://bs-era.net/) of the 7 FP of the European Union, Contract DNS7RP 01/32, of the Ministry of Education and Science of the Republic of Bulgaria.

References

  1. C. F. Claus, British Patent 5958, 1883.
  2. P. F. Cross, UK Patent Application GB 2503294 A, 2012.
  3. Z. Nugeired, EA 000764 B1, 1998.
  4. V. K. Kam-Wang, WO 2001053197 A1 (also US 6214311), 2000.
  5. M. Rameshni, WO2009055104 A2 (also US 7722852 B2), 2009.
  6. T. Shimizu, M. Peglow, K. Yamagiwa, and M. Tanaka, “Comparison among attrition-reaction models of SO2 capture by uncalcined limestone under pressurized fluidized bed combustion conditions,” Chemical Engineering Science, vol. 58, no. 13, pp. 3053–3057, 2003. View at: Publisher Site | Google Scholar
  7. L. Cholpanova, N. Kazanski, and R. Tsacheva, Bulgarian Environmental Projects, Pensoft, Bulgaria, Sofia, 1995.
  8. K. Petrov, “Electrochemical methods for cleansing of H2S and SO2 in industrial and natural contaminated waters. Elcox method,” in Technological Innovations in Sensing and Detection of Chemical, Biological, Radiological, Nuclear Threats and Ecological Terrorism, NATO Science for Peace and Security Series A: Chemistry and Biology, pp. 287–299, Springer, Amsterdam, The Netherlands, 2012. View at: Publisher Site | Google Scholar
  9. A. Midilli, M. Ay, A. Kale, and T. N. Veziroglu, “A parametric investigation of hydrogen energy potential based on H2S in Black Sea deep waters,” International Journal of Hydrogen Energy, vol. 32, no. 1, pp. 117–124, 2007. View at: Publisher Site | Google Scholar
  10. T. Chivers, J. B. Hyne, and C. Lau, “The thermal decomposition of hydrogen sulfide over transition metal sulfides,” International Journal of Hydrogen Energy, vol. 5, no. 5, pp. 499–506, 1980. View at: Publisher Site | Google Scholar
  11. S. Z. Baykara, E. H. Figen, A. Kale, and T. Nejat Veziroglu, “Hydrogen from hydrogen sulphide in Black Sea,” International Journal of Hydrogen Energy, vol. 32, no. 9, pp. 1246–1250, 2007. View at: Publisher Site | Google Scholar
  12. K. Petrov and S. Srinivasan, “Low temperature removal of hydrogen sulfide from sour gas and its utilization for hydrogen and sulfur production,” International Journal of Hydrogen Energy, vol. 21, no. 3, pp. 163–169, 1996. View at: Publisher Site | Google Scholar
  13. L. Goltseva and A. Yutkin, “Black sea,” Inventor, vol. 2, p. 7, 1996. View at: Google Scholar
  14. K. Petrov, S. Z. Baykara, D. Ebrasu, M. Gulin, and A. Veziroglu, “An assessment of electrolytic hydrogen production from H2S in Black Sea waters,” International Journal of Hydrogen Energy, vol. 36, no. 15, pp. 8936–8942, 2011. View at: Publisher Site | Google Scholar
  15. I. Streeter, A. J. Wain, J. Davis, and R. G. Compton, “Cathodic reduction of bisulfite and sulfur dioxide in aqueous solutions on copper electrodes: an electrochemical ESR study,” Journal of Physical Chemistry B, vol. 109, no. 39, pp. 18500–18506, 2005. View at: Publisher Site | Google Scholar
  16. Z. Mao, A. Anani, R. E. White, S. Srinivasan, and A. J. Appleby, “Modified electrochemical process for the decomposition of hydrogen sulfide in an aqueous alkaline solution,” Journal of the Electrochemical Society, vol. 138, no. 5, pp. 1299–1303, 1991. View at: Publisher Site | Google Scholar
  17. J. Zaman and A. Chakma, “Production of hydrogen and sulfur from hydrogen sulfide,” Fuel Processing Technology, vol. 41, no. 2, pp. 159–198, 1995. View at: Publisher Site | Google Scholar
  18. K. Petrov, I. Nikolov, T. Vitanov, D. Uzun, and V. Ognjanov, “Pyrolyzed Co-phtalocyanine as a catalyst for the oxidation of sulphur dioxide,” Bulgarian Chemical Communications, vol. 42, no. 3, pp. 189–193, 2010. View at: Google Scholar
  19. K. T. Chuang, J. C. Donini, A. R. Sanger, and S. V. Slavov, “A proton—conducting solid state H2S-O2 fuel cell 2. Production of liquid sulphur at 120–145°C,” International Journal Hydrogen Energy, vol. 25, no. 9, pp. 887–894, 2000. View at: Publisher Site | Google Scholar
  20. C. Wagner and W. Z. Traud, “Über die deutung von korrosionsvorgängen durch überlagerung von elektrochemischen teilvorgängen und über die potentialbildung an mischelektroden,” Zeitschrift für Elektrochemie und Angewandte Physikalische Chemie, vol. 44, pp. 391–402, 1938. View at: Google Scholar
  21. V. V. Scorcelletti, Theoretical Fundamentals of Corrosion in Metals, Khimia Leningrad: Chemistry, Saint Petersburg, Russia, 1973.
  22. M. Spiro and P. L. Freund, “Polyelectrodes: evidence for and against the wagner and traud additivity hypothesis,” Journal of Electroanalytical Chemistry, vol. 144, no. 1-2, pp. 293–301, 1983. View at: Publisher Site | Google Scholar
  23. K. Vetter, Electrochemical Kinetics, Chemistry, Moscow, Russia, 1967.
  24. B. V. Romanovsky, Fundamentals of Chemical Kinetics, Exam, Moscow, Russia, 2006.
  25. D. Uzun, E. Razkazova-Velkova, V. Beschkov, and K. Petrov, “The electrochemical method for separation of sulphur dioxide and hydrogen sulphide from fluids,” Bulgarian Patent Office, Patent Request Number: 111701, 2014. View at: Google Scholar
  26. D. Uzun, P. Hiev, D. Vladikova et al., “Electrocatalytic oxidation-reduction reactions of metal-hydride alloys with teflon-carbon additives,” Bulgarian Chemical Communications, vol. 42, no. 2, pp. 113–118, 2010. View at: Google Scholar
  27. N. P. Penchev and B. N. Zagorghev, Analytic Chemistry, Quantity Analysis, Science and Art, Sofia, Bulgaria, 1956.
  28. A. Busev and L. Simon, Analytical Chemistry of Sulphur, Science, Moscow, Russia, 1975.
  29. W. Fresenius and G. Jander, Handbook for Analytical Chemistry, Springer, 4th edition, 1967.
  30. N. P. Penchev and B. N. Zagorghev, Analytic Chemistry Qualitative Analysis, Science and Art, Sofia, Bulgaria, 1964.
  31. M. G. Bapat and B. Sharma, “Application of amperometric dead stop end point to iodate procedures in presence of mercuric mercury,” Fresenius' Zeitschrift für Analytische Chemie, vol. 157, no. 4, pp. 258–261, 1957. View at: Publisher Site | Google Scholar
  32. D. Uzun, E. Razkazova-Velkova, K. Petrov, and V. Beschkov, “Electrochemical method for energy production from hydrogen sulfide in the Black sea waters in sulphide—driven fuel cell,” Bulgarian Chemical Communications, vol. 47, no. 3, pp. 859–866, 2015. View at: Google Scholar
  33. A. Carbó, Electrochemistry of Porous Materials, Taylor & Francis Group, 2012.

Copyright © 2016 Dzhamal R. Uzun et al. This is an open access article distributed under the Creative Commons Attribution License, which permits unrestricted use, distribution, and reproduction in any medium, provided the original work is properly cited.


More related articles

6626 Views | 770 Downloads | 0 Citations
 PDF  Download Citation  Citation
 Download other formatsMore
 Order printed copiesOrder

Related articles

We are committed to sharing findings related to COVID-19 as quickly and safely as possible. Any author submitting a COVID-19 paper should notify us at help@hindawi.com to ensure their research is fast-tracked and made available on a preprint server as soon as possible. We will be providing unlimited waivers of publication charges for accepted articles related to COVID-19. Sign up here as a reviewer to help fast-track new submissions.