EP0283785A1 - Process for recovering mercury by electrolysis - Google Patents
Process for recovering mercury by electrolysis Download PDFInfo
- Publication number
- EP0283785A1 EP0283785A1 EP88103269A EP88103269A EP0283785A1 EP 0283785 A1 EP0283785 A1 EP 0283785A1 EP 88103269 A EP88103269 A EP 88103269A EP 88103269 A EP88103269 A EP 88103269A EP 0283785 A1 EP0283785 A1 EP 0283785A1
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- EP
- European Patent Office
- Prior art keywords
- electrolysis
- mercury
- chloride
- chlorine
- cell
- Prior art date
- Legal status (The legal status is an assumption and is not a legal conclusion. Google has not performed a legal analysis and makes no representation as to the accuracy of the status listed.)
- Granted
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- 238000005868 electrolysis reaction Methods 0.000 title claims abstract description 33
- 238000000034 method Methods 0.000 title claims abstract description 19
- QSHDDOUJBYECFT-UHFFFAOYSA-N mercury Chemical compound [Hg] QSHDDOUJBYECFT-UHFFFAOYSA-N 0.000 title claims abstract description 14
- 229910052753 mercury Inorganic materials 0.000 title claims description 7
- 239000003792 electrolyte Substances 0.000 claims abstract description 14
- ZOMNIUBKTOKEHS-UHFFFAOYSA-L dimercury dichloride Chemical compound Cl[Hg][Hg]Cl ZOMNIUBKTOKEHS-UHFFFAOYSA-L 0.000 claims abstract description 10
- 239000000725 suspension Substances 0.000 claims abstract description 10
- 229940008718 metallic mercury Drugs 0.000 claims abstract description 7
- ZAMOUSCENKQFHK-UHFFFAOYSA-N Chlorine atom Chemical compound [Cl] ZAMOUSCENKQFHK-UHFFFAOYSA-N 0.000 claims description 13
- 229910052801 chlorine Inorganic materials 0.000 claims description 13
- 239000000460 chlorine Substances 0.000 claims description 13
- 238000007254 oxidation reaction Methods 0.000 claims description 12
- 230000003647 oxidation Effects 0.000 claims description 11
- VEXZGXHMUGYJMC-UHFFFAOYSA-M Chloride anion Chemical compound [Cl-] VEXZGXHMUGYJMC-UHFFFAOYSA-M 0.000 claims description 8
- LWJROJCJINYWOX-UHFFFAOYSA-L mercury dichloride Chemical compound Cl[Hg]Cl LWJROJCJINYWOX-UHFFFAOYSA-L 0.000 claims description 5
- XEEYBQQBJWHFJM-UHFFFAOYSA-N Iron Chemical compound [Fe] XEEYBQQBJWHFJM-UHFFFAOYSA-N 0.000 claims description 4
- PXHVJJICTQNCMI-UHFFFAOYSA-N Nickel Chemical compound [Ni] PXHVJJICTQNCMI-UHFFFAOYSA-N 0.000 claims description 4
- 239000007788 liquid Substances 0.000 claims description 4
- RYGMFSIKBFXOCR-UHFFFAOYSA-N Copper Chemical compound [Cu] RYGMFSIKBFXOCR-UHFFFAOYSA-N 0.000 claims description 3
- 229910052802 copper Inorganic materials 0.000 claims description 3
- 239000010949 copper Substances 0.000 claims description 3
- 230000008021 deposition Effects 0.000 claims description 3
- 238000011065 in-situ storage Methods 0.000 claims description 3
- 229910052751 metal Inorganic materials 0.000 claims description 3
- 239000002184 metal Substances 0.000 claims description 3
- BQCADISMDOOEFD-UHFFFAOYSA-N Silver Chemical compound [Ag] BQCADISMDOOEFD-UHFFFAOYSA-N 0.000 claims description 2
- ATJFFYVFTNAWJD-UHFFFAOYSA-N Tin Chemical compound [Sn] ATJFFYVFTNAWJD-UHFFFAOYSA-N 0.000 claims description 2
- HCHKCACWOHOZIP-UHFFFAOYSA-N Zinc Chemical compound [Zn] HCHKCACWOHOZIP-UHFFFAOYSA-N 0.000 claims description 2
- 229910045601 alloy Inorganic materials 0.000 claims description 2
- 239000000956 alloy Substances 0.000 claims description 2
- 229910052782 aluminium Inorganic materials 0.000 claims description 2
- XAGFODPZIPBFFR-UHFFFAOYSA-N aluminium Chemical compound [Al] XAGFODPZIPBFFR-UHFFFAOYSA-N 0.000 claims description 2
- 229910052793 cadmium Inorganic materials 0.000 claims description 2
- BDOSMKKIYDKNTQ-UHFFFAOYSA-N cadmium atom Chemical compound [Cd] BDOSMKKIYDKNTQ-UHFFFAOYSA-N 0.000 claims description 2
- 229910052742 iron Inorganic materials 0.000 claims description 2
- 239000000463 material Substances 0.000 claims description 2
- BQPIGGFYSBELGY-UHFFFAOYSA-N mercury(2+) Chemical compound [Hg+2] BQPIGGFYSBELGY-UHFFFAOYSA-N 0.000 claims description 2
- 150000002739 metals Chemical class 0.000 claims description 2
- 229910052759 nickel Inorganic materials 0.000 claims description 2
- 229910052709 silver Inorganic materials 0.000 claims description 2
- 239000004332 silver Substances 0.000 claims description 2
- 229910052718 tin Inorganic materials 0.000 claims description 2
- 229910052725 zinc Inorganic materials 0.000 claims description 2
- 239000011701 zinc Substances 0.000 claims description 2
- KZBUYRJDOAKODT-UHFFFAOYSA-N Chlorine Chemical compound ClCl KZBUYRJDOAKODT-UHFFFAOYSA-N 0.000 description 12
- 229910000497 Amalgam Inorganic materials 0.000 description 2
- QAOWNCQODCNURD-UHFFFAOYSA-N Sulfuric acid Chemical compound OS(O)(=O)=O QAOWNCQODCNURD-UHFFFAOYSA-N 0.000 description 2
- 238000006243 chemical reaction Methods 0.000 description 2
- 238000000151 deposition Methods 0.000 description 2
- 239000010406 cathode material Substances 0.000 description 1
- 238000003487 electrochemical reaction Methods 0.000 description 1
- 238000002474 experimental method Methods 0.000 description 1
- 239000007789 gas Substances 0.000 description 1
- 239000012528 membrane Substances 0.000 description 1
- 238000001465 metallisation Methods 0.000 description 1
- 239000000203 mixture Substances 0.000 description 1
- 238000000746 purification Methods 0.000 description 1
- 150000003839 salts Chemical class 0.000 description 1
- 231100000331 toxic Toxicity 0.000 description 1
- 230000002588 toxic effect Effects 0.000 description 1
Classifications
-
- C—CHEMISTRY; METALLURGY
- C25—ELECTROLYTIC OR ELECTROPHORETIC PROCESSES; APPARATUS THEREFOR
- C25C—PROCESSES FOR THE ELECTROLYTIC PRODUCTION, RECOVERY OR REFINING OF METALS; APPARATUS THEREFOR
- C25C7/00—Constructional parts, or assemblies thereof, of cells; Servicing or operating of cells
- C25C7/02—Electrodes; Connections thereof
-
- C—CHEMISTRY; METALLURGY
- C25—ELECTROLYTIC OR ELECTROPHORETIC PROCESSES; APPARATUS THEREFOR
- C25C—PROCESSES FOR THE ELECTROLYTIC PRODUCTION, RECOVERY OR REFINING OF METALS; APPARATUS THEREFOR
- C25C1/00—Electrolytic production, recovery or refining of metals by electrolysis of solutions
- C25C1/16—Electrolytic production, recovery or refining of metals by electrolysis of solutions of zinc, cadmium or mercury
Definitions
- the invention relates to a method for the deposition of metallic mercury from an electrolyte by means of electrolysis, wherein the mercury-I-chloride (Hg2Cl2) in suspension-containing electrolyte reacts with chlorine, which the mercury-I-chloride to soluble mercury-II-chloride (HgCl2 ) oxidized, which is reduced cathodically to liquid mercury by electrolysis under the influence of chlorine at the anode.
- Hg2Cl2 mercury-I-chloride
- HgCl2 soluble mercury-II-chloride
- the process according to the invention is advantageously used whenever mercury-I chloride present as a suspension is to be separated off and recovered as metallic mercury.
- Mercury-I-chloride for example, often occurs during the purification of gases, which is obtained in a reactor with a solution of mercury-II-chloride.
- the invention avoids these disadvantages. It is based on the object of proposing a method for the deposition of metallic mercury from an electrolyte by means of electrolysis with the features mentioned at the outset, which is distinguished by a noticeably simplified procedure, combined with a noticeably increased yield of deposited metallic mercury.
- the invention is characterized in that when an electrolysis cell is used in which the chlorine developed at the anode during the oxidation can migrate unhindered into the cathode region of the cell, the chlorine formed in the electrolysis cell during the electrolysis in situ for the oxidation of mercury-I-chloride is used to form soluble mercury-II-chloride.
- the separate conduction of the chlorine gas evolving during electrolysis to the oxidation reactor is therefore dispensed with. Rather, the oxidation and the electrolysis are carried out in one and the same electrolysis cell, so that the chlorine gas generated during the electrolysis can also migrate directly and unhindered into the cathode region of the cell.
- the gaseous chlorine formed in the electrolysis is therefore generally dissolved in the electrolyte and transported with the electrolyte, possibly supported by a pump or the like. The entire volume of the electrolyte is thus available for the oxidation of the mercury I chloride to mercury II chloride by means of the (gaseous or dissolved) chlorine.
- a fixed bed electrolysis cell is preferably used for the process described, without a separate anolyte circuit and with a diaphragm which prevents direct contact with the counterelectrode but does not hinder the mass transfer. It is known in a basic embodiment by the German patent specification 26 22 497 and in an improved embodiment by the applicant's DE-PS 29 04 539. A further improved embodiment describes the applicant's DE-PS 35 32 573. All of these embodiments can be used for carrying out the method according to the invention.
- the process according to the invention is carried out in such a way that the electrolyte is used at least initially in such a concentration of mercury-I chloride and / or that the electrolysis voltage and thus the electrolysis current are used at least initially at such a level that metallic mercury is used deposits on the cathode and drips from there. It can then be withdrawn from the bottom of the electrolytic cell.
- Iron, silver, nickel, copper, cadmium, aluminum, zinc, tin or an alloy of these metals is particularly suitable as the material for the cathode.
- the inventive method is based on the theory that at the anode of the electrolysis device Cl ⁇ in Cl2 passes.
- the Cl2 reacts with the Hg2Cl2 in suspension form and gives 2HgCl2, which is dissolved in the electrolyte.
- the HgCl2 is reduced to Hg o + 2Cl ⁇ . This Cl ⁇ is then available for the oxidation of the cathode.
- the electrolyte used had the following composition: 45 g / l Hg2Cl2 as a suspension 30 g / l sulfuric acid 10 g / l chloride.
- the anodic current density was 300 A / m2. It was expanded metal, so that this value relates to the entire area including the gaps.
- the cathodic current density was also 300 A / m2.
- the initial content of water-insoluble Hg2Cl2 was equal to the above-mentioned concentration of the suspension of 45 g / l.
- the initial current density was 600 A / m2.
Landscapes
- Chemical & Material Sciences (AREA)
- Engineering & Computer Science (AREA)
- Chemical Kinetics & Catalysis (AREA)
- Electrochemistry (AREA)
- Materials Engineering (AREA)
- Metallurgy (AREA)
- Organic Chemistry (AREA)
- Electrolytic Production Of Metals (AREA)
Abstract
Description
Die Erfindung betrifft ein Verfahren zur Abscheidung von metallischem Quecksilber aus einem Elektrolyten mittels Elektrolyse, wobei der Quecksilber-I-chlorid (Hg₂Cl₂) in Suspension enthaltende Elektrolyt mit Chlor reagiert, das das Quecksilber-I-chlorid zu löslichem Quecksilber-II-chlorid (HgCl₂) oxidiert, welches mittels der Elektrolyse unter Einwirkung von Chlor an der Anode kathodisch zu flüssigem Quecksilber reduziert wird.The invention relates to a method for the deposition of metallic mercury from an electrolyte by means of electrolysis, wherein the mercury-I-chloride (Hg₂Cl₂) in suspension-containing electrolyte reacts with chlorine, which the mercury-I-chloride to soluble mercury-II-chloride (HgCl₂ ) oxidized, which is reduced cathodically to liquid mercury by electrolysis under the influence of chlorine at the anode.
Das erfindungsgemäße Verfahren wird mit Vorteil immer dann eingesetzt, wenn als Suspension vorhandenes Quecksilber-I-chlorid abgeschieden und als metallisches Quecksilber wiedergewonnen werden soll. Quecksilber-I-chlorid fällt beispielsweise häufig bei der Reinigung von Gasen an, die in einem Reaktor mit einer Lösung von Quecksilber-II-chlorid gewonnen wird.The process according to the invention is advantageously used whenever mercury-I chloride present as a suspension is to be separated off and recovered as metallic mercury. Mercury-I-chloride, for example, often occurs during the purification of gases, which is obtained in a reactor with a solution of mercury-II-chloride.
Ein derartiges Verfahren beschreibt die europäische Offenlegungsschrift 179 040. Das bei der Elektrolyse dort entstehende Chlorgas wird aus dem Elektrolysegefäß abgeleitet und einem Reaktor zugeführt, in dem die Oxidation stattgefunden hat. Damit ist zwar der Vorteil verbunden, daß das beim Verfahren benötigte Chlorgas durch das Verfahren selbst erzeugt wird, jedoch benötigt man eine besondere Chlorgasleitung zwischen der Elektrolysezelle und dem Oxidationsreaktor. Hierbei muß besondere Vorsorge dafür getroffen werden, daß das giftige Chlorgas nicht in die Umwelt gelangt. Auch muß das Chlorgas durch geeignete Maßnahmen in die im Reaktor vorhandene Suspension fein verteilt eingetragen werden, um dort die Oxidationsreaktion durchführen zu können.Such a process is described in European laid-open specification 179 040. The chlorine gas generated there during the electrolysis is discharged from the electrolysis vessel and fed to a reactor in which the oxidation has taken place. This has the advantage that the chlorine gas required in the process is generated by the process itself, but a special chlorine gas line is required between the electrolysis cell and the oxidation reactor. Special precautions must be taken to ensure that the toxic chlorine gas does not get into the environment. The chlorine gas must also be taken by appropriate measures in the reactor existing suspension can be finely divided so that the oxidation reaction can be carried out there.
Diese Druckschrift beschreibt nicht die genaue Ausgestaltung der dort verwendeten Elektrolysezelle. Es muß jedoch vermutet werden, daß es sich um eine mittels einer Membran geteilten Elektrolysezelle handelt, weil der Stand der Technik nach der deutschen Auslegeschrift 20 11 610 allgemein dazu rät, bei einem Elektrolysegang Chlor von der Kathode fernzuhalten, da Chlor an der Kathode reduziert wird und damit die Stromausbeute der dort stattfindenden Metallabscheidung verringert (vergl. hierzu insbesondere Spalte 8, Zeile 63 ff der DE-AS 20 11 610).This document does not describe the exact design of the electrolysis cell used there. However, it must be assumed that the electrolysis cell is divided by means of a membrane, because the state of the art according to German patent specification 20 11 610 generally advises to keep chlorine away from the cathode during an electrolysis cycle, since chlorine is reduced at the cathode and thus reduces the current efficiency of the metal deposition taking place there (cf. in particular column 8, lines 63 ff of DE-AS 20 11 610).
Die Erfindung vermeidet diese Nachteile. Ihr liegt die Aufgabe zugrunde, ein Verfahren zur Abscheidung von metallischem Quecksilber aus einem Elektrolyten mittels Elektrolyse mit den eingangs genannten Merkmalen vorzuschlagen, welches sich durch eine fühlbar vereinfachte Verfahrensführung, verbunden mit einer fühlbar erhöhten Ausbeute an abgeschiedenem metallischen Quecksilber, auszeichnet.The invention avoids these disadvantages. It is based on the object of proposing a method for the deposition of metallic mercury from an electrolyte by means of electrolysis with the features mentioned at the outset, which is distinguished by a noticeably simplified procedure, combined with a noticeably increased yield of deposited metallic mercury.
Zur Lösung dieser Aufgabe ist die Erfindung dadurch gekennzeichnet, daß bei Verwendung einer Elektrolysezelle, in der das bei der Oxidation an der Anode entwickelte Chlor ungehindert in den Kathodenbereich der Zelle wandern kann, das in der Elektrolysezelle bei der Elektrolyse entstehende Chlor in situ für die Oxidation des Quecksilber-I-chlorids zu löslichem Quecksilber-II-chlorid verwendet wird.To achieve this object, the invention is characterized in that when an electrolysis cell is used in which the chlorine developed at the anode during the oxidation can migrate unhindered into the cathode region of the cell, the chlorine formed in the electrolysis cell during the electrolysis in situ for the oxidation of mercury-I-chloride is used to form soluble mercury-II-chloride.
Man verzichtet somit auf die gesonderte Leitung des bei der Elektrolyse entsthenden Chlorgases zum Oxidationsreaktor. Vielmehr werden die Oxidation und die Elektrolyse in ein- und derselben Elektrolysezelle durchgeführt, so daß das bei der Elektrolyse entstehende Chlorgas direkt und ungehindert auch in den Kathodenbereich der Zelle wandern kann. Das bei der Elektrolyse entstehende gasförmige Chlor wird also im allgemeinen im Elektrolyten gelöst und mit dem Elektrolyten transportiert, ggfs. unterstützt durch eine Pumpe oder dergleichen. Das gesamte Volumen des Elektrolyten steht somit für die Oxidation des Quecksilber-I-chlorids zu Quecksilber-II-chlorid mittels des (gasförmigen bzw. gelösten) Chlors zur Verfügung.The separate conduction of the chlorine gas evolving during electrolysis to the oxidation reactor is therefore dispensed with. Rather, the oxidation and the electrolysis are carried out in one and the same electrolysis cell, so that the chlorine gas generated during the electrolysis can also migrate directly and unhindered into the cathode region of the cell. The gaseous chlorine formed in the electrolysis is therefore generally dissolved in the electrolyte and transported with the electrolyte, possibly supported by a pump or the like. The entire volume of the electrolyte is thus available for the oxidation of the mercury I chloride to mercury II chloride by means of the (gaseous or dissolved) chlorine.
Bevorzugt wird für die geschilderte Verfahrensführung eine Festbett-Elektrolysezelle verwendet, ohne separaten Anolytkreislauf und mit einem Diaphragma, das den direkten Kontakt mit der Gegenelektrode verhindert, den Stoffaustausch jedoch nicht behindert. Sie ist in einer grundlegenden Ausführungsform bekannt geworden durch die deutsche Patentschrift 26 22 497 und in einer verbesserten Ausführungsform durch die DE-PS 29 04 539 der Anmelderin. Eine abermals verbesserte Ausführungsform beschreibt die DE-PS 35 32 573 der Anmelderin. Alle diese Ausführungsformen können für die Erfindungsgemäße Verfahrensführung eingesetzt werden.A fixed bed electrolysis cell is preferably used for the process described, without a separate anolyte circuit and with a diaphragm which prevents direct contact with the counterelectrode but does not hinder the mass transfer. It is known in a basic embodiment by the German patent specification 26 22 497 and in an improved embodiment by the applicant's DE-PS 29 04 539. A further improved embodiment describes the applicant's DE-PS 35 32 573. All of these embodiments can be used for carrying out the method according to the invention.
Das erfindungsgemäße Verfahren wird so geführt, daß der Elektrolyt zumindest anfänglich in einer solchen Konzentration an Quecksilber-I-chlorid verwendet wird und/oder daß die Elektrolysespannung und damit der Elektrolysestrom zumindest anfänglich in einer solchen Höhe angewendet werden, daß sich metallisches Quecksilber an der Kathode abscheidet und von dort abtropft. Es kann dann aus dem Boden der Elektrolysezelle abgezogen werden. Als Werkstoff für die Kathode eignet sich hierbei besonders Eisen, Silber, Nickel, Kupfer, Cadmium, Aluminium, Zink, Zinn oder eine Legierung dieser Metalle.The process according to the invention is carried out in such a way that the electrolyte is used at least initially in such a concentration of mercury-I chloride and / or that the electrolysis voltage and thus the electrolysis current are used at least initially at such a level that metallic mercury is used deposits on the cathode and drips from there. It can then be withdrawn from the bottom of the electrolytic cell. Iron, silver, nickel, copper, cadmium, aluminum, zinc, tin or an alloy of these metals is particularly suitable as the material for the cathode.
Abweichend vom Vorschlag der schon erwähnten deutschen Auslegeschrift 20 11 610 wird somit beim erfindungsgemäßen Verfahren anodisch gebildetes Chlor zum Oxidieren des schwer löslichen Quecksilber-I-chlorids verwendet, das dieses Salz dann auflöst, wodurch die Ausgangs-Suspension der Elektrolyse erst zugänglich gemacht wird.Deviating from the proposal of the already mentioned German specification 20 11 610, anodically formed chlorine is thus used in the process according to the invention to oxidize the poorly soluble mercury-I chloride, which then dissolves this salt, whereby the initial suspension is only made accessible to electrolysis.
Versuche haben gezeigt, daß es genügen kann, wenn die Elektrolysespannung und damit der Elektrolysestrom nur anfänglich über eine verhältnismäßig kurze Zeit in einer Spannungsspitze angelegt wird, nämlich solange, bis sich ein erster Quecksilberfilm auf der Oberfläche der Amalgamkathode gebildet hat. Anschließend kann die Spannung auf normale Werte wieder heruntergefahren werden und das Quecksilber scheidet sich weiter in metallischer Form auf der Oberfläche der Amalgamkathode ab. Entsprechendes gilt für die Konzentration an Hg₂Cl₂ im Elektrolyten.Experiments have shown that it can suffice if the electrolysis voltage and thus the electrolysis current are only initially applied in a voltage spike for a relatively short time, namely until a first mercury film has formed on the surface of the amalgam cathode. The voltage can then be reduced to normal values again and the mercury continues to deposit in metallic form on the surface of the amalgam cathode. The same applies to the concentration of Hg₂Cl₂ in the electrolyte.
Dem erfindungsgemäßen Verfahren liegt die Theorie zugrunde, daß an der Anode des Elektrolysegeräts Cl⁻ in Cl₂ übergeht. Das Cl₂ reagiert mit dem in Suspensionsform vorliegenden Hg₂Cl₂ und ergibt 2HgCl₂, welches im Elektrolyten gelöst ist.The inventive method is based on the theory that at the anode of the electrolysis device Cl⁻ in Cl₂ passes. The Cl₂ reacts with the Hg₂Cl₂ in suspension form and gives 2HgCl₂, which is dissolved in the electrolyte.
An der Kathode wird das HgCl₂ zu Hgo+2Cl⁻ reduziert. Dieses Cl⁻ steht dann für die Oxidation der Kathode zur Verfügung.At the cathode, the HgCl₂ is reduced to Hg o + 2Cl⁻. This Cl⁻ is then available for the oxidation of the cathode.
Als elektrochemische Gleichung geschrieben ergibt sich also folgendes:Written as an electrochemical equation, the following results:
Ausgangsreaktion (nur als Beispiel) wie Hg₂Cl₂ als Suspension in einem Elektrolyten entstehen kann:
(A) Hgo (gasförmig) + HgCl₂ (löslich) = Hg₂Cl₂ (schwerlöslich)
Initial reaction (only as an example) of how Hg₂Cl₂ can be formed as a suspension in an electrolyte:
(A) Hg o (gaseous) + HgCl₂ (soluble) = Hg₂Cl₂ (hardly soluble)
(B) Hg₂Cl₂ (schwerlöslich) + Cl₂ (gasförmig) = 2HgCl₂ (löslich)
(B) Hg₂Cl₂ (hardly soluble) + Cl₂ (gaseous) = 2HgCl₂ (soluble)
(C) HgCl₂ (löslich) + elektr. Energie = Hgo (flüssig) + Cl₂ (gasförmig)
(C) HgCl₂ (soluble) + electr. Energy = Hg o (liquid) + Cl₂ (gaseous)
Aus Hgo (gasförmig) + Energie erhält man also Hgo (flüssig)
Das in Stufe C entstehende Cl₂ (gasförmig) wird als solches und in situ in Stufe B verwendet.Hg o (gaseous) + energy gives Hg o (liquid)
The Cl₂ (gaseous) formed in stage C is used as such and in situ in stage B.
Diese elektrochemischen Reaktionen sind ein zumindest grobes Bild für die sich tatsächlich während der Elektrolyse abspielenden Vorgänge. In Wirklichkeit können diese Vorgänge komplizierter ablaufen, beispielsweise über entsprechende Komplexe oder Mehrfach-Reaktionen.These electrochemical reactions are at least a rough picture of the processes actually taking place during electrolysis. In reality, these processes can be more complicated, for example via corresponding complexes or multiple reactions.
Bei einem Ausführungsbeispiel, wobei Kupfer als Kathodenmaterial genommen wurde, hatte der verwendete Elektrolyt die folgende Zusammensetzung:
45 g/l Hg₂Cl₂ als Suspension
30 g/l Schwefelsäure
10 g/l Chlorid.
In one embodiment, using copper as the cathode material, the electrolyte used had the following composition:
45 g / l Hg₂Cl₂ as a suspension
30 g / l sulfuric acid
10 g / l chloride.
Die anodische Stromdichte betrug 300 A/m². Es handelte sich hierbei um Streckmetall, so daß dieser Wert auf die gesamte Fläche einschließlich der Lücken bezogen ist. Die kathodische Stromdichte betrug ebenfalls 300 A/m².The anodic current density was 300 A / m². It was expanded metal, so that this value relates to the entire area including the gaps. The cathodic current density was also 300 A / m².
Der Anfangsgehalt an wasserunlöslichem Hg₂Cl₂ war gleich der schon genannten Konzentration der Suspension von 45 g/l. Die Anfangsstromdichte betrug 600 A/m².The initial content of water-insoluble Hg₂Cl₂ was equal to the above-mentioned concentration of the suspension of 45 g / l. The initial current density was 600 A / m².
Claims (3)
dadurch gekennzeichnet,
daß bei Verwendung einer Elektrolysezelle, in der das bei der Oxidation an der Anode entwickelte Chlor ungehindert in den Kathodenbereich der Zelle wandern kann, das in der Elektrolysezelle bei der Elektrolyse entstehende Chlor in situ für die Oxidation des Quecksilber-I- Chlorids zu löslichem Quecksilber-II-chlorid verwendet wird.1. Process for the deposition of metallic mercury from an electrolyte by means of electrolysis, the mercury -I-chloride (Hg₂Cl₂) in suspension-containing electrolyte reacting with chlorine, which oxidizes the mercury-I-chloride to soluble mercury-II-chloride (HgCl₂) which is reduced cathodically to liquid mercury by means of electrolysis with the development of chlorine at the anode,
characterized by
that when using an electrolysis cell in which the chlorine developed during oxidation at the anode can migrate unhindered into the cathode region of the cell, the chlorine formed in the electrolysis cell during the electrolysis in situ for the oxidation of the mercury-I chloride to soluble mercury II chloride is used.
dadurch gekennzeichnet,
daß eine Festbett-Elektrolysezelle verwendet wird.2. The method according to claim 1,
characterized by
that a fixed bed electrolytic cell is used.
dadurch gekennzeichnet,
daß als Werkstoff für die Kathode Eisen, Silber, Nickel, Kupfer, Cadmium, Aluminium, Zink, Zinn oder eine Legierung dieser Metalle verwendet wird.3. The method according to claim 1 or 2,
characterized by
that iron, silver, nickel, copper, cadmium, aluminum, zinc, tin or an alloy of these metals is used as the material for the cathode.
Priority Applications (1)
| Application Number | Priority Date | Filing Date | Title |
|---|---|---|---|
| AT88103269T ATE76450T1 (en) | 1987-03-21 | 1988-03-03 | METHOD OF SEPARATION OF MERCURY BY MEANS OF ELECTROLYSIS. |
Applications Claiming Priority (2)
| Application Number | Priority Date | Filing Date | Title |
|---|---|---|---|
| DE3709359 | 1987-03-21 | ||
| DE19873709359 DE3709359A1 (en) | 1987-03-21 | 1987-03-21 | METHOD FOR DEPOSITING MERCURY BY ELECTROLYSIS |
Publications (2)
| Publication Number | Publication Date |
|---|---|
| EP0283785A1 true EP0283785A1 (en) | 1988-09-28 |
| EP0283785B1 EP0283785B1 (en) | 1992-05-20 |
Family
ID=6323699
Family Applications (1)
| Application Number | Title | Priority Date | Filing Date |
|---|---|---|---|
| EP88103269A Expired - Lifetime EP0283785B1 (en) | 1987-03-21 | 1988-03-03 | Process for recovering mercury by electrolysis |
Country Status (10)
| Country | Link |
|---|---|
| EP (1) | EP0283785B1 (en) |
| JP (1) | JPS63266085A (en) |
| KR (1) | KR880011373A (en) |
| AT (1) | ATE76450T1 (en) |
| CA (1) | CA1317560C (en) |
| DE (2) | DE3709359A1 (en) |
| ES (1) | ES2031941T3 (en) |
| GR (1) | GR3005241T3 (en) |
| IN (1) | IN168897B (en) |
| PT (1) | PT87018B (en) |
Cited By (1)
| Publication number | Priority date | Publication date | Assignee | Title |
|---|---|---|---|---|
| WO1994009167A1 (en) * | 1992-10-19 | 1994-04-28 | General Electric Company | Extraction of mercury and mercury compounds from contaminated material and solutions |
Citations (3)
| Publication number | Priority date | Publication date | Assignee | Title |
|---|---|---|---|---|
| DE2011610C3 (en) * | 1969-03-11 | 1980-01-03 | Ppg Industries, Inc., Pittsburgh, Pa. (V.St.A.) | Process for obtaining a metal from a solution containing traces of the metal ion by means of electrolysis |
| DD160806A1 (en) * | 1980-08-01 | 1984-03-14 | Buna Chem Werke Veb | PROCESS FOR PROCESSING MICRO-LIQUID ACTIVE CARBON |
| EP0179040A2 (en) * | 1984-10-19 | 1986-04-23 | Boliden Contech Ab | A method for the purification of gases containing mercury and simultaneous recovery of the mercury in metallic form |
Family Cites Families (1)
| Publication number | Priority date | Publication date | Assignee | Title |
|---|---|---|---|---|
| AT11882B (en) * | 1901-12-24 | 1903-05-11 | Siemens Ag |
-
1987
- 1987-03-21 DE DE19873709359 patent/DE3709359A1/en not_active Ceased
-
1988
- 1988-03-03 DE DE8888103269T patent/DE3871202D1/en not_active Expired - Fee Related
- 1988-03-03 ES ES198888103269T patent/ES2031941T3/en not_active Expired - Lifetime
- 1988-03-03 AT AT88103269T patent/ATE76450T1/en not_active IP Right Cessation
- 1988-03-03 EP EP88103269A patent/EP0283785B1/en not_active Expired - Lifetime
- 1988-03-14 IN IN214/CAL/88A patent/IN168897B/en unknown
- 1988-03-17 KR KR1019880002842A patent/KR880011373A/en not_active Application Discontinuation
- 1988-03-17 CA CA000561755A patent/CA1317560C/en not_active Expired - Fee Related
- 1988-03-18 PT PT87018A patent/PT87018B/en not_active IP Right Cessation
- 1988-03-18 JP JP63063739A patent/JPS63266085A/en active Pending
-
1992
- 1992-07-21 GR GR920401575T patent/GR3005241T3/el unknown
Patent Citations (3)
| Publication number | Priority date | Publication date | Assignee | Title |
|---|---|---|---|---|
| DE2011610C3 (en) * | 1969-03-11 | 1980-01-03 | Ppg Industries, Inc., Pittsburgh, Pa. (V.St.A.) | Process for obtaining a metal from a solution containing traces of the metal ion by means of electrolysis |
| DD160806A1 (en) * | 1980-08-01 | 1984-03-14 | Buna Chem Werke Veb | PROCESS FOR PROCESSING MICRO-LIQUID ACTIVE CARBON |
| EP0179040A2 (en) * | 1984-10-19 | 1986-04-23 | Boliden Contech Ab | A method for the purification of gases containing mercury and simultaneous recovery of the mercury in metallic form |
Non-Patent Citations (1)
| Title |
|---|
| CHEMICAL ABSTRACTS, Band 79, Nr. 26, 31. Dezember 1973, Columbus, Ohio, USA T. TAURA et al.; "Removing Mercury from gas" seite 70, spalte 2, Zusammenfassung Nr. 147 804e & JP-B-48 017 690 * |
Cited By (1)
| Publication number | Priority date | Publication date | Assignee | Title |
|---|---|---|---|---|
| WO1994009167A1 (en) * | 1992-10-19 | 1994-04-28 | General Electric Company | Extraction of mercury and mercury compounds from contaminated material and solutions |
Also Published As
| Publication number | Publication date |
|---|---|
| ATE76450T1 (en) | 1992-06-15 |
| IN168897B (en) | 1991-07-06 |
| CA1317560C (en) | 1993-05-11 |
| JPS63266085A (en) | 1988-11-02 |
| PT87018A (en) | 1988-04-01 |
| DE3709359A1 (en) | 1988-09-29 |
| DE3871202D1 (en) | 1992-06-25 |
| GR3005241T3 (en) | 1993-05-24 |
| KR880011373A (en) | 1988-10-28 |
| PT87018B (en) | 1992-06-30 |
| ES2031941T3 (en) | 1993-01-01 |
| EP0283785B1 (en) | 1992-05-20 |
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