US3756930A - Electroly recovery of chlorine and hydrogen from aqueous hydrochloric - Google Patents
Electroly recovery of chlorine and hydrogen from aqueous hydrochloric Download PDFInfo
- Publication number
- US3756930A US3756930A US00157766A US3756930DA US3756930A US 3756930 A US3756930 A US 3756930A US 00157766 A US00157766 A US 00157766A US 3756930D A US3756930D A US 3756930DA US 3756930 A US3756930 A US 3756930A
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- US
- United States
- Prior art keywords
- acid
- cell
- chlorine
- hydrogen
- weight
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- 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.)
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- C—CHEMISTRY; METALLURGY
- C25—ELECTROLYTIC OR ELECTROPHORETIC PROCESSES; APPARATUS THEREFOR
- C25B—ELECTROLYTIC OR ELECTROPHORETIC PROCESSES FOR THE PRODUCTION OF COMPOUNDS OR NON-METALS; APPARATUS THEREFOR
- C25B1/00—Electrolytic production of inorganic compounds or non-metals
- C25B1/01—Products
- C25B1/24—Halogens or compounds thereof
- C25B1/26—Chlorine; Compounds thereof
Definitions
- Aqueous hydrochloric acid is electrolyzed in a di aphragm cell to recover chlorine and hydrogen therefrom.
- the acid to be electrolyzed should have a concentration of from 18 to 28% by weight of HCl and should be degraded by not more than 2% by weight during its passage through the cell.
- the mean temperature in the cell is kept at from 75 to 90 C.
- This object may be achieved for example by appropriate choice of the diaphragm which prevents mixing of the gases formed on the cathode and anode sides but does not impede the flow of current.
- Another possibility is to decrease the resistance in the electrolyte by carrying out the electrolysis in the region of maximum conductivity of hydrochloric acid, or to decrease the hydrogen overvltage at the graphite cathodes generally used.
- the hydrogen overvoltage may be lowered for example in known manner by adding certain metals to the electrolyte, the added metal cations being deposited in the course of the electrolysis on the cathodes and the electrolytic decomposition takes place at the layers of the electrodes thus activated with a decrease in the overvoltage.
- Metals of the platinum group, copper, nickel, antimony, silver, molybdenum and cobalt are preferred as metals and they may be added to the electrolytes either batchwise or continuously.
- acids having an HCl concentration of more than 20% up to about 26% by weight are used.
- the rate of flow of the acid is controlled so that a concentration gradient between the acid introduced into the electrolyzer and the acid withdrawn of more than 3% by weight, for example of 5% by weight, is maintained. Since there is no freedoin as regards the temperature of the acid leaving the cell because of its HCl partial pressure (generally a temperature of the effluent acid of C. should not be exceeded) it is necessary to cool the acid strongly before it enters the cell. In this way the mean temperature in the cell is kept fairly low.
- the temperature range used is therefore one in which the hydrochloric acid has a low conductivity 30 that an increased amount of energy has to be used.
- the acid being electrolyzed is preferably degraded by from 0.5 to 1.6% by weight.
- the low degradation of the hydrochloric acid is achieved by passing the acid to be electrolyzed at an increased rate of flow through the cathode and anode chambers at the known and conventional current densities of from 2000 to 5000 amperes per square meter. In this way it is possible to eliminate the resistance produced by the gas bubbles forming at the electrodes, as the bubbles are rapidly detached from the cathode and anode and entrained. A considerable decrease in the cell potential is thus achieved by simple means.
- Another advantage of the method in accordance with the invention is that it is possible to use a higher mean cell temperature. Because of the increased throughput of acid it is possible to allow the acid to enter at a relatively high temperature and a further gain of potential is achieved because of the higher conductivity of hydrochloric acid at increasing temperatures.
- EXAMPLE A 25% by weight hydrochloric acid is passed through a diaphragm cell (having an anode area of 2.32 m. and consisting of thirty successive individual cells) at such a rate that the concentration of the degraded acid leaving the cell is 21.5%. At a current of 9400 amperes a cell potentail of 2.25 volts is measured. The mean temperature of the acid is 65 C.
- a process as claimed in claim 1 wherein said aqueous hydrochloric acid being electrolyzed is substantially free of metal additives which lower the hydrogen overvoltage at the cathodes of the cell.
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- Chemical & Material Sciences (AREA)
- Inorganic Chemistry (AREA)
- Engineering & Computer Science (AREA)
- Chemical Kinetics & Catalysis (AREA)
- Electrochemistry (AREA)
- Materials Engineering (AREA)
- Metallurgy (AREA)
- Organic Chemistry (AREA)
- Electrolytic Production Of Non-Metals, Compounds, Apparatuses Therefor (AREA)
Abstract
AQUEOUS HYDROCHLORIC ACID IS ELECTROLYZED IN A DIAPHRAGM CELL TO RECOVER CHLORINE AND HYDROGEN THEREFROM. THE ACID TO BE ELCTROLYZED SHOULD HAVE A CONCENTRATION OF FROM 18 TO 28% BY WEIGHT OF HCL AND SHOULD BE DEGRADED BY NOT MORE THAN 2% BY WEIGHT DURING ITS PASSAGE THROUGH THE CELL. THE MEAN TEMPERATURE IN THE CELL IS KEPT AT FROM 75* TO 90*C.
Description
United States Patent O ifice 3,756,930 Patented Sept. 4, 1973 U.S. Cl. 204-429 3 Claims ABSTRACT OF THE DISCLOSURE Aqueous hydrochloric acid is electrolyzed in a di aphragm cell to recover chlorine and hydrogen therefrom. The acid to be electrolyzed should have a concentration of from 18 to 28% by weight of HCl and should be degraded by not more than 2% by weight during its passage through the cell. The mean temperature in the cell is kept at from 75 to 90 C.
In the chlorinating substitution of organic compounds, half of the chlorine originally used is obtained as hydrogen chloride. Since this cannot always be used and nowadays disposal thereof with efiluents is often out of the question, the need for recovery of the chlorine from hydrogen chloride gains continually in importance. Two methods have been adopted: hydrogen chloride is oxidized with air or oxygen in the presence of catalysts, or hydrochloric acid is first formed from the gaseous hydrogen chloride by absorption and the resultant acid is subjected to electrolytic decomposition to recover chlorine and hydrogen. These methods of recovering chlorine differ from the widely used chlor-alkali method in that it is possible to produce chlorine without the simultaneous production of alkali and therefore the alkali-chlorine balance is not affected.
In the electrolytic recovery of chlorine from aqueous hydrochloric acid, which is preferably carried out in diaphragm cells, the energy consumption plays a significant part as in all electrochemical processes. There has therefore been no lack of attempts in the course of the years to decrease the consumption of energy as far as possible by decreasing the achievable cell potential.
This object may be achieved for example by appropriate choice of the diaphragm which prevents mixing of the gases formed on the cathode and anode sides but does not impede the flow of current. Another possibility is to decrease the resistance in the electrolyte by carrying out the electrolysis in the region of maximum conductivity of hydrochloric acid, or to decrease the hydrogen overvltage at the graphite cathodes generally used. The hydrogen overvoltage may be lowered for example in known manner by adding certain metals to the electrolyte, the added metal cations being deposited in the course of the electrolysis on the cathodes and the electrolytic decomposition takes place at the layers of the electrodes thus activated with a decrease in the overvoltage. Metals of the platinum group, copper, nickel, antimony, silver, molybdenum and cobalt are preferred as metals and they may be added to the electrolytes either batchwise or continuously.
In carrying out the hydrochloric acid electrolysis, acids having an HCl concentration of more than 20% up to about 26% by weight are used. The rate of flow of the acid is controlled so that a concentration gradient between the acid introduced into the electrolyzer and the acid withdrawn of more than 3% by weight, for example of 5% by weight, is maintained. Since there is no freedoin as regards the temperature of the acid leaving the cell because of its HCl partial pressure (generally a temperature of the effluent acid of C. should not be exceeded) it is necessary to cool the acid strongly before it enters the cell. In this way the mean temperature in the cell is kept fairly low. The temperature range used is therefore one in which the hydrochloric acid has a low conductivity 30 that an increased amount of energy has to be used.
We have now found that the electrolysis of hydrochloric acid can be carried out with economically favorable current consumption and low potential and without adding substances to decrease the overvoltage when the acid to be electrolyzed has a concentration of from 18 to 28% by weight of HCl, the acid electrolyzed is degraded to the extent of not more than 2% by weight of HCl and the mean temperature of the acid in the cell is kept at from 75 to C.
The acid being electrolyzed is preferably degraded by from 0.5 to 1.6% by weight.
The low degradation of the hydrochloric acid is achieved by passing the acid to be electrolyzed at an increased rate of flow through the cathode and anode chambers at the known and conventional current densities of from 2000 to 5000 amperes per square meter. In this way it is possible to eliminate the resistance produced by the gas bubbles forming at the electrodes, as the bubbles are rapidly detached from the cathode and anode and entrained. A considerable decrease in the cell potential is thus achieved by simple means.
Another advantage of the method in accordance with the invention is that it is possible to use a higher mean cell temperature. Because of the increased throughput of acid it is possible to allow the acid to enter at a relatively high temperature and a further gain of potential is achieved because of the higher conductivity of hydrochloric acid at increasing temperatures.
The following example illustrates the invention.
EXAMPLE (A) A 25% by weight hydrochloric acid is passed through a diaphragm cell (having an anode area of 2.32 m. and consisting of thirty successive individual cells) at such a rate that the concentration of the degraded acid leaving the cell is 21.5%. At a current of 9400 amperes a cell potentail of 2.25 volts is measured. The mean temperature of the acid is 65 C.
(B) If the acid being electrolyzed is degraded from 25% by weight to only 23.5% by weight, the cell potential is 2.03 volts at a mean temperature of the acid in the cell of 77 C.
We claim:
1. In a process for the electrolytic recovery of chlorine and hydrogen by continuous flow of aqueous hydrochloric acid through a diaphragm cell having anode and cathode chambers maintained at a current density of from 2000 to 5000 amperes per square meter, the improvement which comprises introducing into said cell said aqueous 5 hydrochloric acid to be electrolyzed at a concentration of 18 to 28% by weight of HCl, conducting said acid through said cell at a fiow rate which is sufficiently high to degrade theacid by not more than 2% by weight and maintaaining the mean temperature of the acid in the cell at from 75 C. to 90 C.
2. A process as claimed in claim 1 wherein said flow rate of the acid is maintained sufiiciently high so as to degrade the acid by from 0.5 to 1.6% by weight.
3. A process as claimed in claim 1 wherein said aqueous hydrochloric acid being electrolyzed is substantially free of metal additives which lower the hydrogen overvoltage at the cathodes of the cell.
4 References Cited UNITED STATES PATENTS 2/1930 Low 204-128 2/1966 Messner 204-128 Us; Cl. X.R.
Da swimmer a 197? Patent NO "3 1175 6 @930 fi) Gueriith ex Weiss, Heinz Weller and. Ewalci p tified that erfor appears in the above-idehtified patent It is ear at are hereby corrected as shown below:
end that said Letters Pate Column 1, fiemh 11m, "$1213 28, 19% swam mm M July 8, 1970 Column 2, 1m 53, "p0tentai3. 'smuld potential Go1umn'3, line H, "maintaining" mould read maintaining Signed and sealed this 1st day of October 1974.,
(SEAL) Attest:
McCOY M. GIBSON JR Attesting Officer C, MARSHALL DANN Cormissioner of Patents FORM PC4050 I uscoMM-Dc wan-ps9 it U.5. GOVERNMENT PRlNTlNG OFFICE: [9S9 0-386-384,
Applications Claiming Priority (1)
Application Number | Priority Date | Filing Date | Title |
---|---|---|---|
DE19702033802 DE2033802A1 (en) | 1970-07-08 | 1970-07-08 | Process for the electrolytic recovery of chlorine from aqueous hydrochloric acid |
Publications (1)
Publication Number | Publication Date |
---|---|
US3756930A true US3756930A (en) | 1973-09-04 |
Family
ID=5776115
Family Applications (1)
Application Number | Title | Priority Date | Filing Date |
---|---|---|---|
US00157766A Expired - Lifetime US3756930A (en) | 1970-07-08 | 1971-06-28 | Electroly recovery of chlorine and hydrogen from aqueous hydrochloric |
Country Status (5)
Country | Link |
---|---|
US (1) | US3756930A (en) |
BE (1) | BE769632A (en) |
DE (1) | DE2033802A1 (en) |
FR (1) | FR2098096A5 (en) |
GB (1) | GB1346656A (en) |
Cited By (11)
Publication number | Priority date | Publication date | Assignee | Title |
---|---|---|---|---|
US4069120A (en) * | 1976-09-21 | 1978-01-17 | United Technologies Corporation | Photo-electrolytic production of hydrogen |
US4101394A (en) * | 1975-05-09 | 1978-07-18 | Ppg Industries, Inc. | Electrolytic method |
US4105516A (en) * | 1977-07-11 | 1978-08-08 | Ppg Industries, Inc. | Method of electrolysis |
US4160704A (en) * | 1977-04-29 | 1979-07-10 | Olin Corporation | In situ reduction of electrode overvoltage |
US4203814A (en) * | 1978-11-01 | 1980-05-20 | United Technologies Corporation | Hydrogen gas generation utilizing a bromide electrolyte and radiant energy |
US4203813A (en) * | 1978-11-01 | 1980-05-20 | United Technologies Corporation | Method for producing HBr |
US4263111A (en) * | 1979-12-17 | 1981-04-21 | United Technologies Corporation | Hydrogen generation utilizing semiconducting platelets suspended in a divergent vertically flowing electrolyte solution |
US4263110A (en) * | 1979-12-17 | 1981-04-21 | United Technologies Corporation | Hydrogen-bromine generation utilizing semiconducting platelets suspended in a vertically flowing electrolyte solution |
WO2003035938A2 (en) * | 2001-10-23 | 2003-05-01 | Bayer Materialscience Ag | Method for electrolysis of aqueous solutions of hydrogen chloride |
US20040067192A1 (en) * | 2002-10-07 | 2004-04-08 | The Procter & Gamble Company | Conversion of sodium bromide to anhydrous hydrobromic acid and sodium bisulfate |
US20040067191A1 (en) * | 2002-10-07 | 2004-04-08 | The Procter & Gamble Company | Conversion of sodium bromide to anhydrous hydrobromic acid and sodium bisulfate |
-
1970
- 1970-07-08 DE DE19702033802 patent/DE2033802A1/en active Pending
-
1971
- 1971-06-28 US US00157766A patent/US3756930A/en not_active Expired - Lifetime
- 1971-06-29 FR FR7123739A patent/FR2098096A5/fr not_active Expired
- 1971-07-07 GB GB3185871A patent/GB1346656A/en not_active Expired
- 1971-07-07 BE BE769632A patent/BE769632A/en unknown
Cited By (17)
Publication number | Priority date | Publication date | Assignee | Title |
---|---|---|---|---|
US4101394A (en) * | 1975-05-09 | 1978-07-18 | Ppg Industries, Inc. | Electrolytic method |
US4069120A (en) * | 1976-09-21 | 1978-01-17 | United Technologies Corporation | Photo-electrolytic production of hydrogen |
US4160704A (en) * | 1977-04-29 | 1979-07-10 | Olin Corporation | In situ reduction of electrode overvoltage |
US4105516A (en) * | 1977-07-11 | 1978-08-08 | Ppg Industries, Inc. | Method of electrolysis |
US4203814A (en) * | 1978-11-01 | 1980-05-20 | United Technologies Corporation | Hydrogen gas generation utilizing a bromide electrolyte and radiant energy |
US4203813A (en) * | 1978-11-01 | 1980-05-20 | United Technologies Corporation | Method for producing HBr |
US4263111A (en) * | 1979-12-17 | 1981-04-21 | United Technologies Corporation | Hydrogen generation utilizing semiconducting platelets suspended in a divergent vertically flowing electrolyte solution |
US4263110A (en) * | 1979-12-17 | 1981-04-21 | United Technologies Corporation | Hydrogen-bromine generation utilizing semiconducting platelets suspended in a vertically flowing electrolyte solution |
WO2003035938A2 (en) * | 2001-10-23 | 2003-05-01 | Bayer Materialscience Ag | Method for electrolysis of aqueous solutions of hydrogen chloride |
WO2003035938A3 (en) * | 2001-10-23 | 2003-10-09 | Bayer Ag | Method for electrolysis of aqueous solutions of hydrogen chloride |
US20040245117A1 (en) * | 2001-10-23 | 2004-12-09 | Andreas Bulan | Method for electrolysis of aqueous solutions of hydrogen chloride |
US7128824B2 (en) | 2001-10-23 | 2006-10-31 | Bayer Materialscience Ag | Method for electrolysis of aqueous solutions of hydrogen chloride |
US20040067192A1 (en) * | 2002-10-07 | 2004-04-08 | The Procter & Gamble Company | Conversion of sodium bromide to anhydrous hydrobromic acid and sodium bisulfate |
US20040067191A1 (en) * | 2002-10-07 | 2004-04-08 | The Procter & Gamble Company | Conversion of sodium bromide to anhydrous hydrobromic acid and sodium bisulfate |
US6811763B2 (en) | 2002-10-07 | 2004-11-02 | The Procter & Gamble Company | Conversion of sodium bromide to anhydrous hydrobromic acid and sodium bisulfate |
US20050135990A1 (en) * | 2002-10-07 | 2005-06-23 | Schaefer Jared J. | Conversion of sodium bromide to anhydrous hydrobromic acid and sodium bisulfate |
US7045109B2 (en) * | 2002-10-07 | 2006-05-16 | Procter & Gamble | Conversion of sodium bromide to anhydrous hydrobromic acid and sodium bisulfate |
Also Published As
Publication number | Publication date |
---|---|
FR2098096A5 (en) | 1972-03-03 |
BE769632A (en) | 1972-01-07 |
GB1346656A (en) | 1974-02-13 |
DE2033802A1 (en) | 1972-01-20 |
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