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Publication numberUS2390591 A
Publication typeGrant
Publication dateDec 11, 1945
Filing dateNov 8, 1941
Priority dateNov 8, 1941
Publication numberUS 2390591 A, US 2390591A, US-A-2390591, US2390591 A, US2390591A
InventorsJanes Milton
Original AssigneeNat Carbon Co Inc
Export CitationBiBTeX, EndNote, RefMan
External Links: USPTO, USPTO Assignment, Espacenet
Electrolytic method for producing oxygen
US 2390591 A
Abstract  available in
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Claims  available in
Description  (OCR text may contain errors)

Dec. 11, 1945. M. JANES ELECTROLYTIC METHOD FOR PRODUCING OXYGEN Filed NOVFB, 1941 ZZVAVl/AY/l A 4\\ v H .W Wm ma 9 W M wxkwimifir1W:mW m m m l m ATTORNEY stantial production 01 hydrogen peroxide.

Patented Dec. 11, 1945 OFFICE Milton Janes, Lakewood, Ohio, as'signor to Nav I I tional' Carbon Compan New York y, Inc., a corporation of Application November 8, 1941, Serial No. 418,390

3 Claims.

. Electrolysis of aqueous solutions of caustic alkalisor of oxygen-containing acids has been used as a method of obtaining very pure hydrogen and oxygen. The best known types of commercial cells for this purpose comprise electrodes of irongroup metal, usually of nickel-plated iron, separated by an asbestos cloth diaphragm, and as an electrolyte a solution of sodium hydroxide or potassium hydroxide in a concentration between 10% and 35%. Published data indicate that such cells can produce about 150 grams of oxygen per kilowatt-hour. Considered solely as a source of oxygen, electrolysis is so much more costly than air-separation methods that it has not competed with the latter methods; rather, it has been used as a source of pure hydrogen, the oxygen being a by-product.

The electrolytic production of oxygen offers some attractive advantages. The necessary equipment is relatively simple, inexpensive, small in volume, and durable, and requires little labor in operation and maintenance. The cost of the electrical energy is, in fact, the main impediment which has prevented the more widespread use of the electrolytic method. Another item of expense, which under some circumstances is material, is the cost of distilled water which is consumed in the process.

It is the principal object of the present invention to increase the yield of oxygen per unit of electrical energy consumed in the electrolytic production of oxygen. Another object is to provide an electrolytic method for producing oxygen, in which no hydrogen gas is liberated and which consumes no water. A further object is to produce pure oxygen by the electrolysis of aqueous caustic solutions without the use of an interelectrode diaphragm. Another object is a method, capable of producing per unit of electrical energy from two to two and one half, or even -more, times as much oxygen as is produced by electrolytic methods and apparatus heretofore used commercially. Still another object is an electrolytic method which consumes little or no water by electrolysis.

The principal feature of the invention is the use of a continuously depolarized cathode, suitably an air-depolarized porous carbon cathode, in

combination with an insoluble or passive anode in an aqueous electrolyte of potassium hydroxide or sodium hydroxide. I have found that, at convenient current densities, not only is no hydrogen liberated at such a cathode but there is a sub- The hydrogen not oxidized to the peroxide is oxidized to water. When no inter-electrode diaphragm is used, hydrogen peroxide finds its way to the anode where it gives up oxygen and regenerates waten.

By. providing a depolarized cathode," and by eliminating the customary diaphragm, the overall voltage drop through the cell at a given current is materially lowered, thereby decreasing the electrical energy consumption. Oxidation at the anode of peroxideproduced at the cathode yields twice as much oxygen per unit of electrical current as can be produced by the discharge of hydroxyl ions in the absence of hydrogen peroxide. As a result, it is readily possible to produce, per unit of energy, over twice as much oxygen as can be produced in conventional cells.

An example of an electrolytic cell suitable for use in practicing the invention is illustrated in the accompanying drawing'in which:

Fig. 1 isa side sectional view, along Il of Fig. 2, of an electrolytic cell,

Fig. 2 is a top sectional view along 2--2 of Fig. 1, and

Fig. 3 is a 'side sectional fragmentary view, along 3-3 of Fig. 2, showing a detail of the cell of Figs. 1 and 2.

The cell shown in Figs. 1 to 3-comprises an outer container Ill of caustic-resistant insulating material, or of a metal resistant to caustic, such as iron; 2. body of caustic alkali electrolyte H, suitably an aqueous solution containing about 10% to 35% of potassium hydroxide or sodium hydroxide or a mixture thereof, a solution containing 25% potassium hydroxide being preferred; an insoluble or passive metal anode [2, which is preferably hollow and provided with means, such as pipes I5 and I6, for circulating a coolant, and which is preferably composed of one or more metals of the iron group (iron, cobalt, nickel); and a porous carbon cathode I3 sealed into and supported by an insulating frame It in such a manner as to provide a space or well for the access of air to the rear surface of the cathode l3. Above the electrolyte II is an oxygen-collecting manifold from which oxygen may be withdrawn through a conduit ll. Suitable electrical connections l8 and 19 may be provided for the anode and cathode.

The porous cathode l3 should be composed of active carbon, by which is meant herein and in the appended claims carbon of the kind that can transfer oxygen of the air to the cathode: catholyte interface in electrochemically active form where it acts as a depolarizing agent. A

suitable material is that used in air-depolarized primary galvanic cells, made in any of the several known ways, and rendered resistant to penetra tion by the electrolyte. For example, the electrode materials described in Patents 2,010,608,

issued-August 6, 1935, to E. A. Schumacher, V. C. Hamister, and G. W. Heise, and 2,017,280 issued October 15. 1935, to G. W. Heise and E. A. Schumacher, are satisfactory for use in the present invention.

Although the cathode l3 shown in the drawing is a single flat plate, modifications can of course be made. For instance, an electrode of large area may be fabricated from a number ,of smallplates, electrically interconnected, supported in a frame in a manner analogous to glass in a multi-paned window. Instead of a flat plate having one wet face and one dry face, a hollow carbon electrode may be used, the hollow being open to the air. Circulation of the; air to the bottom of the space behind the cathode may be improved by blowing air through the tube 2| shown in Figs. 1 and 2.

The anode is preferably cooled because best efliciencies are obtained when the cell is operated at a low temperature.

Under some circumstances, as at high current densities, it-will be advantageous to have the depolarizing air in the space or well 20 behind the cathode I3 under pressure.

As an example of the results obtainable by the use of the invention, operating data obtained during the use of a cell comprising a nickel gauze anode, a porous carbon air-depolarized cathode, and a 25% solution of potassium hydroxide in water, at an electrolyte temperature of C., are given in the following table:

A 0 th d Average, verage a o e grams of g g current oxygen per voltage p density kilowatthour The foregoing data indicate the general magnitude of the increase in yield of oxygen, per unit of energy, afforded by the invention. The electrolytic cell is of simple'construction, and can be made of inexpensive yet durable materials. Since no hydrogen is produced, the only loss of water is by evaporation and entrainment, there is no problem of collecting and disposing of hydrogen, nor is there any problem of preventing the diffusion of hydrogen to the anode. There is no hazard of hydrogen explosions in the cell room.

Where electric power is cheap, and where because of intermittent or small demand for oxygen, or for other reasons, it is incovenient or unduly expensive to obtain oxygen manufactured by airseparation methods, the present invention provides pure oxygen at moderate cost and with inexpensive pparatus.

I claim:

1. In a, process for producing oxygen by electrolyzing an aqueous solution between an anode and a cathode to produce oxygen at theanode, the improvement which comprises continuously depolarizing the cathode with oxygen'to prevent the evolution of hydrogen, and promptly electrolyzing at the anode the product of such cathodic depolarization. 1 i

2. A process for producing oxygen at a, rate upwards of 300 grams per kilowatt hour of electrical energy which comprises electrolyzing between an anode and a cathode an aqueous caustic alkali solution, collecting the oxygen thereby produced, and depolarizin the cathode continuously with atmospheric oxygen to prevent the evolution of hydrogen, and promptly electrolyzing at the anode the product of such cathodic depolarization.

3. A process for producing oxygen at a rate I upwards of 340 grams per kilowatt hour of electrical energy which comprises electrolyzing between an anode and an air-depolarized carbon cathode n aqueous solution essentially comprising potassium hydroxide, mingling catholyte, containing cathodic depolarization product, with the anolyte, and collecting the oxygen thereby produced.

MILTON J ANES.

Referenced by
Citing PatentFiling datePublication dateApplicantTitle
US2470073 *Aug 16, 1944May 10, 1949Fmc CorpElectrolytic cell and method of operating same
US2681884 *Feb 3, 1950Jun 22, 1954Diamond Alkali CoBrine electrolysis
US2681887 *Feb 3, 1950Jun 22, 1954Diamond Alkali CoElectrolytic cell
US2951802 *Jun 5, 1957Sep 6, 1960Joseph C WhiteElectrolytic oxygen generator
US2984607 *Feb 24, 1958May 16, 1961White Joseph CMethod of producing oxygen and hydrogen by electrolysis
US3057946 *Dec 31, 1959Oct 9, 1962Electric Storage Battery CoFuel cell system
US3124520 *Sep 28, 1959Mar 10, 1964 Electrode
US3188283 *Jan 3, 1961Jun 8, 1965Cons Electrodynamics CorpElectrolytic process for removing moisture
US3236760 *Nov 9, 1959Feb 22, 1966Oronzio De Nora ImpiantiCells for the production of chlorine from hydrochloric acid
US3316167 *Sep 1, 1961Apr 25, 1967Exxon Research Engineering CoMulti-cell reactor in series
US3342717 *Aug 2, 1963Sep 19, 1967Pullman IncElectrochemical cell
US3394062 *Jun 30, 1964Jul 23, 1968Henes Mfg CompanyMethod for the electrolytic production of hydrogen and oxygen
US3888749 *Aug 31, 1972Jun 10, 1975Sun Research DevelopmentElectrolytic separation of oxygen from air
US3915836 *Apr 4, 1974Oct 28, 1975Bayer AgHCl electrolysis frame with a graphite plate arranged therein
US4300987 *Nov 5, 1979Nov 17, 1981Tseung Alfred C CGas extraction
US4302320 *Aug 14, 1979Nov 24, 1981Lewis Arlin CCopper
US5425859 *May 11, 1993Jun 20, 1995Rockwell International CorporationElectrochemical reduction
US5549445 *Nov 1, 1991Aug 27, 1996Schremp; Edward J.Macro-engineering process and system for all-weather at-sea wind-energy extraction
EP0005325A1 *Apr 11, 1979Nov 14, 1979Alfred Chan Chung TseungMethod for separating a gas from a gaseous mixture and electrochemical cell therefor
WO1979000933A1 *Apr 11, 1979Nov 15, 1979S JasemGas extraction
Classifications
U.S. Classification205/635, 204/DIG.300, 204/294
International ClassificationC25B1/02
Cooperative ClassificationY10S204/03, C25B1/02
European ClassificationC25B1/02