Patent Application
20090181312
The present invention relates to a novel type of storage battery which is distinguished by its unique electrochemistry. In the changed condition, the positive electrode comprises lead dioxide and the negative electrode comprises certain alloys that on charging absorb atomic hydrogen to form the metal hydride.
The most common storage battery, found in almost every vehicle, is the lead-acid battery. This battery comprises a lead dioxide positive electrode, a lead metal negative electrode, and sulfuric acid for the electrolyte. Its chief advantage is low cost. Nevertheless, it has a limited energy density and the electrolyte is extremely corrosive. Furthermore, sufficient acid is required to react with the electrodes during discharge. Maintenance-free types avoid the loss of evolved gases, as disclosed in U.S. Pat. No. 3,862,861, but their cycle-life is still restricted.
The search for alternatives to the lead-acid battery has been ongoing. As far back as 1934, Drumm disclosed the nickel-oxide zinc battery and the silver oxide-zinc battery (U.S. Pat. No. 1,955,115). Both of these batteries employ zinc as the negative electrode and caustic potash as the electrolyte. Nickel oxide or silver oxide serves as the positive electrode. These batteries have improved energy densities and for many uses are a good compromise.
The ideal storage battery would combine the best features of existing batteries with none of the drawbacks. The need for such a battery is apparent for backup systems and in mobile applications. Therefore, it is an object of the present invention to provide an improved storage battery, one that is both economical and highly efficient. These and other objects, features, and advantages of the invention will be recognized from the following description and accompanying figure.
A rechargeable battery has been developed in which the positive electrode comprises lead dioxide in the charged condition, a negative electrode comprising at least one of iron, lead, cadmium, and alloys, an alkaline electrolyte and electrical leads attached to the electrodes. Upon discharge, the lead dioxide is reduced to lead oxide and the metal is oxidized to an oxide. These reactions are reversed when the battery is charged.
The alloy of the negative electrode can be a metal hydride. The metal hydride can be, for example, a rare earth or another group made from of a titanium-zirconium composition.
The electrolyte of the cell is alkaline. Aqueous solutions of bases provide the alkalinity. These bases include ammonia and the hydroxides of the alkali metals, namely, lithium, sodium, potassium and cesium. In addition, tetramethyl ammonium hydroxide may be employed.
Other solutions can be used as the electrolyte as well. These include carbonates, borates, silicates, phosphates and sulfates. They may be introduced by the corresponding acids or their respective salts.
The electrodes of a practical embodiment of the invention may be configured as sheets, fibers, or particles thereby to maximize electrode surface area. Interspersed particles of a carbonaceous material may be used to improve the electrical conductivity. A gelling agent may be added to immobilize the electrolyte. As required, a separator may be employed between the positive and negative electrodes to prevent a short circuit.
The chemistry of the lead-alkaline battery is important in order to gain an understanding of its operation. A positive electrode initially made of lead becomes lead dioxide when changed which is reduced to lead oxide during discharge. In the case where the negative electrode comprises, for example, zinc, this metal is oxidized to zinc oxide when the cell is discharged. The electrolyte is alkaline such that the solution contains an excess of hydroxyl ions. The electrode reactions during discharge can be represented by the following equations:
PbO2+H2O+2 e−→PbO+2 OH− (1)
Zn+2 OH−→ZnO+H2O+2 e− (2)
In the above reaction, zinc hydroxide may be an intermediate in the formation of zinc oxide. When these equations are combined, the reaction for the cell is:
PbO2+Zn→PbO+ZnO (3)
In the overall reaction, there is no change in the average composition of the electrolyte during discharge although there may be concentration gradients.
During recharging of the cell, the reactions are reversed. Thus, lead oxide is oxidized to lead dioxide and zinc oxide is reduced to zinc metal. The emf necessary for charging is supplied by an external power source. The discharge-recharge cycle can be repeated endlessly, thus fulfilling the function of a storage battery.
A particularly difficult challenge in designing new batteries is identifying electrode materials that will undergo electrochemical reactions and still withstand corrosion by the electrolyte. Although theory is helpful in this respect, empirical data are required to prove the effectiveness of materials—both for the electrodes and the electrolyte. One measure of the relative performance of a cell is its open-circuit voltage. Another consideration is cycle life.
Zinc is used as an example of a negative electrode that can be used with the lead positive electrode and the electrolyte described herein. However, other materials can be used for the negative electrode, including but not limited to iron, lead, cadmium and metal hydrides. Metal hydrides are materials that comprise certain alloys that on charging absorb atomic hydrogen to form the metal hydride. At least two classes of alloys are suitable to form metal hydrides. One group of alloys is based on rare earths and generally consists of a lanthanum-nickel blend. A second group of alloys is made of a titanium-zirconium composition. The negative electrodes herein are provided by way of example and are not meant to be limiting. It is contemplated that other alloys can be used as a negative electrode in the battery embodiments disclosed herein.
The use of lead in an alkaline cell may seem questionable because lead in the +2 oxidation state commonly forms plumbous salts containing the positive divalent ion Pb++. However, by the action of hydroxides on plumbous compounds it is possible to form the negative ion HPbO2− which is soluble in aqueous solutions. Accordingly, Pb(OH)2 is regarded as an amphoteric hydroxide. In a similar manner, concentrated solutions of alkali hydroxides act upon the dioxide PbO2 to form plumbate ions, PbO4−4 and PbO3−2, which are likewise soluble.
In view of these considerations, one goal of the research on new cells was to control the concentration hydroxides in the electrolyte. This result was made possible by employing solutions of sodium carbonate which react as follows:
Na2CO3+H2ONaOH+NaHCO3 (4)
From this equation it is seen that such solutions are strongly alkaline. The carbonic acid set free on hyrdolysis does not escape when the base is strong but forms the bicarbonate. However, hydrolysis can be reduced by increasing the concentration of the sodium carbonate, thus permitting a degree of control over the formation of hydroxide.
In place of carbonates, borates can be employed to similar advantage. Boric acid is a weak acid, much more mild than carbonic acid. Thus, its salts tend to hydrolyze in solution. The following equation shows the reaction of potassium meta borate in solution to form potassium hydroxide and potassium tetra borate.
2 K2B2O4+H2O2 KOH+K2B4O7 (5)
Again the hydroxyl concentration can be controlled by adjusting the concentration of the potassium borate.
Carbonates and borates are effective not only in controlling the alkalinity of the electrolyte, but they also form insoluble salts with lead. In this manner the corrosion of the positive electrode can be minimized. Not only are carbonates and borates helpful in this regard, but other salts are likewise effective. Silicates, phosphates and sulfates form insoluble salts with lead.
Alkalinity can be provided by compounds of the alkali metals including lithium, sodium, potassium, and cesium. Lithium has certain limitations inasmuch as its carbonate and phosphate are almost insoluble in water. Cesium provides a very strong base but the cost of this material limits its potential applications. While ammonium hydroxide is basic in solution, its volatility restricts its use. Finally, tetramethyl ammonium hydroxide is known to be strongly alkaline, approaching that of sodium hydroxide and potassium hydroxide.
The present invention covers the use of aqueous solutions for the electrolyte. These solutions have the advantage of superior electrical conductivities. Although use of organic solvents including alcohols and glycols is feasible, their performance is inferior.
The configuration of a lead-alkaline cell is not restricted. For purposes of testing various combinations of electrodes and electrolytes, a simple cell was assembled from a glass jar and strips of metal separated, as need be, by a polypropylene sheet. A workable battery, however, would necessarily be designed with the maximum surface areas for the electrodes and minimum volume of electrolyte. Such geometric designs as parallel plates, either flat or spirally wound, are appropriate. Alternatively, particles of lead and metal either alone or interspersed with graphite may be employed. In this manner, the capacity of the cell can be increased and its internal resistance minimized.
To gain a greater appreciation of the present invention,
Applications of a secondary battery as provided by the present invention are almost limitless. The largest application is in vehicles including automobiles powered by new hybrid motors. Other uses include portable electronic devices such as cell phones and laptop computers.
The electrolyte was prepared by heating 100.0 gm. Of potassium bicarbonate in an oven to convert it to potassium carbonate, which was then dissolved in 185 ml. of water. The positive electrode was formed from a 1½ in. wide strip of lead and the negative electrode was a 1½ in. wide strip of steel. The cell comprised a glass jar about 2⅔ in. diameter by 2½ in. high. After charging the cell at 2.5 volts for 21 minutes an open circuit potential of 1.7 volts was observed. At the end of the run both electrodes were in good condition and the electrolyte was water-white.
The electrolyte was prepared by heading 106.3 gm. of sodium bicarbonate in an oven to convert it to sodium carbonate, which was dissolved in 250 ml. of water and 10 ml. of concentrated sulfuric acid. Two strips of lead 2 in. wide were used for the positive and negative electrodes. The cell comprised a glass jar 2½ in. diameter by 4 in. high. After charging the cell at 2.4 volts for 9 minutes an open circuit potential of 1.5 volts was observed. Both electrodes were dimensionally stable.
The same cell was used as in Example 2, but 3.7 gm. of sodium hydroxide pellets were added to the electrolyte. Also, a zinc electrode was substituted for the negative lead electrode. After charging the cell at 2.5 volts for 3 minutes an open circuit of 2.1 volts was obtained. The electrodes remained in excellent condition after repeat cycling.
A cell per Example No. 3 can be constructed using cadmium as the negative electrode.
This application is a continuation-in-part application corresponding to U.S. patent application Ser. No. 11/167,535, filed on Jun. 27, 2005, which is a continuation-in-part application corresponding to U.S. patent application Ser. No. 10/756,015, filed on Jan. 13, 2004.
| Number | Date | Country | |
|---|---|---|---|
| Parent | 11167535 | Jun 2005 | US |
| Child | 12410500 | US | |
| Parent | 10756015 | Jan 2004 | US |
| Child | 11167535 | US |
