Electrochemical energy storage device

Abstract

The invention relates to an electrochemical energy storage device (100) having at least one electrochemical cell (10) which has an electrolyte (13) and at least two electron-conducting materials in the form of electrodes (11, 12) which are connected to the electrolyte (13), wherein an external voltage can be applied between the electrodes (11, 12). In order to provide an increased amount of charge in the form of electrons in the electrochemical cell (10), according to the invention at least one electrode (11, 12) is replaced by at least two partial electrodes (66, 67), which are spatially separated from each other and between which an electron line (71) runs.

Description

[0001] -10-2025-43870601 -Hau ptpost-0014 02-10-2025-43870801-HauPt Pos t-0014 PCT / DE2025 / 000096

[0002] Our reference: DRBH1

[0003] Electrochemical energy storage

[0004] The present invention relates to an electrochemical energy storage device according to the preamble of claim 1.

[0005] Energy storage systems of the type mentioned above are well known and are a determining factor in the further development of electromobility.

[0006] Various electrochemical energy storage types exist, which can be further divided into primary and secondary batteries. Primary batteries, i.e., batteries that can only be discharged once and cannot be recharged. Secondary batteries, i.e., accumulators, are rechargeable.

[0007] Electrochemical energy storage devices such as batteries and accumulators have the electrochemical cell, the so-called galvanic cell, as their smallest unit.

[0008] A galvanic cell contains two electrodes separated by an ion-conducting electrolyte. Electrochemical reactions, i.e., oxidation and reduction reactions, take place at the electrodes.

[0009] During the discharge of a galvanic cell, stored chemical energy is converted into electrical energy through an oxidation reaction at a designated electrode, the anode. In this process, charges in the form of electrons are left behind in the anode, which then flow through the load as an electron current.

[0010] The discharge of a galvanic cell is essentially a two-stage process. At the anode, when a voltage is applied, there is an excess of electrons, while at the other electrode, the cathode, there is a deficiency. This difference in electrons defines the electrical voltage of the galvanic cell, also known as the terminal voltage. A load connected between the two electrodes allows the electrons to first dissipate this voltage. This means that, in addition to the charge exchange through the oxidation reaction, electrons resulting from the excess charge and its subsequent reduction also contribute to the electron flow through the load. To prevent this electron flow from quickly ceasing, a constant supply of electrons is required. This is ensured because the circuit within the electrolyte is closed, allowing for a continuous flow of electrons.This is accomplished by the aforementioned oxidation reaction at the anode and the redox reaction at the cathode.

[0011] The amount of charge in a galvanic cell, i.e., the number of stored electrons, is closely related to the significant capacity -10-2025-43870601 -Hau ptpost-0015 02- 10-2025- 43870601 -Hau P t Po s -t - 0015 PCT / DE2025 / 000096

[0012] 2

[0013] Our reference: DRBH1 of a galvanic cell. Although literature and the state of the art do not present a uniform picture, it is possible to speak of an energy capacity in the case of an electrochemical energy storage device, since the amount of energy delivered is more important, as it is ultimately energy that is stored. This is obtained by multiplying the charge by the electrical voltage, since the voltage is nothing other than the energy per unit of charge. An increase in the number of electrons on the anode side therefore corresponds to an increase in the amount of energy delivered and the energy capacity.

[0014] It is therefore an object of the present invention to increase the number of electrons on the anode side of a galvanic cell and thus also the energy capacity of a galvanic cell.

[0015] This problem is solved by the features of claim 1. Advantageous embodiments of the invention are described in the dependent claims.

[0016] The invention provides that at least one electrode is replaced by at least two partial electrodes which are spatially separated from each other and between which an electron conductor runs.

[0017] The core idea of ​​the invention is that when an electrode is reduced in size, its galvanic potential, i.e., its electrode potential in a galvanic cell, does not change. The electrode potential of the electrode is related to the charge state of the electrode. A higher number of electrons means a more negative electrode potential. Dividing an electrode results in each resulting sub-electrode having the same number of electrons as the undivided electrode. Because an electron conductor runs between the sub-electrodes, it is ensured that if a charge difference is created between them, the electrons flow to the other sub-electrode and are then transferred to the load in the electron current.

[0018] To produce sub-electrodes with identical electrodes, it is advantageous for both sub-electrodes to have the same chemical composition. Within the scope of the invention, it is also conceivable that the sub-electrodes have different electrode potentials. In this case as well, one electrode can be replaced by two small sub-electrodes.

[0019] To prevent charge exchange between the partial electrodes that does not occur via electron conduction, an advantageous embodiment of the invention provides that the partial electrodes are partially electrically insulated from one another, preferably on the sides facing away from the electrolyte. Separating an electrode into two partial electrodes results in a loss of surface area, which, in the case of -10-2025-43870601 -Hau ptpost-0016 02- 10-2025-43870601 -Hau t Pos t-0016 PCT / DE2025 / 000096

[0020] 3

[0021] Our reference: DRBH1

[0022] During discharge and charging, oxidation and reduction processes take place. Therefore, electrical insulation should advantageously be minimal, preferably within the scope of conventional thin-film insulation, in order to minimize the reduction of charge conversions due to oxidation processes at the electrode during the discharge and charging of the galvanic cell.

[0023] The invention will now be explained in more detail with reference to the following drawings.

[0024] They show, in schematic representation:

[0025] Fig. 1a an electrochemical cell according to the prior art;

[0026] Fig. 1b the electrochemical cell from figure aa with a

[0027] external circuit with voltmeter;

[0028] Fig. 2a to

[0029] Fig. 2b shows the electrochemical cell from figure aa during its discharge;

[0030] Fig. 3a shows the electrochemical cell from figure 1a with a circuit including a consumer;

[0031] Fig. 3b shows the electrochemical cell from figure aa during charging;

[0032] Fig. 4a to

[0033] Fig. 4c Construction of a space charge density with corresponding potential difference between a metal electrode and an electrolyte according to the prior art;

[0034] Fig. 5a two electrodes with an electrochemical double layer and the same material, shape and size in an electrolyte;

[0035] Fig. 5b two electrodes with an electrochemical double layer and the same material, but with different shapes and sizes in an electrolyte;

[0036] Fig. 6 shows three electrodes with an electrochemical double layer and the same material, both with different shapes and sizes and with the same shape and size, in an electrolyte;

[0037] Fig. 7 shows a partial section of an electrochemical cell containing an electrode with an electrochemical double layer as shown in Figures 5a to 6; -10-2025-43870601 -Hau ptpost-0017 02- 10-2025- 43870601 -H au P i Po st -0017 PCT / DE2025 / 000096

[0038] 4

[0039] Our reference: DRBH1

[0040] Fig. 8 shows the electrochemical cell from Figure 7, wherein the electrode is divided into a first region and a second region;

[0041] Fig. 9a to

[0042] Fig. 9b Voltages between electrodes with alternating electrical potentials;

[0043] Fig. 10 to

[0044] Fig. 12 shows the different stages of the electrochemical cell from Figure 7 during its discharge;

[0045] Fig. 13a shows an electrochemical energy storage device according to the invention;

[0046] Fig. 13b shows the energy storage device from Figure 13a during its discharge;

[0047] Fig. 14a shows another embodiment of the energy storage device according to the invention;

[0048] Fig. 14b shows the energy storage device from Figure 14a during its discharge;

[0049] Fig. 15a shows another embodiment of the energy storage device according to the invention;

[0050] Fig. 15b shows the electrochemical energy storage device from Figure 15a during its discharge;

[0051] Fig. 16a shows another embodiment of the energy storage device according to the invention;

[0052] Fig. 16b shows the electrochemical energy storage device from Figure 16a during its discharge;

[0053] Fig. 17a of the electrochemical energy storage device from Figure 13a;

[0054] Fig. 17b shows the electrochemical energy storage device from Figure 17a during its operation.

[0055] Charging;

[0056] Fig. 18a of the electrochemical energy storage device from Figure 14a;

[0057] Fig. 18b shows the electrochemical energy storage device from Figure 18a during its operation.

[0058] Charging

[0059] Fig. 19a shows the electrochemical energy storage device from Figure 15a;

[0060] Fig. 19b shows the electrochemical energy storage device from Figure 19a during charging;

[0061] Fig. 20a the electrochemical energy storage device from Figure 16a -10-2025-43870601 -Hau ptpost-0018 02- 10-2025-43870601 -Hau P t Po st -0018 PCT / DE2025 / 000096

[0062] 5

[0063] Our reference: DRBH1

[0064] Fig. 20b shows the electrochemical energy storage device from Figure 20a during charging;

[0065] Fig. 21a to

[0066] Fig. 24b further embodiments of the energy storage device according to the invention.

[0067] Figure 1a shows a conventional electrochemical cell, designated with reference numeral 10, which has the structure of a galvanic cell.

[0068] The basic components of the electrochemical cell shown in Figure 1a are the negative electrode 11, i.e., the anode, and the positive electrode 12, i.e., the cathode, as well as the electrolyte 13, which is located between the electrodes 11 and 12 and on both sides of the separator 14. The electrodes 11 and 12 are made of different metals. The separator 14 is located within and in the center of the electrolyte 13. The separator 14 allows the exchange of ions in the electrolyte 13 on both sides of the separator 14.

[0069] Both electrodes 11, 12 are equipped with conductors 17, 18. The two conductors 17, 18 cover the two electrodes 11, 12 and are arranged on the sides of the electrodes 11, 12 facing away from the electrolyte 13. Electrons can flow into and out of the electrodes 11, 12 via the conductors 17, 18. The phase boundaries 15, 16 are located between the electrodes 11, 12 and the electrolyte 13. Electrochemical double layers 21, 22 form at the phase boundaries 15, 16, which consist of the electrolyte-side and solvated positive ions 19 and the electrode-side electrons 20. Due to the larger number of electrons 20 (symbolized by seven electrons 20 in figure a1a) in the electrochemical double layer 21, electrode 11 is more negative than electrode 12 with its number of electrons (symbolized by four electrons in figure a1a) in the electrochemical double layer 22, i.e., electrode 11 is less noble than electrode 12.The two electrochemical double layers 21, 22 are each in electrochemical equilibrium, i.e., the same number of positive ions 19 pass through the phase boundaries 15, 16 in both directions per unit time (although the numbers differ at the phase boundaries 15, 16). The electrochemical equilibria at the electrodes 11, 12 are different. This results in the different strengths of the negative charge, which is symbolized by the unequal number of electrons 20 in the electrodes 11, 12.

[0070] The electrochemical cell 10 shown in Figure 1a, which represents the state of the art, is—as illustrated in Figure 1b—supplemented by a voltage device 24a, the poles of which are connected via the external conductor 23 to the terminals 17, 18 of the electrodes 11, 12. With the conventional electrochemical cell 10 shown in Figure 1b, it is possible to measure the cell voltage, i.e., the cell voltage of the electrochemical cell 10 in electrochemical equilibrium. For this purpose, the differences between two galvanic voltages are used.

[0071] 6

[0072] Our symbol: DRBH1 combines externally to form the electromotive force EEMK, i.e., the clamping voltage Emem of the electrochemical cell 10, and can be measured by means of the voltage device 24a. Due to the charge separation in the electrochemical double layers 21, 22, an electric field is created within the double layers 21, 22, and thus an electrical voltage, the so-called galvanic voltage. The galvanic voltage for the system electrode and electrolyte solution, i.e., for a system as shown in Figure 1a, is also referred to as the electrode potential.

[0073] A first galvanic voltage, i.e., a first electrical potential difference Acp bA potential difference of εe is established between electrode 11 with the electrical potential εe and electrolyte 13 with the electrical potential εe. A second galvanic potential difference, i.e., a second electrical potential difference εp2, is established between electrode 12 with the electrical potential εe. <p2und dem Elektrolyten 13 mit dem elektrischen Potential <po ein. Die Elektrode 12 mit ihrer Elektronenzahl (in Figur lb symbolisiert durch vier Elektronen) weist gegenüber der Elektrode 11 mit ihrer Elektronenzahl (in Figur lb symbolisiert durch sieben Elektronen) ein positiveres elektrisches Potential auf. Um eine positive elektromotorische Kraft EEMK bzw. positive Klemmenspannung Eitlem zu erhalten, muss daher gelten EKiem=A<p2- A<pi = <p2- epi .

[0074] Due to the high internal resistance of the voltage source 24a, in the embodiment of the conventional electrochemical cell 10 shown in figure 1b, there is no electron current from the electrode 11 to the electrode 12 and thus no discharge of the electrochemical cell 10.

[0075] The de-energized electrochemical cell 10 in Figure 1b is in electrochemical equilibrium, where the cell voltage, i.e., terminal voltage AEKiem, exists between the electrodes 11, 12. In this state, i.e., in the state of electrochemical equilibrium, the electrochemical cell 10 is charged.

[0076] Figure 2a shows a discharge of the electrochemical cell 10 from Figure 1b. In Figure 2a, the voltage device 24a from Figure 1b is replaced by the load 24a. The electrochemical cell 10, which has the structure of a galvanic cell, thus becomes a galvanic cell that discharges spontaneously, i.e., the positive terminal voltage AEKI em ^P2 ~ Cpi • applies.

[0077] As Figure 2a further illustrates, during the discharge, an electron current 25 flows from the negative electrode 11 to the positive electrode 12. The electrons 20 move through the conductor 17 of the negative electrode 11, the external conductor 23, and the conductor 18 of the positive electrode 12 to the electrode 12.

[0078] Here, electrons 20 initially flow from the electrochemical double layer 21 shown in Figures 1a and 1b to electrode 12 due to the excess of electrons in the negative electrode 11 and the deficiency of electrons in the positive electrode 12. The consequence of this charge change is, in turn, as Figure 2a further illustrates, an electron deficiency in the negative electrode 11 and a -10-2025-43870601 -Hau ptpost-0020 02- 10-2025-43870601 -Hau Pt Pc st -0020 PCT / DE2025 / 000096

[0079] 7

[0080] Our reference: DRBH1

[0081] Excess electrons in the positive electrode 12. The positive electrode 1 becomes negatively charged.

[0082] Figure 2b illustrates that, as a consequence of the charge change shown in Figure 2a, oxidation and reduction processes are triggered at electrodes 11 and 12. To maintain the electron flow, the circuit in the electrolyte 13 must also be closed. This is accomplished by the oxidation and reduction processes at electrodes 11 and 12.

[0083] In the prior art electrochemical cell 10, various oxidation and reduction scenarios are possible involving the positive ions 27 shown in Figure 2b. In a first scenario, positive metal ions 27 from the positive electrode 12 are located in the electrolyte 13 between the separator 14 and the positive electrode 12. Because the charge changes result in an increased number of electrons 20 in the positive electrode 12, the positive metal ions 27 move towards the positive electrode 12 during the reduction process in order to accept electrons 20 there (attraction between the positive metal ions 27 and the electrons 20 in the positive electrode 12). Thus, the positive metal ions 27 are deposited on the positive electrode 12.

[0084] The electron current 25 would very quickly equalize the charge difference between electrodes 11 and 12, but the electrochemical cell 10 shown in Figure 2b, which is part of the prior art, supplies further electrons 20 that flow to electrode 12 via the external conductor 23, so that the electron current 25 continues. In addition, after the first metal ions 27 of electrode 11 have dissolved in the electrochemical double layer 21 shown in Figure 1b (as shown in Figure 2a), further metal ions 27 of electrode 11 dissolve in the electrode 11 and migrate away from electrode 11 in the direction 26. This oxidation process also causes electrons 20 to be left behind in electrode 11, which in turn flow to electrode 12 via the external conductor 23.Due to the charging by metal ions 27 of the electrode 11 in the electrolyte 13 between electrode 11 and separator 14, negative ions of the electrolyte 13, not shown in Figure 2b, migrate through the separator 14 into the space between electrode 11 and separator 14.

[0085] The literature describes another scenario of discharge in an electrochemical cell, which also has the structure of a galvanic cell and can be described with reference to Figure 2b. In this scenario, the charge change in the electrochemical cell 10 shown in Figure 2a is also initially balanced by the flow of electrons 25 from the negative electrode 11 to the positive electrode 12. The electrons 20 move through the conductor 17 of the negative electrode 11, the external conductor 23, and the conductor 18 of the positive electrode 12 to electrode 12. The balancing of the charge change results in a further charge change, since an electron deficiency arises in electrode 11 and an electron surplus in electrode 12.This change in charge causes a corresponding change in voltage, which in the currentless state of the electrochemical cell -10-2025-43870601 -Hau ptpost-0021 02~ 10-2025-43870601 -Hau t Po st -00 1 PCT / DE2025 / 000096.

[0086] 8

[0087] Our reference: DRBH1

[0088] The clamping voltage is 10. This voltage change is balanced again by the ion migration in the electrolyte 13. Atoms of the electrode 11 go into solution as positive metal ions 27 and leave electrons 20 behind in the electrode 11. The positive metal ions 27 continue to migrate in the electrolyte 13 towards electrode 12, since the resulting excess of electrons in electrode 12 makes its potential negative relative to the potential of the quenching layer of positive metal ions 27 around electrode 11. The positive metal ions 27 migrating towards electrode 12 are deposited as neutral atoms on electrode 12. Electrode 11 becomes thinner and thinner, and electrode 12 becomes coated with atoms from electrode 11. As soon as electrode 12 is completely covered with atoms from electrode 11, the voltage of the electrochemical cell 10 decreases because there are now practically two identical electrodes 11 and 12 [cf. W.Demtröder: Experimental Physics 2, Chapter 2.8, 7th edition (Springer, Berlin 2017)].

[0089] Regardless of the two scenarios of discharge of the electrochemical cell 10 described here, the electron current 25 in the conventional electrochemical cell 10 shown in Figures 2a to 2b is composed of electrons 20, the causes of which, i.e., their sources, must be distinguished:

[0090] 1. A quantity of electrons 20 resulting from the equalization of the initial charge difference between electrode 11 and electrode 12, as illustrated in Figure 2a and shown in Figure 1b, i.e., from the reduction of the applied clamping voltage and

[0091] 2. A further quantity of electrons 20, which originate from the oxidation processes at electrode 11, i.e., the electrons 20 are left behind in electrode 11 and subsequently flow to electrode 12.

[0092] Thus, essentially two reservoirs for the electrons 20, i.e., two storage possibilities for the electrons 20 in the electrochemical cell 10 resulting from the discharge, can be identified. A first reservoir for the electrons 20 arises from the applied clamping voltage of the electrochemical cell 10. Due to the applied clamping voltage and the associated electrochemical equilibrium, electrons 20 accumulate – as illustrated in Figure 1b – in the electrodes 11, 12.

[0093] Another reservoir for electrons 20 is provided by the reduction process at electrode 12 during the discharge of the electrochemical cell 10. Through the deposition of positive metal ions 27 at electrode 12, electrons 20 are absorbed and "stored" at electrode 12 by the positive metal ions 27.

[0094] Reservoirs for the electrons 20 also manifest themselves—as will be shown below—during the charging of the electrochemical cell 10. During charging, the electrochemical cell 10 functions as an electrolysis cell. The -10-2025-43870601 -Hau ptpost-0022 02“ 10-2025-43870601-HauP -t Pos t -0022 PCT / DE2025 / 000096

[0095] 9

[0096] Our reference: DRBH1

[0097] The electrolysis cell represents the reverse of the galvanic cell, whose function the electrochemical cell 10 fulfills during discharge.

[0098] Figure 3b shows the charging of the electrochemical cell 10. Reference is first made to Figure 3a. Figure 3a shows the electrochemical cell 10 with a voltage source 28, which replaces the load 24a shown in Figures 2a and 2b and whose terminals are also connected via the line 23 to the leads 17, 18 of the electrodes 11, 12. Before the charging of the electrochemical cell 10 can begin, the voltage 29 must be applied by means of the voltage source 28. In order for electrolysis and thus the charging process of the electrochemical cell 10 to be initiated, the voltage 29 must be at least equal to the terminal voltage AE described in Figure 1b. Kiem= <P2 - epi der freiwillig ablaufenden Entladung der elektrochemischen Zelle 10 entsprechen. Diese Potentialdifferenz bzw. die mit der angelegten Spannung 29 einhergehende und in Figur 3a veranschaulichte Ladungsänderung sind - wie auch in Figur 1b - durch die sieben in Figur 3a gezeigten Elektronen 20 in der Elektrode

[0099] 11 and symbolized by the four electrons 20 shown in Figure 3a in electrode 12. The change in charge creates a change between the two electrodes 11,

[0100] 12. An electric field was set up.

[0101] The voltage 29 corresponds to the so-called deposition potential. A certain additional clamping voltage AEKiem= <P2 - epi bzw. Abscheidungspotential muss jedoch aufgebracht werden, um u.a. den ohmschen Widerstand der elektrochemischen Zelle 10 zu überwinden. Die elektrochemische Polarisation der Elektroden 11 , 12 kann zudem eine Überspannung erforderlich machen.

[0102] The charge change associated with the applied voltage 29 results in the processes at electrodes 11, 12 proceeding in the opposite direction in the two discharge scenarios of the electrochemical cell 10 described above. As in electrolysis, the processes at electrodes 11, 12 in the electrochemical cell 10 thus proceed in the opposite direction compared to the galvanic cell. See Figure 3b for further details.

[0103] Figure 3b shows that, due to the electron excess in electrode 11 (or the electric field between the two electrodes 11 and 12) shown in Figure 3a, metal ions 27 of the electrolyte 13 migrate towards electrode 31 of electrode 11 to be reduced and deposited there, absorbing electrons 20. At electrode 12, on the other hand, oxidizing metal atoms from electrode 12 dissolve as positive metal ions 27 and follow the electric field towards electrode 31 of electrode 11. The electrons released during oxidation move as electrons 20 through the conductor 18 of electrode 12, the external conductor 23, and the conductor 17 of electrode 11 to electrode 11. Thus, the oxidation at electrode 12 replenishes electrons 20 for the electrodes.From a certain point in time, the electrodes 11, 12 differ so much that they assume the chemical composition of the electrodes 11, 12 described in Figure 1b in their charged state.

[0104] Regardless of the two charging scenarios of the electrochemical cell 10 described here, the electron current 30 continues in the -10-2025-43870601 -Hau ptpost-0023 02- 10-2025-43870601 -Hau P t Po st -0023 PCT / DE2025 / 000096

[0105] 10

[0106] Our symbol: DRBH1 conventional electrochemical cell 10 shown in figure 3b made up of electrons 20, the causes of which, i.e., their sources, are to be distinguished:

[0107] 1. A quantity of electrons 20 resulting from the migration of electrons 20 shown in Figure 3b due to the applied voltage 29 shown in Figure 3a and

[0108] 2. A further quantity of electrons 20, which originate from the oxidation processes at electrode 12, i.e., are left behind in electrode 12 and subsequently flow to electrode 11 as supplied electrons 20.

[0109] Thus, essentially, two reservoirs for the electrons 20, i.e., two storage possibilities for the electrons 20 in the electrochemical cell 10, can be identified during charging. A first reservoir for the electrons 20 results from the voltage 29 applied to the electrochemical cell 10 as shown in Figure 3a. Due to the applied voltage 29 and the associated charge distribution shown in Figure 3a, electrons 20 accumulate – as illustrated in Figure 3a – in the electrodes 11 and 12.

[0110] Another reservoir for electrons 20 is provided by the reduction process at electrode 11 during the charging of the electrochemical cell 10. Through the deposition of positive metal ions 27 at electrode 11, electrons 20 are absorbed and "stored" at electrode 11 by the positive metal ions 27.

[0111] The electrochemical cell 10 described in Figures 1a to 3b is state of the art.

[0112] For a better understanding of the invention, reference is first made to Figures 4 to 6.

[0113] Figures 4a to 4c each show an electrochemical half-cell 34 filled with an electrolyte 33. The electrolytes 33 in Figures 4a to 4c have the same chemical composition. The electrode 32 is immersed in the electrolyte 33 of the respective half-cell 34. The electrodes are metals of the same chemical composition, such as copper or zinc. However, in the half-cell 34 illustrated in Figure 4c, the electrode 32 is immersed further in the electrolyte 33 than in the half-cells 34 shown in Figures 4b and 4c. As Figures 4a to 4c further illustrate, electrochemical double layers are formed at the electrodes 32, sections 35, 36, and 37 of which are shown. These double layers consist of electrons 39 of concentration ci and positive metal ions 38 of concentration c2. An electrochemical equilibrium exists at the electrochemical double layer.Thus, after the double layer has formed upon negative charging of the electrode 32, i.e., upon establishment of the excess of electrons 39 in the electrode 32, the same number of positive metal ions 38 migrate back and forth per unit time at the boundary between the electrode 32 and the electrolyte 33, i.e., the metal dissolution and the metal deposition -10-2025-43870601 -Hau ptpost-0024 02- 10-2025-43870601 -Hau P t Po st -0024 PCT / DE2025 / 000096.

[0114] 11

[0115] Our symbol: DRBH1 propagates at the same speed at this boundary [cf. CH Hamann, W. Vielstich: Electrochemistry, Chapter 3.1.2, 4th edition (Wiley-VCH, Weinheim 2005)].

[0116] Potential jumps occur at the interface between electrode 32 and electrolyte 33, as further illustrated by the figures. Both electrode 32 and electrolyte 33 exhibit Galvani potentials in electrochemical equilibrium. The difference between these Galvani potentials is the Galvani potential, which, for the system electrode 32 and electrolyte 33 described here, is the electrode potential [cf. C.H. Hamann, W. Vielstich: Electrochemistry, Chapter 3.1.2, 4th edition (Wiley-VCH, Weinheim 2005)]. The electrode potential of the electrode, i.e., also of electrode 12, is given in the electrochemical series, which is used to calculate the voltages of electrochemical energy storage devices such as batteries and accumulators under standard conditions such as temperature, pressure, and electrolyte 33 concentration.

[0117] The standard conditions do not include the dimensions of an electrode, such as size and extent.

[0118] A key insight of the present invention, the first embodiment of which is illustrated in Figure 13, is therefore that, regardless of the dimensions of an electrode, the electrode potential does not change when the electrode is immersed in an electrolyte.

[0119] This realization is also manifested in figures 5 and 6.

[0120] Figure 5a shows a container 41 filled with an electrolyte 33. Two electrodes, both designated with reference numeral 42, are fully immersed in the electrolyte 33. Both electrodes 42 have the same dimensions and chemical composition. In the embodiment shown in Figure 5, the electrodes 42 are made of copper or zinc. Standard conditions prevail in the container 41, and electrochemical double layers 43, 44 have formed in electrochemical equilibrium on each of the electrodes 42. These double layers are composed of electrons 39 in the electrodes 42 and positive metal ions 38 in the electrolyte 33.

[0121] Both electrodes 42 also exhibit Galvani potentials in the electrochemical equilibrium shown in Figure 5a. <pi2 uf. Die Differenz dieser Galvani-Potentiale ist auch hier die Galvani-Spannung, die für das hier beschriebene System von Elektrode 32 und Elektrolyt 33 das Elektrodenpotential ist. Die Galvani-Spannung hängt von der Temperatur der Halbzelle ab [vgl. Wilhelm H. Westphal: Physik, § 177, 25. / 26. Auflage (Springer, Berlin 1970)].

[0122] For the same Galvani potentials < n, < i2 of the electrodes 42, symbolized by the same number of 14 electrons 39 each, the following applies under standard conditions, i.e., regardless of the dimensions of the electrodes 42:

[0123] < 1 1 — <P 12 -10-2025-43870601 -Hau ptpost-0025 02- 10-2025-43870601 -Hau P t Pos i-0025 PCT / DE2025 / 000096

[0124] 12

[0125] Our reference: DRBH1

[0126] Figure 5b illustrates two electrodes 42 under standard conditions and with the same chemical composition, but of different dimensions, immersed in the electrolyte 33. The differently sized electrodes 42 also have the same Galvani potentials cpn, tpi2, symbolized by the same number of 14 electrons 39 each, i.e., the same electrode potentials, and the following also applies here:

[0127] <P 11 - Cp 12

[0128] This is also clearly illustrated: The electrodes with the Galvani potentials <pn, <pi2 verfügen über einen Lösungsdruck, d.h. sie haben die Tendenz unter Auflösung derselben und unter Verbleib von Elektronen 39 in den Elektroden positive Metallionen 38 in den Elektrolyten 33 hineinzusenden. Diesem Lösungsdruck wirkt gemäß der nernstschen Theorie der osmotische Druck von bereits in dem Elektrolyten 33 befindlichen Metallionen 38 entgegen. Durch die entgegengesetzte Aufladung von Elektrode 42 und Elektrolyt 33 entsteht zwischen den beiden ein elektrisches Feld, das den weiteren Austritt von Metallionen 38 aus der Elektrode 42 behindert. Eine weitere negative Aufladung, d.h. eine vermehrte Erzeugung von positiven Metallionen 38 durch eine räumliche Vergrößerung der Elektrode 42 mit dem Galvani-Potential <pn würde durch elektrostatische Rückhaltekräfte beendet.Even in light of Le Chatelier's principle, an increase in the emission of positive metal ions 38 into the electrolyte 33 would result in an increase in the deposition pressure in the electrochemical equilibrium, i.e., the positive metal ions 38 would again be deposited at the electrode 42.

[0129] Figure 6 shows three electrodes 42, each with the same chemical composition, under standard conditions in the electrolyte 33 located in the container 41. As further shown in Figure 6, the electrode 42 with the Galvani potential is <p 13, symbolisiert durch die Anzahl von 14 Elektronen 39, in ihren Ausmaßen etwa doppelt so groß ist wie die Elektroden 42 mit den Galvani- Potentialen cpn, <pi2, symbolisiert durch die gleiche Anzahl von jeweils 14 Elektronen 39. Für die Galvani-Potentiale <pn, <pi2, <p 13 unter Standardbedingungen in dem Behälter 41 gilt auch hier:

[0130] <p 11 — <P12 - <P13

[0131] Figure 6 illustrates that in a half-cell, dividing an electrode that has a Galvani potential under standard conditions doubles the number of electrochemical double layers and thus the number of electrons, with the electrons being distributed equally between the two divided electrodes. The Galvani potential remains unchanged by the division. If the electrode were divided into three parts, the number of -10-2025-43870601 -Hau ptpost-0026 02-10-2025-43870601 -HauP -t Pos t-0026 PCT / DE2025 / 000096

[0132] 13

[0133] Our reference: DRBH1

[0134] Electrons triple in size; each of the three electrodes would receive one-third of the electrons.

[0135] A fundamental idea of ​​the invention, the first embodiment of which is illustrated in Figure 13, is that the amount of charge of the electrochemical cell 10 can be increased by dividing the electrode.

[0136] For this purpose, reference is first made to Figures 7 to 8,

[0137] Figure 7 shows a section 45 of a galvanic cell filled with electrolyte 33. The electrolyte 33 has the potential <po befindet sich eine Elektrode 49 mit dem Galvani-Potential <pi < 0, d.h. bei der Elektrode 46 handelt es sich um ein unedles Metall. Die Elektrode 46 ist beidseitig an ihrer Phasengrenze Elektrode 46 / Elektrolyt 33 mit elektrochemischen Doppelschichten 43, 44 versehen, die sich aus Elektronen 39 in der Elektrode 46 und positiven Ionen 38 in dem Elektrolyten 33 zusammensetzen. Die entgegengesetzte Aufladung an der Phasengrenze Elektrode 46 / Elektrolyt 33 erzeugt die Potentialänderung 48. An der der Elektrolytoberfläche zugewandten Elektrodenseite ist die Elektrode 46 mit einem Stromleiter 46 versehen, der aus dem Elektrolyten 33 herausragt und durch den die Elektronen 39 bei einer Entladung des galvanischen Elements aus der Elektrode 46 hinausfließen können.

[0138] The electrode 46 shown in Figure 7 undergoes a reduction in its spatial dimensions without changing its Galvani potential ee < 0. This is illustrated in Figure 8. Figure 8 shows the partial region 45 of a galvanic cell described in Figure 7, which is filled with the electrolyte 33 with the Galvani potential < 0.

[0139] Electrode 49 is located in the upper region of the electrolyte 33. Electrode 49 has the same chemical composition as electrode 46, which is smaller in size and described in Figure 7. As can be seen from the description of Figures 5 and 6, the Galvani potential of an electrode does not change when its spatial dimensions are changed; that is, the Galvani potentials < i of electrode 46 in Figure 7 and electrode 49 in Figure 8 are the same, which is symbolized by the same number of 14 electrons 39.

[0140] Below electrode 49, i.e. in the lower half of the electrolyte 33, another electrode 50 is arranged, which also has the same chemical composition as the smaller electrode 46 described in Figure 7, i.e., as electrode 49. <pi = < 2.

[0141] The opposing charges at the phase boundaries electrode 59, 50 / electrolyte 33 generate the potential jumps 56.

[0142] On the side of the electrode facing the electrolyte surface, the electrode 49 is provided with a conductor 51 that protrudes from the electrolyte 33 and through which the electrons 39 can flow out of the electrode 49 during a discharge of the galvanic cell. -10-2025-43870601 -Hau ptpost-0027 02- 10-2025-43870601-HauP Pos t-0027 PCT / DE2025 / 000096

[0143] 14

[0144] Our reference: DRBH1

[0145] The two electrodes 49, 50 are connected to each other by the conductor 52, which is arranged between the electrodes 49, 50. The conductor 52 is surrounded by an insulating wall 53, which electrically insulates the conductor 52 from the electrolyte 33. In the embodiment of the partial region 45 of the galvanic cell shown in Figure 8, the insulating wall 53 is made of ceramic. Alternatively, the material of the insulating wall 53 can also be glass.

[0146] Due to the insulating wall 53, no electric field forms between the conductor 52 and the electrolyte 33, i.e., no electrochemical double layer forms along the insulating wall 53, which is indicated by the absence of a potential change 60, whereby the electrical potentials in the conductor 52 and in the electrolyte 33 may well be different.

[0147] The electrochemical double layers 43, 44 in the two electrodes 49, 50 are in electrochemical equilibrium. Charge equalization between the two electrodes 49, 50 is achieved by the conductor 52. This occurs when <pi <p2ist, d.h. wenn ein Potentialunterschied zwischen den Elektroden besteht.

[0148] Another aspect of the invention, the first embodiment of which is illustrated in Figure 13, is that during the discharge of the electrochemical cell 10, the equalization of potential differences between electrodes of the same chemical composition in an electrolyte results in an increased discharge current. Reference is first made to Figures 9 to 12 for further details.

[0149] Figure 9a shows the charge state, i.e., the potentials epi, <p2von zwei Körpern 58, 59, welche Teil eines Systems 57 sind. Bei den Körpern 58, 59 handelt es sich um Elektroden derselben chemischen Zusammensetzung und bei dem System 57 um eine galvanische Zelle. Je mehr Elektronenüberschuss in einem Körper vorhanden ist, desto stärker negativ ist sein Potential. Bei Elektronenmangel ist das Potential eines Körpers positiv. In Figur 9a weist der Körper 58 mehr Elektronen 39 als positive Ionen 39 auf, d.h. sein Potential <pi ist negativ. Der Körper 59 hat dagegen mehr positive Ionen 39 als Elektronen 38, somit ist sein Potential cp2positiv.

[0150] The electrical voltage U is the difference between the two potentials epi, <p2. Zwischen den beiden Körpern 58, 59 kann eine Spannung U = epi - cp2gemessen werden. Der Wert der Spannung U ist positiv, da der Spannungspfeil 60 vom höheren zum niedrigeren Potential weist. Eine Spannung wird auch zwischen zwei positiv geladenen Körpern gemessen, wenn einer der beiden mehr positiv geladen ist als der andere, (vgl. hierzu: https: / / www.professorglasmachers.de / gde_potential-und- spannung / ).

[0151] Figure 9b shows that both bodies 58 and 59 have an excess of electrons. Body 58 has 5 extra electrons, while body 59 has 3 extra electrons. Both bodies 58 and 59 have a negative potential, but body 58 is more negatively charged than body 59. Therefore, a positive voltage acts from body 59 towards body 58. The voltage is positive when the arrow points from the relatively higher to the lower potential (see: https: / / www.professorglasmachers.de / gde_potential-und-spannung / ). -10-2025-43870601 -Hau ptpost-0028 02-10-2025-43870601-HauPtPos i-0028 PCT / DE2025 / 000096

[0152] 15

[0153] Our reference: DRBH1

[0154] When the two bodies 58, 59 are connected by a conductor – such as the conductor 52 illustrated in Figure 8 – an electron current flows from body 58 towards body 59 due to the voltage. The charges equalize in such a way that there are subsequently four extra electrons 39 on both bodies 58, 59. Charge equalization thus functions independently of the number of charges; it is based much more on the difference between charges. The result of charge equalization is therefore not always two electrically neutral, uncharged bodies, but rather two bodies with the same charge. This also applies when there is a difference in charge deficiency between two bodies. If 10,000 electrons are missing in body 58, while 9,000 electrons are missing in body 59, a deficiency of 9,500 electrons will result on both bodies 58, 59 after charge equalization (see: https: / / www.professorglasmachers.de / gde_potential-und-spannung / ).

[0155] The discharge of the electrode 49 shown in Figure 8 is illustrated in Figure 10 and follows the same mechanism as the discharge of the electrochemical cell 10 from Figures 2a to 2b, whereby a possible exchange of positive ions 38 between the electrodes 49, 50 is initially disregarded.

[0156] As illustrated in Figure 10, the electron current 55 initially draws the electrons 39 from the decay of the initially applied voltage during discharge. This also changes the galvanic potential. <pi der Elektrode 49, was durch die Potentialänderung 61 angedeutet ist. Durch den dann einsetzenden Oxidationsvorgang an der Elektrode 49, d.h. mit der Wanderung der positiven Ionen 38 in Richtung 54 der in Figur 10 nicht gezeigten positiven Elektrode und dem damit einhergehenden Zurücklassen von Elektronen 39 in der Elektrode 49 werden Elektronen 39 für den Elektronenstrom 55 nachgeliefert.

[0157] From a certain point onwards, due to the outflow of electrons 39 from electrode 49, a charge difference occurs between electrode 49 and electrode 50, since there is a deficiency of electrons compared to electrode 50, i.e., electrode 49 becomes more positive compared to electrode 50.

[0158] Figure 11 illustrates the effect of this charge difference. As the electrochemical double layers 43, 44 of the electrode 50 shown in Figure 10 dissolve, electrons 59 flow in an electron current 59 towards the electrode 49. This also results in a change 62 of the galvanic potential. <pa der Elektrode 50. Durch den Abfluss der Elektronen 39 der Elektrode 50 kommt es in der Elektrode 50 zu einem Elektronenmangel bei einem gleichzeitig weiteren Elektronenüberschuss in der in Figur 10 nicht gezeigten positiven Elektrode.

[0159] The oxidation process that also begins at electrode 50, i.e., the migration of the positive ions 38 towards electrode 54 (not shown in Figure 1), and the associated leaving of electrons 39 in electrode 50, replenishes electrons 39 for the electron current 59. A migration of the positive ions 38 generated by electrode 50 towards electrode 49 is unlikely, since positive ions 38 are also present at electrode 49 due to the oxidation process taking place there. Therefore, the positive ions 38 from electrodes 49 and 50 repel each other electrostatically. -10-2025-43870601 -Hau ptpost-0029 02- 10-2025-43870601 -Hau t Pos t-0029 PCT / DE2025 / 000096

[0160] 16

[0161] Our symbol: DRBH1 move together in the direction of 54 of the positive electrode not shown in Figure 11.

[0162] As can be seen from Figure 12, the discharge current, i.e., the discharge current 55 during the discharge of the galvanic cell, initially consists of the electrons 39 resulting from the equalization of the charge difference between the negative electrode 49 and the positive electrode of the galvanic cell (not shown in Figure 12), as well as the electrons 39 left behind at the electrode 49 during the oxidation processes. This electron current 55 is associated with a change 63 in the galvanic potential. <p i einher. Elektronen 39 für den Entladestrom, d.h. für den Elektronenstrom 55 werden durch den Elektronenstrom 59 nachgeliefert, der durch den Stromleiter 52 zwischen den Elektroden 50, 49 fließt. Der Elektronenstrom 59 setzt sich wiederum aus Elektronen 39 zusammen, die sich aufgrund der in Figur 10 gezeigten Ladungsdifferenz zwischen den Elektroden 49, 50 in Bewegung setzen und die aufgrund der an der Elektrode 50 stattfindenden Oxidationsvorgänge in der Elektrode 50 zurückgelassenen werden.The electron current 59 is accompanied by a change 65 in the galvanic potential < 2. Because electrons 39 flow into electrode 49 via the electron current, a charge difference is maintained between electrode 49 and the positive electrode of the galvanic cell (not shown in Figure 12). This means that electrode 49 continues to have an excess of electrons compared to the positive electrode (not shown in Figure 12). The load (not shown in Figure 12) then allows this charge difference to be reduced via the electron current 55 with the electrons from electrode 50.

[0163] Figure 13a shows a first embodiment of the electrochemical energy storage device 100 according to the invention, in which the negative electrode 11, i.e., the anode, shown in Figures 1a to 2b is replaced by the two partial electrodes 66, 67. The partial electrodes 66, 67 have the same chemical composition as the electrode 11 in Figures 1a to 2b. Furthermore, both partial electrodes 66, 67 have the same galvanic potential cpc = < i-cpo and thus, since the partial electrodes 66, 67 are located in the electrolyte 13, the same electrode potential as the electrode 11 illustrated in Figures 1a to 3b, which is symbolized by the same number of seven electrons 20 each. At the phase boundaries 69, 70 of the partial electrodes 66, 67 there are also electrolyte-side solvated positive ions 17 of the same number, so that electrochemical double layers are formed here as well, which are in an electrochemical equilibrium.Between the partial electrode 66 and the positive electrode 12, i.e., the cathode of the electrochemical cell 10, and between the partial electrode 67 and the positive electrode 12, the voltage 29, i.e., the terminal voltage of the electrochemical cell 10, prevails. As can be further seen from Figure 13a, the partial electrodes 66, 67 are spatially separated from each other by an intermediate region 68, which is filled with the electrolyte 13.

[0164] Figure 13b shows the discharge of the electrochemical cell 10. The discharge follows the same process as the discharge of the conventional electrochemical cell 10 shown in Figures 2a to 2b, with the difference that the number of electrons 20 in the electron current 25 is increased by the release of electrons 20. -10-2025-43870601 -Hau ptpost-0030 02-10-2025-43870601-HauPtPos t-0030 PCT / DE2025 / 000096

[0165] 17

[0166] Our symbol: DRBH1 of the second sub-electrode 67 is further increased. For this purpose, the reduction of the charge difference between the sub-electrode 66 and the positive electrode 12 is initiated, with the result that - as in the discharge of the conventional electrochemical cell 10 according to figures 1a to 2b - oxidation processes are triggered at the sub-electrode 66, i.e., positive metal ions 27 migrate towards the positive electrode 12, leaving electrons 20 behind in the sub-electrode 66.

[0167] Due to the continuous outflow of electrons 20 from the sub-electrode 66, a charge difference arises between the sub-electrode 66 and that of the sub-electrode 66.

[0168] The current collector 17 and the partial electrode 67 are connected. Due to the lack of electrons 20, the partial electrode 66 becomes more positive not only relative to the positive electrode 12, but also relative to the partial electrode 67. This charge difference is balanced by the movement of electrons 20 from the partial electrode 67 via the current collector 17 towards the partial electrode 66. Thus, more electrons 20 are available for the electron current 25 towards the positive electrode 12, i.e., the amount of charge or the capacity of the electrochemical cell 10 increases. To prevent charge exchange between the current collector 17 in the area of ​​the electron conductor 71 and the electrolyte 13, an electrical insulating layer 76 is arranged in this area between the electron conductor 71 and the electrolyte 13.

[0169] Since there is also an excess of electrons in the positive electrode 12 compared to the sub-electrode 67, positive ions 27 migrate—as with sub-electrode 66—towards 26 of the positive electrode 12 in order to be reduced there. The oxidation process at sub-electrode 67 also releases electrons 20 into the sub-electrode 67.

[0170] 67 back, which flow in the direction of the partial electrode 66, in order to then enrich the electron current 25 and increase the discharge current of the electrochemical cell 10.

[0171] In a further embodiment of the invention, as illustrated in Figures 14a to 14b, the electrochemical cell 10 is provided with an insulating wall 72. The insulating wall 72 is arranged between the phase boundaries 69, 70 of the partial electrodes 66, 69 and shields the intermediate region 68 from the electrolyte 13. In the embodiment of the invention shown in Figures 14a to 14b, the intermediate region 68 is designed as an electrical insulating layer, the dimensions of which are minimal in order to ensure as many charge conversions as possible, i.e., the generation of an increased number of electrons 20 at the partial electrodes 66, 67 during the oxidation processes at the partial electrodes 66, 67. The intermediate area 68, acting as an electrical insulating layer, prevents charge exchange between the two partial electrodes 66, 67, i.e., it ensures that the partial electrodes 66, 67 are electrically insulated from each other on the sides facing away from the electrolyte 13.

[0172] Figures 15a to 16b show another embodiment of the invention. In this embodiment, the partial electrode 66 is provided with a current collector 80 on the side facing away from the electrolyte 13, wherein the electron conductor 78 between the mutually facing sides 77, 78 of the -10-2025-43870601 -Hau ptpost-0031 02-10-2025-43870601-HauPt os t-0031 PCT / DE2025 / 000096

[0173] 18

[0174] Our reference: DRBH1

[0175] The partial electrodes 66, 67 are connected. The sides 73, 75 of the partial electrode 67 and the electron conductor 78 facing away from the electrolyte 13 have no current collector. As can also be seen from Figure 15a, there is a voltage 79 between the electron conductor 78 and the positive electrode 12, which differs from the voltage 29, i.e., the terminal voltage of the electrochemical cell 10. The voltage 79 disappears through the insulating layer 72, which is arranged between the phase boundaries 69, 70 of the partial electrodes 66, 67 and shields the area between the partial electrodes 66, 67 from the electrolyte 14.The area between sides 77, 78 of the partial electrodes 66, 77 and the area next to side 75 of the electron conductor 78 facing away from the electrolyte 13 is designed as an insulating layer, which is also minimal in its dimensions here in order to ensure as many charge conversions as possible at the partial electrodes 66, 67 during the oxidation processes at the partial electrodes 66, 67.

[0176] Figures 17a to 20b show the charging of the electrochemical cell 10 in the various embodiments of the invention. The charging process follows the same procedure as the charging of the conventional electrochemical cell 10 shown in Figures 3a to 3b, with the difference that the electron current 30 is initially supplied to the partial electrode 66. This creates a charge difference between the partial electrodes 66 and 67, i.e., the partial electrode 66 becomes more negative relative to the partial electrode 67 and receives an excess of electrons 20. As a result, the electrons 20 flow further to the partial electrode 67. Through further energy input from the voltage source 28, more electrons 20 reach the partial electrode 66 and then the partial electrode 67 until, due to the processes shown in Figures 9a to 9b, a charge balance is achieved between the partial electrodes 66 and 67.The electrochemical energy storage device 100 according to the invention is then “charged”.

[0177] Figures 21a to 24b illustrate that the positive electrode 12 shown in Figures 1a to 3b can also be replaced by partial electrodes 66, 67 in order to provide an increased storage reservoir for the electrons 20 shown in Figures 1a to 3b during the discharge and charging of the electrochemical cell 10.

Claims

-10-2025-43870601 -Hau ptpost-0033 02-10-2025— 3870601-HauP-t Pos t-0033 PCT / DE2025 / 000096 19 Our reference: DRBH1 Patent claims 1. Electrochemical energy storage device (100) with at least one electrochemical cell (10) comprising an electrolyte (13) and at least two electron-conducting materials in the form of electrodes (11, 12) in contact with the electrolyte (13), wherein an external voltage can be applied between the electrodes (11, 12), characterized in that at least one electrode (11, 12) is replaced by at least two partial electrodes (66, 67) which are spatially separated from each other and between which an electron conductor (71) runs.

2. Energy storage device according to claim 1, characterized in that the partial electrodes (66, 67) have the same chemical composition.

3. Energy storage device according to claim 1 or 2, characterized in that the partial electrodes (66, 67) have the same electrode potentials.

4. Energy storage device according to claim 1 or 2, characterized in that the partial electrodes (66, 67) have different electrode potentials 5. Energy storage device according to one of claims 1 to 4, characterized in that the partial electrodes (66, 67) are partially electrically insulated from each other.

6. Energy storage device according to one of the preceding claims, characterized in that the electrolyte (13) and the electron conductor (71) are electrically insulated from each other.

7. Energy storage device according to claim 5 or 6, characterized in that the partial electrodes (66, 67) are electrically insulated from each other on the sides facing away from the electrolyte (13).

8. Energy storage device according to one of the preceding claims, characterized in that the partial electrodes (66, 67) are provided with a current collector (17), wherein the electron conductor (71) is part of the current collector (17). -10-2025-43870601 -Hau ptpost-0034 02- 10-2025-43870601-HauPt Pos t-0034 PCT / DE2025 / 000096 20 Our reference: DRBH1 9. Energy storage device according to one of the preceding claims, characterized in that the electron conduction (71) runs between the mutually facing sides of the partial electrodes (66, 67).

10. Energy storage device according to claim 9, characterized in that the partial electrode (66) is provided with a current collector (17).

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