A bi-phasic electrolysis cell for carbon dioxide capture, electrocatalysts for use in the cell, related methods and a production facility using the electrolysis cell and the electrocatalysts

Abstract

The present disclosure relates to a bi-phasic electrolysis cell (1) for carbon dioxide capture, using an organic electrocatalyst in solution or anchored to a cathode (15), for conversion of carbon dioxide to a carbon dioxide reduction product chosen from either a C1-2 carboxylic acid or alcohol, such as formic acid or methanol. The disclosure further relates to a method for capturing carbon dioxide by converting the carbon dioxide to a reduction product in the bi- phasic electrolysis cell, organic electrocatalysts, methods for synthesizing organic electrocatalysts, a cathode department for use in the bi-phasic electrolysis cell, and a production facility (2) for use in carbon dioxide capture and / or production of formic acid and / or methanol.

Description

[0001]A bi-phasic electrolysis cell for carbon dioxide capture, electrocatalysts for use in the cell, related methods and a production facility using the electrolysis cell and the electrocatalysts. Technical field The present disclosure relates to the field of carbon capture and utilization, and especially to carbon dioxide capture and conversion to an organic acid like formic acid, which can be used as a fuel and carbon-1 feedstock. More specifically, the disclosure relates to a bi-phasic electrolysis cell for carbon dioxide capture, a method for capturing carbon dioxide by converting the carbon dioxide to a carbon dioxide reduction product in a bi-phasic electrolysis cell, an organic electrocatalyst, a method for synthesizing an organic electrocatalyst, a cathode department and a production facility for use in carbon dioxide capture and / or fuel production. Background art Increased levels of carbon dioxide in the atmosphere, partly resulting from emissions from industry, is a major challenge to be resolved. Methods and systems for capturing carbon dioxide exist, but the present solutions are equipped with limitations and or problems. Use of carbon dioxide reduction products, such as formic acid as a fuel is known from e.g., the following references (1): ACS Energy Lett.2017, 2, 1, 188-195, (2) Nature Communications volume 11, Article number: 3633 (2020), and (3) International Journal of Hydrogen Energy Volume 46, Issue 24, 6 April 2021, Pages 13050-13060. However, there are limitations in finding efficient methods for producing it as a fuel from a carbon capture context. Among the reported organic solutions for carbon capture and conversion, (i) Amine-based systems, (ii) Carbonate-bicarbonate based systems, and (iii) Covalent organic framework- based systems exist (see references below): Sullivan et al. (Nature Catalysis 4, 952-958 (2021) “Coupling electrochemical CO2 conversion with CO2 capture”), Gutiérrez-Sánchez et al. (ChemElectroChem, 2022, https: / / doi.org / 10.1002 / celc.202101540, “A State-of-the-Art Update on Integrated CO2 Capture and Electrochemical Conversion Systems”) and Seo et al. (J. Am. Chem. Soc.2022, 144, 5, 2164-2170, “Electrochemical Carbon Dioxide Capture and Release with a Redox-Active Amine”). (i) Amines, and carbonate systems are known to capture CO2 at ambient temperature but need high temperature for desorption. (ii) Covalent organic frameworks suffer from limited electronic conductivity and chemical stability. (iii) Other metal-free molecular electrocatalysts for CO2reduction suffer from low product selectivity. It mainly results in a mixture of products leading to further costs for product purification and hence large-scale implementation is not cost-effective. Other publications in the field are for e.g., WO2014 / 042781A2, which discloses methods and systems for electrochemical conversion of carbon dioxide to organic products, including formate and formic acid. The anode is e.g., of titanium, which is more expensive than other common metals (e.g., iron and copper) because it is rarer, and because it is typically only found bonded to other elements, which can make processing more expensive. Also, US2021 / 0047743A1 discloses a method for electrochemically reducing carbon dioxide in a three-compartment electrochemical cell, comprising an anode compartment, a cathode compartment, and an aqueous product compartment. Moreover, US2008 / 0296146A1 discloses a process for sequestrating carbon in the form of a mineral, comprising concentrating CO2 in a liquid phase, and electroreduction to a compound such as formic acid, and subsequent re-extraction and mineralization. Also, Xia et al. (Nature Energy 4, 776-785 (2019), ”Continuous production of pure liquid fuel solutions via electrocatalytic CO2 reduction using solid-electrolyte devices”) discloses electrocatalytic reduction of CO2 to e.g., formic acid, for subsequent use as fuel, using a solid electrolyte combined with a Bi-based catalyst. A problem with the solutions of the prior art is that there are limitations in terms of scalability. Also, there are issues in relation to environmental aspects. Further, process efficiency and the need for additional purification of the end product are typical problems. There is thus a need for an improved sustainable electrochemical system for carbon dioxide capture. Summary of the invention It is an object of the present disclosure to mitigate, alleviate or eliminate one or more of the above-identified deficiencies and disadvantages in the prior art and solve at least the above- mentioned problem. According to a first aspect there is provided a bi-phasic electrolysis cell (1) for carbon dioxide capture, comprising a first (10) and a second (30) compartment, at least one inlet (12) connected to the first compartment for allowing carbon dioxide to flow into the first compartment, and means for applying electrical voltage (17) to a first working electrode (cathode), a second counter electrode (anode) (15) and a third reference electrode (16), which electrodes are positioned in the first compartment, wherein: (a) the first compartment comprises (i) an organic phase (14), for facilitating electrocatalytic reduction of carbon dioxide into a carbon dioxide reduction product; (ii) a catalyst outlet (19) for enabling extraction of used electrocatalyst for subsequent regeneration or for changing the organic solvent; (iii) an overpressure outlet (18), and (iv) at least one organic electrocatalyst for conversion of carbon dioxide; (b) the second compartment (30) comprises (i) an aqueous phase (31); (ii) a product outlet (32) for enabling extraction of any carbon dioxide reduction product produced in the electrolysis cell; wherein the first and the second compartments are in fluid communication, so that any carbon dioxide conversion product produced in the first compartment can flow and / or be extracted to the second compartment, wherein the carbon dioxide reduction product is either a C1-2carboxylic acid or alcohol. Hereby, a novel bi-phasic electrolysis cell design (BPCCU) for CCU (carbon capture and utilization) is provided. Carbon dioxide is captured and converted to a carbon dioxide reduction product in an organic phase with the aid of an organic electrocatalyst. As a result of the design of the bi-phasic cell, the electrocatalyst can easily be regenerated, and the carbon dioxide reduction product can easily be extracted from the cell for subsequent use. According to some embodiments, the carbon dioxide reduction product is formic acid or methanol. Hereby, products being useful in many applications are provided. In the context of this electrolysis cell, formic acid and methanol are 2e and 4e reduction products of carbon dioxide, respectively. According to some embodiments, the organic electrocatalyst is dissolved in the organic phase and / or is anchored to the cathode. Hereby, there is flexibility in terms of how the electrocatalyst can be provided and used in the electrolysis cell. For example, when the electrocatalyst is anchored to the cathode, the cathode can be in the form of a structurally optimized molecular cathode, or molecularly designed electrode, e.g., as defined as a cathode department in this disclosure. According to some embodiments, the organic phase comprises a C7-C10-alkane solvent in the presence of an organic acid chosen from heptanoic, octanoic acid, nonanoic acid or decanoic acid. These acids are insoluble in water and therefore preferable for use in the present disclosure. Hereby, optimal conditions for the electrocatalyst to work, i.e., to catalyze the process of converting carbon dioxide to a reduction product, such as formic acid or methanol, are provided. Formic acid is suitable for use as fuel, an excellent hydrogen carrier and will, due to solubility reasons, immediately go to the aqueous phase of the biphasic cell, where it can be stored and subsequently extracted (see also https: / / pubs.acs.org / doi / 10.1021 / acsenergylett “The high volumetric capacity hydrogen generation from formic acid”). The instant removal from the organic phase of the product also allows a longer lifetime for the electrocatalysts. Moreover, by selectively producing formic acid (HCOOH), any further purification costs are limited or avoided. Formic acid can also be used for other purposes than fuel, such as (i) leather tanning, (ii) as a decalcifier and cleaning product, (iii) as a chemical reducing agent, (iv) as a preservative in animal feeds, (v) as a synthon for several chemicals. Methanol is a versatile chemical used in various industries, including chemicals, pharmaceuticals, fuels, and energy storage. In addition, formic acid or methanol produced according to the present disclosure typically exhibits a very low amount of impurities (a purity of about at least 99%) and therefore they are suitable for use as laboratory chemicals, for which a high purity is a requirement. According to some embodiments, the at least one organic electrocatalyst comprises an organic frustrated Lewis pair. Hereby, the reactivity of such electrocatalyst is used for unexpectedly efficient catalyzing of the carbon capture process. In some embodiments, the organic electrocatalyst is metal-free, which typically make them more environmentally friendly. According to some embodiments, the at least one organic electrocatalyst is chosen from the group comprising: 4-(tert-butyl)-N-(4-(tert-butyl)phenyl)-N-((4,4,5,5-tetramethyl-1,3,2- dioxaborolan-2-yl)methyl)aniline [catalyst 1], 4-(tert-butyl)-N-(4-(tert-butyl)phenyl)-N-(2- (4,4,5,5-tetramethyl-1,3,2-dioxaborolan-2-yl)ethyl)aniline [catalyst 2], 4,4,5,5-tetramethyl-2- (((2,4,6-tri-tert-butylphenyl)thio)methyl)-1,3,2-dioxaborolane [catalyst 3] 4,4,5,5-tetramethyl- 2-(2-((2,4,6-tri-tert-butylphenyl)thio)ethyl)-1,3,2-dioxaborolane [catalyst 4] BBIT-4Me [catalyst 5] and Cu2I4BBIT-4Me [catalyst 6]. Hereby, novel electrocatalysts developed for the purposes of the present disclosure are provided, offering unique and unforeseen performance in terms of catalyzing the carbon dioxide conversion process. Catalysts 1-4 are examples of metal-free catalysts. Modifications and variations, such as using other substituents with similar functionalities would also be included in this disclosure, for any of the catalysts 1-6. According to some embodiments, the first working electrode and the second counter electrode comprises graphite foil, and / or the third reference electrode comprises Ag / AgCl. Hereby, an efficient electrochemical cell is provided, enabling the carbon dioxide conversion process. According to some embodiments, the first (organic) compartment is arranged essentially above the second (aqueous) compartment, to allow for an essentially vertical flow of the carbon dioxide reduction product from the first to the second compartment. Hereby, the vertical flow arrangement of the cell will assist in quickly removing the reduction product from the organic phase to the aqueous phase. According to some embodiments, the bi-phasic electrolysis cell comprises an intermittent phase between the first and the second compartments. By having an intermittent phase between the organic phase and the aqueous phase, in which intermittent phase a mix of the water and organic phases are allowed, waste of catalyst can be avoided or limited, since the intermittent phase is typically not replaced, while the product containing the aqueous phase is replaced with a new one. According to some embodiments, the first working and second counter electrodes, acting as cathode, comprises at least one organic electrocatalyst anchored to the cathode surface via a linker. Typically, some electrocatalysts, such as catalyst 1-4 of this disclosure, are amenable to work in solution, e.g. because of structural limitations not allowing anchoring to an electrode surface as for catalyst 5 and 6, whereas some electrocatalysts, such as catalysts 5-6 of this disclosure, work best anchored, e.g. because of low solubility under normal conditions in the electrolysis phase (typically catalyst 5-6 would be soluble in DMSO). Hereby, the electrocatalyst is exposed in a way that is suitable for certain applications and catalysts. For example, by immobilizing the electrocatalyst on the cathode, the cathode (and thereby the electrocatalyst) may easily be exchanged to adapt to changes in flue gas and / or other condition parameters. According to a second aspect there is provided a method for capturing carbon dioxide to a carbon dioxide reduction product in a bi-phasic electrolysis cell according to the first aspect, comprising the steps of: (a) allowing carbon dioxide, such as from flue gas, to flow into the first compartment via the inlet; (b) applying electrical voltage to the electrodes of the electrolysis cell at a level allowing conversion of carbon dioxide to carbon dioxide reduction product in the presence of at least one organic electrocatalyst, wherein the organic electrocatalyst is dissolved in the organic phase and / or is anchored to the cathode; (c) transferring the carbon dioxide reduction product from the first to the second compartment through mechanical shaking / stirring and / or solvent extraction; thereby storing the carbon dioxide reduction product in the aqueous (inorganic / hydrophilic) phase of the second compartment temporarily or for long-term purposes; wherein the carbon dioxide reduction product is a C1-2carboxylic acid or alcohol. Hereby, carbon dioxide is efficiently and environmentally friendly converted to a reduction product, which can be stored temporarily or for long-term purposes in the aqueous phase. According to some embodiments, the method comprises a subsequent step, wherein the carbon dioxide reduction product is collected from the second compartment via the product outlet, and isolated from water by distillation. Thus, the reduction product can be efficiently extracted from the aqueous phase by using an extractive distillation process. According to some embodiments, an electrical voltage of about -0.8V (vs NHE) is applied to the electrodes. Hereby, a selective electrochemical reduction to a C1-2 carboxylic acid or alcohol, such as formic acid or methanol, can be obtained with the cell design of the present disclosure. According to some embodiments, the at least one electrocatalyst is regenerated after prolonged electrolysis by electrochemical oxidation at about 1.2V (vs NHE). Hence, by regenerating the electrocatalyst(s) used in the process, process efficiency and economy is improved and / or optimized. According to some embodiments, the transfer of the carbon dioxide reduction product from the first to the second compartment is improved by mechanical shaking of the electrolysis cell. Hereby, the concentration of the formic acid product can be even further increased in the aqueous phase. According to a third aspect there is provided an organic electrocatalyst, comprising an organic frustrated Lewis pair. Hereby, by providing novel electrocatalysts, and using an organic frustrated Lewis pair, improved catalytic performance for carbon capture purposes is obtained. Typically, under these reaction conditions, for formation of formic acid (HCOOH), the electrocatalyst typically does not need to contain metal, i.e. can be metal-free, and for formation of methanol (MeOH), an electrocatalyst containing 1strow transition metal (e.g., copper or iron) is typically needed. Especially, active organic electrocatalysts can be regarded as superior in comparison to the critical element containing organometallic electrocatalysts for capture and reduction of CO2 as the later often (i) make the overall processes expensive; (ii) produces extra waste in the form of metal oxide that cannot be regenerated; and (iii) 2nd and 3rd row transition metals containing electrocatalysts produce wastes that are not environmentally benign. Also, the electrocatalysts of the present disclosure are especially designed for providing 2e- reduction products, such as formic acid, or 6e- reduction products, such as methanol. According to some embodiments, the frustrated Lewis pair is based on (i) boron, nitrogen, carbon, and hydrogen, or (ii) boron, sulfur, carbon, and hydrogen. Hereby, improved catalytic performance has been observed. According to some embodiments, the organic electrocatalyst is chosen from: [catalyst type I], [catalyst type II], or (iii) benzimidazole hydrides. According to some embodiments, the organic electrocatalyst is chosen from 4-(tert-butyl)-N- (4-(tert-butyl)phenyl)-N-((4,4,5,5-tetramethyl-1,3,2-dioxaborolan-2-yl)methyl)aniline [catalyst 1], 4-(tert-butyl)-N-(4-(tert-butyl)phenyl)-N-(2-(4,4,5,5-tetramethyl-1,3,2-dioxaborolan-2- yl)ethyl)aniline [catalyst 2], 4,4,5,5-tetramethyl-2-(((2,4,6-tri-tert-butylphenyl)thio)methyl)- 1,3,2-dioxaborolane [catalyst 3], 4,4,5,5-tetramethyl-2-(2-((2,4,6-tri-tert- butylphenyl)thio)ethyl)-1,3,2-dioxaborolane [catalyst 4], BBIT-4Me [catalyst 5] and Cu2I4BBIT- 4Me [catalyst 6]. Hereby, catalytic compounds exhibiting outstanding performance in the carbon capture context are provided. These are designed to be used in the bi-phasic carbon capture cell design of this disclosure, where electrolysis occurs in the organic phase and products (such as formic acid or methanol) are stored and extracted / distilled from the aqueous phase. According to a fourth aspect there is provided a method for synthesizing a metal-free organic electrocatalyst chosen from [catalyst type I], wherein n is equal to 1 or 2, or [catalyst type II], wherein X is equal to -C(CH3)3, -H, -OMe or -NH2, comprising the steps of: (a) mixing (i) bis(4-(tert-butyl)phenyl)amine [SM1] or 2,4,6-tri-tert-butylbenzenethiol [SSM1] with 2-(bromomethyl)-4,4,5,5-tetramethyl-1,3,2-dioxaborolane [SM2] or 2-(2- bromoethyl)-4,4,5,5-tetramethyl-1,3,2-dioxaborolane [SSM2]; (b) exposing the mixture of step (a) to an elevated temperature at about 70-80 ^C, in the presence of Et3N; thereby obtaining the metal-free organic electrocatalyst and HBr. Hereby, a novel synthesis process for obtaining electrocatalysts according to the present disclosure is provided. According to some embodiments, the method for synthesizing a metal-free organic electrocatalyst is used for obtaining one of catalysts 1, 2, 3 or 4. Details related to the synthesis procedure for obtaining these catalysts are shown in the synthesis schemes of the example section of this disclosure. According to a fifth aspect, there is provided a method for synthesizing an organic electrocatalyst chosen from benzimidazole hydrides, comprising the steps of: (a) cyanation of terpyridine ligand (A), followed by (b) condensation with benzene 1,2-diamine in the presence of polyphosphoric acid to introduce benzimidazole units attached to terpyridine to get 6,6''-bis(1H-benzo[d]imidazol-2- yl)-2,2':6',2''-terpyridine (D); and (c) methylation of the resulting product (D) with about 6 equivalents of MeI; thereby obtaining catalyst 5 (2,2'-([2,2':6',2''-terpyridine]-6,6''-diyl)bis(1,3-dimethyl-1H- benzo[d]imidazol-3-ium; BBIT-4Me). According to some embodiments, the method further comprises reaction of BBIT-4Me [catalyst 5] with CuI2 for 24 h in methanol under N2, thereby obtaining Cu2I4BBIT-4Me [catalyst 6]. According to a sixth aspect, there is provided a cathode compartment for use in a bi-phasic electrolysis cell according to previous aspects, comprising at least one organic electrocatalyst according to previous aspects, either in (i) solution, or (ii) wherein the electrocatalyst is anchored to the cathode surface via a pyridine linker. According to some embodiments, the cathode surface comprises pyridine modified graphite for immobilization of the catalyst Cu2I4BBIT-4Me, wherein the linker comprises at least two methylene units and a pyridine ring, for formation of methanol. According to some embodiments, the cathode surface comprises the organic catalyst BBIT- 4Me, wherein the linker comprises at least one benzene ring, for formation of formic acid. According to a seventh aspect there is provided a production facility for use in carbon dioxide capture and / or fuel production, comprising at least one bi-phasic electrolysis cell according to the first aspect, wherein carbon dioxide is captured and reduced to a carbon dioxide reduction product chosen from a C1-2carboxylic acid or alcohol. According to some embodiments, the production facility comprises a plurality of serially connected bi-phasic electrolysis cells. According to some embodiments, the production facility comprises a cathode compartment according to previous aspects. According to some embodiments, the production facility comprises means for controlling the production facility including the bi-phasic electrolysis cell(s). Hereby, the bi-phasic electrolysis cell of the present disclosure, and the associated organic electrocatalysts, are provided on an industrial scale, allowing efficient and sustainable carbon dioxide capture and conversion, as well as potential fuel production, in an industrial context. Such scaled-up design may also include a plurality of bi-phasic electrolysis cells of the present disclosure. To summarize some of the advantages and characteristics of the various aspects of the present disclosure: Effects and features of the second through seventh aspects are to a large extent analogous to those described above in connection with the first aspect. Embodiments mentioned in relation to the first aspect are largely compatible with the second through seventh aspects. The present disclosure will become apparent from the detailed description given below. The detailed description and specific examples disclose preferred embodiments of the disclosure by way of illustration only. Those skilled in the art understand from the guidance in the detailed description that changes and modifications may be made within the scope of the disclosure. Hence, it is to be understood that the herein disclosed disclosure is not limited to the particular component parts of the devices described, or the chemical components of the compounds described, or steps of the methods described since such devices, compounds and methods may vary. It is also to be understood that the terminology used herein is for the purpose of describing particular embodiments only and is not intended to be limiting. It should be noted that, as used in the specification and the appended claim, the articles "a", "an", "the", and "said" are intended to mean that there are one or more of the elements unless the context explicitly dictates otherwise. Thus, for example, reference to "a unit" or "the unit" may include several devices, and the like. Furthermore, the words "comprising", "including", "containing" and similar wordings do not exclude other elements or steps. Definitions The term CCU is to be interpreted as “carbon capture and utilization”. Similarly, the term BPCCU is to be interpreted as “bi-phasic carbon capture and utilization”. In the context of this invention “catalyst 1”, “catalyst 2” and so on refers to specific organic molecules, whereas “catalyst type I”, “catalyst type II” and so on refers to a group of electrocatalysts, having potential structural variations within the group. The terms “flue gas” and “exhaust gas” are used interchangeably throughout this disclosure. The term “NHE” is to be interpreted as “normal hydrogen electrode”. A “frustrated Lewis pair” (FLP) is a compound or mixture containing a Lewis acid and a Lewis base that, because of steric hindrance, cannot combine to form a classical adduct. “Solvent extraction” is the process in which a compound transfers from one solvent to another owing to the difference in solubility or distribution coefficient between these two immiscible (or slightly soluble) solvents. The term “carbon dioxide reduction product” or “carbon dioxide reduced product” refers to the carbon containing compound being produced as a result of reducing carbon dioxide. Typically, the carbon dioxide reduction product is a C1-2carboxylic acid or alcohol, such as formic acid or methanol. In the context of this disclosure, related to immobilization or anchoring of an electrocatalyst to a surface, such as a cathode surface, the terms “immobilized” and “anchored” are used interchangeably. In the context of this disclosure, wt% relate to the percentage of weight of the catalyst with respect to the overall electrode (carbon cloth + surface immobilized linker (such as pyridine) + catalyst) weight. Brief descriptions of the drawings The above objects, as well as additional objects, features and advantages of the present disclosure, will be more fully appreciated by reference to the following illustrative and non- limiting detailed description of example embodiments of the present disclosure when taken in conjunction with the accompanying drawings. Figure 1 shows a cell design for a biphasic electrolysis cell (BPCCU) of the present disclosure. Figure 2 shows the expected mechanism for carbon capture converting carbon dioxide to formic acid using a catalyst of type I of the present disclosure. Figure 3 shows a catalyst of type II of the present disclosure. Figure 4 shows a synthesis scheme of catalyst 1 of the present disclosure. Figure 5 shows a synthesis scheme of catalyst 2 of the present disclosure. Figure 6 shows synthesis schemes of catalyst 3 and 4 of the present disclosure. Figure 7 (a-f) shows cyclic voltammograms including electrochemical characterization, CO2reduction, and regeneration using catalysts 1 and 2: (a) electrochemical characterization of catalyst 2, (b) electrochemical reduction of CO2for catalyst 2, (c) electrochemical regeneration and second reduction for catalyst 2, (d) electrochemical characterization (comparison) of catalyst 1 and 2, (e) electrochemical characterization of catalyst 1, and (f) electrochemical regeneration and second reduction for catalyst 1. Figure 8 shows an example of a BPCCU cell. Figure 9 (a-h) shows IUPAC-names of the catalysts 1, 2, 3 and 4, as well as of starting materials SM1, SM2, SSM1 and SSM2. Figure 10 shows schematically the steps to synthesize catalyst 5 (BBIT-4Me) and 6 (Cu2I4BBIT- 4Me). Details are disclosed in the experimental section of Example 5. Figure 11 shows x-ray diffraction crystallographic structures of catalyst 5 and 6. The solvent molecules and counter anions are removed for clarity. Figure 12 shows x-ray diffraction crystallographic structures of 1-hydride (i.e. BBIT-4Me- hydride). Figure 13 shows electrode / cathode design, including immobilized electrocatalyst, for selective formation of formic acid (a) or methanol (b), respectively. Figure 14 shows 400 MHz1H NMR of BBIT-4Me (referred to as compound “1”) (a) in DMSO and after addition of NaBH4 (b). Figure 15 shows 400 MHz1H NMR of BBIT-4Me (a (upper)) and after electrolysis (b (lower)) under CO2saturated conditions. Figure 16 shows 400 MHz1H NMR of BBIT-4Me (a (lower)) and Cu2I4BBIT-4Me (b (upper)) in DMSO-d6 (BBIT-4Me is referred to as compound “1” and Cu2I4BBIT-4Me is referred to as compound “2”). Figure 17 (a-d) shows HRMS (ESI-TOF) data. Figure 18 shows schematically chemical reduction of BBIT-4Me with NaBH4. Detailed description The present disclosure will now be described with reference to the accompanying drawings and examples, in which preferred example embodiments of the disclosure are shown. The disclosure may, however, be embodied in other forms and should not be construed as limited to the herein-disclosed embodiments. The disclosed embodiments are provided to fully convey the scope of the disclosure to the skilled person. Bi-phasic electrolysis cell Figure 1 shows a bi-phasic electrolysis cell design 1 for the purposes of carbon capture and utilization (CCU), which in this context involves carbon dioxide capture and conversion to a carbon dioxide reduction product, such as formic acid or methanol, to be used e.g., as a fuel. In figure 1, carbon dioxide included in exhaust gases 3 from an industrial facility 2, is allowed to flow via an inlet pipe 11 to the inlet 12 to a first compartment 10 of the bi-phasic cell. For example, carbon dioxide may be separated from other exhaust gases before entering the inlet of the first compartment of the bi-phasic cell. In some embodiments, a membrane 13 is positioned in the inlet to the first compartment to prevent flow of liquid from the first compartment to the inlet pipe. Also, the membrane may have the function of purifying and / or separating the incoming exhaust gas comprising carbon dioxide. Also, and / or alternatively, carbon dioxide is selectively captured from the exhaust gas-mixture in the first compartment of the bi-phasic cell, followed by electrochemical reduction of carbon dioxide to e.g., formic acid. The amount of CO2 that is captured depends on the amount of exhaust gas, the amount of CO2 in the exhaust gas, and the electrolysis cell size and concentration of the catalysts. Typically. There, by including more than one electrolysis cell through the overpressure outlet of the first cell, a higher amount of CO2 can be captured. The first compartment of the electrolysis cell is adapted to comprise an organic phase 14 and at least one electrocatalyst, for allowing the carbon dioxide conversion to occur in the first compartment. The first compartment also includes a first and second electrodes 15 (working (cathode) and counter (anode) electrode) and a third electrode 16 (reference electrode). Means for applying electrical voltage 17 to the electrodes are typically positioned at the exterior of the first compartment. Further, the first compartment typically comprises an overpressure outlet 18 for allowing pressure within the first compartment to be reduced when needed. Typically, the overpressure outlet is positioned at the upper part of the first compartment, such as close to the top, above the upper liquid level of the organic phase when in use, to allow for gas to be let out, without letting any liquid out. Also, the first compartment typically comprises a catalyst outlet 19, for enabling extraction / distillation of used electrocatalyst for change or subsequent regeneration. The catalyst outlet is typically positioned at the lower part of the first compartment, such as close to the bottom, to allow electrocatalyst to be extracted / distilled from the first compartment. Moreover, the first compartment may include means for quality testing 20 of the contents of the first compartment during use, so that e.g., concentration of various components, pH, temperature, pressure, efficiency, production rate etc. can be measured and monitored. The second compartment 30 is adapted to comprise an inorganic and / or aqueous phase 31, so that any reduction product, such as formic acid or methanol, produced in the organic phase from the catalyzed carbon dioxide conversion will transfer quickly to the aqueous phase as a result of solvent extraction. The second compartment further comprises a product outlet 32 for allowing any reduction product, such as formic acid or methanol, to be distilled / extracted from the aqueous phase of the second compartment when in use. Typically, the product outlet is positioned at the lower part of the second compartment, such as close to the bottom, to facilitate efficient distillation / extraction. The bi-phasic electrolysis cell may further comprise an intermittent phase 40 between the first and the second compartment, and in liquid connection with both the first and the second compartment, adapted to contain a mix of the organic phase of the first compartment and the inorganic / aqueous phase of the second compartment. To avoid wasting any catalyst of the organic phase, the intermittent phase will not be replaced when exchanging / replacing the product-containing aqueous phase with new water. The amount of aqueous phase that can be removed after a prolonged electrolysis can typically be measured by a volumetric flask. The bi-phasic electrolysis cell may be of any convenient and suitable size, material and shape, allowing for sustainable bi-phasic carbon capture and utilization according to the present disclosure. Thus, the size of the electrolysis cell can be increased or decreased depending on the needs of the industry size and the amount of exhaust gas. For some purposes, the bi- phasic cell may have a volume of 2 liters (1 l organic phase and 1 l aqueous phase) made up of Teflon plastic. The means for quality testing 20, that may be part of the first compartment, can for example be used in the following way: Every 2ndweek or month (depending on the industry and electrolysis cell size) 0.5 ml of organic phase will be collected and subjected to NMR analysis in order to see if the catalysts’ structure is still intact or if the exhaust gas did some damage to the catalyst. Typically, the first compartment is arranged essentially above the second compartment, to allow for an essentially vertical flow from the first to the second compartment. Turning to figure 8, showing an example design of a cylindrically shaped BPCCU cell 101 according to the present disclosure, a BPCCU cell having a total volume of 5 liters is shown. The diameter of the cylindrically shaped cell of this example embodiment is about 11.3 cm. A flue-gas inlet 112 is arranged in the first compartment (height 30 cm) as a pipe 111 having a diameter of about 2.5 cm projecting from the top to the lower part of the first compartment 110 where flue-gas is dissolved in the organic phase. An over-pressure outlet 118 (diameter 1 cm) with a 5bar pressure (safety) valve 125 is arranged at the top part of the first compartment (above the organic phase). The pressure (safety) valve can hold up to 5 bar pressure and is constructed to open-up immediately upon higher pressure. The over-pressure outlet can be attached to a second BPCCU to improve air quality further. A stopper 150 is arranged at the outside of the first compartment that will block the inward-outward flow of the flue gas and the liquid from the electrolysis cell. A catalyst outlet 119 (1 cm diameter) is arranged close to the bottom of the first compartment. The cathode and the anode 115 and 116 (10 cm x 10 cm) can be separated about 3 cm, and the cathode and the reference electrode can be separated by about 1 cm. In the second compartment 130 (height 20 cm), a product outlet 132 (diameter 1 cm) is arranged close to the bottom of the second compartment. Typically, it should be possible to remove the aqueous layer (with products) without disturbing the organic layer. An intermittent phase or layer 140 (such as a plastic / metal plate in the middle of the two phases) is needed for this purpose. The cell should be air-tight with and without (operating mode) the plate in the middle. Thus, the intermittent layer (140) is arranged between the first and the second compartments.140 can be avoided by carefully utilizing a suitable volumetric flask and using concentration and solubility differences of the two phases. The quality of the catalysts after prolonged electrolysis can be tested e.g., through the catalyst outlet 119 utilizing a sampler 151 that is connected to the outlet. Accordingly, the first aspect of this disclosure includes a bi-phasic electrolysis cell for carbon dioxide capture, comprising a first and a second compartment, at least one inlet connected to the first compartment for allowing carbon dioxide to flow into the first compartment, and means for applying an electrical voltage to a first working electrode, second counter electrode and a third reference electrode, which electrodes are positioned in the first compartment comprising: (a) the first compartment comprises (i) an organic phase, comprising at least one organic electrocatalyst for conversion of carbon dioxide to a reduction product, such as formic acid or methanol; (ii) a catalyst outlet for enabling extraction of used electrocatalyst for subsequent regeneration; and (iii) an overpressure outlet; (b) the second compartment comprises (i) an inorganic phase, comprising water; (ii) a product outlet for enabling extraction of any reduction product produced in the electrolysis cell; (c) the first and the second compartment are in fluid communication, so that any reduction product produced in the first compartment can flow and / or be extracted to the second compartment. Typically, the organic phase comprises a C7-C10-alkane in the presence of an organic acid chosen from heptanoic, octanoic acid, nonanoic acid or decanoic acid, whereby the organic acid typically acts as a proton donor (typically pivotal for HCOOH or methanol formation from CO2). The C7-C10 alkane solvent can be chosen from any alkane within this group, even though it is preferred, for handling and environmental reasons, to avoid any hazardous substances, such as hexane. For example, heptane can be used. Typically, a higher molecular weight solvent is preferable, as it may allow a better temperature range. For the best performance of the electrolysis cell, the organic electrocatalysts should be dissolved in a solvent that is immiscible with water and lighter than water, such as pentane, hexane (not ideal due to health hazards), or heptane. In this case, both gravitation and solvent extraction will act in favour of the process. As the organic acid included in the organic phase, any organic acid having no or very low solubility in water may work. For example, heptanoic acid or octanoic acid are alternatives. Typically, the organic acid will be used in about 0.1 M concentration. However, this could vary in an interval of about 0.01-1M, such as for example 0.05-0.5 M. The conversion of carbon dioxide will, depending on conditions and choice of electrocatalyst, result in the production of a carbon dioxide reduction product, such as a C1-2 carboxylic acid or alcohol. In some embodiments of this disclosure, the electrolysis cell is designed to result in production of formic acid, which is suitable for use as fuel. In some embodiments, the electrolysis cell is designed to result in production of methanol. In some embodiments the electrocatalyst is dissolved in the organic phase and in some embodiments the electrocatalyst is immobilized / anchored to the cathode. In some embodiments, the at least one organic electrocatalyst is a metal-free organic electrocatalysts, comprising an organic frustrated Lewis pair, and in some embodiments the organic electrocatalyst comprises metal. Typically, the dissolved organic electrocatalyst will be used in a concentration of about 1 mM. However, this could vary in an interval of about 0.1-10 mM, such as for example 0.5-5 mM, depending on choice of electrocatalyst and set-up of the cell. When used on the cathode (immobilized) the catalyst is typically present at an amount of 3-4 % (weight), However, the actual amount may vary significantly depending on choice of electrocatalyst and set-up of the cathode and the cell, e.g. in the interval from 0.1- 10 % (weight), or from 1 to 5 % (weight). In some embodiments, the at least one organic electrocatalyst is chosen from the group comprising: 4-tert-butyl-N-4-tert-butylphenyl-N-4,4,5,5-tetramethyl-1,3,2-dioxaborolan-2- ylmethylaniline [catalyst 1], 4-tert-butyl-N-4-tert-butylphenyl-N-2-4,4,5,5-tetramethyl-1,3,2- dioxaborolan-2-ylethylaniline [catalyst 2], 4,4,5,5-tetramethyl-2-2,4,6-tri-tert- butylphenylthiomethyl-1,3,2-dioxaborolane [catalyst 3], 4,4,5,5-tetramethyl-2-2-2,4,6-tri-tert- butylphenylthioethyl-1,3,2-dioxaborolane [catalyst 4], BBIT-4Me [catalyst 5] and Cu2I4BBIT- 4Me [catalyst 6]. These are novel electrocatalysts, specifically designed for use in converting carbon dioxide to formic acid (catalyst 1-5) or methanol (catalyst 6). Typically, the first working and counter electrode comprises graphite foil, and the second reference electrode comprises Ag / AgCl. Typically, the reference electrode (Ag / AgCl) is in 3 M KCl. Thus, in some embodiments, the present electrochemical system is the first example where a completely organic, and boron-nitrogen-carbon-hydrogen based frustrated Lewis pair is used for selective carbon-dioxide capture and conversion to formic acid. In some embodiments according to this disclosure, the boron-nitrogen-carbon-hydrogen based frustrated Lewis pair can be exchanged for a boron-sulphur-carbon-hydrogen based frustrated Lewis pair. The system typically requires minimal applied potential of -0.8 V (vs NHE) and simple (cost effective) graphite foil as working and counter electrode. However, the minimum applied potential could vary in an interval of about -0.1 to – 2 V, such as for example -0.5 to 1 V. Ag / AgCl was used as reference electrode. The electrocatalysts are regenerated after the electrolysis through oxidation at 1.2 V (vs NHE), when the product (formic acid) gets released. However, this could vary in an interval of about 0.5 to 2 V, such as for example 1-1.5 V. For methanol production, using another electrocatalyst (such as catalyst 6), the conditions are typically similar / same as for forming formic acid. The biphasic system (BPCCU) allows product separation through solvent extraction which can be improved by mechanical shaking. As the aqueous phase is the lower phase, gravitation also helps the product to reach the aqueous phase. The biphasic electrolysis cell (BPCCU) captures CO2and converts it selectively to a reduction product, such as formic acid or methanol. The cell constitutes an alkane solvent, such as heptane, and water as two phases. The organic electrocatalysts in the alkane solvent, such as heptane (1 mM), in presence of organic acid, such as butanoic or octanoic acid, capture and convert CO2to a reduction product, such as formic acid or methanol. Strategically designed organic frustrated Lewis pair acts as the electrocatalysts. The catalysts can be regenerated after prolonged electrolysis by electrochemical oxidation. The product (typically formic acid or methanol) goes directly to the aqueous layer due to the solubility reasons and concentration of the product can be increased in the aqueous layer by mechanical shaking. The cell is designed in a way which allows prolonged use of it for CCU. Immediate removal of the product from the organic phase (active phase) allows longer lifetime for the electrocatalysts. Method for capturing carbon dioxide using a BPCCU cell The second aspect of this disclosure shows a method for capturing carbon dioxide by converting the carbon dioxide to a carbon dioxide reduction product in a bi-phasic electrolysis cell according to the first aspect, comprising the steps of: (a) allowing carbon dioxide, such as from flue gas (or exhaust gas), to flow into the first compartment via the inlet; (b) applying electrical voltage to the electrodes of the electrolysis cell at a level allowing conversion of carbon dioxide to a carbon dioxide reduction product, such as formic acid or methanol, in the presence of at least one organic electrocatalyst; (c) transferring the reduction product, such as formic acid or methanol, from the first to the second compartment through mechanical shaking / stirring and / or solvent extraction; thereby storing the reduction product, such as formic acid or methanol, in the inorganic phase of the second compartment temporarily or for long-term purposes. The amount of CO2 that is captured depends on the amount of exhaust gas, the amount of CO2 in the exhaust gas, and the electrolysis cell size and concentration of the catalysts. By including more than one electrolysis cell through the overpressure outlet of the first cell, the overall captured amount of carbon dioxide can be increased. Typically, at least about 78% of the CO2 entering the electrolysis cell can be removed / captured (at atmospheric pressure). Using a higher pressure results in a higher removal. Also, in order to obtain a higher removal, two or more electrolysis cells can be serially connected. In the present electrolysis setup, electrocatalysts from 1 mM to 100 mM concentration can typically be used. Ideally, each molecule can capture one CO2molecule, reduce it to reduction product, get regenerated, and capture CO2 again. Figure 2 shows the mechanisms of the carbon capture process using a catalyst of type I, i.e., including for example catalyst 1 and 2 of the present disclosure. In this figure it can be shown how the electrocatalyst facilitates reduction of the carbon dioxide molecule and the resulting conversion to formic acid (HCOOH). The presence of an organic acid, such as octanoic acid, provides the necessary hydrogen atoms that is added to the formic acid product molecule. The nitrogen atom and the boron atom of the electrocatalysts are essential for the reduction of the carbon dioxide molecule to occur. Similarly, when using a catalyst of type II (see figure 3), i.e., including for example catalyst 3 and 4 of the present disclosure, wherein, among other changes, the nitrogen atom has been exchanged for a sulphur atom, a reduction of the carbon dioxide molecule takes place (not shown) resulting in a conversion to formic acid (HCOOH). Typically, the electrolysis system is expected to be equally efficient in the temperature range of 25-60 ^C. The boiling point of the organic phase solvent, i.e., the C5-C10 alkane, will typically be a limiting factor. Typically, the aqueous layer may exhibit a near-neutral pH (6.8-7.2). When storing the reduction product, such as formic acid or methanol, in the aqueous phase, the aqueous phase may for example be replaced / exchanged every week or month (depending on the industry and electrolysis cell size), whereby the reduction product, such as formic acid or methanol can be distilled out. As an alternative or in addition, the method comprises a subsequent step d, wherein the reduction product, such as formic acid or methanol, is collected from the second compartment via the product outlet, and isolated from water by for example extractive distillation, since the boiling point of water and formic acid or methanol are very close. Using an extractive distillation agent (e.g., sulfone), formic acid or methanol can be readily removed from mixtures containing it and water by using extractive distillation. The process of extractive distillation is further described in patent US4642166). During electrolysis, an electrical voltage of about -0.8V (vs NHE) is typically applied to the electrodes. Typically, the at least one electrocatalyst is regenerated after prolonged electrolysis by electrochemical oxidation at about 1.2V (vs NHE). In some embodiments, the transfer of the reduction product, such as formic acid or methanol, from the first to the second compartment is improved by mechanical shaking of the electrolysis cell. For example, mechanical shaking once every day may be preferable to get rid of the product from the active organic phase. Organic electrocatalysts The third aspect of this disclosure shows an organic electrocatalyst, comprising an organic frustrated Lewis pair. In essence, the present inventors have invented a new series of completely organic electrocatalyst that can capture CO2and electrochemically reduce it selectively to formic acid or methanol at -0.8 V (vs NHE). These electrocatalysts can be regenerated after prolonged electrolysis by electrochemical oxidation at 1.2 V (vs NHE). The electrocatalysts are designed to be used in the BPCCU system of the present disclosure (alkane solvent (such as heptane) + water) where electrolysis occurs in the organic phase in presence of an organic acid, such as butanoic acid, and products get stored in the aqueous phase. As part of the research project forming basis for the present disclosure, organic frustrated Lewis pairs (FLPs) have been tested as active electrocatalysts. One focus has been on (metal- free) boron, nitrogen, carbon and hydrogen containing electrocatalysts, i.e., for example catalysts of type I (see figure 2). Other electrocatalysts with similar properties, i.e., space between active centres of the FLPs’, solubility, and electrochemical features may also be used. For example, electrocatalysts wherein the nitrogen atom has been exchanged for a sulphur atom may be used. Examples of sulphur-containing electrocatalysts are catalysts of type II (see figure 3). The catalysts of type I that have been synthesized (catalyst 1 and 2) have been characterized by NMR and HRMS spectroscopy. Also, the formation of the product (formic acid) after electrolysis is confirmed by NMR spectroscopy. Moreover, the electrochemical performance of the electrocatalysts and the possible regeneration have been tested out (see example section). For the electrocatalysts of the present disclosure, it has been found that (i) the presence of electron-deficient boron and electron-efficient nitrogen (or sulphur) close by (ii) the presence of bulky tertiary butyl groups and methyl groups are preferred and / or essential features. Thus, in some embodiments, metal-free electrocatalysts of the present disclosure can be chosen from ^ 4-(tert-butyl)-N-(4-(tert-butyl)phenyl)-N-((4,4,5,5-tetramethyl-1,3,2-dioxaborolan-2- yl)alkyln)aniline, where n = 1 or 2 [catalyst type I] (see figure 2) and ^ 4,4,5,5-tetramethyl-2-(((2,4,6-tri-tert-butylphenyl)thio)alkyln)-1,3,2-dioxaborolane, where n = 1 or 2, and the 4-butyl substituent (-C(CH3)3) can be exchanged for -H, OCH3 or -NH2 [catalyst type II] (see figure 3). In some embodiments, metal-free electrocatalysts of the present disclosure can be chosen from 4-tert-butyl-N-4-tert-butylphenyl-N-4,4,5,5-tetramethyl-1,3,2-dioxaborolan-2- ylmethylaniline [catalyst 1], 4-tert-butyl-N-4-tert-butylphenyl-N-2-4,4,5,5-tetramethyl-1,3,2- dioxaborolan-2-ylethylaniline [catalyst 2], 4,4,5,5-tetramethyl-2-2,4,6-tri-tert- butylphenylthiomethyl-1,3,2-dioxaborolane [catalyst 3] and 4,4,5,5-tetramethyl-2-2-2,4,6-tri- tert-butylphenylthioethyl-1,3,2-dioxaborolane [catalyst 4]. In some embodiments, the organic electrocatalysts can be chosen from benzimidazole hydrides or pyridine-benzimidazole hydrides, such as BBIT-4Me (catalyst 5) and Cu2I4BBIT-4Me (catalyst 6). For the electrocatalyst of benzimidazole hydride type, pyridine is typically used as the linker between the conductive surface and the catalyst, even though other alternatives could also be used as long as similar functionality is achieved. Thus, the linker (such as pyridine) is necessary to anchor the catalyst, and has typically part in the electron and charge transfer but is structurally not part of the catalyst. Variations and alternatives to pyridine as the linker are also included in the present invention. Method for synthesizing metal-free organic electrocatalysts The fourth aspect of this disclosure shows a method for synthesizing a metal-free organic electrocatalyst chosen from [catalyst type I], wherein n is equal to 1 or 2, or [catalyst type II], wherein X is equal to -C(CH3)3, -H, -OMe or -NH2, comprising the steps of: (a) mixing (i) bis(4-(tert-butyl)phenyl)amine [SM1] or 2,4,6-tri-tert-butylbenzenethiol [SSM1] with (ii) 2-(bromomethyl)-4,4,5,5-tetramethyl-1,3,2-dioxaborolane [SM2] or 2-(2-bromoethyl)- 4,4,5,5-tetramethyl-1,3,2-dioxaborolane [SSM2]; (b) exhibiting the mixture of step (a) to an elevated temperature at about 70-80 ^C, in the presence of Et3N; thereby obtaining the metal-free organic electrocatalyst and HBr. In some embodiments, the method for synthesizing comprises obtaining any one of catalysts 1, 2, 3 or 4 by using any of the schemes as shown in figure 4-6. Method for synthesizing an organic electrocatalyst The fifth aspect of this disclosure refers to a method for synthesizing an organic electrocatalyst of benzimidazole hydride-type, such as BBIT-4Me (catalyst 5) and inorganic catalyst Cu2I4BBIT- 4Me (catalyst 6). Figure 10 discloses the scheme and steps for synthesizing catalyst 5 and catalyst 6 (details can be found in the examples). Cathode department The sixth aspect of this disclosure refers to a cathode department for use in the electrolysis cell of the present disclosure, and is disclosed in Figure 13, where it can be shown that the electrocatalyst for use in the carbon reduction reaction is anchored to the cathode. Hereby, the electrocatalyst may e.g. more stable than if in solution. The overall principle and set-up of the electrolysis cell comprising the cathode department is as disclosed in figure 8. The electrocatalyst is anchored through covalent bonding to the cathode material via a linker. The identity of an optimal linker and / or the cathode material may be different depending on various parameters having an effect on the conditions in the electrolysis cell. For example, depending on the flue gas entering the electrolysis cell, the cathode may need to be changed, so that optimal product selectivity and stability are obtained. For example, depending on the presence of particular gases, such as NOxSOxetc., some electrodes or cathodes may work less well, and exchanging the cathode may be preferred or required. Further, the choice of electrocatalyst and therefore desired carbon reduction product, the cathode material and / or the linker may be different and / or need to be changed. As regards size, for a 500 ml electrolysis set-up, a 5 cm x 5 cm cathode can typically be used. However, there are in principle no lower or upper size restrictions of the electrodes as long as they fit in the electrolysis cell. In the context of this disclosure, cathode and cathode department may be used interchangeably in some embodiments. In some embodiments, the cathode surface comprises pyridine modified graphite for immobilization of a catalyst. Modifications other than pyridine modified graphite can also be used depending on the electrocatalyst used and other conditions. In some embodiments, for formation of methanol, the cathode surface comprises pyridine modified graphite for immobilization of the catalyst Cu2I4BBIT-4Me, wherein the linker comprises at least two methylene units and a pyridine ring. In some embodiments, for formation of formic acid, the cathode surface comprises the organic catalyst BBIT-4Me and the linker comprises at least one benzene ring. Production facility for use in the BPCCU The seventh aspect of this disclosure refers to a production facility for use in carbon dioxide capture and / or fuel production, comprising at least one bi-phasic electrolysis cell according to the first aspect, wherein carbon dioxide is captured and converted to a reduction product, such as formic acid or methanol. The production facility 2 can for example be an industrial facility or factory related to industrial production wherein exhaust gases including carbon dioxide 3 are emitted. Thus, according to this aspect, the bi-phasic electrolysis cell of the present disclosure, and the associated organic electrocatalysts, are provided in an industrial scale, allowing efficient and sustainable carbon dioxide capture and conversion, as well as potential fuel production, in an industrial context. Formic acid may for example, when used in a fuel cell, be split into water and carbon dioxide, a process generating electricity / energy, which in turn may be used to power an engine or similar functionality. Methanol can also be used as a fuel, and both formic acid and methanol can be used for laboratory chemical uses. Methanol is a versatile chemical used in various industries, including chemicals, pharmaceuticals, fuels and energy storage. When using the carbon reduction products for fuel purposes, a purity of about 80-90% is typically required, whereas for laboratory standard purposes, a purity of about 99,9% is typically required. The technology of the present disclosure is amenable for use for both these purposes. In some embodiments, one bi-phasic electrolysis cell adapted to the size of the industrial facility and to the amount of exhaust gas including carbon dioxide is provided. In some embodiments, such scaled-up design may also include a plurality of bi-phasic electrolysis cells of the present disclosure, each cell having an independent or parallel function. Some practical considerations to take into account when scaling-up and / or serially connecting a plurality of cells are for example: (i) the scale-up and / or serial connection might result in low energy efficiency in presence of certain flue gas components of certain industries, and (ii) as water is used as one of the phases, in case of below 0 degree temperature (Celsius scale) of the surroundings, it will require additional heating. The present disclosure will now be described with reference to the following examples. Examples Example 1 – Synthesis of electrocatalysts – catalyst 1 See figure 4. Single Step: A clean 100 ml microwave vial was dried in the oven (around 65°C) for 24 hours then cooled under a nitrogen atmosphere before use. Inlet and outlet needles were on the septum to ensure inert gas circulation within the microwave vial while transferring the chemicals to the vial.0.515 g of SM1 (1.21 mmol) was transferred to the microwave vial, followed by 0.4 mL of SM2 (1 eq.) while the reaction mixture was under continuous stirring.5 mL of degassed triethyl amine was added to the mixture afterwards. The reaction mixture in the microwave vial was tightly sealed and heated at 70°C for 3 days in an oil bath, followed by drying under vacuum using the Schlenk line. The resulting product (catalyst 1) was stored under inert atmosphere. A yield was calculated at 95-98 %, and it was estimated based on the1HNMR analysis.1H-NMR 400 MHz CD3CN δ 1.26 (s, 31H), 3.06 (q, 2H), 7.12-7.14 (d, 4H), 7.21-7.23 (d, 4H)13C-NMR 101 MHz CD3CN δ 8.7 ppm, 25.2, 31.9, 35.1, 56.8, 86.6, 117.6, 126.9, 142.8, 143.1 Example 2 – Synthesis of electrocatalysts – catalyst 2 See figure 5. Step 1: Anhydrous THF (25 ml) was transferred from an inert solvent purification system to the two- necked round-bottom flask under an inert atmosphere. The flask with THF was cooled down in a dry ice and acetone bath to -78 °C. To the cooled THF solution, 0.636 g of 1,2-dibromoethane (0.293 ml, 3.38 mmol) was added, followed by the dropwise addition of 2.5 M n-Bu-Li (3.5 ml). Thereafter, trimethyl borate (0.412 ml, 0.384g, 3.69 mmol) was added dropwise. After 17 hours, 4N HCl dioxane (0.45 ml) was added dropwise, and the resulting product was concentrated under a high vacuum to get 0.44g (85% yield) of (2-bromoethyl) boronic acid.1H-NMR 500 MHz CD3OD, δ 3.69 (s, 2OH), 4.88 (s, 4H),13C-NMR 125 MHz CD3OD, δ66.8ppm Step 2: 0.65 g of (2-bromoethyl) boronic acid (4.22 mmol) and pinacol (1 eq.0.50 g, 4.23mmol) were added to a two-necked round-bottom flask under an inert atmosphere. The mixture was then stirred while 30 ml of degassed DCM was transferred into the flask. The reaction mixture was kept under an inert atmosphere at room temperature for 17 hours. Once the reaction was complete, the product was sedimented down, and majority of the solvent was carefully removed with a syringe. The remaining solvent was then removed by heating the crude product at 45°C over a period of 5 h under nitrogen flow, resulting in a 96 % yield (0.95g) of white product.1H-NMR 400 MHz CD3OD, δ 1.23ppm (s, 12H), 3.69ppm (s, 2H), 4.93ppm (s,2H)13C-NMR 100 MHz CD3OD, δ 25.9, 69.0, 76.7 ppm Step 3: A clean 100 ml microwave vial was dried in the oven (around 65°C) for 24 hours then cooled under a nitrogen atmosphere before use. Inlet and outlet needles were on the septum to ensure inert gas circulation within the microwave vial while transferring the chemicals to the vial. First 0.249 g of SM1 (0.88 mmol) was transferred to the vial, followed by 0.208 g of SSM2 (0.88 mmol), while the reaction mixture was stirred continuously. Finally, 5 ml of degassed triethyl amine was transferred to the mixture. The microwave vial containing the reaction mixture was tightly closed with a cap and heated in an oil bath to 80°C for 4 days, followed by drying under vacuum using the Schlenk line. It resulted in 0.375 g of catalyst 2 (off-white product with 98% yield).1H-NMR 500 MHz CD3CN δ 1.25ppm (s, 11H), 1.29ppm (s, 20H), 2.98-3.02ppm (q, 1H), 3.63 (s, 1H), 4.39 (s, 2H), 7.01-7.02ppm (d, 4H), 7.28-7.29ppm (d, 4H)13C-NMR 125 MHz CD3CN δ 25.6, 32.0, 35.1, 67.9, 77.3, 118.9, 127.3, 142.8, 144.3 ppm Example 3 – Synthesis of electrocatalysts – catalyst 3 and 4 See figure 6 for synthesis schemes of respective catalyst belonging the catalyst type II, i.e., containing sulfur instead of nitrogen. Overall synthesis conditions are similar to the synthesis of catalysts 1 and 2 as shown in previous examples. Example 4 – Catalyst 1 and 2 - Cyclic voltametric and electrolysis experiments, CO2 capture and electroreduction, and HCOOH formation Both catalysts 1 (1 mM) and 2 (1 mM) have been tested for CO2 capture and electroreduction at room temperature in 15 mL heptane, acetonitrile, and dichloromethane solution. Graphite foils (1 cm x 1 cm) were used as working and counter electrodes. Ag / AgCl was used as a reference electrode. Tetrabutylammonium hexafluorophosphate (TBAPF6) (0.1 M) was used as the supporting electrolyte. See Figure 7 (a-f), wherein figure 7a-c refers to catalyst 2, figure 7d compares catalyst 1 and 2, and figure e-f refers to catalyst 1. More specifically, figure 7a relates to CO2 capture by catalyst 2, figure 7b relates to CO2 reduction to formic acid by catalyst 2, figure 7c relates to regeneration of the electrocatalyst 2, figure 7d relates to comparison between catalysts 2 and 1, figure 7e relates to CO2 capture by catalyst 1 and figure 7f relates to CO2 reduction to formic acid by catalyst 1 and regeneration. ^ Both the catalysts showed immediate interaction with CO2in CO2-saturated acetonitrile solution (see below), reflected by the increasing area under the cyclic voltammogram, which also indirectly indicates an increase of the capacitance behaviour under the CO2-saturated condition (figure 7a, d and e). ^ Control potential electrolysis (CPE) experiments were conducted at -1.2 V (vs Ag / AgCl) for 4 h to get the CO2 electroreduction product in the presence of catalysts 1 and 2 in two separate experiments (figure 7 b and e). The formation of HCOOH was confirmed by13C (1H) NMR (singlet at 172.9 ± 0.1 ppm) and 500 MHz1HNMR experiments. ^ The addition of 0.5 V% of water (additional proton source) improved the HCOOH formation. In this case, the formation of HCOOH could be confirmed within 1 h of electrolysis by NMR. ^ After the CPE experiments, upon bubbling the post-electrolysis solution with CO2 for 2 min, the electrocatalyst 2 returns to its original electrochemical response. confirming the regeneration of the catalyst and the release of the product (HCOOH) (figure 7 c). ^ In the case of the biphasic system, such regeneration will not be necessary frequently, as the product is expected to be easily separated out. ^ Following a similar procedure, regeneration of catalyst 1 is not obtained to the same extent as catalyst 2 (figure 7 c and f) ^ Overall, catalyst 2 exhibits better performance than catalyst 1 for carbon dioxide capture, reduction, and catalyst regeneration under the tested reaction conditions. Example 5 - Molecular electrodes for selective formation of formic acid and methanol from CO2 To promote the selective formation of methanol (MeOH) from the electrochemical reduction of CO2, a multiple-hydride transfer approach utilizing benzimidazole hydrides is employed. The ligand framework is designed to position the transition metal close to the benzimidazole units, enabling the catalytic generation of reactive hydride intermediates in the vicinity of transient metal-hydrides (M–H). Benzimidazole hydrides are previously reported for reducing CO2to formate (HCOO-) via hydride transfer. Three consecutive hydride transfers to the substrate CO2 are mandatory before the product is released to achieve the six-electron reduction necessary for methanol production. In recent years, Copper (Cu) containing electrocatalysts have shown great promise for CO2electroreduction to value-added products. Keeping all these in mind, the inventors have designed and synthesized ligand framework 1 [2,2'- ([2,2':6',2''-terpyridine]-6,6''-diyl)bis(1,3-dimethyl-1H-benzo[d]imidazol-3-ium)] (also referred to as catalyst 5 in the context of this disclosure) and corresponding Cu complex (2, Cu2I4BBIT) (also referred to as catalyst 6 in the context of this disclosure). The ligand framework (1) was synthesized using a multiple-step process (Figure 10), starting from cyanation of terpyridine ligand (A), followed by condensation with benzene 1,2-diamine in the presence of polyphosphoric acid to introduce benzimidazole units attached to terpyridine to get 6,6''- bis(1H-benzo[d]imidazol-2-yl)-2,2':6',2''-terpyridine (D). The methylation of the resulting product (D) with an excess of MeI resulted in 1 (2,2'-([2,2':6',2''-terpyridine]-6,6''-diyl)bis(1,3- dimethyl-1H-benzo[d]imidazol-3-ium; BBIT-4Me) with overall 35% yield. The NMR spectra and mass envelop at 524.25 (m / z) confirmed the molecular identity of 1 [calculated for C33H29N7+ ([M+H+]) 524.2557 (m / z), found 524.2566]. The copper complex (2) was prepared by the reaction of 1 with CuI2 for 24 h in methanol under N2. The recrystallization from the MeOH solution resulted reddish-brown solid which was dissolved in 1:2 MeOH: Acetonitrile mixture at 500C and followed by slow evaporation resulted in shining orange-colored X-ray diffraction quality crystals of 2 (Figure 11 (a, b)) The methanol solution of 2 showed a mass envelop at 1029.82 (m / z) confirmed the molecular identity of 2 [calculated for C33H29Cu2I3N7([M+]) 1029.8205 (m / z), found 1029.8215 (m / z)]. Before testing the electrocatalytic CO2 reduction efficiency of 2, both D and 1 were tested under CO2-saturated conditions in dimethyl sulfoxide (DMSO), using a three-electrode setup using glassy carbon as the working (see detail in the experimental section). In the case of D, no hydride intermediate could be formed [electrochemically or chemically (NaBH4induced)], whereas with 1, a hydride intermediate could be easily formed both electrochemical and chemical pathways, confirmed by 1H NMR signal at 4.11 ppm (figure 14). A control potential electrolysis experiment at -1.4 V (vs NHE) under CO2 saturated conditions and 0.1 V% of water for 4 h duration resulted a new peak at 8.05 ppm (figure 15), corresponding to formic acid species with a 72% yield. It was further supported by a distinct13C NMR peak at 165 ppm. No other products were isolated under this reaction conditions. An X-ray diffraction quality crystal from the NaBH4-induced reduction (Figure 12) under inert conditions could be isolated. The disappearance of this hydride signal upon the purging of CO2into the DMSO solution of 1 and followed by the appearance of a new signal at 8.05 ppm confirms that CO2 can be directly inserted into the benzimidazole hydride (C – H) bonds of and result in 2e reduced formic acid species. The discrepancy in behaviour between D and 1, under reductive conditions shows clear impact of the N-methyl units. Nevertheless, the X-ray diffraction structure of 1 displays the hydride units are far apart (distance between two benzimidazole carbons having the hydrides > 11.85 Å) from each other, which is unfavourable for multiple hydride transfer to the same CO2 molecule, resulting in formic acid species as the only product from the electrochemical and the chemically induced reduction. Inside the Cu-complex (2), this distance decreases (< 7 Å) to a significant extent. Moreover, the distance between the Cu-centre and the benzimidazole carbons that can form hydrides is less than 3.25 Å, a distance that can be suitable for the multiple hydrides. From the previously published reports and the kinetic data, we can assume that M – H species will form and interact faster with the incoming substrate (CO2) than the benzimidazole-hydrides. In order to form methanol from CO2, it needs three consecutive hydrides transfer and thus to make it possible the organic hydride donors must be closely spaced to the metal centres. Although the molecular electrocatalysts allow this sort of structural optimization and detail investigation of reaction mechanisms, they are well-known to undergo decomposition, deactivation, or copolymerization under the reaction conditions. This can be avoided by anchoring the structurally optimized electrocatalysts on the solid conductive surface (figure 13). Following the previously reported procedure of the inventors (DOI: 10.1039 / D3TA00071K (Paper) J. Mater. Chem. A, 2023, 11, 13331-13), 2 was possible to anchor onto a pyridine modified graphite surface using ligand exchange mechanism. The resulting electrode (2PG; 2 anchored on pyridine modified graphite surface) surface was characterized using EDX, SEM, and TEM spectroscopy. A control potential electrolysis experiment at -2.5 V (vs NHE) under CO2 saturated conditions and 0.1 V% of water in acetonitrile for 2 h duration resulted a new singlet peak at 2.8 ppm, corresponding to methanol with a 35% faradaic efficiency (FE). Increasing the water concentration to 0.15 V% improved the FE 41%, but further increment to 0.3 V% decreases the yield significantly and resulted only 28% FE for CH3O- production. No other liquid phase products were isolated. Experimental: Synthesis of [2,2':6',2''-terpyridine] 1,1''-dioxide (B). See figure 10, step (i). A solution of 3 (210.0 mg, 0.9 mmol, 1 equiv.) in dichloromethane (9 mL) was added to a solution of m-chloroperbenzoic acid (756.5 mg, 3.4 mmol, 3.8 equiv.) in dichloromethane (9 mL). The resulting mixture was stirred at room temperature for 15 h. The mixture was extracted with a 10% sodium carbonate solution (2 x 20 mL). The organic layer was separated, dried over magnesium sulfate, filtered, and evaporated, resulting in a yellow solid. The crude mixture was subsequently purified using column chromatography on silica gel, using a gradient of 5-25% methanol in dichloromethane. 4 was isolated as a white solid (129.0 mg, 54%).1H NMR (400 MHz, CDCl3, 298.2 K) δ: 8.94 (d, J= 8.0 Hz, 2H), 8.34 (dd, J= 6.3, 1.3 Hz, 2H), 8.20 (dd, J= 8.0, 2.2 Hz, 2H), 7.98 (t, J= 8.0 Hz, 1H), 7.38 (td, J= 7.7, 1.3 Hz, 2H), 7.33 – 7.27 (m, 2H);13C NMR (101 MHz, CDCl3, 298.1 K) δ: 149.5, 147.3, 140.9, 136.8, 128.1, 126.2, 125.8, 125.5. Synthesis of [2,2':6',2''-terpyridine]-6,6''-dicarbonitrile (C) See figure 10, step (ii). Trimethylsilyl cyanide (186 µL, 1.5 mmol, 3.0 equiv.) was added to a solution of 4 (129.0 mg, 0.49 mmol, 1 equiv.) in dichloromethane (6 mL). N,N-Dimethylcarbamyl chloride (134 µL, 1.5 mmol, 3.0 equiv.) was added, and the mixture was stirred at room temperature for 72 h. The solution was diluted with dichloromethane (4 mL), and a 10% potassium carbonate solution (5 mL) was added. Continuous stirring at room temperature for 15 min led to effervescence. The phases were then separated, and the aqueous layer was extracted with dichloromethane (2 x 10 mL). The combined organic layers were dried over magnesium sulfate, evaporated, and subjected to purification by column chromatography on silica gel, using 30% ethyl acetate in n- pentane as the eluent.5 was isolated as a white solid (94.3 mg, 68% yield).1H NMR (400 MHz, CDCl3, 298.1 K) δ: 8.81 (dd, J= 8.1, 1.1 Hz, 2H), 8.57 (d, J= 7.9 Hz, 2H), 8.07 – 7.97 (m, 3H), 7.75 (dd, J= 7.6, 1.1 Hz, 2H);13C NMR (101 MHz, CDCl3, 298.1 K) δ: 157.9, 153.7, 138.7, 138.1, 133.5, 128.5, 124.3, 122.8, 117.4. Synthesis of [2,2':6',2''-terpyridine]-6,6''-dicarbonitrile (D). See figure 10, step (iii). Finely grounded o-phenylenediamine (47.5 mg, 0.44 mmol, 2.1 equiv.) and 5 (59.0 mg, 0.21 mmol, 1 equiv.) were added to polyphosphoric acid (1.5 mL). The mixture was stirred at 200 °C for 16 h. After cooling to room temperature, the mixture was poured into water (15 mL), leading to precipitation. The resulting precipitate was collected by filtration, suspended in water (15 mL), and neutralized with aqueous ammonia (32%). Following filtration, the dried precipitate was dissolved in the minimum amount of dimethyl sulfoxide. Shiny gold-colored crystals of BBIT were obtained via methanol vapor diffusion (53.0 mg, 55% yield).1H NMR (400 MHz, DMSO-d6, 295.2 K) δ: 13.17 (s, 2H), 9.09 (d, J= 7.8 Hz, 2H), 8.81 (dd, J= 7.8, 1.1 Hz, 2H), 8.42 (dd, J= 7.8, 1.1 Hz, 2H), 8.34 (t, J= 7.8 Hz, 1H), 8.23 (t, J= 7.8 Hz, 2H), 7.72 (d, J= 27.5 Hz, 4H), 7.29 (s, 4H);13C NMR (101 MHz, DMSO-d6, 298.2 K) δ: 155.0, 154.3, 150.7, 148.1, 144.0, 138.8, 138.4, 134.9, 123.4, 122.0, 121.7, 121.4, 119.5, 112.1; HRMS (ESI-TOF): calcd for C29H19N7+([M+H+]) 466.1775 m / z, found 466.1765 m / z. See figure 17(a). Synthesis of 2,2'-([2,2':6',2''-terpyridine]-6,6''-diyl)bis(1,3-dimethyl-1H-benzo[d]imidazol-3- ium) (1). See figure 10, step (iv). D (232.8 mg, 0.5 mmol, 1.0 equiv.) was added to a solution of potassium carbonate (248.8 mg, 1.8 mmol, 3.6 equiv.) in acetonitrile (3 mL). Methyl iodide (405 µL, 6.5 mmol, 13 equiv.) was added, and the mixture was stirred at 100 °C for 36 h. The mixture was cooled down to room temperature and the acetonitrile solvent was evaporated using a rotary evaporator. The crude mixture was purified by column chromatography on silica gel, using a gradient of 5-10% methanol in dichloromethane. BBIT-4Me was isolated as an off-white solid (262.0 mg, 67% yield).1H NMR (400 MHz, DMSO-d6, 298.2 K) δ: 9.11 (dd, J= 8.1, 1.0 Hz, 2H), 8.62 (d, J= 7.9 Hz, 2H), 8.54 (t, J= 7.9 Hz, 2H), 8.34 (dd, J= 7.7, 1.0 Hz, 2H), 8.30 – 8.19 (m, 5H), 7.89 – 7.80 (m, 4H), 4.19 (s, 12H) (figure 16);13C NMR (101 MHz, DMSO-d6, 298.2 K) δ: 156.0, 153.7, 147.2, 140.5, 139.7, 139.4, 131.8, 128.8, 127.3, 124.2, 122.2, 113.8, 33.4; HRMS (ESI-TOF): calcd for C33H29N7+([M+H+]) 524.2557 m / z, found 524.2566 m / z. See figure 17(b). Synthesis of the Cu-complex (CuBBIT-4Me). See figure 10, step (v). A solution of BBIT-4Me (80.0 mg, 0.1 mmol, 1 equiv.) in methanol / dichloromethane (10 mL, 1:1) was added dropwise to a solution of copper (II) iodide (63.4 mg, 0.2 mmol, 2 equiv.) in methanol (10 mL) under inert atmosphere. An immediate color change and the formation of a dark solution were noted. The mixture was stirred at room temperature for 24 h. Cooling the crude mixture in the fridge for 15 min at 4°C resulted in the formation of a precipitate which was collected and washed with diethyl ether. CuBBIT-4Me was isolated as a dark brown solid (74.2 mg, 62% yield). HRMS (ESI-TOF): calcd for C33H29Cu2I3N7([M+]) 1029.8205 m / z, found 1029.8215 m / z. See figure 17 (c). Chemical reduction of BBIT-4Me with NaBH4. See figure 18. BBIT-4Me (20.0 mg, 0.026 mmol, 1 equiv.) was dissolved in deuterated DMSO (1 mL). Upon addition of NaBH4 (2.9 mg, 0.077 mmol, 3 equiv.), an immediate color change and bubbling were noted. The reaction was stirred at room temperature for 5 min, after which the mixture was subjected to analysis using HRMS and NMR (figure 14). HRMS (ESI-TOF): calcd for C33H31N7 ([M-H+]) 524.2557 m / z, found 524.2553 m / z. See figure 17(d). The person skilled in the art realizes that the present disclosure is not limited to the preferred embodiments described above. The person skilled in the art further realizes that modifications and variations are possible within the scope of the appended claims. For example, alternative designs of the bi-phasic cell depending on context may be contemplated, as well as alternative electrocatalysts, as long as the overall effects are achieved. Additionally, variations to the disclosed embodiments can be understood and effected by the skilled person in practicing the claimed disclosure, from a study of the drawings, the disclosure, and the appended claims.

Claims

CLAIMS 1. A bi-phasic electrolysis cell (1) for carbon dioxide capture, comprising a first (10) and a second (30) compartment, at least one inlet (12) connected to the first compartment for allowing carbon dioxide to flow into the first compartment, and means for applying electrical voltage (17) to a first working electrode (cathode), a second counter electrode (anode) (15) and a third reference electrode (16), which electrodes are positioned in the first compartment, wherein: (a) the first compartment comprises (i) an organic phase (14), for facilitating electrocatalytic reduction of carbon dioxide into a carbon dioxide reduction product; (ii) a catalyst outlet (19) for enabling extraction of used electrocatalyst for subsequent regeneration or for changing the organic solvent; (iii) an overpressure outlet (18), and (iv) at least one organic electrocatalyst for conversion of carbon dioxide; (b) the second compartment (30) comprises (i) an aqueous phase (31); (ii) a product outlet (32) for enabling extraction of any carbon dioxide reduction product produced in the electrolysis cell; wherein the first and the second compartments are in fluid communication, so that any carbon dioxide conversion product produced in the first compartment can flow and / or be extracted to the second compartment, wherein the carbon dioxide reduction product is either a C1-2 carboxylic acid or alcohol.

2. The bi-phasic electrolysis cell according to claim 1, wherein the carbon dioxide reduction product is formic acid or methanol.

3. The bi-phasic electrolysis cell according to claim 1 or 2, wherein the organic electrocatalyst is dissolved in the organic phase and / or is anchored to the cathode.

4. The bi-phasic electrolysis cell according to any one of the preceding claims, wherein the organic phase comprises a C7-C10-alkane in the presence of an organic acid chosen from heptanoic, octanoic acid, nonanoic acid or decanoic acid.

5. The bi-phasic electrolysis cell according to any one of the preceding claims, wherein the at least one organic electrocatalyst comprises an organic frustrated Lewis pair.

6. The bi-phasic electrolysis cell according to any one of the preceding claims, wherein the at least one organic electrocatalyst is chosen from the group comprising: 4-(tert-butyl)-N- (4-(tert-butyl)phenyl)-N-((4,4,5,5-tetramethyl-1,3,2-dioxaborolan-2-yl)methyl)aniline [catalyst 1], 4-(tert-butyl)-N-(4-(tert-butyl)phenyl)-N-(2-(4,4,5,5-tetramethyl-1,3,2-dioxaborolan-2- yl)ethyl)aniline [catalyst 2], 4,4,5,5-tetramethyl-2-(((2,4,6-tri-tert-butylphenyl)thio)methyl)- 1,3,2-dioxaborolane [catalyst 3], 4,4,5,5-tetramethyl-2-(2-((2,4,6-tri-tert- butylphenyl)thio)ethyl)-1,3,2-dioxaborolane [catalyst 4], BBIT-4Me (catalyst 5) and Cu2I4BBIT- 4Me (catalyst 6).

7. The bi-phasic electrolysis cell according to any one of the preceding claims, wherein (i) the first working electrode and the second counter electrode (15) comprises graphite foil, and / or the third reference electrode (16) comprises Ag / AgCl.

8. The bi-phasic electrolysis cell according to any one of the preceding claims, wherein the first compartment (10) is arranged essentially above the second compartment (30), to allow for an essentially vertical flow of the carbon dioxide reduction product from the first to the second compartments.

9. The bi-phasic electrolysis cell according to any one of the preceding claims, further comprising an intermittent phase (40) in-between the first (10) and the second compartments (30).

10. The bi-phasic electrolysis cell according to any one of the preceding claims, wherein the first working and the second counter electrode, acting as cathode, comprises at least one organic electrocatalyst anchored to the cathode surface via a linker.

11. A method for capturing carbon dioxide by converting the carbon dioxide to a carbon dioxide reduction product in a bi-phasic electrolysis cell according to claims 1-7, comprising the steps of: (a) allowing carbon dioxide, such as from flue gas, to flow into the first compartment via the inlet; (b) applying electrical voltage to the electrodes of the electrolysis cell at a level allowing conversion of carbon dioxide to carbon dioxide reduction product in the presence of at least one organic electrocatalyst, wherein the organic electrocatalyst is dissolved in the organic phase and / or is anchored to the cathode; (c) transferring the carbon dioxide reduction product from the first to the second compartment through mechanical shaking / stirring and / or solvent extraction; thereby storing the carbon dioxide reduction product in the aqueous phase of the second compartment temporarily or for long-term purposes;wherein the carbon dioxide reduction product is a C1-2carboxylic acid or alcohol.

12. The method according to claim 11, comprising a subsequent step (d), wherein the carbon dioxide reduction product is collected from the second compartment via the product outlet, and isolated from water by distillation.

13. The method according to claim 11 or 12, wherein an electrical voltage of about - 0.8V (vs NHE) is applied to the electrodes.

14. The method according to any one of claims 11 to 13, wherein at least one electrocatalyst is regenerated after prolonged electrolysis by electrochemical oxidation at about 1.2V (vs NHE).

15. The method according to any one of claims 11 to 14, wherein the transfer of the carbon dioxide reduction product from the first to the second compartment is improved by mechanical shaking of the electrolysis cell.

16. An organic electrocatalyst, comprising an organic frustrated Lewis pair.

17. The organic electrocatalyst according to claim 16, wherein the frustrated Lewis pair is based on (i) boron, nitrogen, carbon and hydrogen, or (ii) boron, sulfur, carbon and hydrogen.

18. The organic electrocatalyst of claim 16 or 17, chosen from: (i) [catalyst type I], (ii) [catalyst type II] or (iii) benzimidazole hydrides.

19. The organic electrocatalyst of claim 18, chosen from 4-(tert-butyl)-N-(4-(tert- butyl)phenyl)-N-((4,4,5,5-tetramethyl-1,3,2-dioxaborolan-2-yl)methyl)aniline [catalyst 1], 4- (tert-butyl)-N-(4-(tert-butyl)phenyl)-N-(2-(4,4,5,5-tetramethyl-1,3,2-dioxaborolan-2- yl)ethyl)aniline [catalyst 2], 4,4,5,5-tetramethyl-2-(((2,4,6-tri-tert-butylphenyl)thio)methyl)- 1,3,2-dioxaborolane [catalyst 3], 4,4,5,5-tetramethyl-2-(2-((2,4,6-tri-tert- butylphenyl)thio)ethyl)-1,3,2-dioxaborolane [catalyst 4], BBIT-4Me (catalyst 5) and Cu2I4BBIT- 4Me (catalyst 6).

20. A method for synthesizing a metal-free organic electrocatalyst chosen from [catalyst type I], wherein n is equal to 1 or 2, or [catalyst type II], wherein X is equal to - C(CH3)3, -H, -OMe or -NH2, comprising the steps of: (a) mixing (i) bis(4-(tert-butyl)phenyl)amine [SM1] or 2,4,6-tri-tert-butylbenzenethiol [SSM1] with (ii) 2-(bromomethyl)-4,4,5,5-tetramethyl-1,3,2-dioxaborolane [SM2] or 2-(2- bromoethyl)-4,4,5,5-tetramethyl-1,3,2-dioxaborolane [SSM2]; (b) exposing the mixture of step (a) to an elevated temperature at about 70-80 ^C, in the presence of Et3N;thereby obtaining the metal-free organic electrocatalyst and HBr.

21. The method for synthesizing a metal-free organic electrocatalyst according to claim 20, obtaining any one of catalysts 1, 2, 3 or 4.

22. A method for synthesizing an organic electrocatalyst chosen from benzimidazole hydrides, comprising the steps of: (a) cyanation of terpyridine ligand (A), followed by (b) condensation with benzene 1,2-diamine in the presence of polyphosphoric acid to introduce benzimidazole units attached to terpyridine to get 6,6''-bis(1H-benzo[d]imidazol-2- yl)-2,2':6',2''-terpyridine (D); and (c) methylation of the resulting product (D) with about 6 equivalents of MeI; thereby obtaining catalyst 5 (2,2'-([2,2':6',2''-terpyridine]-6,6''-diyl)bis(1,3-dimethyl-1H- benzo[d]imidazol-3-ium; BBIT-4Me).

23. The method of claim 22, further comprising reaction of BBIT-4Me [catalyst 5] with CuI2for 24 h in methanol under N2, thereby obtaining Cu2I4BBIT-4Me [catalyst 6].

24. A cathode compartment for use in a bi-phasic electrolysis cell according to any one of claims 1-10, comprising at least one organic electrocatalyst according to claims 16-19, either in (i) solution, or (ii) wherein the electrocatalyst is anchored to the cathode surface via a pyridine linker.

25. The cathode compartment according to claim 24, wherein the cathode surface comprises pyridine modified graphite for immobilization of the catalyst Cu2I4BBIT-4Me, wherein the linker comprises at least two methylene units and a pyridine ring, for formation of methanol.

26. The cathode compartment according to claim 24, wherein the cathode surface comprises the organic catalyst BBIT-4Me, wherein the linker comprises at least one benzene ring, for formation of formic acid.

27. A production facility (2) for use in carbon dioxide capture and / or fuel production, comprising at least one bi-phasic electrolysis cell (1) according to any one of claims 1-10, wherein carbon dioxide is captured and reduced to a carbon dioxide reduction product chosen from a C1-2 carboxylic acid or alcohol.

28. The production facility of claim 27, comprising a plurality of serially connected bi- phasic electrolysis cells.

29. The production facility of claims 27-28, further comprising a cathode compartment according to claims 24-26.

30. The production facility of claims 27-29, further comprising means for controlling the production facility including the bi-phasic electrolysis cell(s).

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