Patent Application
20160102112
This application claims the benefits of the Taiwan Patent Application Serial Number 103135209, filed on Oct. 9, 2014, the subject matter of which is incorporated herein by reference.
1. Field of the Invention
The present invention relates to dinitrosyl iron complexes, a use thereof and a water splitting device using the same and, more particularly dinitrosyl iron complexes for effectively splitting water to generate hydrogen gas, a use thereof and a water splitting device using the same.
2. Description of Related Art
A growing awareness of issues to air pollution and climate change has made the search for clean and sustainable energy. Herein, fuel cells using hydrogen gas is one of the alternative energy without using carbon source. One of the current methods for generating hydrogen gas is water splitting.
To effectively split water to generate hydrogen gas at room temperature, a Pt electrode is usually used as a working electrode. Although Pt electrode has high catalytic activity for water splitting, its high cost prohibits its widespread application. Hence, heavy research is made to synthesize earth-abundant element-containing molecular catalysts for hydrogen generation from water.
The known catalysts for hydrogen generation include complexes containing Co, Ni or Mo, winch can improve the water splitting rate through electrocatalytic or photocatalytic reaction. However, these complexes have poor alkali resistance, so buffer solution has to be added into the water to adjust the pH value. Meanwhile, these molecular catalysts can not serve as the efficient catalysts for long-term generation of H2.
Therefore, it is desirable to provide a novel catalyst, which can be applied on the water splitting to effectively generate hydrogen gas.
An object of the present invention is to provide a dinitrosyl iron complex and a use thereof, wherein the dinitrosyl iron complex can efficiently catalyze water splitting to generate hydrogen.
Another object of the present invention is to provide a water splitting device, wherein the dinitrosyl iron complex of the present invention is added into the water, so that the water splitting device can efficiently split the water to generate hydrogen.
To achieve the object, the dinitrosyl iron complex of the present invention is represented by the following formula (I):
[(R1R2N(CH2)nNR3(CH2)mNR4R5)Fe(NO)2]z (I)
wherein, each R1, R2, R3, R4 and R5 is independently selected from the group consisting of H, halogen, alkyl, alkoxy, aryl, and heteroaryl; n is 2, 3 or 4; m is 2, 3, or 4; and z is −2, −1, 0, +1 or +2.
In the present invention, alkyl, alkoxy, aryl, and heteroaryl mentioned herein include both substituted and unsubstituted moieties, unless specified otherwise. Possible substituents on alkyl, alkoxy, aryl, and heteroaryl include, but are not limited to, alkyl, halogen, alkoxy, heterocyclic group or aryl.
In the present invention, “halogen” includes F, Cl, Br and I; preferably is F, Cl or Br; and more preferably is Cl or Br. The term “alkyl” refers to linear and branched alkyl; preferably, includes linear or branched. C1-20 alkyl; more preferably, includes linear or branched C1-12 alkyl; and most preferably, includes linear or branched C1-6 alkyl. Specific examples of alkyl include, but are not limited to methyl, ethyl, n-propyl, iso-propyl n-butyl, sec-butyl, iso-butyl, tert-butyl, pentyl, neo-pentyl or hexyl. The term “alkoxy” refers to a moiety that the alkyl defined in the present invention coupled with an oxygen atom; preferably includes linear or branched C1-20 alkoxy; more preferably, includes linear or branched C1-12 alkoxy; and most preferably, includes linear or branched C1-6 alkoxy. Specific examples of alkoxy include, but are not limited to, methoxy, ethoxy, n-propoxy, iso-propoxy, n-butoxy, iso-butoxy, sec-butoxy tert-butoxy pentyloxy neo-pentyloxy or hexyloxy. The term “alkenyl” refers to a linear or branched hydrocarbon moiety that contains at least one double bond; preferably, includes a linear or branched hydrocarbon moiety containing at least one double bond; more preferably, includes a linear or branched hydrocarbon C2-12 moiety containing at least one double bond; and most preferably, includes a linear or branched hydrocarbon C2-6 moiety containing at least one double bond. Specific examples of alkenyl include, but are not limited to, ethenyl, propenyl, allyl, or 1,4-butadienyl. The term “aryl” refers to a monovalent 6-carbon monocyclic, 10-carbon bicyclic, or 14-carbon tricyclic aromatic ring system. Specific examples of aryl include, but are not limited to, phenyl, naphthyl, pyrenyl, anthracenyl or phenanthryl; and preferably, the aryl is phenyl. The term “heterocyclic group” refers to a 5-8 membered monocyclic, 8-12 membered bicyclic or 11-14 membered tricyclic heteroaryl or heterocycloalkyl having at least one heteroatom which is selected from the group consisting of O, S and N. Specific examples of heterocyclic group include, but are not limited to, pyridyl, furyl, thiazolyl, imidazolyl or thienyl.
In the dinitrosyl iron complex of the present invention, each R1, R2, R3, R4 and R5 can be independently selected from the group consisting of H, halogen, alkyl, alkoxy, aryl, and heteroaryl; preferably, each R1, R2, R3, R4 and R5 is independently selected from the group consisting of H, alkyl, aryl, and pyridine; more preferably, each R1, R2, R3, R4 and R5 is independently H or alkyl; further more preferably, each R1, R2, R3, R4 and R5 is independently selected from the group consisting of H, methyl, ethyl, n-propyl, iso-propyl, n-butyl, sec-butyl, iso-butyl and tert-butyl; and most preferably, each R1, R2, R3, R4 and R5 is independently selected from the group consisting of H, methyl and ethyl.
In addition, in the dinitrosyl iron complex of the present invention, R1, R2, R3, R4 and R5 can be identical to or different from each other. Preferably, R1 and R2 are identical, and R4 and R5 are identical. More preferably, all R1, R2, R3, R4 and R5 are identical substituents. Further more preferably, all R1, R2, R3, R4 and R5 are identical substituents, and are H, methyl, ethyl, n-propyl, iso-propyl, n-butyl, sec-butyl, iso-butyl or tert-butyl. Most preferably, all R1, R2, R3, R4 and R5 are identical substituents, and are H, methyl or ethyl.
Furthermore, in the dinitrosyl iron complex of the present invention, n and m can be identical to or different from each other, and are integers between 2 and 4. Preferably, n and m are the same integers between 2 and 4. More preferably, both n and m are 2.
In addition, in the dinitrosyl iron complex of the present invention, z can be −2, −1, 0, +1 or +2. Preferably, z is −1, 0 or +1. More preferably, z is 0 or +1.
In the dinitrosyl iron complex of the present invention, the dinitrosyl iron complex represented by the formula (I) can be the dinitrosyl iron complex represented by the following formula (II) or (III), and preferably the dinitrosyl iron complex represented by the following formula (III):
wherein the definitions of R1, R2, R3, R4 and R5 are the same as those illustrated above.
In addition, the present invention further provides a use of the aforementioned dinitrosyl iron complex for splitting water to generate hydrogen.
Furthermore, the present invention further provides a water splitting device using the aforementioned dinitrosyl iron complex, which comprises: a container; water disposed in the container, wherein the aforementioned dinitrosyl iron complex is added into the water; a first electrode, disposed in the container and immersed in the water; and a second electrode, disposed in the container, immersed in the water and opposite to the first electrode.
In the present invention, the term “water” refers to pure water or any other aqueous solution. Specific examples thereof include, but are not limited to pure water or sea water. Especially when the water is sea water, splitting the sea water can generate not only hydrogen but also chlorine due to the sea water containing chloride ions.
Co, Ni and Mo complexes are usually used to catalyze water splitting to generate hydrogen for those devices using hydrogen such as fuel cells. However, the alkali resistances of the Co, Ni and Mo complexes are not good enough. In addition, the water splitting has to be performed in the presence of organic solvents when using the Co, Ni and Mo complexes as catalysts. In order to improve the limitations of the water splitting using the Co, Ni and Mo complexes as the catalyst, the present invention provides a novel dinitrosyl iron complex having high alkali resistance to replace the conventional Co, Ni and Mo complexes. When the dinitrosyl iron complex of the present invention is applied to the water splitting process and device, it can efficiently catalyze the water splitting, and no acids and organic solvents have to be added. In addition, the dinitrosyl iron complex of the present invention has high alkali resistance, and thus the expensive Pt electrode can be replaced with the cheap glass-carbon electrode as the working electrode. Meanwhile, if the dinitrosyl iron complex of the present invention is used to catalyze the sea water splitting, another benefit is that chlorine can also be simultaneously produced.
Other objects, advantages, and novel features of the invention will become more apparent from the following detailed description when taken in conjunction with the accompanying drawings.
The present invention has been described in an illustrative manner, and it is to be understood that the terminology used is intended to be in the nature of description rather than of limitation. Many modifications and variations of the present invention are possible in light of the above teachings. Therefore, it is to be understood that within the scope of the appended claims, the invention may be practiced otherwise than as specifically described.
Compounds [Na][NO2] (10.0 mmol, (1690 g) and 18-crown-6-ether (10.0 mmol, 2.643 g) were dissolved in THF in the 50 mL Schlenk flask, and the commercial [Fe(CO)5] (10.0 mmol, 1.348 mL) was added into the THF mixture solution at 0° C. The resulting solution was stirred at ambient temperature overnight. The reaction was monitored with FTIR. IR spectrum (IR 1983 m, 1877 s (νCO), 1647 m (νNO) cm−1 (THF)) was assigned to the formation of [Na-18-crown-6-ether][Fe(CO)3(NO)]. Then, hexane was added to precipitate the yellow solid [Na-18-crown-6-ether][Fe(CO)3(NO)] (3.885 g, 85%). Compounds [Na-18-crown-6-ether][Fe(CO)3(NO)] (2.0 mmol, 0.914 g) and [NO][BF4] (2.0 mmol, 0.234 were loaded into 25 mL Schlenk flask, and 20 mL of THF was added at 0° C. The resulting solution was stirred about 30 min at 0° C. and IR spectrum (IR 2088 s, 2037 s (νCO), 1808 s, 1760 s (νNO) cm−1 (THF)) was assigned to the formation of [Fe(CO)2(NO)2].
THF solution (20 mL) of Fe(CO)2(NO)2 (˜1.0 mmol) and pentamethyldiethylenetriamine (PMDTA) (1.0 mmol, 0.11 mL) were reacted for 4 hr at ambient temperature, followed by adding hexane into the reaction solution to precipitate the brown solid [(CH3)2N(CH2)2NCH3(CH2)2N(CH3)2)Fe(NO)2]0 represented by the formula (I-1).
In addition, THF solution (20 mL) of Fe(CO)2(NO)2 (˜1.0 mmol) and diethylenetriamine (DTA) (1.0 mmol, 0.21 mL) were also reacted for 4 hr at ambient temperature, followed by adding hexane into the reaction solution to precipitate the brown solid [H2N(CH2)2NH(CH2)2NH2)Fe(NO)2] represented by the formula (I-2).
Each crystal was mounted on a glass fiber and quickly coated with an epoxy resin. Unit-cell parameters were obtained by least-squares refinement. Herein, diffraction measurements for complexes (I-1) and (I-2) were carried out on a Bruker Kappa Apex DUO diffractometer with graphite-monochromated Mo Kα radiation (λ=0.7107 Å). Least-squares refinement of the positional and anisotropic thermal parameters of all non-H atoms and fixed H atoms was based on F2. A SADABS absorption correction was made. The SHELXTL structural refinement program was employed. The single-crystal X-ray structure of the dinitrosyl iron complex (I-2) is shown in
Herein, cyclic voltammetry was performed to obtain the reduction-oxidation reactivity of the complexes (I-1) and (I-2) toward water. Electrochemical measurements were performed with a CHI model 621b potentiostat (CH Instrument) instrumentation. Cyclic voltammograms were obtained from 2.0 mM analyte concentration in O2-free MeCN using 0.1 M [n-Bu4N][PF6] as the supporting electrolyte. The potential was measured at 298 K vs a Ag/AgNO3 reference electrode by using a glassy carbon working electrode (surface area=(0.0707 cm2) and a platinum wire auxiliary electrode at a scan rate of 0.05 V/s. The results indicate that, when 2 mM of the complexes (I-1) and (I-2) in MeCN reacted with 0.1 M [n-Bu4N][PF6], the reversible electrochemical interconversion occurs at E1/2=−0.92 V and −0.81 V (versus Fc/Fc+) respectively. In addition, infrared spectroscopy was also performed on complexes of (I-1) and (I-2). Infrared spectra of the νNO stretching frequencies were recorded on a PerkinElmer model Spectrum One B spectrometer with sealed solution cells (0.1 mm, CaF2 windows) or KBr. The results indicate that, in THF, IR νNO frequencies of 1697, 1643 cm−1 are exhibited by the complex (I-1), compared to 1686, 1634 cm−1 exhibited by the complex (I-2). The IR spectra of the complexes (I-1) and (I-2) are shown in
Upon addition of one equiv of [NO][BF4] to the CH3CN solution of the complex (I-1), IR νNO frequencies shifting from (1697, 1643 cm−1) shown in
In addition, upon addition of one equiv of [NO][BF4] to the CH3CN solution of the complex (I-2), IR νNO frequencies shifting from (1686, 1634 cm−1) shown in
Hereinafter, the obtained complexes (I-3) and (I-4) were used to perform water splitting reaction.
0.1 M KCl aqueous solution, 0.1 M Na2SO4 aqueous solution or sea water as a proton provider was respectively placed into containers. A glassy carbon electrode as a working electrode and a Pt electrode as an glassy auxiliary electrode were immersed into the container. In addition, the complexes (I-3) and (I-4) were also added into the KCl aqueous solution, Na2SO4 aqueous solution or the sea water for water splitting. Then, voltage was provided onto the working electrode and the auxiliary electrode to perform the water splitting reaction.
Compared to the high potential of −1.04 V for direct reduction of water using glassy carbon as working electrode, aerobic aqueous solution of 1 mM of the complex (I-3) with 0.1 M KCl electrolyte exhibits a reduction response as a tail rising up from −0.63 V (versus standard hydrogen electrode (SHE) as a reference electrode) in addition to the reversible redox peaks at E1/2=−0.34 V (vs SHE). This sharp increase in current indicates the catalytic reduction of 0.1 M KCl aerobic aqueous solution to afford H2 in the presence of 1 mM of the complex (I-3), as evidenced by GC analysis of gas samples in the headspace.
Herein, saturated calomel electrode (SCE) was used as a reference electrode, a glassy carbon electrode (area=0.0707 cm2) was used as a working electrode, and cyclic voltammetry was performed to obtain the oxidation-reduction potential of 0.1 M Na2SO4 aqueous solution (or 0.1 M KCl aqueous solution) in the presence (1 mM) and absence (0 mM) of the complex (I-4), at a scan rate of 0.1 Vs (or 0.05 V/s). The results are shown in
In addition,
Furthermore, to expand from a reactive inorganic complex toward water reduction, the catalytic efficacy of the complex (I-3) for H2-generation was evaluated by controlled potential electrolysis (CPE). Considering the practical application, CPE experiment was conducted in the absence of buffer reagents, while 0.1 M Na2SO4 was added as electrolyte to minimize internal resistance.
The catalytic turnover frequency for H2-generation by adding 1 mM of complex (I-3) into 3.0 M KCl aqueous solution (25 mL), on a glassy carbon electrode (A=0.0707 cm2), is 3.76 moles (current density 71.28 mA/cm2) under the controlled potential electrolysis (CPE) experiment using an applying potential of −1.2 V (vs. SHE) for 14 hours. That is 52.64 moles of H2 is produced per mole of the complex (I-3) using −1.2 V overpotential at pH 7 for 14 hours.
In a similar fashion, the complex (I-3) exhibits steady seawater (Taiwan strait) reduction to produce H2, under the controlled potential electrolysis (CPE) experiment using an applying potential of −1.25 V (vs. SHE) for 136 hours, with a turnover number of 650.78 (that is 650.78 moles H2 produced per mole of the complex (I-3)) and current density 90.71 mA/cm2 (on a glassy carbon electrode (A=0.0707 cm2)). That is, 325.39 moles of H2 is produced per mole of the complex (I-3) using −1.25 V overpotential for 136 hours. These results indicate that the dinitrosyl iron complexes of the present invention indeed can be used to split sea water to generate hydrogen gas, and the catalytic property thereof can be maintained after long term operation. Furthermore, chlorine gas was also generated at the auxiliary electrode when sea water was oxidized.
According to the aforementioned results, the dinitrosyl iron complexes of the present invention can be used as a catalyst to generate hydrogen gas effectively. Even though a glassy carbon electrode is used as a working electrode for water splitting, the effect for generating hydrogen gas still can be maintained. In addition, when the dinitrosyl iron complexes of the present invention are used to split sea water or an aqueous solution containing chloride ions, not only hydrogen gas but also chlorine gas can be obtained at the same time. Furthermore, even though the dinitrosyl iron complexes of the present invention are used for a long time, the catalytic activity thereof is still maintained, and the complexes can split water steadily. Herein, the electrocatalytic mechanism of water splitting promoted by the dinitrosyl iron complexes of the present invention is described in the following Scheme I.
In addition,
Although the present invention has been explained in relation to its preferred embodiment, it is to be understood that many other possible modifications and variations can be made without departing from the spirit and scope of the invention as hereinafter claimed.
| Number | Date | Country | Kind |
|---|---|---|---|
| 103135209 | Oct 2014 | TW | national |
