PROCESS FOR PREPARATION OF METAL OXIDES NANOCRVSTALS AND THEIR USE FOR WATER OXIDATION

Abstract

The present application refers to a process for preparing of nanostructured metal oxides such as cobalt oxide and transition metal incorporated cobalt oxides and nickel aluminium oxides and nickel metal supported on aluminium oxide using plant material such as spent tea leaves as a hard template and the use of such catalysts for water oxidation.

Claims

1. Process for preparing a nanostructured metal oxide, said process comprising the steps of: a) impregnating a solid plant material derived from plant leaves which are optionally broken with the solution of at least one metal salt to yield impregnated plant material; b) drying the obtained impregnated plant material; c) subjecting the impregnated plant material to a high temperature treatment in the range of 150 to 400 C. under an oxygen containing atmosphere whereby the at least one metal salt is converted into the respective metal oxide; d) subjecting the impregnated plant material to a further high temperature treatment in the range of 400 to 1000 C. whereby the plant material is removed to yield nanostructured metal oxide; and e) cooling down the obtained nanostructured metal oxide to room temperature.

2. Process according to claim 1, wherein the solid plant material derived from plant leaves is derived from tea leaves, preferably spent tea leaves.

3. Process according to claim 2, wherein the tea leaves have been pretreated before use by extraction with a solvent until no soluble components are extracted by the solvent.

4. Process according to claim 1, wherein the plant material is impregnated with an aqueous solution of the at least one metal salt.

5. Process according to claim 1, wherein the at least one metal salt is a catalytically active metal salt of a metal selected from the group consisting of Ti, V, Cr, Mn, Fe, Co, Ni, Cu, Zn, Al, Mo, Se, Sn, Pt, Ru, Pd, W, Ir, Os, Rh, Nb, Ta, Pb, Bi, Au, Ag, Sc, Y, Bi, Sb, and mixtures thereof.

6. Process according to claim 1, wherein the drying step b) and the high temperature treatment step c) are carried out as a one-step treatment by increasing the temperature at a ramping rate sufficient to dry the impregnated material before the at least one metal salt is completely converted into the respective metal oxide.

7. Process according to claim 1, wherein the high temperature treatment steps c) and d) are carried out as a one-step treatment at a ramping rate allowing the conversion of the metal salt to the metal oxide to be completed before the combustion of the plant material.

8. Process according to claim 1, wherein the product obtained in step d) is subjected to a treatment with a diluted acid and subsequently washed with water.

9. Process according to claim 1, wherein the obtained nanostructured metal oxide or oxides which may be partially reduced to the metal, is selected from Al.sub.2O.sub.3, NiO/Al.sub.2O.sub.3, Co.sub.3O.sub.4, transition metal (Cu, Ni, Fe, Mn) incorporated cobalt oxides, CoO and Co/CoO.

10. Process according to claim 1, wherein the product obtained in step d) or e) is subjected to a post treatment with a reducing agent.

11. Nanostructured metal oxide obtained by the process of claim 1.

12. A process comprising conducting a catalyzed chemical reaction in the presence of a catalyst, wherein the catalyst or a carrier for a metal catalytically active in the chemical reaction is the nanostructured metal oxide according to claim 11.

13. A process comprising oxidizing water in the presence of a catalyst, wherein the catalyst is the nanostructured metal oxide according to claim 11.

14. Process for enhancing the activity of a nanostructured metal oxide as electrocatalyst for water oxidation, said process comprising subjecting a nanostructured metal oxide according to claim 11 to a cyclic voltammetry in an alkaline electrolyte.

15. Process according to claim 14, wherein the nanostructured metal oxide is a NiCo based nanostructured metal oxide electrocatalyst.

Description

[0030] In the Figures, the following is illustrated:

[0031] FIG. 1. TEM images of STL templated Co.sub.3O.sub.4 and Cu, Ni, Fe, Mn incorporated mixed oxides.

[0032] FIG. 2. SEM images (a, b), cross-section SEM image (c) and HRTEM image (d) of STL templated NiCo.sub.3O.sub.4.

[0033] FIG. 3. Wide angle XRD patterns of STL templated Co.sub.3O.sub.4 and Cu, Ni, Fe, Mn incorporated mixed oxides.

[0034] FIG. 4. N.sub.2-sorption isotherms (a) and pore size distribution (b) of STL-templated Co.sub.3O.sub.4 and mixed oxides. The isotherms are plotted with an offset of 30 cm.sup.3/g.

[0035] FIG. 5. TEM images of STL-templated Co.sub.3O.sub.4 prepared using the large scale synthesis (60 g dried leaves, 750 mL water, 30 g of cobalt nitrate hexahydrate).

[0036] FIG. 6. TEM images of templated Co.sub.3O.sub.4 prepared from various commercial tea species. (a, b) Chinese green tea; (c, d) Westcliff Pfefferminze (peppermint tea); (e, f) Westcliff Salbei (herbal tea); (g, h) Westcliff Earl Grey (black tea) and (i, j) Westcliff Melisse (herbal tea). The values of the measured BET surface areas are shown in the figures.

[0037] FIG. 7. Thermogravimetric analysis of pre-treated tea leaves.

[0038] FIG. 8. XRD patterns and TEM images of CoO (a,c) and Co/CoO composite material (b,d) prepared by reduction of Co.sub.3O.sub.4 under different atmospheres.

[0039] FIG. 9. TEM images of as-prepared NiAl oxide (a,b) and samples obtained after reduction at 300 C. for 2 h (c,d), 500 C. for 4 h (e,f) and 900 C. for 4 h (g,h).

[0040] FIG. 10. XRD patterns of obtained materials after NiAl oxide being reduced at various temperatures.

[0041] FIG. 11. N.sub.2 sorption isotherms of obtained materials after NiAl oxide being reduced at various temperatures. The isotherms are plotted with an offset of 100 cm.sup.3/g.

[0042] FIG. 12. TEM image (a) and oxygen evolution linear scan (b) of Co.sub.3O.sub.4 obtained from direct thermal decomposition of cobalt nitrate hexahydrate. The linear scan of STL-tem plated Co.sub.3O.sub.4 is shown for comparison as the black trace.

[0043] FIG. 13. a) Initial oxygen evolution linear scans, b) Tafel plots and c) Cyclic voltammetry curves of tea leave-templated Co.sub.3O.sub.4 and Cu, Ni, Fe, Mn incorporated mixed oxides in 1 M KOH electrolyte (catalyst loading 0.12 mg/cm.sup.2).

[0044] FIG. 14. a) Stabilized oxygen evolution linear scans of tea leaf-templated Co.sub.3O.sub.4 and Cu, Ni, Fe, Mn incorporated mixed oxides in 1 M KOH electrolyte (catalyst loading 0.12 mg/cm.sup.2) after CV measurements. b) Detailed linear scan comparison of NiCo.sub.3O.sub.4 (before and after activity) with pristine Co.sub.3O.sub.4. c) Tafel plots derived from FIGS. 5c and d) Controlled-current electrolysis of activated NiCo.sub.3O.sub.4 by applying a current density of 10 mA/cm.sup.2 for 12 h.

[0045] FIG. 15. Illustrated formation process of metal oxide nanocrystals templated from spent tea leaves (STL).

EXPERIMENTAL SECTION

Material Characterization:

[0046] All of the chemicals and reagents were purchased from Sigma Aldrich and used without further purification. Wide angle XRD patterns collected at room temperature were recorded on a Stoe theta/theta diffractometer in Bragg-Brentano geometry (Cu K1/2 radiation). The measured patterns were evaluated qualitatively by comparison with entries from the ICDD-PDF-2 powder pattern database or with calculated patterns using literature structure data. TEM images of samples were obtained with an H-7100 electron microscope (100 kV) from Hitachi. EDX spectroscopy was conducted on Hitachi S-3500N. The microscope is equipped with a Si(Li) Pentafet Plus-Detector from Texas Instruments. HR-TEM and SEM images were taken on HF-2000 and Hitachi S-5500, respectively. Samples for cross section images were prepared on 400 mesh Au-grids in the following way: 1. Two-step embedding of the sample in Spurr resin (hard mixture). 2. Trimming with LEICA EM TRIM. 3. Sectioning with a 35 diamond-knife at a REICHERT ULTRA-CUT microtome. 4. Transferring from the water surface area on a lacey-film/400 mesh Au-grid. N.sub.2-sorption isotherms were measured with an ASAP 2010 adsorption analyser (Micrometrics) at 77 K. Prior to the measurements, the samples were degassed at 150 C. for 10 h. Total pore volumes were determined using the adsorbed volume at a relative pressure of 0.97. BET surface areas were determined from the relative pressure range between 0.06 and 0.2. Pore size distribution curves were calculated by the BJH method from the desorption branch.

Synthesis of Tea Leaf-Templated Co.sub.3O.sub.4 and Transition Metal Doped Co.sub.3O.sub.4:

[0047] The tea leaves (Goran Mevlana, Ceylon Pure Leaf Tee) were first treated in a Soxhlet extractor with boiled water for 48 hours and then dried at 90 C. before being used as templates. Alternatively, the spent tea leaves could be used directly without any treatment. In a typical templating process, the aqueous solution of metal salt precursors was added to the treated tea leaves and the mixing was conducted at room temperature for 2 h. The weight ratio of tea to metal salt was 2 to 1 throughout this experiment. Afterwards, the mixture was dried at 60 C. and the obtained solid was calcined at 550 C. for 4 h with a ramping rate of 2 C./min. Finally the product was obtained after being washed with 0.1 M HCl solution and cleaned with deionized water.

[0048] In the large scale synthesis of Co.sub.3O.sub.4, the tea leaves were first cleaned using hot water until no color was visible in the tea water. After drying, 60 g of dried tea leaves were used as the templates. To make the cobalt precursor solution, 30 g of cobalt nitrate hexahydrate were dissolved in 750 mL deionized water. Then the solution was added to the tea leaves and the mixing was conducted using gentle stirring for 2 h. Afterwards the mixture was heated at 70 C. until the water was completely evaporated. In the final step, the cobalt loaded tea leaves were calcined and the obtained solids were cleaned following the same procedure.

[0049] The same synthesis protocol was also applied to the following commercial tea leaves without variation on the experimental conditions: Chinese green tea, Westcliff Pfefferminze (peppermint tea), Westcliff Salbei (herbal tea), Westcliff Earl Grey (black tea) and Westcliff Melisse (herbal tea).

Synthesis of Tea Leaf-Templated CoO and Co/CoO Composite Materials:

[0050] Pure phase nanostructured CoO was obtained by reducing Co.sub.3O.sub.4 under ethanol/argon flow (100 mL/min). In detail, N.sub.2 was purged from the bottom of a round-bottom flask contains 200 mL absolute ethanol and the flow was further directed to a tube furnace. The reaction was completed in 4 h at 270 C. The Co/CoO composite material was prepared by reducing Co.sub.3O.sub.4 with 5% H.sub.2/argon flow (100 ml/min) at 300 C. for 4 h. The sample was then slowly oxidized in 1% O.sub.2/argon atmosphere.

Synthesis of Tea Leave Templated Al.sub.2O.sub.3:

[0051] 2 g of treated tea leave are impregnated with 1 g of Al(NO.sub.3).sub.3.6H.sub.2O. After drying at 60 C. overnight, the solid mixture is calcined at 550 C. for 4 h (ramping rate 2 K/min). Finally the sample is washed with 0.1 M HCl solution and cleaned with water.

Synthesis of Tea Leaves Templated NiAl Oxide:

[0052] 2 g of treated tea leave are impregnated with 0.5 g of Al(NO.sub.3).sub.3.6H.sub.2O and 0.5 g of Ni(NO.sub.3).sub.2.6H.sub.2O. After drying at 60 C. overnight, the solid mixture is calcined at 550 C. for 4 h (ramping rate 2 K/min). Finally the sample is washed with 0.1 M HCl solution and cleaned with water.

Reduction Procedure of NiAl Oxide:

[0053] Synthesized NiAl oxide was treated by 5% H.sub.2/argon flow (100 ml/min) at temperatures of 300 C. for 2 h, 500 C. for 4 h, 900 C. for 4 h with a ramping rate of 2 C./min.

Electrochemical Measurements:

[0054] Electrochemical water oxidation measurements were carried out in a three-electrode configuration (Model: AFMSRCE, PINE Research Instrumentation) with a hydrogen reference electrode (HydroFlex, Gaskatel) and Pt wire as counter electrode. 1 M KOH was used as the electrolyte and argon was purged through the cell to remove oxygen before each experiment. The temperature of the cell was kept at 298 K by a water circulation system. Working electrodes were fabricated by depositing target materials onto glassy carbon (GC) electrodes (5 mm in diameter, 0.196 cm.sup.2 surface area). The surface of the GC electrodes was polished with Al.sub.2O.sub.3 suspension (5 and 0.25 m, Allied High Tech Products, INC.) before use. 4.8 mg catalyst was dispersed in a mixed solution of 0.75 ml H.sub.2O, 0.25 ml isopropanol and 50 L Nafion (5% in a mixture of water and alcohol) as the binding agent. Then the suspension was sonicated for 30 min to form a homogeneous ink. After that, 5.25 L of catalyst ink was dropped on GC electrode and then dried under light irradiation. The catalyst loading was calculated to be 0.12 mg/cm.sup.2 in all cases. All linear scans were collected in a rotating disc electrode configuration by sweeping the potential from 0.7 V to 1.7 V vs. RHE with a rate of 10 mV/s and rotation of 2000 rpm. Cyclic voltammetry measurements were carried out in the potential range between 0.7-1.6 V vs RHE with a scan rate of 50 mV/s. The nickel containing electrocatalysts were activated by conducting long-term CV measurements until the linear scan was stabilized. In all measurements, the IR drop was compensated at 85%. Stability tests were carried out by controlled current electrolysis in 1 M KOH electrolyte where the potential was recorded at 10 mA/cm.sup.2 over a time period of 12 h. The reproducibility of the electrochemical data was checked on multiple electrodes.

Results and Discussion

[0055] Herein, the utilization of spent tea leaves (STL) as hard templates to prepare cobalt oxide and mixed oxide nanocrystal is presented. The morphology of the as-prepared STL-templated oxides after calcination was first characterized using electron microscopy. As seen from the low magnification TEM images (FIG. 1), all samples exhibit a unique nanostructure which consists of nano-sized crystallites. After calcination, the obtained nanoparticles of metal oxides are sintered in all cases and that results in a sheet-like nanostructure. This was further supported by SEM investigation of the morphology of NiCo.sub.3O.sub.4 (FIGS. 2a and b). One can clearly see well-packed nanoparticles that are connected to form a sheet-like nanostructure with a domain size of few hundred nanometers. The size of the particles are in the range of 1015 nm. The sintering of particles is also shown in the cross-section image (FIG. 2c). Moreover, the high resolution TEM image of NiCo.sub.3O.sub.4 (FIG. 2d) displays distinct atomic planes in various directions, indicating a high degree of poly-crystallinity.

[0056] The crystal structure of the as-prepared Co.sub.3O.sub.4 and mixed oxides was then examined using wide-angle X-ray diffraction and the patterns are shown in FIG. 3. As seen, tea leaf-templated cobalt oxide showed distinct reflections at 31.2, 36.7, 38.4, 44.7, 55.6, 59.2 and 65.2 2 theta values. This can be assigned to spinel structure of Co.sub.3O.sub.4 with cobalt atoms located at both tetrahedral and octahedral centers. Once the second transition metal species were introduced into the oxides, the XRD patterns displayed characteristic reflections at same positions as pure cobalt oxide, indicating the cobalt atoms in the spinel structure were successfully substituted by incorporated metal cations without forming additional phases was formed. However, the substituted cobalt sites vary depending on the incorporated metal species. According to the literature, in Ni and CuCo.sub.3O.sub.4, the tetrahedrally coordinated Co.sup.2+ is substituted by Cu.sup.2+, while in Fe and Mn incorporated Co.sub.3O.sub.4, the octahedrally coordinated Co.sup.3+ is substituted. Moreover, the broadness of the reflection peaks suggests the nano-crystallinity of all samples although the average crystal size for obtained oxides was different. As calculated using the Scherrer equation, the average crystal size of pure Co.sub.3O.sub.4 was 13 nm and the value for Cu, Ni, Fe and Mn incorporated Co.sub.3O.sub.4 were determined to be 15, 12, 9 and 8 nm respectively. In the case of NiCo.sub.3O.sub.4, the calculated particle size was in good agreement with the electron microscopic investigation (FIGS. 1 and 2).

[0057] In order to confirm the successful incorporation of the second metal species, elemental analysis was conducted to gain information on the material composition as well as the possible residues that can be left from the tea leaves. Besides carbon, tea leaves contain other elements such as Ca, Mg, Na, Al, S, P, Mn and their elemental composition might vary depending on the type and nature of the tea..sup.48 After the calcination of tea/metal precursor composites, one should note that the treatment of the calcined materials with diluted HCl is necessary in the inventor's case since a small amount of CaCO.sub.3 was present after calcination at 500 C. Table S1 shows the elemental analysis results of the HCl treated Co.sub.3O.sub.4 and mixed oxides that were conducted using energy dispersive spectroscopy in a scanning electron microscope.

TABLE-US-00001 CuCo.sub.3O.sub.4 NiCo.sub.3O.sub.4 FeCo.sub.3O.sub.4 MnCo.sub.3O.sub.4 Element Atom % Element Atom % Element Atom % Element Atom % O 59.64 O 57.80 O 58.95 O 61.19 Mg 0.49 P 0.19 Mg 0.49 Mg 0.49 Al 0.69 Al 0.73 Al 0.70 Al 0.69 Si 0.17 Si 0.24 Si 0.15 Si 0.22 S 0.17 S 0.19 S 0.25 S 0.10 Ca 0.35 Ca 0.46 Ca 0.84 Ca 0.55 Mn 0.12 Mn 0.09 Mn 0.11 Cu 0.1 Co 36.53 Co 36.01 Co 34.33 Co 31.90 Cu 1.84 Ni 4.29 Fe 3.84 Mn 4.56

[0058] Although residues such as Al, S, P, Mg and Ca were detected in the final products, the total atomic ratio was lower than 3%. More importantly, the relative ratio of the incorporated transition metal cations to the cobalt cations matched well with the expected value (1/8) except in the case of Cu, where a relative ratio of 1/20 was obtained instead. This is due to the reason that a small amount of CuO phase was formed during calcination. Since HCl solution dissolves CuO in the cleaning step, the copper content in the sample is significantly lower. The textural parameters of the templated metal oxides were further determined using N.sub.2 sorption measurements and the isotherms are depicted in FIG. 4a. As presented, all materials show type IV isotherms which are characteristic for mesoporous materials. The calculated BET surface area of Co.sub.3O.sub.4 and the mixed oxides shows clear correlation with the crystal size calculated from XRD patterns as MnCo.sub.3O.sub.4 showed the highest BET surface area of 63 m.sup.2/g, nearly doubled that of pure cobalt oxide (34 m.sup.2/g) and Cu doped counterpart (35 m.sup.2/g). Ni and Fe incorporated cobalt oxide have BET surface areas of 40 m.sup.2/g and 53 m.sup.2/g respectively. The pore size distribution as determined from the desorption branches of isotherms are plotted in FIG. 4b. As shown, all samples possess pores with the size between 3 and 4 nm. This can be attributed to the space between neighboring nanocrystals.

[0059] Moreover, this preparation method can be easily scaled up and Co.sub.3O.sub.4 with the same morphology (FIG. 5) and textural parameters was acquired when 60 g of tea leaves were used as the templates. More than 8 g of Co.sub.3O.sub.4 with the BET surface area of 40 m.sup.2/g was obtained as the final product. In order to investigate the applicability of the synthesis protocol, 5 other commercially available tea species (refer to experimental for details) were selected and used as hard templates. As can be seen from FIG. 6, Co.sub.3O.sub.4 as the final product in all cases shows similar nanostructure with distinguishable nanocrystals. The measured BET surface areas for these samples are in the range of 6090 m.sup.2/g, depending on the tea species.

[0060] The data presented above suggest the successful replication of mixed transition metal oxides using spent tea leaves as the hard template. The formation of such nanostructures is illustrated in FIG. 15. The tea leaves were first intensively treated in boiled water. Afterwards, the transition metal precursors were impregnated on treated tea leaves (SEM image shown in FIG. 15) using water as the solvent. Upon immersion into the water, the leaves tend to swell and accommodate the metal precursors. Besides, due to the pretreatment process, additional porosity is likely to be created that is beneficial for the absorption of metal cations due to the release of organic compounds. Once the water is evaporated, calcination is applied to obtain crystalline oxides and meanwhile remove the template. By considering the results from electron microscopy studies, the inventors propose that the nanoparticles are first formed on STL from the thermal decomposition of metal precursors. Due to the role of the substrate, the particles were well-packed and the sheet-like nanostructure was already present at the first stage. Afterwards, the tea leaves, which mostly consist of carbon, were combusted at higher temperatures and thus the nanostructured of metal oxides was maintained. One key aspect concerning this process is that the decomposition temperature of the metal nitrates has to be higher than combustion temperature of tea leaves. Otherwise the hard template (STL in this case) will vanish prior to the formation of metal oxides and this will lead to the formation of larger particles. Therefore, the combustion temperature of the tea leaves was checked using thermogravimetric analysis. As shown in FIG. 7, no clear weight loss was observed at temperatures lower than 260 C. Since the decomposition temperature of metal nitrates was reported to be lower, the inventors could be confident that the formation of interconnected nanoparticles already took place before the removal of tea template at higher calcination temperatures.

[0061] The transformation of Co.sub.3O.sub.4 to pure phase CoO and Co/CoO composite was also performed by reduction under ethanol/Ar and 5% H.sub.2/Ar flow. The crystalline phases were characterized by XRD and the TEM images show that the nanostructure of the starting Co.sub.3O.sub.4 was preserved through the reduction process (FIG. 8). Furthermore, this method can be applied to prepare NiO/Al.sub.2O.sub.3 and, when the materials is treated with H.sub.2 at different temperatures, mixture of NiO/Ni and pure metallic Ni nanoparticle supported on Al.sub.2O.sub.3 could be prepared.

[0062] As can be observed, the as-prepared NiAl mixed oxide shows NiO phase and aggregated nanoparticles can be seen from the TEM images (FIG. 9a, b). After reduction at 300 C. for 2 h, the XRD pattern (FIG. 10) did not show any change, suggesting the reduction condition is not sufficient to obtained metallic Ni. When the reduction temperature was increased to 500 C., after 4 h a mixed phase of NiO and metallic Ni was observed from the XRD pattern. It is worth pointing out that the broad reflection of metallic Ni indicates crystallites in nano size and it is difficult to see from the TEM images (FIG. 9e, f). However, when the mixed oxide was reduced at even higher temperature (900 C. for 4 h), the reflection of Ni became much sharper and particles in the size of 520 nm can be observed clearly from TEM images (FIG. 9g, h).

[0063] The BET surface areas of Ni Al mixed oxides reduced at different temperatures are measured by N.sub.2 sorption. The isotherms are shown in FIG. 11. As calculated, the BET surface areas are around 100 m.sup.2/g for samples reduced at 300 C. and 500 C. while a lower surface area of 38 m.sup.2/g was measured when the mixed oxide was reduced at 900 C. for 4 h.

Electrocatalyst Test

[0064] In order to indicate the application of prepared nanocrystals, the materials were tested as electrocatalysts for water oxidation. The catalytic activity towards electrochemical water oxidation was then evaluated following the benchmark protocol proposed by Jaramillo's group. The measurements were carried out in a three-electrode configuration and the catalyst was dropcast onto the glassy carbon electrode with a loading of 0.12 mg/cm.sup.2 in all cases. The comparison was first made between STL templated Co.sub.3O.sub.4 and bulk Co.sub.3O.sub.4 which was obtained from the direct thermal decomposition of Co(NO.sub.3).sub.2.6H.sub.2O. As shown in FIG. 12, direct calcination of cobalt precursor resulted in Co.sub.3O.sub.4 with a particle size of 6080 nm. In terms of water oxidation activity, although a similar onset potential was shown in both samples, STL templated Co.sub.3O.sub.4 exhibited higher current density and lower Tafel slopes than its bulk counterpart. This clearly demonstrates the advantage of using STL as the template. FIG. 13a depicts the initial linear sweep voltammetry (LSV) curves of Co.sub.3O.sub.4 and mixed oxides collected in 1 M KOH electrolyte. As shown, the influence of transition metal cations on the OER activity of cobalt oxide was clearly present, as Mn showed detrimental effect while Cu, Ni and Fe doped ones exhibited enhanced activity over pristine Co.sub.3O.sub.4 to similar extent. To reach a current density of 10 mA/cm.sup.2, pure Co.sub.3O.sub.4 requires an overpotential of 401 mV, which is comparable to the benchmarked nanoparticulate water oxidation catalyst. In comparison, the overpotential negatively shifted to 382 mV for Cu(Ni)Co.sub.3O.sub.4 and 378 mV for FeCo.sub.3O.sub.4 respectively, indicating enhanced water oxidation activity and this matches well with the inventor's previous study on ordered mesoporous materials and other research work conducted on transition metal oxides. The OER kinetics were investigated and the Tafel plots of as-made catalyst are depicted in FIG. 13b. As calculated, the highest Tafel slope was 63 mV/dec in the case of MnCo.sub.3O.sub.4, indicating relatively sluggish OER kinetics. Pure Co.sub.3O.sub.4 and other mixed oxides showed Tafel slopes in the range of 4553 mV/dec, being in good agreement with values obtained from cobalt-based nanoparticulate OER catalysts. The cyclic voltammetry curves of as-made catalyst in 1 M KOH were also collected. As shown in FIG. 13c, all samples exhibit one redox couple with a broad anodic peak prior to the onset of water oxidation reaction. This is correlated with the formation of oxyhydroxide species and oxidation of Co(III) to Co(IV). As shown, Mn-doped Co.sub.3O.sub.4 showed much lower oxidation current compared with others, indicating that the oxidation of cobalt cations to higher valence was strongly inhibited by the addition of Mn cations despite the highest BET surface area. On the contrary, the oxidation peak of FeCo.sub.3O.sub.4 and NiCo.sub.3O.sub.4 was significantly larger than that of Co.sub.3O.sub.4, suggesting higher population of active sites and this can be related with relatively higher surface area. However, the enhanced OER activity should not be fully correlated with this factor as the CV curve of CuCo.sub.3O.sub.4 showed nearly identical shape as Co.sub.3O.sub.4 but the former exhibited higher OER activity. The interaction between Co and metal dopants should also be taken into account as the active property of metal cations can be altered due to the local environment generated by neighboring metal atoms. Furthermore, the incorporation of the second metal can also increase the conductivity of catalyst and in turn facilitate the charge transfer.

[0065] Since continuous cyclic voltammetry scans can be regarded as an approach for monitoring the material variation during the reaction and evaluating the material's stability, the inventors cycled the electrocatalyst in the same electrolyte from 0.7 V to 1.6 V vs. RHE with a scan rate of 50 mV/s and collected the linear scan afterwards. As plotted in FIG. 14a, after conducting the cyclic voltammetry, pristine Co.sub.3O.sub.4 showed nearly identical polarization curves as the initial one, indicating good chemical stability under alkaline condition. Slight deactivation was observed in the case of Fe and Cu doped Co.sub.3O.sub.4 as the overpotential at j=10 mA/cm.sup.2 shifted to 394 and 385 mV respectively. Interestingly, in the case of NiCo.sub.3O.sub.4, it was found that the catalyst was gradually activated during the CV measurements. Upon further activation, the performance was stabilized and the current density of 10 mA/cm.sup.2 was reached at an overpotential of 368 mV. The direct comparison of the linear scan with that of Co.sub.3O.sub.4 and its non-activated counterpart are shown in FIG. 14b. To be more specific, the activated NiCo.sub.3O.sub.4 reached a current density of 3.79 mA/cm.sup.2 at n=0.35 V, being 4.6 times higher than that of Co.sub.3O.sub.4. The turnover frequency was then calculated based on the assumption that all the metal atoms on the GC electrode are electrochemically active and a TOF of 0.0064 s.sup.1 was obtained for activated NiCo.sub.3O.sub.4. The Tafel slope also decreased from 50 mV/dec to 38 mV/dec, indicating substantially enhanced OER kinetics (FIG. 14c). Moreover, the activated catalyst demonstrated outstanding stability in constant current electrolysis as the overpotential required to reach 10 mA/cm.sup.2 remained at 365 mV for at least 12 h (FIG. 14d).

[0066] As it can be seen from the above, it was demonstrated for the first time that by using spent tea leaves as the hard template, metal oxides such as Al.sub.2O.sub.3, NiO/Al.sub.2O.sub.3, Co.sub.3O.sub.4 and transition metal (Cu, Ni, Fe, Mn) incorporated cobalt oxides could be prepared by a simple impregnation-calcination procedure. After a post treatment reduction process Ni/Al.sub.2O.sub.3, CoO and Co/CoO nanocrystals could be prepared as well. Electron microscopic studies revealed that all products possess a unique nanostructure which was constructed by nano-sized crystallites in the size of 10 nm. TG measurement suggested that the tea leaves first functioned as the hard template for the formation of nanoparticles and then were removed by combustion at higher temperatures. As proof of concept, prepared oxides were then tested for electrochemical water oxidation and the Cu, Ni and Fe incorporated cobalt oxides were found to exhibit higher activity than pristine and non-templated Co.sub.3O.sub.4. Moreover, NiCo.sub.3O.sub.4 was found to be significantly activated after continuous potential cycling and the performance remained stable for at least 12 h. Furthermore, these classes of new nanostructured materials have large potential to find applications in various fields of research and industry.