Synthesis and application of zinc cobalt oxide/sulfide nanorods for photocatalytic water splitting and carbon dioxide reduction

Abstract

There is disclosed photoactive, one-dimensional zinc and cobalt-based bimetallic oxide and sulfide nanorods (ZnCo.sub.2O.sub.4 NRs, ZnCo.sub.2S.sub.4 NRs) and their heterojunction composites (1D/1D ZnCo.sub.2O.sub.4/ZnCo.sub.2S.sub.4) to be used as photocatalysts for hydrogen production and carbon dioxide reduction using solar energy. Also disclosed herein, is a method of synthesizing these compounds via hydrothermal processes and a self-assembly approach. 1D/1D heterojunctions of ZnCo.sub.2O.sub.4/ZnCo.sub.2S.sub.4 composites exhibit favourable interface interactions. The photocatalytic performance of both pure and composite materials is evaluated through water splitting to produce hydrogen and CO.sub.2 reduction to yield CO and CH.sub.4 using slurry phase and fixed bed photoreactor systems. ZnCo.sub.2S.sub.4 NRs demonstrate superior hydrogen production whereas CO.sub.2 reduction is more pronounced with ZnCo.sub.2O.sub.4. The highest photocatalytic efficiency is achieved using the heterojunction composites attributed to efficient charge carrier separation facilitated by a suitable band structure. The invention underscores the successful synthesis of highly efficient 1D structured materials for photocatalytic applications.

Claims

1. A photocatalyst composition for producing hydrogen (H.sub.2) by photocatalytic water splitting and for reducing CO.sub.2 into useful chemicals comprising: one-dimensional photoactive zinc cobalt oxide nanorods (1D ZnCo.sub.2O.sub.4 NRs) of uniform size and shape; one-dimensional photoactive zinc cobalt sulfide nanorods (1D ZnCo.sub.2S.sub.4 NRs) of uniform size and shape; and 1D/1D ZnCo.sub.2O.sub.4/ZnCo.sub.2S.sub.4 heterojunction nanocomposites exhibiting good interface interactions.

2. The photocatalyst composition of claim 1, wherein raw materials for producing the 1D ZnCo.sub.2O.sub.4 NRs by hydrothermal synthesis comprise 0.2 g of zinc acetate (ZnC.sub.4H.sub.6O.sub.4), 0.32 g of cobalt nitrate (Co(NO.sub.3).sub.2.Math.6H.sub.2O), 0.60 g oxalic acid, urea of double the amount than oxalic acid, 20 mL ethanol and 20 mL DI (deionized) water.

3. The photocatalyst composition of claim 1, wherein 0.05 to 0.2 g of ZnCo.sub.2O.sub.4, 0.2 to 2 g of thioacetamide and 40 mL DI water act as raw materials for producing the 1D ZnCo.sub.2S.sub.4 NRs by replacing oxygen with sulfur via hybrid hydrothermal synthesis.

4. The photocatalyst composition of claim 1, wherein raw materials for producing 1D/1D heterojunction ZnCo.sub.2O.sub.4/ZnCo.sub.2S.sub.4 composites in a self-assembly approach comprise ZnCo.sub.2O.sub.4 and ZnCo.sub.2S.sub.4 of equal amounts homogenously dispersed in methanol and oven-dried at 100 C. for 24 hours.

5. The photocatalyst composition of claim 1, wherein the 1D ZnCo.sub.2O.sub.4 NRs and the 1D ZnCo.sub.2S.sub.4 NRs have a spinel crystal structure with zinc, cobalt and respective oxygen or sulfur ions arranged in a lattice and have stability over multiple cycles of photocatalytic reactions.

6. The photocatalyst composition of claim 5, wherein the 1D/1D ZnCo.sub.2O.sub.4/ZnCo.sub.2S.sub.4 heterojunction composites have higher charge separation efficiency, photocatalytic efficiency and stability over multiple cycles compared to single constituent materials ZnCo.sub.2O.sub.4 and ZnCo.sub.2S.sub.4.

7. The photocatalyst composition of claim 1, wherein the 1D ZnCo.sub.2S.sub.4 NRs, due to the presence of sulfur, are more suitable for hydrogen production than the 1D ZnCo.sub.2O.sub.4 NRs, whereas the 1D ZnCo.sub.2O.sub.4 NRs, due to oxides groups and surface defects, are more suitable for CO.sub.2 reduction than the 1D ZnCo.sub.2S.sub.4 NRs.

8. The photocatalyst composition of claim 7, wherein the 1D/1D ZnCo.sub.2O.sub.4/ZnCo.sub.2S.sub.4 heterojunction composites produce the highest H.sub.2 production of 290.2 ppm and the highest CO production of 179.24 molg.sup.1 than the 1D ZnCo.sub.2O.sub.4 and the 1D ZnCo.sub.2S.sub.4.

9. A method for synthesizing a photocatalyst composition comprising photoactive zinc and cobalt based oxides and sulfides nanorods of one-dimensional structure, comprising: synthesizing zinc cobalt oxide nanorods (1D ZnCo.sub.2O.sub.4 NRs) of uniform size and shape using a facile hydrothermal method with specific amounts of raw materials; synthesizing zinc cobalt sulfide nanorods (1D ZnCo.sub.2S.sub.4 NRs) of uniform size and shape using a hybrid hydrothermal method with specific amounts of raw materials; and fabricating further 1D/1D ZnCo.sub.2O.sub.4/ZnCo.sub.2S.sub.4 heterojunction composites using a self-assembly approach, wherein the photocatalyst composition uses solar energy to produce hydrogen (H.sub.2) by photocatalytic water splitting and to convert CO.sub.2 into useful chemicals by photocatalytic CO.sub.2 reduction.

10. The method of claim 9, wherein the hydrothermal method for synthesizing the 1D ZnCo.sub.2O.sub.4 NRs comprise dissolving 0.2 g of zinc acetate (ZnC.sub.4H.sub.6O.sub.4), 0.32 g of cobalt nitrate (Co(NO.sub.3).sub.2.Math.6H.sub.2O), 0.60 g of oxalic acid and urea in double amount than oxalic acid in 20 mL of DI water and 20 mL ethanol; heating the solution at 140 C. for 12 hours; washing resultant 1D ZnCo.sub.2(OH).sub.2 nanorods (NRs) with water or ethanol followed by drying at 100 C. for 24 hours; and heating the 1D ZnCo.sub.2(OH).sub.2 NRs at 350 C. for 2 hours.

11. The method of claim 9, wherein the hybrid hydrothermal method for synthesizing the 1D ZnCo.sub.2S.sub.4 NRs comprise mixing 0.05 to 0.2 g of ZnCo.sub.2O.sub.4 and 0.2 to 2 g of thioacetamide in 40 mL DI water; heating the suspension at 140 C. for 12 hours; washing resultant product with DI water; and drying it at 100 C. for 24 hours.

12. The method of claim 9, wherein the self-assembly approach for synthesizing the 1D/1D ZnCo.sub.2O.sub.4/ZnCo.sub.2S.sub.4 heterojunction composites comprise homogeneously dispersing equal amounts of ZnCo.sub.2O.sub.4 and ZnCo.sub.2S.sub.4 in methanol by stirring and ultrasonication; and oven-drying final product at 100 C. for 24 hours.

13. The method of claim 9, wherein the 1D ZnCo.sub.2O.sub.4 NRs and the 1D ZnCo.sub.2S.sub.4 NRs have a spinel crystal structure with zinc, cobalt and respective oxygen or sulfur ions arranged in a lattice and have stability over multiple cycles of photocatalytic reactions.

14. The method of claim 13, wherein the 1D/1D ZnCo.sub.2O.sub.4/ZnCo.sub.2S.sub.4 heterojunction composites have higher charge separation efficiency, photocatalytic efficiency and stability over multiple cycles compared to single constituent materials ZnCo.sub.2O.sub.4 and ZnCo.sub.2S.sub.4.

15. The method of claim 9, wherein the photocatalytic water splitting for producing H.sub.2 comprises injecting the photocatalyst into a slurry phase photoreactor system integrated with a light source; and analyzing using a micro-Gas Chromatography (GC) fusion.

16. The method of claim 9, wherein the photocatalytic CO.sub.2 reduction for converting CO.sub.2 into CO and CH.sub.4 comprises exposing the photocatalyst and reactants to a light source; maintaining a constant flow rate of high-purity CO.sub.2 gas using mass flow controllers; and analyzing using a micro-GC (fusion).

17. The method of claim 9, wherein the 1D ZnCo.sub.2S.sub.4 NRs are more suitable for hydrogen production than the 1D ZnCo.sub.2O.sub.4 NRs due to the presence of sulfur, and the 1D ZnCo.sub.2O.sub.4 NRs are more suitable than the 1D ZnCo.sub.2S.sub.4 NRs for CO.sub.2 reduction due to oxides groups and surface defects.

18. The method of claim 17, wherein the 1D/1D ZnCo.sub.2O.sub.4/ZnCo.sub.2S.sub.4 heterojunction composites produce the highest H.sub.2 production of 290.2 ppm and the highest CO production of 179.24 molg.sup.1 than the 1D ZnCo.sub.2O.sub.4 and the 1D ZnCo.sub.2S.sub.4.

Description

BRIEF DESCRIPTION OF THE DRAWINGS

(1) The subject matter that is regarded as the invention is particularly pointed out and distinctly claimed in the claims at the conclusion of the specification. The foregoing and other aspects, features, and advantages of the invention are apparent from the following detailed description taken in conjunction with the accompanying drawings in which:

(2) FIG. 1 shows the synthesis of ZnCo.sub.2(OH).sub.2 and ZnCo.sub.2O.sub.4 using hydrothermal process, in accordance with the present invention.

(3) FIG. 2 shows the synthesis of ZnCo.sub.2S.sub.4 using hydrothermal process, in accordance with the present invention.

(4) FIG. 3 shows the synthesis of ZnCo.sub.2O.sub.4/ZnCo.sub.2S.sub.4 composite using self assembly approach, in accordance with the present invention.

(5) FIG. 4A shows XRD analysis of ZnCo.sub.2(OH).sub.2, ZnCo.sub.2O.sub.4 and ZnCo.sub.2S.sub.4 samples, in accordance with the present invention.

(6) FIG. 4B shows UV-visible analysis of ZnCo.sub.2(OH).sub.2, ZnCo.sub.2O.sub.4 and ZnCo.sub.2S.sub.4 samples, in accordance with the present invention.

(7) FIG. 4C shows PL analysis of ZnCo.sub.2(OH).sub.2, ZnCo.sub.2O.sub.4 and ZnCo.sub.2S.sub.4 samples, in accordance with the present invention.

(8) FIG. 5A, FIG. 5B and FIG. 5C show EDX analysis of ZnCo.sub.2(OH).sub.2, ZnCo.sub.2O.sub.4 and ZnCo.sub.2S.sub.4 samples respectively, in accordance with the present invention.

(9) FIG. 6 shows the EDX spectra of ZnCo.sub.2O.sub.4/ZnCo.sub.2S.sub.4 composite with element composition, in accordance with the present invention.

(10) FIG. 7A, FIG. 7B, FIG. 7C, FIG. 7D and FIG. 7E show XPS analysis of Zn 2p, C is, Co 2p, O 1s and S 2p for ZnCo.sub.2S.sub.4, in accordance with the present invention.

(11) FIG. 7F shows XPS analysis of wide spectra for valance band position for ZnCo.sub.2S.sub.4, in accordance with the present invention.

(12) FIG. 8 shows the photocatalytic hydrogen production with ZnCo.sub.2(OH).sub.2, ZnCo.sub.2O.sub.4, ZnCo.sub.2S.sub.2 and ZnCo.sub.2O.sub.4/ZnCo.sub.2S.sub.4 composites, in accordance with the present invention.

(13) FIG. 9 shows the photocatalytic CO.sub.2 reduction with H.sub.2O over various photocatalysts for the production of CO and CH.sub.4 under visible light irradiation, in accordance with the present invention.

(14) FIG. 10A shows the production of CO and CH.sub.4 over ZnCo.sub.2O.sub.4 in photocatalytic CO.sub.2 reduction with H.sub.2O, in accordance with the present invention.

(15) FIG. 10B shows the production of CO and CH.sub.4 over 1D/1D ZnCo.sub.2O.sub.4/ZnCo.sub.2S.sub.4 composite in photocatalytic CO.sub.2 reduction with H.sub.2O, in accordance with the present invention.

DETAILED DESCRIPTION OF THE INVENTION

(16) The aspects of the proposed zinc and cobalt-based bimetallic oxides and sulfides nanocomposites as photocatalystsaccording to the present invention will be described in conjunction with FIGS. 1-10. In the Detailed Description, reference is made to the accompanying figures, which form a part hereof, and which is shown by way of illustration specific embodiments by which the invention may be practiced. It is to be understood that other embodiments may be utilized and logical changes may be made without departing from the scope of the present invention. The following detailed description, therefore, is not to be taken in a limiting sense, and the scope of the present invention is defined by the appended claims.

(17) The present invention proposes synthesis of zinc cobalt oxide (ZnCo.sub.2O.sub.4)/zinc cobalt sulfide (ZnCo.sub.2S.sub.4) nanorods as photoactive materials for energy and environment applications. They are synthesized primarily for photocalalytic CO.sub.2 reduction into useful products and for photocalalytic water splitting to produce hydrogen, using solar energy. These zinc and cobalt-based semiconductors are produced as one-dimensional structure (1D) nanorods (ie; 1D zinc cobalt oxide nanorods (ZnCo.sub.2O.sub.4 NRs), 1D zinc cobalt sulfide nanorods (ZnCo.sub.2S.sub.4)) using a facile hydrothermal approach. They serve as low-cost and highly efficient photocatalyst, active under visible light (photoactive). In an embodiment of the invention, it is further proposed the fabrication of 1D/1D ZnCo.sub.2O.sub.4/ZnCo.sub.2S.sub.4 hybrid nano-composites using a self-assembly approach. In another embodiment, the present invention also discloses the performance of the pure and the composite zinc cobalt-based oxides and sulfides in photocatalytic water splitting to produce hydrogen and photocatalytic CO.sub.2 reduction to produce green fuels such as CO and CH.sub.4 under visible light irradiation. These synthesized materials attain higher visible light absorbance over the entire irradiation time.

(18) According to the disclosure, photocatalytic water splitting using the synthesized photocatalysts, that is 1D ZnCo.sub.2(OH).sub.4 NRs, 1D ZnCo.sub.2O.sub.4 NRs, and 1D ZnCo.sub.2S.sub.4 NRs, results in H.sub.2 production of 82.75, 126.62, and 249.22 ppm respectively. Production of H.sub.2 is higher over ZnCo.sub.2S.sub.4 compared to ZnCo.sub.2(OH).sub.4 and ZnCo.sub.2O.sub.4 samples. The highest H.sub.2 production is obtained over 1D/1D ZnCo.sub.2O.sub.4/ZnCo.sub.2S.sub.4 composites with a yield of 290.2 ppm, which is 1.16, 2.29, and 3.51 folds higher than using pure ZnCo.sub.2S.sub.4, ZnCo.sub.2O.sub.4 and ZnCo.sub.2(OH).sub.4, respectively. The photocatalytic CO.sub.2 reduction with H.sub.2O is able to produce CO and CH.sub.4 as the main products over all types of photocatalysts. The CO production of 32.6, 45.42 and 25.91 mol g.sup.1 h.sup.1 is obtained over ZnCo.sub.2(OH).sub.4, ZnCo.sub.2O.sub.4 and ZnCo.sub.2S.sub.4 samples, respectively. Production of CO is higher over zinc cobalt oxides compared to zinc cobalt sulfides. Using 1D/1D ZnCo.sub.2O.sub.4/ZnCo.sub.2S.sub.4 composite, the highest CO production of 179.24 mol g.sup.1 is obtained which is 1.47 folds higher than using ZnCo.sub.2O.sub.4 photocatalyst respectively. All these results, thereby confirm the successful fabrication of 1D structured materials and their higher photocatalytic efficiency for water splitting and CO.sub.2 reduction applications.

(19) ZnCo.sub.2O.sub.4 and ZnCo.sub.2S.sub.4 are structured compounds with a cubic crystal structure. These compounds have different properties due to the different elements involved, which is oxygen and sulfur, respectively. The characteristics of ZnCo.sub.2O.sub.4(Zinc Cobalt Oxide) are it has a spinel crystal structure, where oxygen ions form a face-centered cubic lattice, and zinc and cobalt ions occupy some of the octahedral and tetrahedral sites within this lattice. ZnCo.sub.2O.sub.4 exhibits mixed conductivity, wherein it has both electronic and ionic conductivity. This property makes it potentially useful in various electrochemical applications, such as fuel cells, sensors, and batteries. It has catalytic properties which makes it suitable for catalytic activity, particularly in oxygen reduction reactions (ORR) and oxygen evolution reactions (OER), which are crucial processes in energy conversion devices like fuel cells and water electrolyzers. ZnCo.sub.2O.sub.4 exhibits good thermal stability, which is important for many high-temperature applications. ZnCo.sub.2S.sub.4(Zinc Cobalt Sulfide), similar to ZnCo.sub.2O.sub.4 also possesses a spinel crystal structure in which, instead of oxygen, sulfur ions occupy the anion positions in the lattice. Since ZnCo.sub.2S.sub.4 is a semiconductor material, its electrical conductivity lies between that of a conductor and an insulator, making it useful in applications such as photocatalysis, solar cells, and sensors. It exhibits optical properties, including absorption and emission characteristics, depending on its exact composition and structure. As a result, it is potentially useful in optoelectronic devices. Similar to ZnCo.sub.2O.sub.4, ZnCo.sub.2S.sub.4 also possesses catalytic properties, particularly in hydrogen evolution reactions (HER) and other electrochemical processes. These characteristics of ZnCo.sub.2O.sub.4 and ZnCo.sub.2S.sub.4, as described herein are of prominence in various fields, particularly the renewable energy and these compounds can be used for applications including energy storage, catalysis, and sensing.

(20) The significance of the present invention is that it provides an approach for the synthesis of visible light active zinc cobalt oxide/sulfides nanorods (ZnCo.sub.2O.sub.4 and ZnCo.sub.2S.sub.4) as a low-cost and highly efficient photocatalyst puts forward a method of producing ZnCo.sub.2O.sub.4 and ZnCo.sub.2S.sub.4-based materials for photocatalytic applications, particularly in the realm of H.sub.2 production and CO.sub.2 reduction using solar energy. Greenhouse gas carbon dioxide (CO.sub.2) is a significant contributor to climate change. When CO.sub.2 gets released into the atmosphere primarily by human activities such as burning fossil fuels (coal, oil, and natural gas) for energy, industrial processes, deforestation, and agricultural practices, it traps heat, leading to global warming and other climate-related disruptions. The present invention puts forward a method of producing ZnCo.sub.2O.sub.4 and ZnCo.sub.2S.sub.4-based materials for photocatalytic conversion of greenhouse CO.sub.2 gas into green fuels and useful chemicals using renewable solar energy. These semiconductor-based photocatalytic systems, due to their enhanced light absorption, charge separation capabilities and catalytic activity, improves the overall process efficiency in harnessing solar energy and results in higher yields of the desired products.

(21) Hydrogen has a huge potential as a viable alternative to fossil fuels with its sustainability, extended storage capacity, and eco-friendly properties as a green fuel. H.sub.2 can be produced efficiently by the process of photocatalytic water splitting that involves harnessing the sunlight using a suitable semiconductor. This process also stands out for its environmental sustainability, contributing to a net-zero carbon footprint. The present approach describes herein, a strategic manipulation of catalyst composition to optimize its performance in hydrogen evolution reactions. ZnCo.sub.2O.sub.4, is a p-type semiconductor, and is inexpensive, nontoxic, earth abundant, and has narrow energy band. When compared to single metal oxides, ZnCo.sub.2O.sub.4 exhibits greater stability, electron conductivity, and richer redox reaction sites. The ZnCo.sub.2S.sub.4 is an n-type semiconductor with narrow energy band (Eg), abundance on earth, environmental friendliness, and low cost. The unique crystal shape and the combined influence of two metal species confer upon ZnCo.sub.2S.sub.4 superior photoelectrochemical consistency, electron conductivity, and a greater number of redox reaction sites compared to single metal sulfides such as ZnS and Co.sub.3S.sub.4. The advantageous properties render ZnCo.sub.2O.sub.4 and ZnCo.sub.2S.sub.4-based materials most suitable for photocatalytic applications for H.sub.2 production and CO.sub.2 reduction and the present invention proposes the synthesis of one dimensional nanorods with higher charge transfer efficiency devoid of charge recombination, larger surface area, suitable band structure, higher visible light absorption, and good stability, for harnessing solar energy for photocatalysis.

(22) The bandgap of a photocatalyst determines its ability to absorb light of certain wavelengths. Ideally, the photocatalyst should have a bandgap corresponding to the solar spectrum to maximize light absorption. The proposes idea suggests synthesis of a suitable photocatalyst through band gap engineering and constructing heterojunction. Bandgap engineering involves modifying the composition or structure of the photocatalyst to optimize its bandgap for efficient light utilisation and charge separation.

(23) Zinc and cobalt-based bimetallic photocatalysts have potential for enhancing photocatalytic activity and stability compared to their monometallic counterpart. The combination of zinc and cobalt in bimetallic photocatalysts can lead to synergistic effects that enhance the photocatalytic activity. Cobalt ions in the bimetallic photocatalyst can act as redox centres, facilitating the generation, transfer, and utilization of photogenerated charge carriers (electrons and holes) during photocatalysis. This can enhance the efficiency of charge separation and reduce the recombination of electron-hole pairs, leading to improved photocatalytic activity. The introduction of cobalt can also extend the light absorption range of the photocatalyst, leading to improved utilization of solar energy for photocatalytic reactions. The presence of cobalt helps to mitigate photo corrosion of zinc-based photocatalysts, thereby enhancing their long-term performance under photocatalytic conditions. In an embodiment of the invention, bimetallic zinc cobalt oxide (ZnCo.sub.2O.sub.4) is used for photocatalytic CO.sub.2 reduction and water splitting to produce hydrogen under solar energy. ZnCo.sub.2O.sub.4 is a mixed metal oxide semiconductor material that is used as a photocatalyst due to its unique electronic structure and photocatalytic properties. ZnCo.sub.2O.sub.4 possesses a spinel crystal structure composed of zinc (Zn), cobalt (Co), and oxygen (O) atoms arranged in a cubic lattice. The electronic structure of ZnCo.sub.2O.sub.4 is characterized by the presence of Co (III) and Co (II) oxidation states, as well as oxygen vacancies, which contribute to its photocatalytic activity. ZnCo.sub.2O.sub.4 exhibits broad absorption in the visible region of the electromagnetic spectrum, which allows it to harness sunlight for photocatalytic reactions. This is attributed to the presence of d-d transition bands associated with the Co ions in the crystal structure. ZnCo.sub.2O.sub.4 exhibits a suitable band structure for promoting charge separation, with photogenerated electrons transferring to the conduction band and holes remaining in the valence band.

(24) Bimetallic sulfur-based photocatalysts, which incorporate two different metals along with sulfur, exhibits enhanced photocatalytic activity and selectivity compared to their monometallic counterparts. In another embodiment of the present invention, ZnCo.sub.2S.sub.4, or zinc cobalt sulfide, which is a ternary metal sulfide compound is used for photocatalysis due to the unique properties of three materials. ZnCo.sub.2S.sub.4 crystallizes in a cubic spinel structure, consisting of zinc (Zn), cobalt (Co), and sulfur (S) atoms arranged in a lattice. In the spinel structure, cobalt ions occupy both tetrahedral and octahedral sites, while zinc ions occupy only octahedral sites. Thus, ZnCo.sub.2S.sub.4 is made suitable for photocatalytic CO.sub.2 reduction and water splitting to produce hydrogen under solar energy.

(25) An embodiment of the present invention combines ZnCo.sub.2O.sub.4 with ZnCo.sub.2S.sub.4 to construct ZnCo.sub.2O.sub.4/ZnCo.sub.2S.sub.4 composites, that provides the properties of both metal oxides and metal sulfides. The combination of ZnCo.sub.2O.sub.4 and ZnCo.sub.2S.sub.4 in a composite material leads to synergistic effects, enhancing the photocatalytic activity and stability compared to individual components. The different electronic properties and band structures of the two phases can promote efficient charge separation and utilization of visible light for photocatalytic reactions.

(26) In an embodiment of the disclosure herein, one-dimensional bimetallic zinc cobalt hydroxide nanorods (1D ZnCo.sub.2(OH).sub.2 NRs), one-dimensional bimetallic zinc cobalt hydroxide nanorods (1D ZnCo.sub.2O.sub.4 NRs) and one-dimensional trimetallic zinc cobalt sulfide nanorods (1D ZnCo.sub.2S.sub.4 NRs) are synthesized using facile hydrothermal methods. In another embodiment of the invention, the performance of these photocatalysts are tested for photocatalytic CO.sub.2 reduction to produce fuels as well as water splitting to produce hydrogen (H.sub.2) in a fixed bed and slurry phase photoreactor systems respectively. The invention proposes in an embodiment, constructing 1D/1D heterojunctions of ZnCo.sub.2O.sub.4/ZnCo.sub.2S.sub.4 composites with good interface interactions and investigating the influential effects of 1D ZnCo.sub.2O.sub.4 and 1D ZnCo.sub.2S.sub.4. According to the disclosure, ZnCo.sub.2O.sub.4 is suitable for photocatalytic CO.sub.2 reduction, whereas ZnCo.sub.2S.sub.4 is more beneficial for solar hydrogen production. However, the highest photocatalytic efficiency is achieved using the heterojunction composites due to efficient charge carrier separation with a suitable band structure to maximize the photocatalytic efficiency.

(27) In an embodiment of the present invention, a hydrothermal method with specific amounts of raw materials such as zinc acetate, cobalt nitrate, urea and oxalic acids of their specific ratios, is used to grow one dimensional zinc cobalt oxide nanorods (1D ZnCo.sub.2O.sub.4 NRs) of uniform size and shape. The hydrothermal method involves, synthesis of 1D ZnCo.sub.2(OH).sub.2 nanorods as well. For the synthesis of ZnCo.sub.2(OH).sub.2 and ZnCo.sub.2O.sub.4, the chemicals used are zinc acetate, cobalt nitrate, oxalic acid, urea and ethanol with their high-purity grade. FIG. 1 shows a schematic illustration of the synthesis of ZnCo.sub.2(OH).sub.2 and ZnCo.sub.2O.sub.4 using the hydrothermal method according to the present embodiment of the invention. The ZnCo.sub.2(OH).sub.2 is synthesized using the following steps. First, 0.2 g of zinc acetate (ZnC.sub.4H.sub.6O.sub.4) with 0.32 g of cobalt nitrate (Co(NO.sub.3).sub.2.Math.6H.sub.2O) are dissolved with 20 mL of DI water (Deionized water) under continuous stirring. The amount of zinc acetate and cobalt nitrate can be adjusted to get different morphologies of the final products. After stirring the mixture for 30 minutes to get a clear solution, a specific amount of oxalic acid (0.60 g) is added to the above solution and stirred well for another 30 minutes. In the next stage, double the amount of urea than oxalic acid, is added to the above solution under continuous stirring. In the final stage, 20 mL ethanol is added to the above solution and after stirring for 30 minutes, it is transferred to a Teflon-lined autoclave. The autoclave is transferred to the furnace, and it is heated at 140 C. for 12 h. The final product is rinsed repeatedly with water and ethanol before being dried at 100 C. to get the final pink colour product of 1D ZnCo.sub.2(OH).sub.2 nanorods (NRs). For the synthesis of ZnCo.sub.2O.sub.4, a specific amount (0.5 to 1 g) of ZnCo.sub.2(OH).sub.2, washed and then dried at 100 C. for 24 h in the previous step is used. ZnCo.sub.2(OH).sub.2 is heated at 350 C. for 2 hours. The final product obtained is of a blackish colour, which is 1D ZnCo.sub.2O.sub.4 nanorods or 1D ZnCo.sub.2O.sub.4 NRs.

(28) In an embodiment of the present invention, a hybrid approach of double hydrothermal method is used for the synthesis of one-dimensional zinc cobalt sulfide nanorods ((1D ZnCo.sub.2S.sub.4NRs)) of uniform size and shape. In this case, 1D ZnCo.sub.2O.sub.4 NRs of uniform size and shape acts as the raw material and the additional precursors employed is thioacetamide as the source of sulfur. Using hybrid hydrothermal method, oxygen gets replaced with sulfur producing 1D ZnCo.sub.2S.sub.4 NRs with the same size and shape but with higher solar energy harvesting efficiency and products selectivity. FIG. 2 shows a schematic illustration of the synthesis of ZnCo.sub.2S.sub.4 nanorods using the hydrothermal process according to the present embodiment of the invention. The hydrothermal process uses ZnCo.sub.2O.sub.4 and thioacetamide, as the raw materials. A specific amount of ZnCo.sub.2O.sub.4 (0.05 to 0.2 g) is dispersed in 40 mL DI water under stirring. In the next stage, a specific amount of thioacetamide (0.2 to 2 g) is added to the above suspension and is stirred for 30 minutes. The mixture is then placed in a Teflon-lined autoclave and heated at 140 C. for 12 hours. The product is centrifuged, washed with DI water, and dried at 100 C. for 24 hours to get one-dimensional (1D) nanorods of ZnCo.sub.2S.sub.4.

(29) In another embodiment of the present invention, the hybrid composites of 1D/1D ZnCo.sub.2O.sub.4/ZnCo.sub.2S.sub.4 nanorods is synthesized using a self-assembly approach. The self-assembly process involves bringing together ZnCo.sub.2O.sub.4 and ZnCo.sub.2S.sub.4 together under specific conditions to allow them to interact and form a composite material. FIG. 3 shows a schematic illustration of the synthesis of ZnCo.sub.2O.sub.4/ZnCo.sub.2S.sub.4 nanotextures using the self-assembly approach, as per the embodiment of the invention. Equal amounts of ZnCo.sub.2O.sub.4 (e.g., 0.5 g) and ZnCo.sub.2S.sub.4 (e.g., 0.5 g) are dispersed in methanol and the mixture is subjected to stirring for 6 h and ultrasonication to ensure homogenous dispersion. The final product is oven-dried at 100 C. for 24 hours and 1D/1D ZnCo.sub.2O.sub.4/ZnCo.sub.2S.sub.4 nanorods are obtained.

(30) The crystal structure of the samples of 1D ZnCo.sub.2(OH).sub.2, ZnCo.sub.2O.sub.4, ZnCo.sub.2S.sub.4 and 1D/1D ZnCo.sub.2O.sub.4/ZnCo.sub.2S.sub.4 nanorods are analysed for characterization of their structure, in different embodiments of the present disclosure. The samples are subjected to X-ray diffraction (XRD) in an embodiment. A Rigaku Bruker Advance D8 X-ray diffractometer, which has a 40-kV working voltage and a 40-mA working current is used for XRD. The morphological and structural characteristics of the pure and composite materials is examined through the application of Scanning Electron Microscopy (SEM), utilizing the JEOL 6010 PLUS/LA apparatus. X-ray photoelectron spectroscopy (XPS) is employed as an embodiment, to ascertain the elemental states and an Axis ultra-DLD Shimadzu is used for the purpose. All of the elements' high-resolution peaks are calibrated using the binding energy of C 1s, which is 284.60 eV. The efficiency of materials charge separation is assessed through photoluminescence (PL) spectroscopy employing a 325 nm wavelength laser from HORIBA Scientific, in an embodiment. Additionally, a Raman investigation is conducted using a HORIBA Scientific Spectrophotometer and a 532 nm laser to explore the interaction among composite elements. UV-visible diffuse reflectance absorbance spectra is also conducted using Carry 100 Agilent UV-vis spectrophotometer (model #G9821A).

(31) Both 1D ZnCo.sub.2O.sub.4 NRs and 1D ZnCo.sub.2S.sub.4 NRs have a larger surface area, higher visible absorption, efficient charge production, suitable band structure and good stability. The hybrid sulfides/oxides (ZnCo.sub.2O.sub.4/ZnCo.sub.2S.sub.4 NRs) composites are found to have higher charge separation efficiency and photocatalytic efficiency when compared to single materials.

(32) FIG. 4A shows XRD patterns of ZnCo.sub.2(OH).sub.2, ZnCo.sub.2O.sub.4 and ZnCo.sub.2S.sub.4 samples. For the bare ZnCo.sub.2(OH).sub.2, the XRD signals have appeared at 2 of 20.18, 28.54, 47.53, and 56.44, which confirms the synthesis of zinc cobalt hydroxide. When ZnCo.sub.2(OH).sub.2 is heated at 350 C., for two hours, the peaks are shifted towards higher 2 values to produce zinc cobalt oxide (ZnCo.sub.2O.sub.4). The signals at 31.17, 36.46, 44.60, 58.980 and 64.89 of ZnCo.sub.2O.sub.4 are assigned to the (2 2 0), (3 1 1), (4 0 0), (5 1 1) and (4 4 0) crystal planes, respectively and similar results are reported previously. This shows the successful synthesis of ZnCo.sub.2O.sub.4 with high purity and crystallinity. When the sulfur (S) is added to ZnCo.sub.2(OH).sub.2, it produces similar peaks, however, oxygen is replaced with sulfur to produce ZnCo.sub.2S.sub.4. Using UV-vis diffuse reflection spectroscopy (DRS), the optical performance of the synthesized samples, ZnCo.sub.2(OH).sub.2, ZnCo.sub.2O.sub.4 and ZnCo.sub.2S.sub.4 are measured, and the results are as shown in FIG. 4B. The absorption edges of 614 nm, 731 nm and 815 nm are obtained for ZnCo.sub.2(OH).sub.2, ZnCo.sub.2O.sub.4 and ZnCo.sub.2S.sub.4 samples, respectively. It is interesting to note that all these samples show absorbance in the visible region, which could help with photocatalytic CO.sub.2 reduction and H.sub.2 generation performance. The band gaps of ZnCo.sub.2(OH).sub.2, ZnCo.sub.2O.sub.4 and ZnCo.sub.2S.sub.4 are determined to be 2.09, 1.70 eV and 1.52 eV, respectively. Previously, ZnCo.sub.2O.sub.4 is analyzed through UV-visible and similar results are obtained. FIG. 4C shows the PL spectra of ZnCo.sub.2(OH).sub.2, ZnCo.sub.2O.sub.4 and ZnCo.sub.2S.sub.4 samples. Using ZnCo.sub.2 (OH).sub.2, lower peak intensity is observed, which is possibly due to lower production of charges. However, a higher peak intensity is obtained for ZnCo.sub.2O.sub.4 due to more production and recombination of charge carriers. This reveals the semiconducting characteristics of zinc cobalt oxide. Furthermore, in the case of ZnCo.sub.2S.sub.4, the peak intensity is significantly dropped, which may be due to lower production of charges or their less recombination in the presence of sulfur. In the literature, peak intensity for ZnCo.sub.2O.sub.4 is not observed, however, in the current disclosure, due to morphological difference and 1D structure, an obvious peak is obtained. The morphology of the materials is further investigated using scanning electron microscopy (SEM) and the results are obtained. The morphology of ZnCo.sub.2(OH).sub.2 shows large size one dimensional (1D) nanorods. It is observed that all the rods are uniform in size and shape, which are produced using the hydrothermal approach with a specific ratio of Zn/Co and oxalic acid/urea. Similarly, the morphology of ZnCo.sub.2O.sub.4 presents that the ZnCo.sub.2O.sub.4 consists of 1D nanorods and all of them are in uniform size and shape, which are produced after heating the ZnCo.sub.2(OH).sub.2 at 350 C. for two hours. This reveals the successful fabrication of zinc cobalt hydroxide and zinc cobalt oxide using a facile hydrothermal method. Furthermore, the SEM images of ZnCo.sub.2S.sub.4 shows that, similar to 1D ZnCo.sub.2O.sub.4 nanorods, ZnCo.sub.2S.sub.4 also consists of 1D nanorods with uniform size and shape, which are synthesized using the hydrothermal method with thioacetamide as the sulfur precursor. However, the surface of 1D ZnCo.sub.2S.sub.4 is rough compared to the smooth surface of ZnCo.sub.2O.sub.4 nanorods, which is possibly due to the replacement of oxygen with sulfur and also due to treating ZnCo.sub.2O.sub.4 with water as the solvent at high temperature.

(33) The EDX analysis of the ZnCo.sub.2(OH).sub.2, ZnCo.sub.2O.sub.4 and ZnCo.sub.2S.sub.4 samples is further conducted, and their results are presented in FIG. 5A, FIG. 5B and FIG. 5C. FIG. 5A shows EDX spectra of 1D ZnCo.sub.2(OH).sub.2 nanorods. The elements observed are Zn, Co, and O with their composition of 35.44%, 18.73% and 45.83%, respectively. On the other hand, FIG. 5B shows the EDX spectrum of 1D ZnCo.sub.2O.sub.4 nanorods. The elements observed are Zn, Co and O with their compositions of 60.21%, 26.72% and 13.07%, respectively. It can be observed that higher oxygen is observed in ZnCo.sub.2(OH).sub.2 due to the presence of water absorbed and hydroxyl groups, due to use as synthesizing material without calcination. Comparatively, a higher amount of Zn and Co is observed in the ZnCo.sub.2O.sub.4 sample, due to heating the precursor at 350 C. for 2 hours, which is useful to remove water and also some adsorbed oxygen. The EDX results of ZnCo.sub.2S.sub.4 are shown in FIG. 5C. EDX spectra show the peaks of Zn, Co, S and O elements with their compositions of 22.05%, 19.86%, 19.72% and 38.37%, respectively. These results are different from the composition of ZnCo.sub.2(OH).sub.2 and ZnCo.sub.2O.sub.4. The composition of Zn and Co is decreased in ZnCo.sub.2S.sub.4 samples due to adding the sulfur, however, the amount of oxygen is increased compared to ZnCo.sub.2O.sub.4 due to using water for the synthesis and also because of using the sample without heating, in which possible oxygen and OH groups would be adsorbed. In general, all of these results confirm successful synthesis of ZnCo.sub.2(OH).sub.2, ZnCo.sub.2O.sub.4 and ZnCo.sub.2S.sub.4 samples and can be further used for photocatalytic applications.

(34) The morphology of 1D/1D ZnCo.sub.2O.sub.4/ZnCo.sub.2S4 heterojunction composite is obtained and investigated using scanning electron microscopy (SEM). The composite consists of 1D nanorods of ZnCo.sub.2O.sub.4 and 1D nanorods of ZnCo.sub.2S.sub.4 to produce 1D/1D heterojunction. A good interface interaction between ZnCo.sub.2O.sub.4/ZnCo.sub.2S.sub.4 nanorods is observed due to using a self-assembly approach in the synthesis. Both materials also have identical morphology as discussed previously, however, their structure is slightly altered due to continuous stirring. The EDX mapping analysis of ZnCo.sub.2O.sub.4/ZnCo.sub.2S4 shows that all the elements Zn, Co, S and O are uniformly and entirely distributed over the composite surface. The distribution of Zn, Co, S and O elements is further investigated through colour images and it further confirms their unfirm distribution within the composite samples. FIG. 6 shows the EDX spectrum of ZnCo.sub.2O.sub.4/ZnCo.sub.2S4, which confirms the presence of Zn, Co, S and O elements. The compositions of Zn, Co, S and S obtained are 46.33%, 25.18%, 9.04% and 19.45%. These results are in good agreement with the previous results of the pure ZnCo.sub.2O.sub.4 and ZnCo.sub.2S.sub.4 samples. Compared to ZnCo.sub.2S.sub.4, the amount of S is decreased, whereas the amount of Zn and O are increased due to adding ZnCo.sub.2O.sub.4 to synthesize ZnCo.sub.2O.sub.4/ZnCo.sub.2S4 composite. All these results confirm the successful synthesis of the composite materials and is useful for producing 1D/1D heterojunctions with higher photocatalytic efficiency.

(35) The elemental state is further investigated using XPS analysis and the results are shown in FIG. 7A-7F. FIG. 7A shows the XPS spectra of Zn 2p with binding energies 1022.01 eV and 1044.79 eV, associated with Zn 2p.sub.3/2 and Zn 2p.sub.1/2, respectively. The corresponding difference of 22.64 eV, confirms the existence of Zn (II) valence ions (Zn.sup.2+) FIG. 7B shows XPS analysis of C1 s with four peaks having binding energies 283.2 eV, 284.6 eV, 285.6 eV and 286.1 eV. The peak at 283.2 eV is ascribed to carbon attached with some intermediates, whereas the other three peaks with binding energies 284.6 eV, 285.6 eV and 286.1 eV can be attributed to CC, CO and CO, respectively. FIG. 7C shows XPS spectra of Co 2p with binding energies 779.4 eV, 781.9 eV, 785.4 eV, 795.5 eV and 802.9 eV. The peak at 779.4 eV identifies the existence of cobalt as the metallic state. The peaks at 781.9 eV and 795.5 eV are attributed to the existence of CO.sub.2.sup.+ and Co.sup.3+ with satellite peaks having binding energies of 785.4 eV and 802.9 eV. FIG. 7D shows XPS spectra of O 1s with binding energies 530.3 eV, 531.3 eV and 532.9 eV, ascribed to crystal lattice oxygen, adsorbed oxygen and oxygen vacancies, respectively. The XPS spectrum of S 2p is shown in FIG. 7E with binding energies 160.2 eV, and 162.9 eV with typical S 2p.sub.3/2 and S 2p.sub.1/2 relevant features, which can be ascribed to corresponding metal sulfides (S.sup.2) with 168.6 eV satellite peak. All these results show the presence of elements as Zn.sup.2+, CO.sub.2.sup.+, Co.sup.3+ and S.sup.2 in the ZnCo.sub.2S.sub.4 nanorods. Furthermore, FIG. 7F shows wide spectra with a valance band position of 2.487 eV for the ZnCo.sub.2S.sub.4, and it can be used to calculate the conductance band with the help of band gap energy.

(36) In an embodiment of the present invention, the pure zinc, cobalt-based materials, and the hybrid nanotextures are tested for photocatalytic water splitting to produce hydrogen and photocatalytic CO.sub.2 reduction to produce green fuels for the climate action with higher efficiency and products selectivity. In one embodiment, 1D ZnCo.sub.2O.sub.4 NRs are promising to effectively convert CO.sub.2 to green fuels in a fixed bed photoreactor under solar energy irradiations. The materials have suitable redox potentials to produce CO and CH.sub.4 with their higher photoactivity and stability. 1D ZnCo.sub.2O.sub.4 NRs are promising for efficient photocatalytic water splitting to produce hydrogen in a slurry type photoreactor system under solar energy irradiations. The materials have suitable redox potentials to produce hydrogen with higher photoactivity and stability. In another embodiment of the present invention, 1D ZnCo.sub.2S.sub.4 NRs are promising to effectively convert CO.sub.2 to green fuels in a fixed bed photoreactor under solar energy irradiations. The materials have suitable redox potentials to produce CO and CH.sub.4 with their higher photoactivity and stability. In an embodiment of the invention, 1D ZnCo.sub.2S.sub.4 NRs are promising for efficient photocatalytic water splitting to produce hydrogen in a slurry type photoreactor system under solar energy irradiations. The materials have suitable redox potentials to produce hydrogen with higher photoactivity and stability. Comparatively, 1D ZnCo.sub.2S.sub.4 NRs are more promising for hydrogen production due to the presence of sulfur, whereas 1D ZnCo.sub.2O.sub.4 NRs are more promising for CO.sub.2 reduction due to oxides groups and surface defects. In another embodiment of the disclosure, the hybridizing 1D ZnCo.sub.2O.sub.4 NRs/1D ZnCo.sub.2S.sub.4 NRs are found to be promising for CO.sub.2 reduction to CO and CH.sub.4, and water splitting to produce hydrogen under the same reaction conditions. 1D ZnCo.sub.2O.sub.4 NRs and 1D ZnCo.sub.2S.sub.4 NRs are also found to be stable in multiple cycles for continuous hydrogen production.

(37) As mentioned, in an embodiment of the invention, pure 1 D ZnCo.sub.2(OH).sub.2, 1 D ZnCo.sub.2O.sub.4 and 1 D ZnCo.sub.2S.sub.4 NR samples and the hybrid composites of 1D ZnCo.sub.2O.sub.4 NRs/1D ZnCo.sub.2S.sub.4 NRs are tested for both photocatalytic water splitting to produce hydrogen and CO.sub.2 reduction to produce green fuels such as CO and CH.sub.4. For photocatalytic water splitting for hydrogen production, a slurry phase Pyrex glass photoreactor system having a total volume of 60 mL is used to examine the performance of all the photocatalysts. A 500 W Xenon lamp serves as the visible light source with a light intensity of 100 mW/cm.sup.2. 25 mg of photocatalyst is disseminated in a 5 vol % aqueous solution of methanol as sacrificial reagents having a total volume of 50 mL and homogenized by magnetic stirring. Utilizing a vacuum flow system and constant nitrogen flow, the reactor and piping systems are cleaned, and efficiency is determined based on the amount of hydrogen produced. The online micro-GC (Gas Chromatography) fusion is integrated with the reactor for the continuous analysis of the amount of H.sub.2 produced. GC is installed with two Thermal Conductivity Detectors (TCDs) connected with argon and helium carrier gases and products are injected into GC after 20 minutes of interval.

(38) In a slurry photoreactor with 5% methanol as the sacrificial reagents and 25 mg of photocatalyst loading, the performance of all the samples is conducted and the results are shown in FIG. 8. Initially, for the first 20 minutes, the lower yield of H.sub.2 is obtained, which is significantly increased after 60 minutes but these trends are continuously increasing over the reaction time. The lower amount of hydrogen production at the beginning could be due to the existence of an activation process of the photocatalyst. Another possible reason can be due to using a continuous process with online injection of samples to GC after 20 minutes of interval. In this case, there is no accumulation of hydrogen in the reactor and the pipelines which are connected to GC. For example, in the initial injection, only a small portion reaches GC, whereas, with increasing reaction time, hydrogen is reached in sufficient quantity to GC inlet, resulting in a higher production rate. Previously, similar patterns are obtained during photocatalytic water splitting to produce H.sub.2 in a continuous flow photoreactor system. The amount of hydrogen produced over ZnCo.sub.2(OH).sub.4 is 82.75 ppm, which is produced after 80 minutes of reaction time with 25 mg of catalyst loading and 5 vol. % sacrificial reagents. This shows that ZnCo.sub.2(OH).sub.4 have semiconducting characteristics and enables to production significant amount of hydrogen. Furthermore, the production of hydrogen is increased to 126.62 ppm with 1D ZnCo.sub.2O.sub.4 NRs photocatalyst, which is 1.53 folds higher than using 1D ZnCo.sub.2(OH).sub.4 NRs under the same reaction conditions and catalyst loading. This increase in hydrogen production is due to more production of photo-induced charge carriers in ZnCo.sub.2O.sub.4 as evidenced by PL analysis. A further increase in hydrogen production is obtained with ZnCo.sub.2S.sub.4 with hydrogen production of 249.22 ppm. This reveals, that introducing sulfur is beneficial to promoting hydrogen production. This amount of hydrogen production is 3.01 and 1.97 folds more than using ZnCo.sub.2(OH).sub.4 and ZnCo.sub.2O.sub.4 samples, respectively. Previously, the H.sub.2 production rate of 123 mol g.sup.1 h.sup.1 is obtained with ZnCo.sub.2O.sub.4 nanoparticles using a 300 W Xe lamp with 20 vol % of triethanolamine (TEOA) in a batch process.

(39) The performance of ZnCo.sub.2O.sub.4 and ZnCo.sub.2S.sub.4 photocatalysts is further investigated by constructing 1D/1D heterojunctions and their results are presented in FIG. 8. Like ZnCo.sub.2O.sub.4 and ZnCo.sub.2S.sub.4, continuous hydrogen production is obtained with the binary composites. The maximum hydrogen amount of 290.2 ppm is obtained with 1D/1D ZnCo.sub.2O.sub.4/ZnCo.sub.2S.sub.4 composite. This amount of hydrogen production is 1.16, 2.29, and 3.51 folds more obtained than using ZnCo.sub.2S.sub.4, ZnCo.sub.2O.sub.4 and ZnCo.sub.2(OH).sub.4 samples, respectively. This significantly enhanced photocatalytic efficiency is due to the efficient production and separation of charge carriers over the binary 1D/1D ZnCo.sub.2O.sub.4/ZnCo.sub.2S.sub.4 composite under visible light irradiation.

(40) In another embodiment of photocatalytic CO.sub.2 reduction, a fixed bed photoreactor system is used to examine the performance of all the photocatalysts. The photocatalytic system consists of an online product analysis system, a central reactor chamber, and mass flow controllers (MFC). The main light source, a 300 W Xenon lamp, is positioned at the top of the reactor glass window and generates light with an intensity of 100 mW/cm.sup.2. A water saturator is incorporated into the reactor system to transport CO.sub.2 and water vapors. In every experiment, 150 mg of powder catalyst is utilized, evenly distributed inside the reactor bottom surface. The primary exposed region is the bottom surface of the reactor chamber, which is where the catalyst, reactants, and light source interact. During each experiment, the MFC maintains a constant flow rate of high-purity CO.sub.2 gas at 20 mL/min. Before the commencement of testing, a feed mixture comprising CO.sub.2 and H.sub.2O is continuously circulated through the reactor for 30 minutes to ensure thorough saturation of the catalyst surface. The products are analyzed using GC-TCD (thermal conductivity detectors)/FID (flame-ionisation detectors) connected with different columns for the identification of CO, CH.sub.4 and other products.

(41) Initially, blank tests are conducted using all the photocatalysts in the process of reducing CO.sub.2 with water and methanol. During these blank experiments, which involves the absence of light, CO.sub.2, and photocatalyst, no additional products are detected in the gas phase. These findings reinforce the purity of the photocatalysts and affirm that the generation of products only occurs when CO.sub.2 is actively reduced in the presence of light and photocatalyst. The absence of products in the blank experiments eliminates the possibility of contamination or interference, underscoring the reliability of the observed outcomes and confirming that the observed reactions are indeed driven by the photocatalysts. FIG. 9 illustrates the photocatalytic process of reducing CO.sub.2 with H.sub.2O to generate CO and CH.sub.4 in a gas-phase photocatalytic system. In all the samples, both CO and CH.sub.4 are produced, however, the production of CO is higher compared to CH.sub.4. Using ZnCo.sub.2(OH).sub.4, CO and CH.sub.4 yields of 32.6 and 24.42 mol g.sup.1 h.sup.1 are produced. Similarly, CO and CH.sub.4 yields of 45.42 and 33.33 mol g.sup.1 h.sup.1 are obtained under identical reaction conditions on using ZnCo.sub.2O.sub.4. The higher CO and CH.sub.4 production over the ZnCo.sub.2O.sub.4 compared to the ZnCo.sub.2(OH).sub.4 is obviously due to more production of charge carriers as evidenced by PL analysis. However, using ZnCo.sub.2S.sub.4, amount of CO and CH.sub.4 is reduced with a lower yield rate of 25.91 and 18.14 molg.sup.1 h.sup.1 compared to using ZnCo.sub.2O.sub.4 and ZnCo.sub.2(OH).sub.4 samples. This shows that sulfur-based materials are not efficient for CO.sub.2 reduction compared to their oxides. This can be explained based on different characteristics and reaction pathways. The highest photoactivity is obtained with ZnCo.sub.2O.sub.4/ZnCo.sub.2S.sub.4 composite with their equal ratios, enabling to produce CO and CH.sub.4 production rates of 71.21 and 35.27 mol g.sup.1 h.sup.1. This provides information about the importance of 1D/1D binary composite of two different materials and their influence on the oxidation and reduction reactions during the photocatalysis process.

(42) The effect of irradiation time on the performance of ZnCo.sub.2O.sub.4 and ZnCo.sub.2O.sub.4/ZnCo.sub.2S.sub.4 1D/1D composite is further investigated for the production of CO and CH.sub.4 and the results are shown in FIG. 10A and FIG. 10B respectively. FIG. 10A shows the photoactivity of ZnCo.sub.2O.sub.4, in which continuous production of CO and CH.sub.4 is obtained over the entire irradiation time. The CO and CH.sub.4 yields of 121.34 and 75.33 mol g.sup.1 are obtained after two hours of irradiation time under visible light irradiation. The production of CO is 1.61 folds higher than the CH.sub.4 formation, which shows that ZnCo.sub.2O.sub.4 is more selective towards CO formation with a selectivity of 61.70%. This is possibly due to a more negative conduction band position and less production of electrons because only 2 electrons are required for CO formations, whereas CH.sub.4 is produced with the involvement of 8 electrons. The performance of 1D ZnCo.sub.2O.sub.4 NRs is further investigated by combining with ZnCo.sub.2S.sub.4 to construct 1D/1D composites of ZnCo.sub.2O.sub.4/ZnCo.sub.2S.sub.4. FIG. 10B shows the production of CO and CH.sub.4 over 1D/1D ZnCo.sub.2O.sub.4/ZnCo.sub.2S.sub.4 composites. Continuous production of CO and CH.sub.4 can be observed over the entire irradiation time. The maximum CO and CH.sub.4 production of 179.24 and 49.2 mol g.sup.1 is obtained after 2 hours of irradiation time. Similar to other photocatalysts, selective CO production is obtained with selectivity of 78.46%. Comparatively, on using 1D/1D ZnCo.sub.2O.sub.4/ZnCo.sub.2S.sub.4 composites, the production of CO is 1.48 folds higher than it is produced by using only 1D ZnCo.sub.2O.sub.4 NRs. The increase in photocatalytic activity is due to efficient visible light utilization and proficient charge carrier separation.

(43) Benefits of the proposed approach for the synthesis of one dimensional visible light active (photoactive) zinc cobalt oxides/sulfides nanorods (ZnCo.sub.2O.sub.4 and ZnCo.sub.2S.sub.4) in accordance with the present invention include a low-cost but highly efficient photocatalyst to convert solar energy to convert CO.sub.2 into green fuels such as CO and CH.sub.4 and for water splitting process to produce hydrogen. Semiconductor-based photocatalytic systems exhibit enhanced efficiency in harnessing solar energy, resulting in optimal yields of desired products. Enhancing the efficiency of semiconductors' light absorption, charge separation, and catalytic activity improves the overall process efficiency of photocatalysis for efficient H.sub.2 production and CO.sub.2 reduction harnessing the sunlight and contributing to environmental sustainability, with a net-zero carbon footprint. The bimetallic oxide/sulphide nanocomposites synthesized herein can meet the growing demand for photocatalysts that are both efficient and stable, particularly under visible light conditions. Besides photocatalytic applications, ZnCo.sub.2O.sub.4 and ZnCo.sub.2S.sub.4 compounds can be used in widespread applications in various other fields of energy storage, catalysis, and sensing such as in electrocatalysis, supercapacitors, batteries etc. The electrical conductivity properties of ZnCo.sub.2O.sub.4 make them potentially useful in various electrochemical applications, such as fuel cells, sensors, and batteries and their catalytic activity, particularly in oxygen reduction reactions (ORR) and oxygen evolution reactions (OER), make them crucial for energy conversion devices like fuel cells and water electrolyzers. ZnCo.sub.2O.sub.4 are thermally stable and can be employed in high-temperature applications. ZnCo.sub.2S.sub.4 is a semiconductor material which makes it useful in applications such as photocatalysis, solar cells, and sensors. It exhibits catalytic properties in hydrogen evolution reactions (HER) and other electrochemical processes. ZnCo.sub.2S.sub.4 possesses interesting optical properties, including absorption and emission characteristics, making it potentially useful in optoelectronic devices. Zinc cobalt oxide/sulfide nanorods are of significant market interest for solar energy utilization and storage, batteries, catalysts, CO.sub.2 capture and utilization, H.sub.2 production and water treatment.

(44) Many changes, modifications, variations and other uses and applications of the subject invention will become apparent to those skilled in the art after considering this specification and the accompanying drawings, which disclose the preferred embodiments thereof. All such changes, modifications, variations and other uses and applications, which do not depart from the spirit and scope of the invention, are deemed to be covered by the invention, which is to be limited only by the claims, which follow.