Enhanced Photocatalytic Hydrogen Evolution from Water Splitting on Ta2O5/SrZrO3 Heterostructures Decorated with CuxO/RuO2 Cocatalysts.

Photocatalytic H2 generation by water splitting is a promising alternative for producing renewable fuels. This work synthesized a new type of Ta2O5/SrZrO3 heterostructure with Ru and Cu (RuO2/CuxO/Ta2O5/SrZrO3) using solid-state chemistry methods to achieve a high H2 production of 5164 μmol g-1 h-1 under simulated solar light, 39 times higher than that produced using SrZrO3. The heterostructure performance is compared with other Ta2O5/SrZrO3 heterostructure compositions loaded with RuO2, CuxO, or Pt. CuxO is used to showcase the usage of less costly cocatalysts to produce H2. The photocatalytic activity toward H2 by the RuO2/CuxO/Ta2O5/SrZrO3 heterostructure remains the highest, followed by RuO2/Ta2O5/SrZrO3 > CuxO/Ta2O5/SrZrO3 > Pt/Ta2O5/SrZrO3 > Ta2O5/SrZrO3 > SrZrO3. Band gap tunability and high optical absorbance in the visible region are more prominent for the heterostructures containing cocatalysts (RuO2 or CuxO) and are even higher for the binary catalyst (RuO2/CuxO). The presence of the binary catalyst is observed to impact the charge carrier transport in Ta2O5/SrZrO3, improving the solar to hydrogen conversion efficiency. The results represent a valuable contribution to the design of SrZrO3-based heterostructures for photocatalytic H2 production by solar water splitting.

Introduction

ABO3 is an inorganic perovskite with a mixed metal oxide composition, where the A-element is an alkaline (earth) or a lanthanide, and the B-element is a transition metal. An example of ABO3 is zirconate (AZrO3), known for its ferroelectric, piezoelectric, and photocatalytic properties.[1,2] In photocatalysis, the H2 production efficiency of AZrO3 remains low due to its limited visible light absorption (Eg > 4 eV) and poor carrier generation.[3,4] Strategies to stimulate photocarrier generation as a means to improve H2 water splitting under visible light are key for AZrO3. A way forward is producing a semiconductor via cation replacement (A = Ba, Ca, Sr) in AZrO3, followed by band alignment interfacing AZrO3 with another semiconductor to form a heterostructure.[5−9] First, cation replacement can be done by introducing Sr into AZrO3 to form SrZrO3, which has an orthorhombic crystal structure with a Pbnm space group.[10,11] SrZrO3 is an indirect band gap semiconductor. The valence band (VB) lies lower than the water oxidation potential, while the conduction band (CB) is located higher than the hydrogen reduction potential.[12] Photogenerated carriers through VB and CB can recombine, reaching the SrZrO3 surface and induce the chemical transformation of 2H2O into 2H2 and O2. However, due to its wide band gap (Eg ∼ 4 eV),[8] SrZrO3 requires UV light to photogenerate enough carriers to produce 50 μmol g–1 h–1.[6] The H2 production can be improved to reach 5310 μmol g–1 h–1 using UV light and electron donor species, such as Na2S and Na2SO3.[7] Although the addition of electron donor species is an option,[7] the main challenge remains with the photocatalyst. An ideal catalyst should effectively promote charge transport and retain similar H2 water-splitting performances under visible light.

The heterostructure concept involves band alignment,[13] which ideally can be used to modulate charge transport. This can be done by incorporating Ta compounds, such as Ta2O5 and other tantalates, recognized as active photocatalysts for H2 water splitting.[14] The band gap structure in tantalum oxide consists of O 2p orbitals formed by the VB and the CB, with a d0 electronic configuration that provides electron mobility access.[15] Depending on the synthetic approach,[16] the addition of Ta can lead to doping via SrZrO3 substitution or yield Ta segregates to form Ta2O5, especially when treated at high temperatures.[17] Notably, both Ta-substitution and Ta segregate formation can promote mobility access in photocatalysts.[18] However, H2 water splitting in tantalates has been mainly promoted with UV irradiation.[15] From this aspect, the next desired step for Ta-containing SrZrO3 catalysts is to retain charge transport properties under visible light.[5,6,8,19] This entails the increase of photocarrier density using visible light by coupling other chemical species, such as cocatalysts (or binary catalysts, hereafter bicatalysts), to Ta-containing SrZrO3. From this point of view, the heterostructure concept with the incorporation of a cocatalyst or bicatalyst has not been applied to Ta-containing SrZrO3 yet, opening new opportunities to design SrZrO3-based photocatalysts.[20,21]

Coupling a narrow band gap to a wide band gap semiconductor enhances light absorption in the visible spectrum.[22,23] In essence, this entails band gap tunability via band alignment to reduce the recombination of photogenerated charges.[24] Copper oxide can function as a narrow band gap p-type semiconductor (Cu2O),[25,26] catalyst (CuO),[26] or both, especially when Cu2O and CuO species are combined (hereafter, CuO).[27] It could then be expected to improve the exchange of photocarriers when interfaced with wide-band semiconductors enabling high catalytic activity. Furthermore, interfacing CuO with an oxide-based hydrogen evolution catalyst, such as RuO2, is an attractive option to improve H2 production during water splitting.[23] The combination of CuO and RuO2 has been successfully applied in photocathodes[23] and is now proposed to improve the photocatalytic activity of Ta-containing SrZrO3.

This work synthesized a novel SrZrO3 heterostructure of mixed oxides (RuO2/CuO/Ta2O5/SrZrO3) via solid-state chemistry. The functionality of the heterostructure is benchmarked during water splitting, achieving 5164 μmol g–1 h–1 of H2. The photocatalytic performance of the heterostructure is compared with that of Ta2O5/SrZrO3 loaded with RuO2, CuO, or RuO2/CuO to understand the role of each heterostructure component. The RuO2/CuO/Ta2O5/SrZrO3 heterostructure is also compared with Pt, a more costly catalyst than Ru or Cu.[28] In-depth chemical and structural analyses were carried out by X-ray photoelectron spectroscopy (XPS), electron energy-loss spectroscopy (EELS), and transmission electron microscopy (TEM) to understand the chemical states of the RuO2/CuO/Ta2O5/SrZrO3 components. Ta2O5 has been observed to be distributed at the surface and between grain boundaries in SrZrO3 nanocrystallites, facilitating charge mobility during photocatalytic water splitting. Ru and Cu have been found as oxides, that is, RuO2, Cu2O, and CuO. RuO2 has been seen to be shaped as nanorods over Ta2O5/SrZrO3, whereas CuO remains distributed over Ta2O5/SrZrO3 with no particular shape. The photocatalytic activity of the heterostructure is attributed to a synergistic effect that allows charge transfer through energy channels, enabling charge carriers to recombine and reach the interface of the RuO2/CuO bi-catalyst. To the best of our knowledge, this is the first report on the coupling of RuO2/CuO to Ta2O5/SrZrO3 for photocatalytic water splitting under visible light. Our results can contribute to the design of efficient SrZrO3-based photocatalysts for hydrogen evolution.

Materials and Methods

Synthesis of Ta2O5/SrZrO3 Photocatalysts

SrCO3 (99%, Sigma-Aldrich 472018), ZrO2 (99%, Merck 230693), and Ta2O5 (99%, Sigma-Aldrich 303518) were ground in an agate mortar for 10 min, adding 0.1 mL of acetone as a dispersant. Ta2O5 amounts added were 0.8, 1.6, 2.4, 3, and 3.9 wt %. The homogenized mixture was placed in a platinum crucible and then thermally treated for 12 h at 1100 °C in air, with a 3 °C.min–1 heating rate.

RuO, CuO, and Pt Cocatalyst Deposition

RuCl3 (Sigma-Aldrich 208523), CuCl2 (Sigma-Aldrich 222011), and H2PtCl6 (Sigma-Aldrich 520896) were impregnated into the Ta2O5/SrZrO3 photocatalysts. The final weight percentages were 0, 0.1, 0.3, 0.5, 1.0, 1.3, and 1.5 wt %. The samples were kept in solution at 80 °C for 4 h under constant stirring. The samples were dried at 80 °C. The obtained powders were annealed in an air atmosphere at 400 °C for 2 h. For Pt deposition, H2PtCl6 was added to a Ta2O5/SrZrO3 suspension in propanol. The powder was centrifuged and also dried at 80 °C for 4 h.

TEM, Energy-Dispersive X-ray Spectrometry, and EELS

Scanning transmission electron microscopy (STEM), energy-dispersive X-ray spectrometry (EDXS), and EELS were carried out using a Cs-corrected microscope JEOL ARM 200CF equipped with an JEOL SSD EDX spectrometer and a Gatan Dual EELS Quantum spectrum-imaging filter. The operational voltage was 200 kV. The photocatalyst powders were dispersed in ethanol and were deposited over different carbon-coated Au, Cu, and Ni grids before the inspection.

X-ray Diffraction

The structural characterization was performed with X-ray diffraction (XRD) in a θ – 2θ arrangement, employing a Bruker D8 Advance diffractometer operating at 40 kV and 40 mA with CuKα radiation (λ = 1.5406 Å), from 10 to 70° (2θ).

Chemical Analysis by XPS

For the X-ray photoelectron spectroscopy (XPS) measurements, a Quantera SXM (Physical Electronics) was used. The X-rays were Al Kα, monochromatic at 1486.6 eV with a beam size of 200 μm. The binding energies were corrected according to the C 1s peak (284.8 eV). Samples were located on millimetric-sized indium cups, forming a pellet for sample homogeneity. In every sample, three different areas were probed with an area size of 600 × 300 μm2.

Optical Characterization

The optical properties were analyzed using a UV–vis NIR spectrophotometer (Cary 5000) in the diffuse reflectance mode. The band gap was calculated with the Tauc method, which involves plotting (α h ν)1/ versus (h ν). The value of the exponent n denotes the nature of the sample transition, the value is 2, considering indirect allowed transitions. A linear region was used to extrapolate to the X-axis intercept to find the band gap values. Photoluminescence spectra were collected in an Agilent Cary Eclipse spectrophotometer using a 254 nm excitation. Prior to UV–vis-NiR or PL, the samples were sieved and pelletized.

Photoelectrochemical Characterization

The photoelectrochemical measurements were carried out in a three-electrode quartz cell connected to a potentiostat from AUTOLAB. Pt was used as a counter electrode and Ag/AgCl (3 M KCl) as a reference electrode. The working electrode was fabricated by depositing the photocatalyst over an ITO substrate. For this process, 2 mg/mL of the photocatalyst suspension in ethanol was deposited using a spin coater at 2000 rpm. The samples were dried at 80 °C for 10 min. Once dried, the samples are immersed in 0.5 M Na2SO4 and used as an electrolyte. Electrochemical impedance spectroscopy (EIS) measurements for obtaining Mott Schottky plots were performed under dark conditions in a potential range of 0.8 to −0.8 V vs. Ag/AgCl at a frequency of 100 kHz–100 MHz and an AC perturbation of 10 mV. The potential versus Ag/AgCl, EAg/AgCl, was converted to reversible hydrogen electrode potential, E, using the Nernst equation. For the photocurrent response experiment, a constant potential of 0.3 V vs. Ag/AgCl is applied. The electrode was illuminated with a solar simulator (Xe lamp 100 mW/cm2) for 300 s, and the photocurrent was obtained considering the electrode area (1 cm2).

Photocatalytic H2 Evolution

The photocatalytic experiments were performed in a Pyrex reactor of 250 mL. In a typical experiment, 0.1 g of the photocatalyst was dispersed in 200 mL of deionized water. Before each experiment, the reactor was purged with N2 for 30 min and irradiated with a wide range UV–vis xenon lamp (simulated solar light). The photocatalyst was stimulated with irradiation between 400 and 900 nm at 100 mW/cm2 in demineralized water. The oxygen and hydrogen products were analyzed using a gas chromatograph (Thermo Scientific) coupled with a thermal conductivity detector. No buffer or electrolyzer was added during the reaction, and the starting pH was 7. No external potential was applied during photocatalytic experiments.

The solar to hydrogen conversion efficiency (STH) was estimated from eq ,[29] using the H2 production, the Gibbs free energy for the reaction, the incident power of the solar simulator (100 mW/cm2 AM1.5G), and the area of irradiation.

The quantum efficiency (QE) was calculated with eq ,[29] at 420 nm, where NH2 is the number of H2 molecules produced in seconds and N is the photon flux.

Computational Methods

Periodic DFT calculations using the projected augmented wave (PAW) formalism were performed with the Vienna Ab Initio Simulation Package (VASP 5.4.4).[30,31] The revised Perdew–Burke–Ernzerhof for solids (PBEsol) were selected for cell-optimization as it reduces PBE’s tendency to overestimate unit cell parameters.[32,33] The one-electron Kohn–Sham orbitals were expanded on a plane-wave basis with a kinetic energy cutoff for the plane waves of 800 eV (PBEsol calculations). PAW potentials were employed to describe the interaction between the valence electrons and the core electrons.[34] Reciprocal space integration over the Brillouin zone was approximated with finite sampling using Monkhorst–Pack k-point grids of 7 × 7 × 7.[35,36] The bulk unit cell of SrZrO3 was optimized until the largest force on all atomic coordinates became smaller than 0.01 eV/Å. Furthermore, the convergence criterion for the self-consistent electric field (SCF) problem was set to 10–6 eV for all optimizations, and the symmetry group was preserved throughout all simulations. The unit cell volume was kept fixed at different cell volumes, followed by a constant volume cell optimization to verify the strain effect on the band gap. The unit cell of both structures was scaled proportionally to investigate the effect of strain on the band gap. Furthermore, a band gap evaluation on the optimized PBEsol structures was performed employing the HSE06[37] hybrid functional and a kinetic energy cutoff of 550 eV using a k-point grid of 3 × 3 × 3 as well as similar electronic and force convergence criteria.

Results and Discussion

A SrZrO3 heterostructure of mixed oxides (RuO2/CuO/Ta2O5/SrZrO3) synthesized via solid-state chemistry has been produced. The synergy between the RuO2/CuO/Ta2O5/SrZrO3 heterostructure components is investigated structurally, chemically, and optically. The application of the RuO2/CuO/Ta2O5/SrZrO3 heterostructure is assessed during photocatalytic water splitting and contrasted with other SrZrO3 compositions to select the most suitable heterostructure that yields the highest H2 efficiency. The results are then correlated to the charge transport in RuO2/CuO/Ta2O5/SrZrO3. Finally, a mechanism is proposed to shed light on charge transfer in the RuO2/CuO/Ta2O5/SrZrO3 heterostructure.

RuO2/CuO/Ta2O5/SrZrO3 Heterostructure Synergy

Structural Analysis of the RuO2/CuO/Ta2O5/SrZrO3 Heterostructure

STEM and EDXS analyses are assessed to unveil the morphology of the heterostructure components. First, the characterization of SrZrO3 is examined (Figure ), followed by a discussion on the higher-order heterostructures, such as RuO2/CuO/Ta2O5/SrZrO3 (Figure ). In Figure a, the morphology of SrZrO3 consists of agglomerated particles of ten to hundreds of nanometer sizes with a uniform distribution of chemical elements Sr, Zr, and O. The crystal structure of SrZrO3 is visualized along the [100] zone axis in Figure b,c that corresponds to the perovskite orthorhombic phase. An atomic model of the SrZrO3 structure is depicted in Figure d. The identification and orientation of the crystal lattice planes are extracted from the fast Fourier transform (FFT) shown in Figure e.

Figure 1

a) HAADF and EDXS maps of SrZrO3 nanocrystallites. b) HAADF and c) BF high-resolution imaging of the SrZrO3 structure along with the [100] orientation. d) Atomic (ball and stick) model of the SrZrO3 structure viewed along the [100] zone axis. e) Corresponding FFT with the identified [100] zone axis and crystal lattice planes (020) and (004).

Figure 2

(a) HAADF imaging and EDXS mapping of 0.1%RuO2/1%CuO/3%Ta2O5/SrZrO3 showing the distribution of chemical elements. The Ru signal is detected only on the nanorods, and the Ta signal is observed scattered and accumulated in small regions (marked by white circles). (b) HAADF images of SrZrO3 crystallites showing Ta segregating at the grain boundaries, (c) at the surface, and (d) clustering. (e) EELS signal corresponding to Ta O2,3 and Zr N2,3.

In Figure a, the STEM-EDXS maps of 0.1%RuO2/1%CuO/3%Ta2O5/SrZrO3 heterostructure show the distribution of Sr, Zr, and O, corresponding to the SrZrO3 nanocrystallite formation. The Ru EDXS signal map indicated the growth of nanorods characterized in detail in Figures S1 and S2. The composition of the nanorods is RuO2 (Figures S1 and S2), and they are distributed at various locations over the heterostructure, ranging in size from 10 to 30 nm in width and 100 to 200 nm in length. In the case of Cu, the overlapping signals of Cu Kα 8.04 with Ta Lα 8.140 (and Hf Lα 7.898 present as an impurity from the synthesis precursor) turned the EDXS mapping problematic for small quantities. However, when the amount of Cu is significant, it is possible to detect Cu among the SrZrO3 nanocrystallites (see Figure S3). The Cu morphology is found not as distinctive as the RuO2 nanorods but rather in the form of agglomerates, in a mixture state of CuO and Cu2O according to EELS observations (Figure S3d).

The distribution of Ta is observed in various parts of the SrZrO3 nanocrystallites: (i) dispersed over the SrZrO3 nanocrystallites and (ii) accumulated in selected regions (Figures a and S4). A closer look at RuO2/CuO/Ta2O5/SrZrO3 revealed that Ta segregated between the grains, as seen in the HAADF image in Figure b (see also Figure S4b). This can be distinguished by the higher contrast observed at the grain boundaries, corresponding to an accumulation of Ta (a higher Z = 73 element compared to Sr = 38 and Zr = 40). A similar observation in Figure c revealed Ta at the surface of the SrZrO3 nanocrystallites (see also Figure S4d). To verify our hypothesis (and discard the presence of Hf Z = 72), EDXS and EELS are carried out in these distinct regions (Figure S4). The Ta O2,3 edge was detected when collecting the EELS signal from the high contrast region in the HAADF image (Figure S4d); likewise, by performing EDXS in a similar area, the presence of the Ta Lα 8.140 peak was observed in the spectra (as shown Figure S4c). This detailed examination revealed that when Ta accumulates preferentially more in some grains than in others, it segregates at the grain boundaries and decorates the nanocrystallite surface. In addition, Ta is found forming clusters around the crystallites as seen in Figure d and confirmed by the Ta O2,3 edge in the EELS signal in Figure e.

Chemical Species at the Surface of the RuO2/CuO/Ta2O5/SrZrO3 Heterostructure

The elemental compositions and chemical environments of RuO2/CuO/Ta2O5/SrZrO3 and comparative and control samples are investigated with XPS. Figure shows the XPS spectra of (a1–d1) Sr 3d, (a2–d2) Zr 3d, (a3–d3) Ta 4d, and (a4–d4) O 1s. The analyzed samples are displayed per row. In this case, (a1–a4) SrZrO3, (b1–b4) 3%Ta2O5/SrZrO3, (c1–c4) 1%CuO/3%Ta2O5/SrZrO3, and (d1–d4) 0.1%RuO2/1%CuO/3%Ta2O5/SrZrO3. Irrespective of the sample structure, the Sr 3d and Zr 3d core level XPS spectra show almost superimposable envelopes. The position of the Sr 3d5/2, Sr 3d3/2, Zr 3d5/2 and Zr 3d3/2 components located at 132.9, 134.7, 181.2, and 183.6 eV, respectively, indicate Sr2+ and Zr4+ in a SrZrO3 environment (Table S1).[7,38] The specific area ratios (2/3) and spin–orbit splitting values for Sr 3d (1.8 eV) and Zr 3d (2.4 eV) suggest no secondary phase. For Ta 4d (a3–d3), unsurprisingly, the pure SrZrO3 sample (a3) shows no Ta presence. The Ta 4d envelopes of the three other samples are identical and show two main contributions at 229.2 eV (Ta 4d5/2) and 241.6 eV (Ta 4d3/2) assigned to Ta5+ in Ta2O5.[39−41] A less-resolved contribution is also observed at lower binding energies (ca. 224.3 eV) and is attributed to Ta 4d5/2 of hydrated Ta species. Finally, the O 1s core-level XPS spectra (a4–d4) display broad envelopes that can be fitted with three components. The first contribution at lower binding energies, ca. 529.2 eV, is assigned to O2– in metal oxides (i.e., SrZrO3, CuO, and RuO2). The contribution at 531.2 eV is attributed to oxygen adsorbed in SrZrO3,[7] while the contribution at the highest binding energies, ca. 532.6 eV, could be associated with O–H.[42] It can be concluded that there is no significant difference in the chemical environments of Sr, Zr, Ta, and O species for SrZrO3, 3%Ta2O5/SrZrO3, 1%CuO/3%Ta2O5/SrZrO3, and 0.1%RuO2/1%CuO/3%Ta2O5/SrZrO3.

Figure 3

XPS spectra of (a1–d1) Sr 3d, (a2–d2) Zr 3d, (a3–d3) Ta 4d, and (a4–d4) O 1s. The analyzed samples are displayed per row. In this case, (a1–a4) SrZrO3, (b1–b4) 3%Ta2O5/SrZrO3, (c1–c4) 1%CuO/3%Ta2O5/SrZrO3, and (d1–d4) 0.1%RuO2/1%CuO/3%Ta2O5/SrZrO3.

The Cu 2p and Ru 3p core-level XPS spectra of the heterostructure samples containing Cu and Ru, that is, 1%CuO/3%Ta2O5/SrZrO3 (Figure a1,a2) and 0.1%RuO2/1%CuO/3%Ta2O5/SrZrO3 (Figure b1,b2), are presented in Figure . Although the spectra have a low signal-to-noise ratio, the Cu 2p and Ru 3p peaks still provide valuable information. It should be noted that Ru 3d is not reported due to the elemental overlap with C, as observed in Figure S5. In Figures a1,b1, two contributions in the form of 932.7 and 934.2 eV peaks assigned to Cu2O and CuO are observed.[8,43] In this set of samples, the additional contribution at 942.4 eV is assigned to Cu 2p3/2 satellites.[8,43] The coexistence of the Cu+ and Cu2+ oxidation states is corroborated by the Cu LMM spectrum (Figure S5). The presence of the Cu2O and CuO phases is observed even after the water-splitting reaction (Figure S5). The presence of Cu+ and Cu2+ also agrees with EELS measurement (Figure S3). XPS confirms the presence of Ru in the 0.1%RuO2/1%CuO/3%Ta2O5/SrZrO3 heterostructure (Figure b2). The binding energy of Ru 3p3/2 of ca. 463.0 eV agrees with the presence of Ru4+ in RuO2 (Table S1).[44] The chemical information, elemental composition, and chemical environments are summarized in Tables and S1. The chemical environment of Sr and Zr and the Sr/Zr ratio are notably constant for all the studied heterostructures and unaltered even after the photocatalytic test (Figure S5 and Table S1). However, a small reduction in Ta, Cu, and Ru is found after the photocatalytic water splitting for the 0.1%RuO2/1%CuO/3%Ta2O5/SrZrO3 heterostructure (Table ).

Figure 4

XPS spectra of Cu 2p and Ru 3p in CuO/3%Ta2O5/SrZrO3 (a1–a2) and in 0.1%RuO2/1%CuO/3%Ta2O5/SrZrO3 (b1–b2).

Table 1

Sr/Zr Ratio and Elemental Composition of Different SrZrO3-Based Catalysts, Including the 0.1%RuO2/1%CuO/3%Ta2O5/SrZrO3 Heterostructurea

sample	Sr/Zr	Ta	Cu	Ru
SrZrO3	1.11	(at. %)	(at. %)	(at. %)
3%Ta2O5/SrZrO3	1.35	1.1
1%CuxO/3%Ta2O5/SrZrO3	1.48	1.0	0.35
0.1%RuO2/1%CuxO/3%Ta2O5/SrZrO3	1.31	1.5	0.37	0.4
0.1%RuO2/1%CuxO/3%Ta2O5/SrZrO3*	1.27	0.6	0.2	0.2

Values reported in atomic percent (at.%). (*) at. % after photocatalytic water splitting.

Optical Properties of the RuO2/CuO/Ta2O5/SrZrO3 Heterostructure Components

The light absorption and charge photogeneration properties of the heterostructure components are shown in Figure . Figures a,b displays the UV–vis and photoluminescence spectra for various Ta2O5 loadings. The inset in Figure a shows the Tauc plots estimated from the UV–vis spectra. Band gap for Ta2O5/SrZrO3 has been found between 3.85 and 4 eV. A redshift to lower energies is observed for the highest Ta2O5-loaded samples. A reduction in the absorption band near a wavelength (λ) of 250 nm is seen in the UV–vis spectrum for 3 wt % Ta2O5, probably due to the participation of Ta 5d orbitals affecting the CB.[45] It should be mentioned that such an effect can promote charge separation, resulting in a significant benefit for a photocatalytic process. The results are in good agreement with photoluminescent (PL) measurements in Figure b, indicating a reduction in charge recombination for 3%Ta2O5/SrZrO3.

Figure 5

(a) UV–vis diffuse reflectance spectra and Tauc plots (inset). (b) Photoluminescence spectra for various Ta2O5 loadings from (a). (c) UV–vis diffuse reflectance spectra and Tauc plots (inset) for various heterostructure constructions. (d) Photoluminescence spectra of the synthesized heterostructures from (c).

Light absorption in the visible range increases with CuO and RuO2 in 3%Ta2O5/SrZrO3 (Figure c). The results show a considerable increase in light absorption for the 0.1%RuO2/1%CuO/3%Ta2O5/SrZrO3 heterostructure, which is more significant than those for 1%CuO/3%Ta2O5/SrZrO3 and 1%RuO2/3%Ta2O5/SrZrO3. Therefore, it can be argued that the 0.1%RuO2/1%CuO/3%Ta2O5/SrZrO3 heterostructure reduces further charge recombination, as shown in Figure d. The results in Figure d suggest that by controlling RuO2/CuO ratios, visible light absorption can be optimized to maintain the photocatalytic rate high.[7] It should be noted that in Figure d, the PL spectrum of 3%Ta2O5/SrZrO3 overlaps with the 1%CuO/3%Ta2O5/SrZrO3 spectrum. Both spectra are also comparable to that of 1%RuO2/3%Ta2O5/SrZrO3.

Structural Characterization

Structural characteristics with XRD for Ta2O5/SrZrO3 and RuO2/CuO/Ta2O5/SrZrO3 heterostructure are assessed to understand how Ta2O5 and RuO2/CuO loadings affect the optical properties as shown in Figure . The synthesized SrZrO3 exhibits a highly crystalline pattern (Figure a1) and corresponds to the orthorhombic phase (JCPDS/ 44–0161). The other SrZrO3 samples with various Ta2O5 loadings in Figure a2–a4 retain the SrZrO3 phase. No distinct Ta2O5 peaks have been identified. Interestingly, from the diffractogram in Figure b, a peak shift from 30.75 to 30.90° in 2θ is observed. A slight shift to higher 2θ theta values is pronounced for large Ta2O5 loadings in Figure b2–b4. The shift has been suggested to be a substitution effect from Ta5+ (0.64 Å) and Zr4+ (0.72 Å) in the crystalline structure of SrZrO3,[19] distorting the lattice.

Figure 6

(a) XRD patterns of (1) SrZrO3 and SrZrO3 with various Ta2O5 loadings, i.e., (2) 0.8%, (3) 1.6%, and (4) 3%. The 0.1%RuO2/1%CuO/3%Ta2O5/SrZrO3 heterostructure is presented in (5). (b) Enlarged region of XRD patterns between 2θ = 30–32°.

From the XRD results of Ta2O5/SrZrO3, a reduction in the cell volume is found. The results are in agreement with band gap changes to higher energy in Figure a. Our attributions are supported by density functional theory in Figure , in which the band gap is studied as a function of the unit cell volume. In this case, the unit cell of both the Pnma and Pnmb SrZrO3 structures is scaled proportionally to investigate the effect of strain on the band gap. Via subsequent constant volume optimization at PBEsol,[33,34] it is possible to verify the strain effect on the band gap. At the PBEsol level of theory, the band gap for both SrZrO3 structures increases when applying compressive strain and decreases with tensile strain. Furthermore, a rigorous evaluation of the band gap using the hybrid functional of Heyd–Scuseria–Ernzerhof (HSE06)[37,46] is employed. It has been found that the HSE06 functional is superior in localizing valence electrons of transition metals (e.g., those in Cu 3d orbitals) more correctly than (semi)local density functionals.[47] An experimental band gap close to 5.6 eV for single SrZrO3 crystals is typical, and HSE06 predicts theoretical band gaps of about ∼5.0 eV,[48] which is in line with the HSE06-calculated band gaps of 5.09 eV (Pnma) and 5.11 eV (Pnmb) in Figure . For all unit cell volumes, it is clear that the HSE06 calculated band gaps are higher than those obtained from PBEsol. However, the trend remains the same. The results suggest that strain effects may originate from the presence of Ta2O5 after the synthesis procedure. Ta in SrZrO3 induces compressive strain on the lattice, leading to lower unit cell volumes. Computationally, it has been found that compressive strain increases the band gap, while tensile strain leads to lower band gaps, as in low-loaded SrZrO3 (Figure a). The effect is primarily due to (i) Zr+4 substitution by Ta+5 or (ii) strain effects on SrZrO3 caused by segregated Ta2O5, both leading to a broader band gap.

Figure 7

Simulation of the band gap decrement as a function of the unit cell volume. Unit cells of Pnma and Pnmb symmetry groups are optimized at chosen unit cell volumes between 0.943, 0.953, ..., 1.053 and 1.063 of their optimized cell volume, that is, 277.3 and 274.2 Å3 respectively.

In the case of 0.1%RuO2/1%CuO/3%Ta2O5/SrZrO3 heterostructure, the presence of RuO2, CuO, or their combination RuO2/CuO leads to broader photoadsorption over a larger part of the visible spectrum (Figure c). The rationale behind this is that these oxides have lower band gaps compared to Ta2O5/SrZrO3 (Figure a).[49] The measured UV–vis diffuse reflectance spectra (Figure c) of the RuO2/CuO bi-catalyst in 3%Ta2O5/SrZrO3 help to extend the heterostructure absorption edge into the visible range. A small shift is found for the 0.1%RuO2/1%CuO/3%Ta2O5/SrZrO3 heterostructure in Figure b5 (2θ = 30.80), particularly when compared to 3%Ta2O5/SrZrO3 in Figure b. The results indicate that 0.1%RuO2/1%CuO/3%Ta2O5/SrZrO3 has a smaller reduction in the cell volume than 3%Ta2O5/SrZrO3. This 2θ shift agrees with the estimated band gap of 3.6 eV of the 0.1%RuO2/1%CuO/3%Ta2O5/SrZrO3 heterostructure in Figure c. Although there is a band gap difference of 0.4 eV between heterostructures with or without a bicatalyst, the role of Ta is imminent, either substituting Zr4+ or compressive strain[19] in the SrZrO3 lattice (Figure ). It should be mentioned that no peak characteristics of RuO2, CuO, or CuO2 have been found in the XRD pattern, possibly due to the low cocatalyst amounts used (lower than 5%).

In short, a detailed analysis of the heterostructure components and the effect of Ta2O5 in SrZrO3 has been carried out optically (Figure a). Ta2O5 has a positive effect by lowering charge recombination, as indicated by the photoluminescent measurements in Figure b. The effect of Ta2O5 in the SrZrO3 structure leads to band gap tunability and has been studied further in Figures and 7. The results show that the role of tantalum is imminent, by either substituting Zr4+ or introducing compressive strain in the SrZrO3 lattice. Lattice constraints in SrZrO3 due to the presence of Ta are not observed in TEM, pointing toward shallow Ta5+ doping. Although this lattice effect is not seen locally in Figure , the XRD pattern in Figure b reveals cell volume contraction for Ta2O5/SrZrO3. Therefore, Ta-substitution or ejected strain in SrZrO3 should not be disregarded in Ta2O5/SrZrO3 and 0.1%RuO2/1%CuO/3%Ta2O5/SrZrO3 heterostructures. The chemical composition of the 0.1%RuO2/1%CuO/3%Ta2O5/SrZrO3 heterostructure consisting of RuO2 and CuO contributes to extending the light absorption in the visible region (Figure c), promoting high photocatalytic activity, demonstrated in the next section.

Heterostructure Synergy to Promote Photocatalytic Water Splitting

The photocatalytic activity for SrZrO3 is evaluated for various Ta2O5 loadings in Figure a (i.e., 0.8, 1.6, 2.4, 3, and 3.9 wt %). H2 production under simulated solar light for SrZrO3 is 132 μmol g–1 h–1, increasing the H2 production rate to 1297 μmol g–1 h–1 as Ta2O5 reaches 3 wt % (hereafter, 3% Ta2O5). The higher catalytic activity is attributed to Ta2O5 improving charge transport at the SrZrO3 interface. In this sense, Ta2O5 can provide a large number of states, where electrons might be trapped, reducing hole–electron recombinations.[50] For still larger Ta2O5 loadings (i.e., 3.9 wt %), the H2 evolution activity reduces to 959 μmol g–1 h–1. The results indicate that Ta2O5 loadings can also affect the overall catalyst performance. It can then be hypothesized that there is a trade-off between charge mobility[15] and trapped states for different Ta2O5 loadings. From the results, Ta2O5 in SrZrO3 is maintained fixed to 3 wt %, as it shows the highest amount of H2 produced in Figure a. It should be noted that during experiments shown in Figure a, the production of O2 has not been observed.

Figure 8

(a) H2 production rates under simulated solar light for Ta2O5/SrZrO3 with various Ta2O5 loadings. (b) Kinetic curves of the H2 evolution vs time for RuO2/1%CuO/3%Ta2O5/SrZrO3 with various RuO2 loadings. (c) H2 and (d) O2 production rates for RuO2/1%CuO/3%Ta2O5/SrZrO3 with various RuO2 loadings. (e) H2 and (f) O2 production rates in 3%Ta2O5/SrZrO3 loaded with CuO, RuO2, and Pt cocatalyst.

The H2 production is further improved by incorporating various RuO2/CuO loadings to 3%Ta2O5/SrZrO3. Insights on the kinetics of H2 evolution on RuO2/CuO heterostructures are presented in Figure b. The results reveal that the H2 production in the first 3 h shows a linear tendency. After this time, the production rate is diminished, showing a plateau effect, which several authors correlate to limitations in the surface area and the available active sites on the photocatalyst.[51] However, we should not disregard possible elemental losses after the reaction (Table ). We also assess potential changes in the chemical environment and crystalline structure in 0.1%RuO2/1%CuO/3%Ta2O5/SrZrO3 with XPS and XRD after the reaction (Figures S5 and S6 and Table S1). In this case, no significant changes are observed; only the Ta at % reduces nearly 2-fold at the surface (Table ), possibly explaining the changes in Figure b after 3 h. The cumulative H2 production is presented in Figure c. Figure c shows that 0.1%RuO2/1%CuO is the ideal ratio, yielding a H2 production rate of 5164 μmol g–1 h–1, which is even higher than those of several cocatalysts (e.g., RuO2, CuO, and Pt) and other zirconates and perovskite heterostructures as shown in Figure e and Table S2. The photocatalytic activity of 0.1%RuO2/1%CuO has also been estimated to support our attributions. In this case, the H2 production rate remains approximately 184 lower (28 μmol g–1 h–1) than the H2 rate obtained for 0.1%RuO2/1%CuO coupled to the 3%Ta2O5/SrZrO3 heterostructure (5164 μmol g–1 h–1). The experiments indicate that charge transfer through the different heterostructure components is improved by adding 0.1%RuO2/1%CuO to 3%Ta2O5/SrZrO3. The photocatalytic activity for 0.1%RuO2/1%CuO is also attributed to the strong electronic coupling with Ta2O5/SrZrO3.

The H2 production rate for the RuO2/1%CuO/3%Ta2O5/SrZrO3 heterostructure of varied RuO2 contents and other heterostructures of lower-order with CuO, RuO2, and Pt (Figure c,e) is contrasted with the O2 production rate to demonstrate the overall water-splitting process (Figure d,f). The trends for the O2 production rates in Figure d are compared to those in Figure c. The results show an O2 to H2 ratio of 1:2 for the RuO2/CuO/3%Ta2O5/SrZrO3 heterostructure.[52] Similar ratios for lower-order heterostructures decorated with RuO2, CuO, and Pt cocatalysts can be seen in Figure e,f. Among the results, it should be noted that the O2 production rate for the 0.1%RuO2/1%CuO/3%Ta2O5/SrZrO3 prevails as the highest without evident chemical changes after reaction (Figures S5 and S6, and Table S1). Overall, the results suggest the favorable effect of the cocatalyst and bicatalyst on promoting the kinetics of O2 evolution.[52]

Although the 0.1%RuO2:1%CuO/3%Ta2O5/SrZrO3 heterostructure prevails the highest, it is essential to reflect on the results from CuO, RuO2, and Pt carefully (Figure e). In this case, various loadings have been assessed (i.e., 0.1, 0.3, 0.5, 1, 1.3, and 1.5 wt %) for the three RuO2, CuO, and Pt cocatalysts, as shown in Figure e. We compare 3%Ta2O5/SrZrO3 (1297 μmol g–1 h–1) with 1 wt % RuO2. A nearly 3-fold increase (4986 μmol g–1 h–1) is achieved. As for the catalyst with 1 wt % CuO, a 2-fold increase (3282 μmol g–1 h–1) has been found. For Pt, a very low loading of ca. 0.1 wt % is required to obtain an activity close to 2744 μmol g–1 h–1, which is comparable to that of either 0.5 wt % CuO or 0.5 wt % RuO2. However, the H2 evolution activity of Pt decreases substantially comparable to that of catalysts with RuO2 and CuO loadings (i.e., 0.1 wt %). In all cases, a high cocatalyst content does not necessarily improve the production of H2 due to parasitic recombination losses as the amount of either CuO increases, that is, (>1 wt %), RuO2 (>1 wt %), or Pt (>0.1 wt %).[53] Additionally, high loadings can also promote the formation of large metal (metal oxide) particles or aggregates detrimental to the overall catalytic activity during water splitting.[22] Overall, the photocatalytic activity of 0.1 wt % CuO and 0.1 wt % RuO2 can be attributed to the strong electronic coupling with Ta2O5/SrZrO3, where hole–electron recombination might be reduced. To support our attribution, the photocatalytic activity of RuO2 and CuO has been measured. The H2 production rate for RuO2 and CuO remains low, ca. 14 and 26 μmol g–1 h–1. This indicates that Ta2O5/SrZrO3 provides the necessary transfer of charges to RuO2 or CuO, reaching the solid–liquid interface to promote H2 water splitting. To this end, an important aspect to highlight is the reduction of the use of noble catalysts such as Ru or Pt without compromising photocatalytic activity. Even if Ru is a less costly catalyst than Pt,[28] Ru usage can be reduced when combined with other catalysts, such as CuO. Therefore, the photocatalytic performance of binary cocatalysts composed of RuO2/CuO has also been assessed. Various RuO2 loadings, that is, 0.01 wt % (0.01%RuO2) and 1 wt % (1%RuO2), are incorporated to 1%CuO/Ta2O5/SrZrO3 (Figure c,d).

The QE at λ = 420 nm and the photocatalysts’ STH are calculated according to eqs and 2 to compare our heterostructures with other systems.[54] The efficiencies obtained are summarized in Table . The QE and STH of SrZrO3 are at the lowest end of the photocatalysts. The incorporation of 3%Ta2O5/SrZrO3 increases the QE and STH. Among the heterostructures containing either RuO2 or CuO, 1%RuO2/3%Ta2O5/SrZrO3 has superior performance, even better than the Pt cocatalyst. However, the RuO2 content is relatively high compared to 0.1%RuO2/1%CuO/3%Ta2O5/SrZrO3, which shows a similar if not even better QE and STH performances than 1%RuO2/3%Ta2O5/SrZrO3. The estimated QE and STH values of 0.1%RuO2/1%CuO/3%Ta2O5/SrZrO3 are 41 and 0.40%, which are competitive with either QE or STH values from other photocatalysts[54−60] and other perovskite heterostructure of high order (Table S2). For example, this is the case of the SrTiO3-based photocatalyst with a QE of 30% at λ = 360 nm.[57] Compared to bare and decorated SrZrO3 with Ni, Cu, Fe, and Co, our 0.1%RuO2/1%CuO/3%Ta2O5/SrZrO3 heterostructure surpasses the known STH values by nearly 4-fold.[8]

Table 2

Solar to Hydrogen Efficiency, STH, and Quantum Efficiency, QE, Obtained from the Experimental Results in Figure

material	STH (%)	QE (%) at 420 nm
SrZrO3	0.01	1.0
3%Ta2O5/SrZrO3	0.10	10
1%RuO2/3%Ta2O5/SrZrO3	0.39	39
1%CuxO/3%Ta2O5/SrZrO3	0.26	26
0.1%Pt/3%Ta2O5/SrZrO3	0.21	22
1%RuO2/1%CuxO/3%Ta2O5/SrZrO3	0.26	26
0.1%RuO2/1%CuxO/3%Ta2O5/SrZrO3	0.40	41
0.01%RuO2/1%CuxO/3%Ta2O5/SrZrO3	0.29	30

After assessing the overall water-splitting performance of the heterostructures, it is clear that the 0.1%RuO2/1%CuO/3%Ta2O5/SrZrO3 composition has the highest H2 or O2 production rate and STH. Regarding QE, 0.1%RuO2:1%CuO/3%Ta2O5/SrZrO3 has the highest among the synthesized SrZrO3 heterostructures.[8] The QE (Table ) of 0.1%RuO2/1%CuO/3%Ta2O5/SrZrO3 is comparable to, if not better, than other QE values reported for perovskite heterostructures shown in Table S2.

The next step is to understand the effect of the heterostructure component during charge transfer to provide a plausible picture of the water-splitting mechanism.

Donor Density and Charge Transfer Resistance in the RuO2/CuO/Ta2O5/SrZrO3 Heterostructure

EIS is used to obtain information on the conductivity type, flat band potential, and donor density in the photocatalysts through the Mott Schottky plots (Figure a). The samples exhibit a positive slope, evidencing the n-type conductivity. The donor density, Nd, has an inverse relationship with the capacitance through the Mott–Schottky formula, eq .[61]where C is the differential capacitance, ε is the dielectric constant of SrZrO3 (e = 60),[62] ε0 is the vacuum permittivity, e is the electron charge, Nd is the donor density, A is the active electrode area, V is the applied potential, VFB is the flat band potential, T is the temperature (in kelvin), and kB is the Boltzmann constant. The donor density is estimated using the Mott–Schottky plot slope, and a value of 60 is estimated for the dielectric constant of SrZrO3. These values are summarized in Table .

Figure 9

(a) Mott–Schottky plots (dark conditions, 10 kHz) and (b) photocurrent response of the photocatalysts at 0.3 V versus Ag/AgCl.

Table 3

Summary of the Donor Density Values Calculated from the Mott–Schottky Plots; The Results of This Table are Derived From Figure a

photocatalyst	Nd (cm–3)
SrZrO3	6.37 × 1015
3%Ta2O5/SrZrO3	3.59 × 1016
1%CuxO/3%Ta2O5/SrZrO3	3.78 × 1016
1%RuO2/3%Ta2O5/SrZrO3	4.26 × 1016
0.1%RuO2/1%CuxO/3%Ta2O5/SrZrO3	5.02 × 1017

In Table and Figure a, the donor density of SrZrO3 is affected by the incorporation of Ta2O5 and the different co-/bicatalysts. The addition of Ta2O5 increased the donor density from 6.37 × 1015 to 3.59 × 1016 cm–3. The donor density can be further improved with cocatalyst incorporation. For example, 1%CuO/3%Ta2O5/SrZrO3 has a donor density of 3.78–4.26 × 1016 cm–3, and 1%RuO2/3%Ta2O5/SrZrO3 has a similar donor density of ca. 4.26 × 1016 cm–3. Remarkably, the bicatalyst (0.1%RuO2/1%CuO) surpasses the obtained values for 1%CuO and 1%RuO with a donor density of ca. 5.02 × 1017 cm–3. This confirms our observations in Figure and indicates that the photoactivity of 3%Ta2O5/SrZrO3 can be tuned using 0.1%RuO2/1%CuO. Donor density mobility in the 0.1%RuO2/1%CuO/3%Ta2O5/SrZrO3 heterostructure can be associated with a reduction in charge recombination (Figure ).

To this end, transient photocurrent measurements are evaluated under simulated solar light (100 mW cm–2) to understand the photocatalyst response in Figure b. 0.1%RuO2/1%CuO/3%Ta2O5/SrZrO3 promoted the higher photoresponse associated with charge carrier separation in this heterostructure. This higher photocurrent is also attributed to the increase in light absorption. Light absorption around 250 nm or higher is improved, as shown in Figure c. Hence, one can assume that photogeneration of electrons and holes occurs more efficiently at the 0.1%RuO2:1%CuO/3%Ta2O5/SrZrO3 interface than in other photocatalysts, as shown in Table .

For insights into the reaction kinetics, impedance analyses are carried out. The semicircle in the impedance spectra in the Nyquist plots (Figure ) shows the charge transfer resistance. The diameter of the semicircle describes the reaction kinetics. A smaller diameter implies faster reaction kinetics. Figure also shows the corresponding equivalent circuit, where Rs is the resistance associated with the electric connection, electrolyte, and substrate. R1 is the charge transference resistance in the electrode–electrolyte interface, and CPE is the constant phase element (Table ). 0.1%RuO2/1%CuO/3%Ta2O5/SrZrO3 shows the smallest diameter among the other heterostructures and control (e.g., SrZrO3). This high-order heterostructure also exhibits the lowest R1 (ca. 1.97640 × 105 Ω), which indicates enhanced charge transport in the heterostructure when 0.1%RuO2/1%CuO and 3%Ta2O5/SrZrO3 are combined. Through this comparison, it is possible to show the beneficial effect on the charge transport kinetics of the 0.1%RuO2/1%CuO/3%Ta2O5/SrZrO3 heterostructure. It should be noted that the prepared electrodes show relatively high charge transfer resistance values due to the physical form of the catalyst, that is, the powder form. Low charge transfer resistance values are expected for denser layers, such as thin films.[63]

Figure 10

Nyquist plots for the prepared electrodes measured at OCP in 0.5 M Na2SO4 in a frequency range of 105–10–2 Hz under illumination.

Table 4

EIS Parameters from the Equivalent Circuit Fitting of Nyquist Plots of SrZrO3-Based Electrodes Measured in 0.5 M Na2SO4

sample	Rs (Ω)	R1 (Ω)	CPE1 (F)
SrZrO3	252.5	3.9 × 106	0.97
3%Ta2O5/SrZrO3	125.1	2.3 × 106	0.95
1%CuxO/3%Ta/SrZrO3	64.2	2.0 × 106	0.97
1%RuO2/3%Ta/SrZrO3	61.3	1.4 × 106	0.97
0.1%RuO2/1%CuxO/3%Ta/SrZrO3	59.4	1.9 × 105	0.97

Charge Transfer Mechanism

Mott–Schottky plots are used to estimate the flat band potential (Figure S7 and Table S3) by extrapolating the x-axis intercept of the linear plot (1/C2 vs E). A positive slope is characteristic of n-type semiconductors, and a negative slope is representative of p-type semiconductors. Note that the Fermi level and the majority charge carrier band [CB (ECB) for n-type and VB (EVB) for p-type] can vary approximately ±0.1 V versus. NHE.[61,64,65] Therefore, it is safe to say that the band energy diagram is estimated using the Mott–Schottky and the semiconductor band gap (Eg) values. These values are used in eq . Note that the Eg values for SrZrO3 and 3%Ta2O5/SrZrO3 are based on Figure . The band gaps of RuO2, CuO, Cu2O, and Ta2O5 are taken from the literature.[66−69] It should also be noted that the same values are used to construct SrZrO3-based heterostructures containing either Ta2O5, RuO2, or CuO shown in Figure S8. The results from Table S3 are used to understand the charge transfer mechanism (Figure ).

Figure 11

Charge transfer pathway for 0.1%Ru2O/1%CuO/3%Ta2O5/SrZrO3 under solar light irradiation.

The charge transfer mechanism in Figure is proposed for the 0.1%Ru2O/1%CuO/3%Ta2O5/SrZrO3 heterostructure to elucidate the possible charge pathways that led to high photocatalytic water splitting shown in Figure . It should be noted that other mechanisms might involve during charge transfer (e.g., Figure S9), but the mechanism in Figure might be the most plausible one. The structural, morphological, chemical, optical, and electrochemical characterization results are used to derive our proposition (Figure ). In this heterostructure, electrons are transferred from tantalum-doped strontium zirconate to Ta2O5 and Cu2O to overcome the evolution of H2. Meanwhile, the electrons in CuO move toward the RuO2 CB. After that, these electrons recombine with Cu2O holes. RuO2 holes are transferred to CuO, performing the O2 evolution reaction. Holes in Ta2O5 move to tantalum-doped strontium zirconate, where they carry out O2 evolution reactions (Figure ). For other heterostructures, the possible mechanism is presented in Figure S8.

Conclusions

SrZrO3-based heterostructures of mixed oxides are synthesized. The highest H2 production is ca. 5164 μmolg–1 h–1 for 0.1%RuO2/1%CuO/3%Ta2O5/SrZrO3, which is comparable if not even higher than that of SrZrO3 and reported QE values for other perovskite heterostructures. In-depth structural analysis revealed the presence of Ta2O5 in SrZrO3. Ta2O5 has been found segregating at the surface and grain boundaries of SrZrO3, which improved the photocatalytic activity in SrZrO3. Yet, the photocatalytic activity of Ta2O5/SrZrO3 is further improved with RuO2 or CuO as a cocatalyst or RuO2/CuO as a binary catalyst. An optimum activity for the RuO2/CuO heterostructure components has been found, surpassing RuO2 or Pt activity. DFT, structural, optical, and electrochemical characterization generates insights on band gap tunability for the different heterostructure components and demonstrates enhanced charge transfer for RuO2/CuO/Ta2O5/SrZrO3. The results are valuable in demonstrating that SrZrO3-based heterostructure can harvest visible light to improve the hydrogen evolution reaction.