The efficiency of sunlight-driven reduction of carbon dioxide (CO2), a process mimicking the photosynthesis in nature that integrates the light harvester and electrolysis cell to convert CO2 into valuable chemicals, is greatly limited by the sluggish kinetics of oxygen evolution in pH-neutral conditions. Current non-noble metal oxide catalysts developed to drive oxygen evolution in alkaline solution have poor performance in neutral solutions. Here we report a highly active and stable oxygen evolution catalyst in neutral pH, Brownmillerite Sr2GaCoO5, with the specific activity about one order of magnitude higher than that of widely used iridium oxide catalyst. Using Sr2GaCoO5 to catalyze oxygen evolution, the integrated CO2 reduction achieves the average solar-to-CO efficiency of 13.9% with no appreciable performance degradation in 19 h of operation. Our results not only set a record for the efficiency in sunlight-driven CO2 reduction, but open new opportunities towards the realization of practical CO2 reduction systems.
The increasing atmospheric carbon dioxide (CO2) level has alarmed the urgent demand of action to mitigate the substantial consequence on our climate. It promotes extensive interest in the development of green alternatives to fossil fuels. A promising approach to meet this challenge is to store solar energy in chemical bonds through sunlight-driven reduction of CO21. This process pairs two half-reactions of CO2 reduction (CO2R) and oxygen evolution reaction (OER) and powers the electrochemical cell using the photocurrents generated from one or more light absorbers. Significant improvements have been achieved in studying CO2R and OER in half-cells2,3, and various valuable carbon-based products have been synthesized in the lab demonstration of integrated devices, including carbon monoxide (CO), formate, hydrocarbons, and oxygenates4,5,6,7,8,9,10.
In the sunlight-driven electrolysis, the overall efficiency to convert solar energy into chemicals are critically determined by the factors of the performance of light absorber, the ohmic and Nernstian losses, and, the most importantly, the activity of catalysts to drive kinetically sluggish reactions11,12. For CO2R, the dissolution of CO2 in high pH solution forms less electrochemically active bicarbonate or carbonate and the reduction in low pH faces the competition with hydrogen evolution, hence restricting the most effective environment in neutral pH. On the other hand, for oxygen evolution non-noble metal oxide catalysts work most efficiently under strongly alkaline conditions and experience detrimental cation leaching that severely depresses the activity in neutral solution13. Furthermore, the accumulation of the leached metal species onto the cathode can be poisoning to CO2R catalyst; hence the cation leaching, even in trace amount, significantly affects the long-term stability of the integrated system7. Thus, searching an oxygen evolution catalyst with simultaneously high catalytic activity and compositional stability for integrated CO2 reduction in neutral pH remains a critical open challenge to improve the overall solar to fuel (STF) efficiency. Previous studies widely used noble metal oxide such as IrO2 to catalyze OER in neutral pH;4,5,6,14 but the moderate activity of IrO2 limited the STF efficiency below 7%11. Alternately, this challenge was circumvented by isolating CO2R and OER in different pH-valued solutions using bipolar membrane (BPM)8,9,10. Whereas the introduction of BPM allowed the operation of CO2R and OER in optimal environments to achieve higher STF efficiency over 10% and potentially benefited the separation of product gases, it not only caused additional membrane-derived voltage losses and raised extra complexity of optimization14,15,16, but the ion crossover due to imperfection of the BPM is still a concern for a long-term operation8.
Here, we report a significant improvement of STF efficiency enabled by the discovery of a highly active OER catalyst in neutral pH. The OER catalyst reported herein, Sr2GaCoO5 (SGC), belongs to the family of Brownmillerite oxides, with the general formula of ABO2.5 or A2B’BO5, where A is a larger sized cation, B and B’ are smaller cations octahedrally and tetrahedrally bonded to oxygen, respectively. As an oxygen-deficient derivative of perovskite, the crystalline structures of Brownmillerite oxides include several variations of oxygen vacancy ordering17,18. The compositional degree of freedom, as well as the structural polymorphism of Brownmillerite oxides, offers a great platform to tune the functionality in various oxygen-related applications, such as oxygen storage materials19, heterogeneous catalysts20,21 and oxygen-ion conductors;22,23 but the usage of these compounds as OER catalyst has seldom been explored24,25. In the current study, we found that SGC had the specific activity about one order of magnitude higher than that of IrO2 and showed superior durability without observable performance degradation in neutral pH. Paring the SGC anode and anodized silver (a-Ag) cathode and coupling the electrolysis cell with triple-junction GaInP/GaInAs/Ge solar cell in a BPM-free device, the integrated device achieved the average solar-to-CO efficiency of 13.9%, setting a record of STF for sunlight-driven CO2 reduction.
Synthesis and structure of SGC
The synthesis of SGC was carried out in a solid-state reaction route (see the Methods for more details). The Rietveld refinement of X-ray diffraction (XRD) pattern showed a pure orthorhombic Brownmillerite structure of space group Icmm for the as-synthesized product (Fig. 1a and see Supplementary Table 1 for the refined lattice parameters) with no XRD-detectable impurity. In the structure model, oxygen atom is missed from octahedral GaO6 in a normal perovskite, resulting in CoO6 octahedra and GaO4 tetrahedra stacked alternatingly, which are clearly visible in the high-angle annular dark-field scanning transmission electron microscopy (HAADF-STEM) image (Fig. 1b). Interestingly, the Rietveld refinement suggested nearly full occupancy of Co and Ga at B and B’ site, respectively, in contrast to the normally observed partial occupancies at both sites in other Brownmillerite oxides17,18. The full occupancy of Co at octahedral site reduced the distribution of cobalt in less active tetrahedral site26, hence improving the utilization of active species.
In a normal perovskite such as LaCoO3, cobalt is bound to six CoO6 units in a crystal field with an Oh-like symmetry, favoring a diamagnetic ground state of low spin (LS) Co3+ with six electrons in the t2g orbitals and empty eg states27,28. In the Brownmillerite SGC two of six surrounding CoO6 units are replaced by GaO4, lowering the Oh symmetry to D4h (Fig. 1c). As a result, the degeneracy of both the t2g and eg orbitals is broken (Fig. 1d), stabilizing the ground state of Co3+ in intermediate spin (IS, t2g5eg1) configuration29, as shown by the electronic structure calculations (Fig. 1d and Supplementary Fig. 1) and confirmed by the magnetization measurements (Supplementary Fig. 2). The stabilization of IS-Co3+ crucially benefits the OER activity as the occupancy of eg filling in Co3+ increases from theoretically zero in LS state to approaching the optimal value of ~1.2 for OER catalyst30,31,32. Furthermore, the Jahn-Teller effect caused by IS-Co3+ elongates Co–O bonds along  direction (2.26 Å versus 1.97 Å for Co–O bonds along (010) plane), lifting the corresponding oxygen p-state towards Fermi level (green area in Fig. 1d). Both these effects are positive to enhance the OER performance32,33,34. Using the computational hydrogen electrode method35, the activities of two cobalt-containing Brownmillerite oxides, SGC and Sr2AlCoO5 (SAC), were predicted in the proximity of the optimum of OER catalysts (Supplementary Figs. 3 and 4). In fully agreement with this theoretical picture, SGC and SAC showed remarkably high OER activities in alkaline solution (0.1 M KOH, pH 13, Supplementary Fig. 5). In particular, the overpotential (η) of SGC at the current density of 500 μA·cm−2oxide (normalized to the oxide surface areas from Brunauer–Emmett-Teller measurements, BET) was 0.33 V measured using a glassy carbon rotating disk electrode (GC-RDE), which was lower than several perovskite catalysts (0.35–0.41 V)36, and comparable to double perovskite (0.29–0.33 V) and recently reported CaCu3Fe4O12 catalyst (0.31 V, see Supplementary Figs. 6 and 7 for details)32,33,34.
The high OER activity of SGC persisted when the measurement was performed in pH-neutral solution, a mixture of 0.4 M NaH2PO4 and 0.6 M Na2SO4 with pH tuned to 7.0 by proper amount of NaOH. Due to the limited literature data on the OER activity in neutral solutions, we also measured the performance of the golden standard catalyst, IrO2, and thoroughly compared it to that of SGC. In the linear sweep voltammogram, SGC displayed an earlier onset potential and exhibited higher current density than commercial IrO2 toward oxygen evolution reaction (Fig. 2a). At the current density of 50 μA·cm−2oxide, the SGC required an η of 0.30 V, which was 0.07 V and about 0.18 V lower than that of IrO2 and a recently discovered NiCoFeP oxyhydroxide catalyst37, respectively. The iR-corrected Tafel plot of SGC and IrO2 further confirmed the higher intrinsic OER activity of SGC throughout the measured potential range (Fig. 2b). The fitted Tafel slope was 75 mV·decade−1 for SGC and 87 mV·decade−1 for IrO2, while the exchange current density of SGC was 5.5 × 10–6 mA·cm−2oxide, about two times higher than that of IrO2 (2.5 × 10−6 mA·cm−2oxide). Using these results, the intrinsic activity of SGC is about 7.8–18.3 times to that of IrO2 at the applied potential of 1.53–1.73 V vs RHE, and the mass activity is 2.0–4.8 times to that of IrO2. In Supplementary Fig. 8, the OER performance recorded in 0.1 M KHCO3 electrolyte showed only marginal difference with that in NaH2PO4/Na2SO4 solution, further demonstrating the intrinsically high OER activity of SGC in neutral conditions instead of being sensitive to the choice of electrolyte.
The OER performance of SGC was highly sustainable for a long-time operation, as shown in the cyclic voltammetry (CV), galvanostatic and potentiostatic tests (Fig. 2d–f). The current density at 1.65 V vs RHE was measured at 1.7 mA/cm2oxide with the retention after five hours of operation at 96%, demonstrating the superior stability to deliver high current at moderate overpotentials.
The comparison of pH 7 and pH 13 results showed that the OER performance of SGC barely depends on the pH value of electrolyte. At current densities no higher than 100 μA·cm−2oxide the overpotential in pH 7 solution was only 0.01–0.02 V higher than that in pH 13 (Fig. 2f). For comparison, the η of IrO2 in pH 7 was 0.05–0.07 V higher than those in pH 13 in the same current density range. Even at the current density of 500 μA·cm−2oxide (10.5 mA·cm−2geo) the measured η of SGC was only 0.04 V higher in pH 7 solution. This weak pH-dependence of η was seldom observed in other perovskite catalysts. For example, for perovskite Ba0.5Sr0.5Co0.8Fe0.2O3-δ, LaMO3 (M=Mn, Fe, Co, and Ni) and double perovskite PrBaCo2O5+δ, the OER activities are severely reduced due to the detrimental dissolution of cations in neutral pH even at the current density as low as 5 μA·cm−2oxide13, resulting in the increase of η by over 0.1–0.3 V compared to that in alkali conditions13,38. As Tsuji et al. reported, the OER activity of Brownmillerite-type Ca2FeCoO5 was strongly affected by the concentration of KOH solution25. Another Brownmillerite oxide studied in the current work, SAC, had the overpotential increased by ~0.03 V in neutral pH at low current densities, but exhibited a large increase of η at 100 μA·cm−2oxide (Fig. 2f and Supplementary Figs. 9–11), which signaled severe performance degradation at moderate to high current densities. Therefore, the observed weak pH-dependence of η should be related to both the Brownmillerite structure and the unique composition of SGC.
While the GC-RDE setup allowed us to firmly establish the intrinsic activity and stability of SGC for oxygen evolution in neutral solution, we also evaluated the potential of using SGC towards practical applications. To do this we drop-casted the catalyst ink on a carbon paper electrode and measured the performance in a three-electrode setup. For the catalyst loading of 1 mg·cm−2geo, the measured overpotential was 0.38 V at the current density of 10 mA·cm−2geo and barely changed in the testing of 72 h (Supplementary Fig. 12). Due to the mass transfer resistance in the porous electrode, this value was about 0.05 V higher than that estimated from the GC-RDE measurements. Increasing the loading effectively decreased the overpotential at the same current density. For the loading of 3 mg·cm−2geo37, the overpotential was reduced to 0.35 V, only 0.02 V higher than the NiCoFeP oxyhydroxide catalyst. Even at a high current density of 100 mA·cm−2geo, the voltages remained highly stable with an increase of less than 0.015 V in the testing of 32 h. While engineering the loading and electrode structure to optimize the performance will be left to future work, these results clearly demonstrated the remarkable performance of SGC in conditions for practical applications.
These results highlighted an intrinsically high, sustainable and weakly pH-dependent performance of SGC to catalyze oxygen evolution. To shed light on these observations, we conducted the X-ray photoelectron spectroscopy (XPS) studies to probe the effect of OER operation on the chemical states of cations in SGC. Whereas the XPS spectra clearly showed the surface adsorption of hydroxyl groups after soaking the sample in the electrolyte for four hours or after 100 CV cycles (Supplementary Fig. 13), little difference was observed for Sr, Co, and Ga signals after contacting the aqueous electrolyte see Fig. 3a. More importantly, the XPS spectra collected on the fresh surface and after Ar+ etching for ~10 nanometers (16 min, assuming an etching rate of around 0.5−1 nm/min39) did not exhibit any appreciable difference on metal signals, indicating no evidence for surface reconstruction beyond XPS-detectable level that tuned the chemical state of active species for OER activity as observed in other Co-based OER catalysts40,41,42,43,44. By integrating the area of the Co 2p and Ga 2p peak, the quantitative difference between the cation contents on the surface and in the bulk was estimated to be less than 5% (Supplementary Fig. 14), which was likely within the instrumental accuracy of estimating elemental content with XPS spectra. Therefore, the XPS results suggested that SGC must be chemically stable against possible OER-induced structural and compositional changes in neutral solutions. On the contrary, the XPS spectra of SAC showed the decrease of Al signals on the surface of CV cycled sample (Fig. 3b), suggesting the appreciable dissolution of Al during the OER operation.
To further study the influence of OER operation on the surface and bulk structure of SGC, we investigated the crystalline structures using high-resolution transmission electron microscopy (HRTEM). Well crystallized surface was observed for as-synthesized samples. After 100 CV cycles in neutral pH, the particle remained high crystallinity with lattice fringes extending to the surface (Fig. 3c and additional images in Supplementary Fig. 15). Based on the energy dispersive spectroscopy (EDS), we found that the OER operation did not introduce any appreciable difference on the surface composition than simply soaking SGC in the electrolyte (Fig. 3e and Supplementary Tables 2–4), in consistent with the XPS results. These results confirmed the high structural and compositional stability of SGC during OER operation in neutral environment. On the contrary, apparent amorphous layer coated on the crystalline SAC particles was observed after CV cycling in neutral pH (Fig. 3d). In consistent with the XPS results shown in Fig. 3c, d, the EDS showed a statistically significant decrease of Al amount in the surface layer (Fig. 3f and Supplementary Tables 5–7), therefore attributing the amorphourization to Al-dissolution induced destruction of crystalline surface.
Combining the XPS, HRTEM, and EDS results provided the mechanistic picture of the high OER performance of SGC in neutral solution. Due to the presence of IS-Co3+ ions in their Brownmillerite structures, both SGC and SAC have intrinsically high activity towards oxygen evolution in alkaline solutions. However, in neutral solutions, only SGC maintains the active crystalline surface for oxygen evolution while the surface of SAC experiences Al-leaching induced amorphourization. Consequently, the activity of SAC showed appreciable degradation in neutral solution especially at high current conditions, while the performance of SGC is highly sustainable and nearly pH-independent. Considering the compositional and structural similarity between SGC and SAC, the difference in stability is attributed to the thermodynamic driving force of dissolving aluminum oxide and gallium oxide at the OER operation condition in neutral pH, as indicated by the wider range of stability for solid gallium oxide in the computational Pourbaix diagrams (Supplementary Figs. 16–18). We note that this simple argument does not consider the complexity brought by the co-existence of Sr and Co or the kinetics of cation leaching. A detailed mechanistic picture for the stability of Brownmillerite oxides in neutral-pH OER should be the key subject of future studies.
Sunlight-driven CO2 reduction
We then proceeded the evaluation by pairing the SGC anode for OER and a-Ag cathode for CO2R in an BPM-free electrolysis cell, as illustrated in Supplementary Fig. 19. We used a-Ag for its high selectivity towards CO generation under a moderate overpotential around 0.5 V45. Taken into account the overpotentials for both electrodes, an operating voltage around 2.2 V is expected., A triple junction of GaInP/GaInAs/Ge photovoltaic with an open-circuit voltage of 2.51 V was therefore used to effectively drive the electrolysis. The room temperature current density–voltage (J–V) profile of the triple junction intersected with the J–V curves of the electrochemical system close to the maximum power point of solar-to-electric energy conversion (Fig. 4a), allowing effective conversion of solar energy into electricity. For comparison, using the same solar cell and a-Ag cathode but commercial IrO2 anode for OER, the J–V curves intersected farther from the maximum power point at lower current densities, leading to poorer utilization of solar energy for conversion (Supplementary Fig. 20).
The high compositional stability of SGC in neutral solution reduced the possible metal ion contamination on CO2-reduction cathode, allowing the sustainable operation without necessarily refreshing the electrolyte for a long period. We, therefore, carried out the electrolysis over the total course of 19 h, the longest time of operation in the sunlight-driven CO2 reduction and far exceeding those employing non-noble metal catalysts for OER in neutral-pH solutions7,37. The integrated system delivered a nearly constant current density of 11.9 mA·cm−2 at an average voltage of 2.26 V (Fig. 4b). The current and voltage fluctuated less than 6% and 3%, respectively, not only confirming the stable performance of the BPM-free device but also reflecting the superior stability of both electrodes under real operating conditions. By monitoring the electrode potential using reference Ag/AgCl electrode, the average iR-uncorrected overpotential was estimated to be 0.56 and 0.37 V at the a-Ag cathode and SGC anode, respectively. Considering the extra mass transfer resistance and the Ohmic loss in the integrated device, both values were in good agreement with those estimated from the half-cell measurements (Supplementary Fig. 21), indicating little performance degradation from the integration of half-cells. For comparison, devices using BPM to isolate CO2R and OER in different pH-valued solutions had extra voltage losses in the order of 0.2–0.5 V due to the resistance of BPM and the necessary overpotential for water dissociation8,10.
The Faraday efficiency for CO generation varied between 85% and 89% and the average value in the 19-h period of operation was 87.2%. The solar-to-CO conversion (STFCO) efficiency was peaked at 14.4% and the average over 19 h was 13.9%. Taking into account both products of CO and H2, the STF efficiency peaked at 16.3% and the average was 15.6%. For comparison, using IrO2 anode for OER, the STFCO efficiency was 9.7% and the STF efficiency was 10.9% after 5 h of operation, about 30% less than the same device using SGC anode. Using IrO2 anode, oxidized gold electrode cathode and perovskite solar cell, Schreier et al. achieved solar to CO efficiency of 6.5%4. Therefore, we may attribute the usage of triple junction solar cell and a-Ag cathode in current study contributed to ~3% of efficiency improvement, while using SGC for OER further improved the efficiency by ~4%. Table 1 summarizes the current results in comparison with previous studies of sunlight-driven CO2 reduction devices. Compared to other experimental results, the STF was improved by at least 130% compared to IrO2-involved systems, and 12% for BMP-based devices, hence setting the benchmark record for future improvements.
While developing high-performed OER catalysts in neutral solution has become a hurdle in realizing a practical CO2-reduction system, our results suggested the critical role of controlling the stability of catalyst in neutral conditions to achieve a highly active and sustainable oxygen evolution. In addition to Sr2GaCoO5 and Sr2AlCoO5, we screened several other A2BB’O5 type Brownmillerite oxides with A=Ca or Sr, B=Mn, Fe or Co, and B’=Ga or Al for oxygen evolution without attempting to optimize the recorded performance. The results summarized in Supplementary Table 8 suggested good potential of Brownmillerite oxides to catalyze oxygen-related reactions. Because the current work studied the activity of as-synthesized stoichiometric Sr2GaCoO5 crystallized in micron-sized particles (Supplementary Fig. 22), it is optimistic to expect further improving activity through strategies established from other perovskite family of catalysts46. In addition, the discovery of SGC as a highly active neutral-pH OER catalyst enables the pairing with various catalysts for efficient BPM-free CO2 reduction (Supplementary Note 1). Examples to generate possible products such as formate, hydrocarbon and oxygenate are assessed in the Supplementary Figure 23. The examination of these devices is therefore of great interest towards the realization of practical sunlight-driven CO2 reduction systems.
Density functional theory (DFT) calculations
DFT calculations were performed with the Vienna ab initio Simulation Package (VASP) using projector-augmented waves (PAW) pseudopotentials and the exchange-correlation functionals parametrized by Perdew, Burke, and Ernzerhof for the generalized gradient approximation (GGA)47,48,49. Numerical convergence to about 2 meV per formula unit was ensured by using a cutoff energy 520.0 eV and appropriate Gamma centered k-point meshes. The electronic structure was calculated using GGA+U method with the U value set as 3.3 for Co. The adsorption of OER intermediates (OH, O, and OOH) was evaluated on the Co-exposed (010) plane of Sr2GaCoO5 and Sr2AlCoO5. To mitigate the interaction between periodic images, a vacuum layer of 15 Å thickness was applied in the supercell.
Materials synthesis and characterization
To synthesize Sr2GaCoO5, stoichiometric amounts of SrCO3, Ga2O3, and Co3O
4 (all 99.9%, from Sigma Aldrich) were ball milled together and placed in an alumina crucible for the calcination at 1100 °C for 24 h. The mixtures were carefully ground in a mortar, followed by sintering at 1100 °C for 216 h with 3 intermediate re-grounding. The as-synthesized product was then ball-milled. The synthesis of Sr2AlCoO5 followed the same procedure using stoichiometric amount of SrCO3, Al2O3 and Co3O4 as the precursors and the sintering was carried out at 1250 °C for total 288 h with 4 intermediate re-grounding. The X-ray diffraction was collected using a Rigaku Smart Lab diffractometer equipped with a Cu Kα radiation (λ = 1.54178 Å) source at a scan rate of 0.1°/minute. Rietveld refinement of the XRD data was performed using the GSAS/EXPGUI package. X-ray photoelectron spectroscopy (XPS) spectra were collected with a PHI 5000 VersaProbe II X-ray photoelectron spectrometer using an Al Kα source. The X-ray parameter conditions were 15 kV, 25 W, pass energy of 23.5 eV and at a resolution of 0.2 eV/step. The sample was mounted on double-sided carbon tape and tilted at 45 degrees. An alternating Ar+ ion source was used for sputtering at 1 kV. The HRTEM study was performed using a JEM-2200FS high-resolution transmission electronic microscope with an in-column energy filter operated at 200 kV. The energy dispersive spectroscopy was taken with the Oxford INCA system at the energy resolution of 140 eV. High-angle annular dark-field scanning transmission electron microscopy imaging was carried out on a FEI Titan80–300 S/TEM microscope equipped with a probe spherical aberration corrector and the operation voltage was 300 kV. The collection angles of the annular dark-field detector for the inner and outer were 55 and 220 mrad, respectively. The magnetization measurements were performed using Magnetic Property Measurement System (MPMS) by Quantum Design.
Oxygen evolution reaction
To prepare the electrode for oxygen evolution, a catalyst ink was first prepared by sonicating a mixture of active catalyst (Sr2GaCoO5 after ball milling or commercial IrO2 purchased from Alfa Aesar, 99.99%), acid-treated carbon black (CB, Alfa Aesar), Na+-exchanged Nafion® solution (5 wt%, Ion Power) in tetrahydofuran (THF, Sigma-Aldrich), and then drop-casted (10 μL) onto pre-polished glassy carbon disk electrodes (5 mm in diameter, Pine Instruments)42. The catalyst film was dried at room temperature for 12 h and the final composition of the film was 250, 50, and 50 µg/cm2 for the catalyst, CB, and Nafion®, respectively.
The OER experiments in neutral pH used the CO2-saturated solution of 0.4 M NaH2PO4 and 0.6 M Na2SO4 and proper amount of NaOH that tuned the pH to 7.0. The tests were performed at room temperature in three-electrode cells using a VSP multichannel potentiostat (Bio-logic). The counter electrode was a Pt coil isolated from the main electrochemical cell using a fritted glass tube. The working electrodes rotated at 1600 rpm using a rotating disc electrode system (Pine Instruments). Cyclic voltammetry (CV) was reported at a scan rate of 10 mV/s while linear sweep voltammogram (LSV) was performed at 1 mV/s. The potentials were measured versus a Ag/AgCl (4 M KCl) reference electrode. Except otherwise mentioned, all the potentials reported in the paper was corrected for IR drop and converted to the reference hydrogen electrode (RHE). The current density was evaluated based on the BET surface area of the catalyst
where I is the measured current, A is the total surface area of the catalyst, m is the amount of catalyst on the electrode and SBET is the BET surface area. The BET current density can be converted to the geometric current density
where Ageo is the geometric area of the electrode.
Sunlight-driven CO2 reduction
To prepare the Sr2GaCoO5 anode for the test of CO2 reduction, a catalyst ink was prepared in the same way as described above and was subsequently drop-coated onto a carbon paper (FuelCellStore). The total apparent electrode size was 1.1 cm2 and the loading of Sr2GaCoO5 was 1 mg·cm−2. The anodized Ag electrodes were prepared from a silver foil (Alfa Aesar, 99.998%, 0.25 mm in thickness) polished and sonicated with deionized water before anodization. The anodization was conducted was carried out at 0.6 V potential for a total charge of 5.5 coulombs using platinum counter electrode, Ag/AgCl reference electrode and 0.1 M NaNO3 electrolyte. The apparent electrode sizes for the anode and cathode were the same.
Sunlight-driven CO2 reduction experiments were carried out in a prototype cell integrating a triple-junction GaInP/GaInAs/Ge photovoltaic cell (SpectroLab) and a two-chamber electrolyzer. The two electrodes were separated by a Nafion®117 membrane and only the product gases from a-Ag electrode was collected. The area of the photovoltaic cell was 0.555 × 0.555 cm (0.308 cm2). Before the electrochemical test, the PV characteristics of the photovoltaic cell was measured. The short circuit current was 0.0041 A. The current and voltage at the maximum power point was 0.0039 A and 2.255 V, respectively, corresponding to the maximum efficiency of 28.5% under 1 sun irradiation. The electrolytes were first saturated with CO2 for 30 min before the electrolysis. Gas phase product was sampled from the headspace of the cathode cell chamber using a gas-tight syringe (Hamilton) periodically every half an hour. A Thermo Scientific Trace GC Ultra gas chromatograph equipped with a VICI pulsed discharge detector and SUPELCO CarboxenTM 1010 PLOT column was used to determine the amount of H2 and CO in the product. Ultra-pure (>99.999%) helium was used as carrier gas.
The data that support the findings of this study are available from the corresponding author upon request.
Goeppert, A., Czaun, M., Prakash, G. K. S. & Olah, G. A. Air as the renewable carbon source of the future: an overview of CO2 capture from the atmosphere. Energy Environ. Sci. 5, 7833–7853 (2012).
Qiao, J., Liu, Y., Hong, F. & Zhang, J. A review of catalysts for the electroreduction of carbon dioxide to produce low-carbon fuels. Chem. Soc. Rev. 43, 631–675 (2014).
Suen, N. T. et al. Electrocatalysis for the oxygen evolution reaction: recent development and future perspectives. Chem. Soc. Rev. 46, 337–365 (2017).
Schreier, M. et al. Efficient photosynthesis of carbon monoxide from CO2 using perovskite photovoltaics. Nat. Commun. 6, 7326 (2015).
Gurudayal et al. Efficient solar-driven electrochemical CO2 reduction to hydrocarbons and oxygenates. Energy Environ. Sci. 10, 2222–2230 (2017).
Arai, T., Sato, S. & Morikawa, T. Monolithic device for CO2 photoreduction to generate liquid organic substances in a single-compartment reactor. Energy Environ. Sci. 8, 1998–2002 (2015).
Jiang, K. et al. Transition-metal single atoms in a graphene shell as active centers for highly efficient artificial photosynthesis. Chem 3, 950–960 (2017).
Schreier, M. et al. Solar conversion of CO2 to CO using Earth-abundant electrocatalysts prepared by atomic layer modification of CuO. Nat. Energy 2, 17087 (2017).
Urbain, F. et al. A prototype reactor for highly selective solar-driven CO2 reduction to synthesis gas using nanosized earth-abundant catalysts and silicon photovoltaics. Energy Environ. Sci. 10, 2256–2266 (2017).
Zhou, X. et al. Solar-driven reduction of 1 atm of CO2 to formate at 10% energy-conversion efficiency by use of a TiO2-protected III–V tandem photoanode in conjunction with a bipolar membrane and a Pd/C Cathode. ACS Energy Lett. 1, 764–770 (2016).
Singh, M. R., Clark, E. L. & Bell, A. T. Thermodynamic and achievable efficiencies for solar-driven electrochemical reduction of carbon dioxide to transportation fuels. Proc. Natl Acad. Sci. USA 112, E6111–E6118 (2015).
Winkler, M. T., Cox, C. R., Nocera, D. G. & Buonassisi, T. Modeling integrated photovoltaic–electrochemical devices using steady-state equivalent circuits. Proc. Natl Acad. Sci. USA 110, E1076–E1082 (2013).
Han, B. et al. Activity and stability trends of perovskite oxides for oxygen evolution catalysis at neutral pH. Phys. Chem. Chem. Phys. 17, 22576–22580 (2015).
Sriramagiri, G. et al. Toward a practical solar-driven CO2 flow cell electrolyzer: designand optimization. ACS Sustain. Chem. Eng. 5, 10959–10966 (2017).
Chabi, S., Papadantonakis, K. M., Lewis, N. S. & Freund, M. S. Membranes for artificial photosynthesis. Energy Environ. Sci. 10, 1320–1338 (2017).
Li, Y. C. et al. Electrolysis of CO2 to syngas in bipolar membrane-based electrochemical cells. ACS Energy Lett. 1, 1149–1153 (2016).
Anderson, M. T., Vaughey, J. T. & Poeppelmeier, K. R. Structural similarities among oxygen-deficient perovskites. Chem. Mater. 5, 151–165 (1993).
D'Hondt, H. et al. Tetrahedral chain order in the Sr2Fe2O5 Brownmillerite. Chem. Mater. 20, 7188–7194 (2008).
Motohashi, T. et al. Oxygen storage capability of Brownmillerite-type Ca2AlMnO5+δ and its application to oxygen enrichment. Chem. Mater. 25, 372–377 (2013).
Jeen, H. et al. Orienting oxygen vacancies for fast catalytic reaction. Adv. Mater. 25, 6459–6463 (2013).
Jee, H. et al. Reversible redox reactions in an epitaxially stabilized SrCoOx oxygen sponge. Nat. Mater. 12, 1057–1063 (2013).
Goodenough, J. B., Ruiz-Diaz, J. E. & Zhen, Y. S. Oxide-ion conduction in Ba2In2O5 and Ba3In2MO8 (M=Ce, Hf, or Zr). Solid State Ion. 44, 21–31 (1990).
Paulus, W. et al. Lattice dynamics to trigger low temperature oxygen mobility in solid oxide ion conductors. J. Am. Chem. Soc. 130, 16080–16085 (2008).
Ling, C., Zhang, R. & Jia, H. Quantum chemical design of doped Ca2MnAlO5+δ as oxygen storage media. ACS Appl. Mater. Interfaces 7, 14518–14527 (2015).
Tsuji, E. et al. Brownmillerite-type Ca2FeCoO5 as a practicable oxygen evolution reaction catalyst. ChemSusChem 10, 2864–2868 (2017).
Wei, C. et al. Cations in octahedral sites: a descriptor for oxygen electrocatalysis on transition‐metal spinels. Adv. Mater. 29, 1606800 (2017).
Korotin, M. A., Ezhov, S. Y., Solovyev, I. V. & Anisimov, V. I. Intermediate-spin state and properties of LaCoO3. Phys. Rev. B 54, 5309–5316 (1996).
Knížk, K. et al. Structure and physical properties of YCoO3 at temperatures up to 1000 K. Phys. Rev. B 73, 214443 (2006).
Qian, D. et al. Electronic spin transition in nanosize stoichiometric lithium cobalt oxide. J. Am. Chem. Soc. 134, 6096–6099 (2012).
Tong, Y. et al. Spin-state regulation of perovskite cobaltite to realize enhanced oxygen evolution activity. Chem 3, 812–821 (2017).
Zhou, S. et al. Engineering electrocatalytic activity in nanosized perovskite cobaltite through surface spin-state transition. Nat. Commun. 7, 11510 (2015).
Suntivich, J., May, K. J., Gasteiger, H. A., Goodenough, J. B. & Shao-Horn, Y. A perovskite oxide optimized for oxygen evolution catalysis from molecular orbital principles. Science 334, 1383–1385 (2011).
Grimaud, A. et al. Double perovskites as a family of highly active catalysts for oxygen evolution in alkaline solution. Nat. Commun. 4, 2439 (2013).
Yagi, S. et al. Covalency-reinforced oxygen evolution reaction catalyst. Nat. Commun. 6, 8249 (2015).
Man, I. C. et al. Universality in oxygen evolution electrocatalysis on oxide surfaces. ChemCatChem 3, 11591–11165 (2011).
Wei, C. et al. Recommended practices and benchmark activity for hydrogen and oxygen electrocatalysis in water splitting and fuel cells. Adv. Mater. 31, 1806296 (2018).
Zheng, X. et al. Theory-driven design of high-valence metal sites for water oxidation confirmed using in situ soft X-ray absorption. Nat. Chem. 10, 149-154 (2017).
McCrory, C. C. L., Jung, S., Peters, J. C. & Jaramillo, T. F. Benchmarking heterogeneous electrocatalysts for the oxygen evolution reaction. J. Am. Chem. Soc. 135, 16977–16987 (2013).
Zhang, R. & Ling, C. Unveil the chemistry of olivine FePO4 as magnesium battery cathode. ACS Appl. Mater. Interfaces 8, 18018–18026 (2016).
Burke, M. S., Kast, M. G., Trotochaud, L. & Smith, A. M. Cobalt−iron (oxy)hydroxide oxygen evolution electrocatalysts: the role of structure and composition on activity, stability, and mechanism. J. Am. Chem. Soc. 137, 3638–3648 (2015).
May, K. J. et al. Influence of oxygen evolution during water oxidation on the surface of perovskite oxide catalysts. J. Phys. Chem. Lett. 3, 3264–3270 (2012).
Jia, H. et al. Different catalytic behavior of amorphous and crystalline cobalt tungstate for electrochemical water oxidation. RSC Adv. 2, 10874–10881 (2012).
Fabbri, E. et al. Dynamic surface self-reconstruction is the key of highly active perovskite nano-electrocatalysts for water splitting. Nat. Mater. 16, 925–931 (2017).
Grimaud, A. et al. Activating lattice oxygen redox reactions in metal oxides to catalyse oxygen evolution. Nat. Chem. 9, 457–465 (2017).
Zhou, L. Q., Ling, C., Jones, M. & Jia, H. Selective CO2 reduction on a polycrystalline Ag electrode enhanced by anodization treatment. Chem. Commun. 51, 17704–17707 (2015).
Chen, D., Chen, C., Baiyee, Z. M., Shao, Z. & Ciucci, F. Nonstoichiometric oxides as low-cost and highly-efficient oxygen reduction/evolution catalysts for low-temperature electrochemical devices. Chem. Rev. 115, 9869–9921 (2015).
Kresse, G. & Furthmuller, J. Efficient Iterative schemes for ab initio total-energy calculations using a plane-wave basis set. Phys. Rev. B 54, 11169–11186 (1996).
Kresse, G. & Hafner, J. Ab initio molecular-dynamics simulation of the liquid-metal–amorphous-semiconductor transition in germanium. Phys. Rev. B 49, 14251–14269 (1994).
Kresse, G. & Joubert, D. From ultrasoft pseudopotentials to the projector augmented-wave method. Phys. Rev. B 59, 1758–1775 (1999).
C.M.W. thanks the support of LDRD of Pacific Northwest National Laboratory for carrying out part of the TEM work, which was carried in the William R. Wiley Environmental Molecular Sciences Laboratory (EMSL), a national scientific user facility sponsored by DOE’s Office of Biological and Environmental Research and located at PNNL. PNNL is operated by Battelle for the Department of Energy under Contract DE-AC05–76RLO1830. H.Z. and M.S.W. thank the support of NECCES, an Energy Frontier Research Center funded by the U.S. Department of Energy, Office of Science, Office of Basic Energy Sciences under Award Number DE-SC0012583. C.-W.C. acknowledges support by the U.S. Air Force Office of Scientific Research under Grant No. FA9550-15-1-0236, the T.L.L. Temple Foundation, the John J. and Rebecca Moores Endowment, and the State of Texas through the Texas Center for Superconductivity at the University of Houston. Y.Y. thanks the support of Scialog: Advanced Energy Storage award from Research Corporation for Science Advancement (award number 25751), UH Technical Gap Fund, and UH High Priority Area Large Equipment Grant.
The authors declare no competing interests.
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