In this study, the S-LFP-derived slag (HS-LFP) catalyst was prepared by acid leaching [Supplementary Figure 1]. Initially, S-LFP battery black powder was selected as the starting material. The S-LFP cathode black powder was obtained from discarded commercial LFP batteries provided by Changzhou Liyuan New Energy Technology Co., Ltd. Prior to processing, the spent batteries were fully discharged in 1 mol L^-1 NaCl solution to a cut-off voltage of 0.5 V to eliminate residual electrical charge and ensure operational safety. After discharge, impurities were removed via mechanical dismantling and thermal treatment. The cathode was calcined at 350 °C for 2 h under an air atmosphere to remove residual organic binders and carbonaceous additives, and the LFP powder was scraped off the aluminum current collector. Subsequently, the collected powder was subjected to acid leaching in 2 mol L^-1 HCl solution at room temperature for 10 min using a solid-liquid ratio of 0.1 g mL^-1, aiming to liberate lithium (Li) from the S-LFP framework. The Li recovery efficiency was quantified by ICP-OES based on the Li contents in the initial S-LFP powder and the acid-leached solid residue HS-LFP. The Li content decreased from 1.62 mmol g^-1 in S-LFP to 0.08 mmol g^-1 in HS-LFP, giving a Li recovery/removal efficiency of 95.06% according to [(1.62 - 0.08)/1.62] × 100%. The remaining precipitate was collected by filtration, repeatedly washed with deionized water and ethanol to remove residual acid and soluble impurities, and then dried at 60 °C for 4 h to obtain the Li-extracted slag, which is the HS-LFP employed in subsequent experiments.

The schematic illustrations and graphical abstract were created by the authors using Photoshop, Adobe Illustrator, and Microsoft PowerPoint. Data plots were prepared using OriginPro. Structural models and DFT-related images were visualized using VESTA. Microscopy images were processed only for standard presentation purposes, such as cropping, scale-bar labeling, and brightness/contrast adjustment, using ImageJ. This information has been added to the manuscript as requested.

To clarify the structural evolution of the S-LFP-derived slag (HS-LFP) and identify the nature of its active centers, X-ray diffraction (XRD), transmission electron microscopy (TEM), scanning electron microscopy (SEM), energy dispersive X-ray spectroscopy (EDS), high-angle annular dark-field imaging (HAADF), and X-ray photoelectron spectroscopy (XPS) characterizations were conducted and systematically compared with S-LFP and commercial LFP and FePO₄ (FP).

As shown in Figure 2A, both LFP and S-LFP exhibit the characteristic diffraction features of olivine structure. The diffraction peak positions of S-LFP remain consistent with the standard pattern, while the attenuated peak intensity compared with that of LFP indicates partial loss of crystallinity after cycling. FP displays sharp and well-defined diffraction peaks, characteristic of a highly crystalline phase with long-range structural order. In contrast, HS-LFP shows no obvious diffraction features assignable to either LiFePO₄ or highly crystalline FePO₄, but only weak and broadened reflections, indicating substantial disruption of the long-range order of the parent lattice during acid leaching. A broad peak at around 26°, assigned to the graphite (002) plane, is also observed, originating from the carbon matrix. SEM [Supplementary Figure 2] reveals distinct morphological differences. LFP shows uniform spherical particles, while pure FP exhibits dense irregular bulks. In contrast, HS-LFP displays broken, rough-surfaced fragments, confirming acid-leaching-induced structural reconstruction rather than simple delithiation to S-LFP.

TEM images further show that S-LFP and HS-LFP exhibit significant differences in their microstructures. S-LFP primarily consists of relatively large flake- or lump-like particles with distinct boundaries, and its overall structure is relatively dense [Supplementary Figure 3]; high-resolution TEM images [Supplementary Figure 4] still reveal locally ordered regions. Fast Fourier transform (FFT) analysis of the selected area [Supplementary Figure 5A] gives an interplanar spacing of approximately 0.29 nm, which can be assigned to the (121) plane of an LiFePO₄-related structure, indicating that the material retains a relatively intact crystal framework even after service. In contrast, HS-LFP exhibits an irregular, agglomerated, loose flake-like/flocculent structure with blurred particle edges [Figure 2B], accompanied by distinct fracturing features, reflecting the significant disruption of the original particle structure caused by the acid leaching process. In its HRTEM images [Figure 2C], most regions lack continuous lattice striations, with only a few short-range ordered regions remaining. FFT analysis [Supplementary Figure 5B] of the enlarged local region gives an interplanar spacing of approximately 0.327 nm, which can be assigned to the (102) plane of a FePO₄-related structure, indicating that minor local FePO₄ structural motifs are retained despite the destruction of long-range crystallinity. Meanwhile, another local region exhibits no discernible lattice fringes and is characteristic of a disordered domain. Combined with the XRD results, these observations confirm that the HS-LFP catalyst is not a uniform crystalline material, but a reconstructed system consisting of a disordered matrix and short-range ordered FePO₄ structural units.

The dispersion state of Fe sites was further examined by HAADF-STEM [Figure 2D]. No obvious Fe-based nanoparticles or clusters were detected; instead, uniformly dispersed isolated bright dots were observed on the reconstructed matrix. Given the Z-contrast mechanism of HAADF imaging, these observations suggest the presence of atomically dispersed Fe species. Elemental mapping [Supplementary Figure 6] further confirms that Fe atoms are homogeneously dispersed and closely co-localized with O species, supporting the presence of highly dispersed Fe species coordinated with surrounding oxygen species, without observable Fe aggregation at the nanoscale. Collectively, these results suggest that acid-leaching-induced reconstruction stabilizes highly dispersed Fe-O_x species on the carbon-containing framework rather than inducing particle aggregation. XPS further reveals the chemical environment of the Fe centers [Figure 2E and F and Supplementary Figures 7 and 8]. Relative to S-LFP, HS-LFP exhibits a weakened Li 1s signal, indicating partial surface delithiation after acid leaching. The Fe 2p spectrum evolves from predominantly Fe²⁺ in S-LFP to a Fe³⁺-enriched state in HS-LFP, together with residual Fe²⁺ and satellite features, evidencing delithiation-induced oxidation and electronic reconstruction of Fe sites. Meanwhile, the retained phosphate-region P 2p signal and the dominant PO_x/FeO_x component in O 1s indicate that Fe remains anchored in an oxygen-coordinated phosphate matrix. The coexistence of Fe²⁺/Fe³⁺ species suggests multiple local Fe-O coordination environments, and the Fe³⁺-enriched state of HS-LFP suggests substantial reconstruction of the local Fe-O coordination environment, possibly involving under-coordinated Fe species. Combined with the HRTEM and HAADF-STEM results, these data indicate that the Fe centers are stably anchored in oxygen-coordinated phosphate frameworks featuring coexisting short-range order and disorder regions. These observations are consistent with highly dispersed Fe-O_x species embedded in a heterogeneous Fe-P-O coordination environment, rather than a single uniform Fe coordination state.

In addition, EDS elemental mapping provides further evidence for the spatial distribution of elements. Compared with S-LFP [Supplementary Figures 9 and 10], the HS-LFP [Supplementary Figures 11-13] exhibits Fe, P, and Al loss and homogeneous distributions of Fe throughout the selected region, indicating good compositional uniformity of the framework. In particular, the Fe signal does not show localized aggregation, in agreement with the atomically dispersed Fe identified by HAADF-STEM. Elemental analysis of C and F further reveals an increased carbon content in HS-LFP (rising from 4.636% to 11.051%), which corroborates the retention of the carbon framework [Supplementary Figure 14].

Taken together, acid-leaching-induced Li extraction transforms S-LFP from its original long-range ordered olivine framework into a reconstructed structure composed of a disordered matrix with residual short-range ordered FePO₄-related units and highly dispersed Fe-O_x species. This architecture is fundamentally different from the regular bulk coordination environment in both S-LFP and LFP. The coexistence of structural disorder, short-range FePO₄-related domains, and highly dispersed Fe-O_x species is expected to increase the accessibility of Fe electrocatalytic centers and to reconstruct the local Fe-O-P coordination environment.

Prior to evaluating the NO₃^-RR performance, the textural properties of HS-LFP were examined. The Li-extracted slag exhibits a dramatically enlarged specific surface area and porous structure. According to the N₂ adsorption-desorption results [Supplementary Figure 15], the specific surface area of HS-LFP reaches 139.00 m² g^-1, markedly higher than those of S-LFP (44.80 m² g^-1), FP (0.58 m² g^-1), and LFP (9.39 m² g^-1). This order-of-magnitude increase indicates that acid-leaching-induced reconstruction markedly increases the accessible surface area and interfacial exposure of the reconstructed Fe-P-O framework. Combined with the structural characterization, this enlarged surface is expected to expose more catalytically accessible Fe-O_x sites, thereby providing an important structural basis for enhanced reactant adsorption, electron transfer, and interfacial reaction kinetics during NO₃^-RR.

To evaluate the intrinsic electrocatalytic activity of different iron phosphate-based materials toward nitrate reduction, linear sweep voltammetry (LSV) measurements were first carried out in 1 M KOH and 1 M KOH + 0.1 M KNO₃ [Figure 3A]. All three electrodes display enhanced cathodic responses after the introduction of NO₃^-, indicating the participation of nitrate species in the cathodic reduction process. Notably, compared with FP and LFP, the HS-LFP electrode exhibits a more positive onset potential [-0.05 V vs. reversible hydrogen electrode (RHE)] and delivers consistently higher reduction current densities over the entire potential range, with a more pronounced current enhancement in the nitrate-containing electrolyte. This result clearly suggests a stronger intrinsic catalytic activity of HS-LFP toward electrochemical NO₃^- reduction. To further clarify the kinetic origin of the outstanding catalytic behavior, electrochemical impedance spectroscopy (EIS) measurements were carried out. As shown in Figure 3B, the Nyquist plots reveal distinct differences in charge-transfer properties among the electrodes. Compared with FP and LFP, the HS-LFP electrode displays a smaller semicircle diameter, indicative of a lower charge-transfer resistance (R_ct) and faster interfacial electron transfer. A smaller R_ct means that the electron-coupled conversion of NO₃^- and its intermediates proceeds more readily on the electrode surface, which is particularly beneficial for the overall kinetics of this multi-electron reduction reaction. The electrochemically active surface area (ECSA) was estimated from the double-layer capacitance derived from cyclic voltammetry (CV) measurements [Figure 3C and Supplementary Figure 16]. The HS-LFP electrode exhibits the largest increase in capacitive current density with increasing scan rate, corresponding to the highest electrochemical double-layer capacitance (C_dl), which indicates a larger ECSA and thus more exposed real catalytic sites. This result is in excellent agreement with the specific surface area measurements, suggesting that the active sites generated after Li extraction not only provide a much larger physical surface area but also translate electrochemically into more accessible and operative interfacial active regions. Taken together, the LSV, EIS, and C_dl results suggest that the superior NO₃^-RR performance of HS-LFP arises from the reconstructed Fe-O/P coordination environments, the increased exposure of electrochemically accessible Fe-O_x sites within the heterogeneous Fe-P-O framework, and improved interfacial charge transfer.

As shown in Figure 3D, during continuous electrolysis from -0.2 to -0.6 V vs. RHE, the current density at each potential remains generally stable with time after a short initial transient decay. This initial decrease is commonly associated with double-layer rearrangement, gradual establishment of surface adsorbates, and stabilization of the local mass-transfer environment; the step-like fluctuations observed at -0.6 V vs. RHE are likely associated with bubble nucleation/detachment under high cathodic current density. In particular, near -0.4 V vs. RHE, the current response remains stable, and the current density reaches ~ 200 mA cm^-2, which is close to industrial scale, indicating that the HS-LFP electrode can sustain a relatively stable interfacial reaction state and continuous electron transfer process under NO₃^-RR. The step-like fluctuations in the -0.6 V curve arise from periodic H₂ bubble formation and detachment on the electrode surface under high cathodic potential, which temporarily alters the active area and local mass transport. This stable electrochemical behavior provides kinetic support for its simultaneously high Faradaic Efficiency (FE) and NH₃ yield. Prior to product quantification, the concentrations of NO₃^-, NO₂^-, and NH₄⁺ were calibrated by ultraviolet-visible spectroscopy (UV-Vis) spectrophotometry using the corresponding standard curves [Supplementary Figure 17]. The high linear correlation coefficients (R² ≥ 0.998) confirm the reliability of the detection method for subsequent performance calculations. Selectivity and ammonia production capability of the three electrodes were then quantitatively compared through product analysis. The HS-LFP electrode exhibits a superior FE(NH₃) over the most investigated potential range relative to the reference electrodes [Figure 3E]. In particular, at -0.4 V vs. RHE, the FE(NH₃) of HS-LFP reaches 98.28%, which is significantly higher than those of LFP and FP at the same potential. This result indicates that HS-LFP substantially suppresses the competing hydrogen evolution reaction (HER) under these conditions and directs electrons preferentially toward the NH₃ formation pathway. It is worth noting that further negative shifting of the potential to -0.5 and -0.6 V leads to a decrease in FE(NH₃) of HS-LFP (from 80.8% to 62.0%). This trend generally suggests that at higher overpotentials, interfacial HER begins to compete more strongly for active sites and electron supply, thereby compromising ammonia selectivity. In contrast, although LFP/FP also exhibit a certain degree of NH₃ selectivity at some potentials, their overall FE values remain clearly lower than that of HS-LFP. Consistent with the potential-dependent FE trend, the NH₃ yield results shown in Figure 3F further verify the performance advantage of HS-LFP. As the applied potential shifts from -0.2 to -0.6 V vs. RHE, the NH₃ yield of all three electrodes gradually increases, indicating that a more negative potential is beneficial for enhancing the overall reduction rate of NO₃^-RR. Importantly, the HS-LFP electrode maintains the highest NH₃ production rate throughout the entire potential window and achieves an ammonia yield of 14,232 μg h^-1 mg_cat^-1 at -0.4 V vs. RHE, together with an FE(NH₃) of 98.28%, demonstrating the optimal balance between activity and selectivity. Although the NH₃ yield can still increase at more negative potentials, the accompanying decline in FE indicates that the system gradually departs from the optimal selectivity window. Therefore, -0.4 V vs. RHE can be identified as the optimal operating potential for efficient NO₃^--to-NH₃ conversion on the HS-LFP electrode.

Finally, the NO₃^--to-NH₃ performance of the HS-LFP electrode was compared with representative catalysts reported in the literature [Supplementary Table 1 and Figure 3G]. The results show that HS-LFP can achieve a FENH₃ as high as 98.28% and an ammonia yield of 14,232 μg h^-1 mg_cat^-1 in a mild alkaline electrolyte, which compares favorably with many representative catalysts reported under comparable conditions. The ability to selectively generate NH₃ at a high rate is particularly meaningful because ammonia can function as a hydrogen carrier for future carbon-free energy systems. Considering that HS-LFP is derived from the Li-extraction slag generated during S-LFP recycling, this result not only demonstrates that the discarded iron phosphate fraction can be transformed from a low-value solid waste into a high-value electrocatalyst, but also highlights that Li-deficient reconstruction and interfacial engineering can effectively unlock the catalytic potential of Fe-O₄/Fe-O₆/FePO₄ sites in waste slags for NO₃^- reduction.

To clarify the origin of NH₃ formation and the intrinsic catalytic mechanism of HS-LFP toward nitrate electroreduction, a series of isotope-labeling, in situ spectroscopic, and theoretical analyses were carried out. As shown in Supplementary Figure 18, negligible NH₃ was produced when using a blank carbon paper (CP) electrode in the presence of NO₃^- or when using the HS-LFP catalyst in a nitrate-free electrolyte. The high ammonia yield was only achieved when both the HS-LFP catalyst and NO₃^- ions were present, ruling out the possibility of nitrogen contamination from the environment or catalyst decomposition. This was further corroborated by ¹⁵N isotope labeling experiments [Figure 4A]. The hydrogen-1 nuclear magnetic resonance (¹H NMR) spectrum of the electrolyte after electrolysis with ¹⁵NO₃^- as the nitrogen source exhibited a distinct doublet characteristic of ¹⁵NH₄⁺, while a triplet was observed when ¹⁴NO₃^- was used. The isotope-tracing observations confirm that the synthesized ammonia originates exclusively from the electroreduction of NO₃^-. The regulation of hydrogen-related intermediates is an important factor in achieving high FE for NO₃^-RR. We utilized electron paramagnetic resonance (EPR) spectroscopy with DMPO as a spin-trapping agent to monitor the behavior of reactive hydrogen species at the catalyst interface [Figure 4B]. In the nitrate-free electrolyte, a robust 1:2:2:1 quadruple signal characteristic of DMPO-H was observed, indicating the accumulation of DMPO-detectable hydrogen-related species on the electrode surface. Conversely, upon the introduction of NO₃^-, the DMPO-H signal intensity drastically diminished. This decrease indicates that DMPO-detectable hydrogen-related species no longer accumulate to a measurable level under NO₃⁻RR conditions. However, this signal decrease should not be interpreted solely as direct evidence of H* consumption, because competitive adsorption or site blocking by NO₃^-/nitrate-derived intermediates may also suppress the steady-state generation or accumulation of hydrogen-related species. Therefore, the EPR results suggest that, in the presence of NO₃^-, hydrogen-related intermediates are preferentially involved in nitrate hydrogenation and/or prevented from accumulating because of nitrate-related surface adsorption processes, thereby contributing to the high NH₃ selectivity.

The evolution of adsorbed intermediates was monitored by in situ FTIR spectroscopy under different applied potentials [Figure 4C]. As cathodic polarization increases, the spectral features of nitrate-derived species evolve continuously, indicating a potential-dependent transformation of surface adsorbates/intermediates during the NO₃^-RR process. Based on prior in situ FTIR studies, the bands observed at around 1,090, 1,160, 1,236, 1,349 and 1,479 cm^-1 can be tentatively associated with nitrate-reduction-related surface species, including N-O stretching / NH₂OH-related species, NO₂^--related vibrations, NO₃^--related vibrations and NH₄⁺/NH₃ -related deformation modes. The broad feature near 1,638 cm^-1 may also include a significant contribution from the bending vibration of interfacial H₂O. Therefore, some of these assignments should be regarded as tentative because overlap from interfacial water, hydroxyl species, electrolyte-derived species, and the phosphate-containing catalyst framework cannot be fully excluded. Nevertheless, the overall spectral evolution supports a stepwise nitrate-to-ammonia conversion pathway involving multiple oxygenated and hydrogenated nitrogen intermediates^[49-52].

To elucidate the structural origin of the exceptional catalytic performance of HS-LFP, particularly the possible synergy among highly dispersed Fe-O_x sites and neighboring FePO₄ motifs within the reconstructed framework, DFT calculations were performed using two representative structural models, namely, a FePO₄ model and a heterogeneous FeO₄/FeO₆/FePO₄ model. The latter is not intended to represent the exact structure of HS-LFP, but rather an experimentally constrained local coordination model. This choice is based on the combined characterization results: XRD and HRTEM indicate that HS-LFP mainly consists of a disordered matrix with residual short-range ordered FePO₄ domains, while HAADF-STEM and XPS suggest highly dispersed Fe species embedded in heterogeneous Fe-O/P coordination environments with multiple Fe valence/coordinative states. Therefore, the FePO₄ unit was used to represent the retained short-range ordered phosphate-related motif, and the FeO₄ and FeO₆ units were introduced to mimic the coexistence of low-coordinated and relatively saturated Fe-O sites in the reconstructed matrix. This model was thus designed to capture the essential local coordination heterogeneity and the possible electronic synergy among adjacent Fe-O motifs in HS-LFP [Figure 4D]. It should also be noted that the graphene support used in the calculation is an idealized conductive carbon model rather than an exact representation of the carbon phase in the real electrode. The experimental carbon environment contains both disordered carbon components and relatively more graphitized carbon paper. Therefore, the calculations are mainly used to reveal qualitative electronic-structure trends of the Fe-O-P active motif at a conductive interface, while possible quantitative effects from the real non-ideal carbon support cannot be fully excluded. The charge-density-difference results further support the above conclusion. As shown in Figure 4E, the yellow and blue colors represent electron accumulation and electron depletion, respectively. Upon adsorption, pronounced charge redistribution is observed around the Fe-O₄ sites and their adjacent coordination environment, indicating strong interfacial electronic coupling between the adsorbate and catalyst surface. Notably, the Fe-O₄/Fe-O₆/FePO₄ model exhibits a larger magnitude of charge transfer upon adsorption (-1.03 e^-) than the reference model (-0.80 e^-), suggesting a more substantial electron reorganization induced by adsorption. This result suggests that neighboring Fe-O₆ sites can modulate the local electronic environment of low-coordination Fe sites through a cooperative effect. Such localized charge polarization is expected to facilitate the activation of nitrate-derived species and optimize the adsorption strength of key intermediates, thereby promoting the overall reaction kinetics. This electronic modulation is also reflected in the projected density of states (PDOS) results [Figure 4F]. For the FePO₄ model, the d-band center is located at -1.71 eV, whereas for the FeO₄/FeO₆/FePO₄ model, it shifts upward to -1.40 eV, closer to the Fermi level (E_F = 0 eV). The upshift of the d-band center indicates that the reconstructed coordination-synergistic structure endows the Fe-O₄ site with a more suitable electronic configuration for interacting with nitrate-derived intermediates, thereby enhancing intermediate adsorption and activation and facilitating subsequent conversion steps. The adsorption-energy comparison shown in Figure 4G provides additional evidence for this synergistic effect. The FeO₄/FeO₆/FePO₄ model exhibits a more favorable adsorption energy of -0.92 eV, significantly lower than that of the FePO₄ model (-0.36 eV), indicating stronger interaction with nitrate-related species. This result suggests that the Fe-O₄-centered synergistic configuration is more capable of capturing and activating nitrate at the initial stage of the reaction. The calculated free-energy profiles further reveal the origin of the improved catalytic performance [Figure 4H]. Both models follow a multistep pathway involving *NO₃, *NO₂, *NO, *NOH, *NHOH, *NH₂OH, *NH₂, and *NH₃ intermediates before the final NH₃ release [Supplementary Figures 19 and 20]. Notably, the FeO₄/FeO₆/FePO₄ model consistently exhibits a lower free-energy profile than the FePO₄ model, especially for the uphill hydrogenation step associated with the formation of *NOH. This step is identified as the rate-determining step, and the corresponding energy barrier decreases from 1.8802 eV on FePO₄ to 1.718 eV on the Fe-O₄-centered synergistic model.

Overall, the mechanistic results collectively demonstrate that the excellent NO₃^-RR performance of HS-LFP is attributed to reconstructed Fe-O_x active sites within a heterogeneous Fe-P-O coordination environment, together with electronic synergy from adjacent coordination motifs. In the model, the Fe-O₄ site acts as the primary catalytic center for nitrate adsorption and conversion, while the surrounding Fe-O₆/FePO₄ environment tunes its charge distribution, shifts the d-band center toward the Fermi level, strengthens nitrate adsorption, and reduces the rate-determining barrier from 1.8802 to 1.718 eV. This coordination-synergistic mechanism provides a clear explanation for the enhanced activity and selectivity of HS-LFP toward ammonia electrosynthesis from nitrate.

Ammonia is an important value-added chemical and a promising hydrogen carrier. Therefore, the practical performance of HS-LFP for ammonia production requires further verification. Since HS-LFP possesses high intrinsic activity and favorable interfacial regulation for nitrate reduction, we further evaluated its performance in terms of continuous-flow compatibility, cycling durability, stability, and techno-economic feasibility. As illustrated in Figure 5A, a flow-cell system was constructed to evaluate the application potential of HS-LFP for electrocatalytic nitrate-to-ammonia conversion. The corresponding current-density response over 30 successive cycles is provided in Supplementary Figure 21 (with the cycle number on the x-axis), showing that HS-LFP maintains a stable cathodic current throughout repeated operations. As shown in Supplementary Figures 22-24, the bright isolated contrast features assigned to atomically dispersed Fe species are still clearly observed after the cycle-stability test, and no obvious Fe aggregation, nanoparticle formation, or phase segregation is detected. Meanwhile, XRD and XPS analyses demonstrate that no obvious degradation occurs to the catalyst upon repeated stability testing, with the chemical environment of Fe largely preserved [Supplementary Figures 25-27]. Moreover, the catalyst does not lose its nitrate reduction capability at 100 ppm; rather, it still sustains a measurable and non-negligible NH₃ selectivity even when the nitrate concentration is reduced to the millimolar level [Supplementary Figure 28].

A photograph of the assembled flow-cell system is shown in Supplementary Figure 29. In this configuration, nitrate-containing wastewater is continuously supplied to the cathode compartment, where HS-LFP serves as the NO₃^-RR catalyst, while the anodic side drives the oxygen evolution reaction. This design highlights a direct utilization route of S-LFP-derived HS-LFP for continuous nitrate conversion.

The operational robustness of the HS-LFP catalytic system and its resistance to competitive ions were first assessed by a 30-cycle test in simulated wastewater containing 1 M KOH, 0.1 M KNO₃, 0.1 M KCl, and 0.1 M K₂SO₄ at a constant potential of -0.4 V vs. RHE. As shown in Figure 5B, both the FE(NH₃) and NH₃ yield remain highly stable over repeated cycling, with the FE maintained at around 95% and the ammonia yield rate remaining nearly unchanged throughout 30 consecutive runs. These results indicate that HS-LFP possesses good tolerance to representative coexisting anions such as chloride and sulfate under the tested conditions and can sustain stable nitrate reduction performance in complex electrolyte environments. To further assess its durability under continuous operation, HS-LFP was examined in the flow-cell mode over extended electrolysis.

As shown in Figure 5C, the FE(NH₃) remains at a high level during the initial stage of continuous operation and shows a moderate decline after prolonged electrolysis. This decline is likely related to the combined effects of bulk nitrate consumption, progressively enhanced interfacial mass-transport limitation, and local microenvironment variation during sustained operation, rather than solely reflecting intrinsic catalyst deactivation. As nitrate is continuously consumed, insufficient nitrate replenishment near the catalyst surface weakens the kinetic advantage of NO₃^- RR over HER, leading to a gradual decrease in NH₃ selectivity.

Beyond electrochemical performance, HS-LFP also exhibits low-cost preparation potential. As shown in Supplementary Figure 30 and Figure 5D, the estimated cost of HS-LFP is approximately 0.01 USD g^-1 when considering direct preparation cost only. This value represents a theoretical lower-bound estimate rather than a full production cost, as it excludes battery collection, disassembly, waste neutralization, labor, and capital-related expenses. Therefore, the comparison with literature-reported Fe-N-C/metal-organic framework (MOF) and Fe-N-C/single-atom catalyst (SAC) catalysts should be interpreted with caution because of the different accounting boundaries. Even under more conservative assumptions that include waste neutralization and minimum manual handling (see Supplementary Materials), HS-LFP still retains a clear feedstock-cost advantage owing to the near-zero raw material cost of the S-LFP-derived slag. These results highlight the economic attractiveness of waste-derived HS-LFP as a catalyst platform for nitrate-to-ammonia electrosynthesis.