milerssliu/battery-device-data-qa huggingface dataset:
The electrocatalytic application of HEA NPs in the selective CO2 reduction reaction (CO2RR) has also been reported recently. For example, Nellaiappan et al. reported quinary fcc-AuPtAgPdCu NPs as an efficient CO2RR electrocatalyst toward CH4 and C2H4 in the low overpotential region. The five elements in the quinary HEA NPs were homogeneously distributed, whose chemical environments adopt metallic characteristics determined by XPS analysis except for Cu; a small amount of Cu2+ content was observed. The quinary fcc-AuPtAgPdCu NPs obtained superior selectivity toward the CO2RR in the low overpotential region, that is, FEmethane = 38.2% and FEethylene = 29.5% at −0.9 VAg/AgCl (−0.3 VRHE) in a CO2-saturated 0.5 M K2SO4 electrolyte (FE: faradaic efficiency). Based on their DFT calculation, the excellent electrocatalytic activity toward the CO2RR has mainly originated from redox-active Cu content in AuPtAgPdCu, while other elements provide an additional synergy in the CO2RR. Also, the long-term stability of the catalyst was verified by a chronoamperometry test for 5 h in a CO2-saturated 0.5 M K2SO4 electrolyte.

Question: What's the electrolyte?
Answer: 0.5 M K2SO4
The electrocatalytic application of HEA NPs in the selective CO2 reduction reaction (CO2RR) has also been reported recently. For example, Nellaiappan et al. reported quinary fcc-AuPtAgPdCu NPs as an efficient CO2RR electrocatalyst toward CH4 and C2H4 in the low overpotential region. The five elements in the quinary HEA NPs were homogeneously distributed, whose chemical environments adopt metallic characteristics determined by XPS analysis except for Cu; a small amount of Cu2+ content was observed. The quinary fcc-AuPtAgPdCu NPs obtained superior selectivity toward the CO2RR in the low overpotential region, that is, FEmethane = 38.2% and FEethylene = 29.5% at −0.9 VAg/AgCl (−0.3 VRHE) in a CO2-saturated 0.5 M K2SO4 electrolyte (FE: faradaic efficiency). Based on their DFT calculation, the excellent electrocatalytic activity toward the CO2RR has mainly originated from redox-active Cu content in AuPtAgPdCu, while other elements provide an additional synergy in the CO2RR. Also, the long-term stability of the catalyst was verified by a chronoamperometry test for 5 h in a CO2-saturated 0.5 M K2SO4 electrolyte.

Question: What's the electrolyte?
Answer: CO2-saturated 0.5 M K2SO4
The concentration of 7Li electrolyte as a function of time is, ce7(t) = [Li+]fe7(t) with the initial condition for the fraction of 7Li in the electrolyte, fe7(0) = 0.92 (the natural abundance of 7Li). Since the diffusion coefficient in lithium metal, Dm, is more than four orders of magnitude smaller than the diffusion Li+ coefficient in the electrolyte (Table 1), the diffusion of Li+ throughout the electrolyte is considered instantaneous.

Question: What's the electrolyte?
The Li3V2(PO4)3 (LVP) electrode slurry was prepared by mixing LVP, carbon black (Super P), and polyvinylidene fluoride (PVDF) in a weight ratio of 8:1:1 in N-methyl pyrrolidone (NMP); this slurry was coated on the Al foil followed by drying at 120 °C for 24 h. Then, the electrodes were cut into disks with a diameter of 14.0 mm and used for coin cell assembly. The mass loading of the LVP electrodes was 2.3–2.6 mg cm−2. The primary batteries (CR2016, coin-type cell) were assembled using the Li3V2(PO4)3 cathode, Celgard 2325 separator, electrolytes, and Li metal anode in an argon-filled glove box.

Question: What's the cathode?
Answer: Li3V2(PO4)3
The Li3V2(PO4)3 (LVP) electrode slurry was prepared by mixing LVP, carbon black (Super P), and polyvinylidene fluoride (PVDF) in a weight ratio of 8:1:1 in N-methyl pyrrolidone (NMP); this slurry was coated on the Al foil followed by drying at 120 °C for 24 h. Then, the electrodes were cut into disks with a diameter of 14.0 mm and used for coin cell assembly. The mass loading of the LVP electrodes was 2.3–2.6 mg cm−2. The primary batteries (CR2016, coin-type cell) were assembled using the Li3V2(PO4)3 cathode, Celgard 2325 separator, electrolytes, and Li metal anode in an argon-filled glove box.

Question: What's the anode?
Answer:  Li metal
The Li3V2(PO4)3 (LVP) electrode slurry was prepared by mixing LVP, carbon black (Super P), and polyvinylidene fluoride (PVDF) in a weight ratio of 8:1:1 in N-methyl pyrrolidone (NMP); this slurry was coated on the Al foil followed by drying at 120 °C for 24 h. Then, the electrodes were cut into disks with a diameter of 14.0 mm and used for coin cell assembly. The mass loading of the LVP electrodes was 2.3–2.6 mg cm−2. The primary batteries (CR2016, coin-type cell) were assembled using the Li3V2(PO4)3 cathode, Celgard 2325 separator, electrolytes, and Li metal anode in an argon-filled glove box.

Question: What's the electrolyte?
Fig. 4c shows the electrochemical impendence spectra of the full cell in the Na–H2O–urea–DMF electrolyte before cycling, after the first cycle and after 100 cycles. The Rs value of the battery in the Na–H2O–urea–DMF electrolyte, connected to the intercept on the real impedance axis at a high frequency in the EIS spectra, is relatively small and equal for the pristine state and after cycling, which suggests good ion diffusion in the electrolyte and good stability of the electrode materials before and after cycling. The Rct value represented the charge transfer resistance increase after the first cycle and after 100 cycles, indicating that a passivation layer may be formed on the NTP anode, which could be a significant factor in the improvement of the cycling performance of the NVP/NTP full cell. Moreover, the XRD patterns (Fig. S16†) and SEM images (Fig. S17†) of NVP/C and NTP/C before and after 500 cycles were recorded, respectively. The results indicate that the Na–H2O–urea–DMF electrolyte is conducive to achieving excellent stability of the NVP cathode. In addition, a NiHCF//NTP full cell displays 80% capacity retention after 2000 cycles at 2C rate (Fig. 4d).

Question: What's the cathode?
Answer: NVP
Fig. 4c shows the electrochemical impendence spectra of the full cell in the Na–H2O–urea–DMF electrolyte before cycling, after the first cycle and after 100 cycles. The Rs value of the battery in the Na–H2O–urea–DMF electrolyte, connected to the intercept on the real impedance axis at a high frequency in the EIS spectra, is relatively small and equal for the pristine state and after cycling, which suggests good ion diffusion in the electrolyte and good stability of the electrode materials before and after cycling. The Rct value represented the charge transfer resistance increase after the first cycle and after 100 cycles, indicating that a passivation layer may be formed on the NTP anode, which could be a significant factor in the improvement of the cycling performance of the NVP/NTP full cell. Moreover, the XRD patterns (Fig. S16†) and SEM images (Fig. S17†) of NVP/C and NTP/C before and after 500 cycles were recorded, respectively. The results indicate that the Na–H2O–urea–DMF electrolyte is conducive to achieving excellent stability of the NVP cathode. In addition, a NiHCF//NTP full cell displays 80% capacity retention after 2000 cycles at 2C rate (Fig. 4d).

Question: What's the anode?
Answer: NTP
Fig. 4c shows the electrochemical impendence spectra of the full cell in the Na–H2O–urea–DMF electrolyte before cycling, after the first cycle and after 100 cycles. The Rs value of the battery in the Na–H2O–urea–DMF electrolyte, connected to the intercept on the real impedance axis at a high frequency in the EIS spectra, is relatively small and equal for the pristine state and after cycling, which suggests good ion diffusion in the electrolyte and good stability of the electrode materials before and after cycling. The Rct value represented the charge transfer resistance increase after the first cycle and after 100 cycles, indicating that a passivation layer may be formed on the NTP anode, which could be a significant factor in the improvement of the cycling performance of the NVP/NTP full cell. Moreover, the XRD patterns (Fig. S16†) and SEM images (Fig. S17†) of NVP/C and NTP/C before and after 500 cycles were recorded, respectively. The results indicate that the Na–H2O–urea–DMF electrolyte is conducive to achieving excellent stability of the NVP cathode. In addition, a NiHCF//NTP full cell displays 80% capacity retention after 2000 cycles at 2C rate (Fig. 4d).

Question: What's the electrolyte?
Answer: Na–H2O–urea–DMF
Herein, we report a new finding that 3Mg/Mg2Sn alloy can be a promising solution to the aforementioned issues in Sn-based alloy-type MIB anodes. It is shown that 3Mg/Mg2Sn, which is composed of ternary phases (crystalline Mg-rich (c-Mg), amorphous Mg-rich (a-Mg), and intermetallic Mg2Sn phases), reversibly magnesiates/de-magnesiates a significant amount of Mg2+ ions in a non-Grignard and Lewis acid-free electrolyte even under high rates of C/D. In Table 1, the unprecedented electrochemical performance of 3Mg/Mg2Sn is compared with that of other popular alloy-type anodes. The origin of high capacities and excellent rate-capabilities is also discussed in the context of structural features. Finally, we describe the compatibility of 3Mg/Mg2Sn with versatile conventional electrolytes and the optimality of using 3Mg/Mg2Sn with Mg2+-trapping cathodes (e.g., Mo6S8).

Question: What's the cathode?
Answer: Mo6S8
Herein, we report a new finding that 3Mg/Mg2Sn alloy can be a promising solution to the aforementioned issues in Sn-based alloy-type MIB anodes. It is shown that 3Mg/Mg2Sn, which is composed of ternary phases (crystalline Mg-rich (c-Mg), amorphous Mg-rich (a-Mg), and intermetallic Mg2Sn phases), reversibly magnesiates/de-magnesiates a significant amount of Mg2+ ions in a non-Grignard and Lewis acid-free electrolyte even under high rates of C/D. In Table 1, the unprecedented electrochemical performance of 3Mg/Mg2Sn is compared with that of other popular alloy-type anodes. The origin of high capacities and excellent rate-capabilities is also discussed in the context of structural features. Finally, we describe the compatibility of 3Mg/Mg2Sn with versatile conventional electrolytes and the optimality of using 3Mg/Mg2Sn with Mg2+-trapping cathodes (e.g., Mo6S8).

Question: What's the anode?
Answer: Sn-based alloy-type MIB
Herein, we report a new finding that 3Mg/Mg2Sn alloy can be a promising solution to the aforementioned issues in Sn-based alloy-type MIB anodes. It is shown that 3Mg/Mg2Sn, which is composed of ternary phases (crystalline Mg-rich (c-Mg), amorphous Mg-rich (a-Mg), and intermetallic Mg2Sn phases), reversibly magnesiates/de-magnesiates a significant amount of Mg2+ ions in a non-Grignard and Lewis acid-free electrolyte even under high rates of C/D. In Table 1, the unprecedented electrochemical performance of 3Mg/Mg2Sn is compared with that of other popular alloy-type anodes. The origin of high capacities and excellent rate-capabilities is also discussed in the context of structural features. Finally, we describe the compatibility of 3Mg/Mg2Sn with versatile conventional electrolytes and the optimality of using 3Mg/Mg2Sn with Mg2+-trapping cathodes (e.g., Mo6S8).

Question: What's the electrolyte?
Answer: non-Grignard and Lewis acid-free
Herein, we report a new finding that 3Mg/Mg2Sn alloy can be a promising solution to the aforementioned issues in Sn-based alloy-type MIB anodes. It is shown that 3Mg/Mg2Sn, which is composed of ternary phases (crystalline Mg-rich (c-Mg), amorphous Mg-rich (a-Mg), and intermetallic Mg2Sn phases), reversibly magnesiates/de-magnesiates a significant amount of Mg2+ ions in a non-Grignard and Lewis acid-free electrolyte even under high rates of C/D. In Table 1, the unprecedented electrochemical performance of 3Mg/Mg2Sn is compared with that of other popular alloy-type anodes. The origin of high capacities and excellent rate-capabilities is also discussed in the context of structural features. Finally, we describe the compatibility of 3Mg/Mg2Sn with versatile conventional electrolytes and the optimality of using 3Mg/Mg2Sn with Mg2+-trapping cathodes (e.g., Mo6S8).

Question: What's the anode?
Answer:  alloy-type
To elucidate the practical applicability, HSABs were assembled using metallic Na as the anode immersed in 1 M NaClO4 in TEGDME organic electrolyte, NASICON solid electrolyte as the separator, O2-saturated 0.1 M NaOH aqueous as the aqueous electrolyte, Pt3Ni1/NixFe LDHs, 20% Pt/C, and RuO2 loaded on Ni foam as the cathode (Fig. 1a). During the discharge process, the Na metal on the anode side is oxidized to Na+ and moves into the NaOH aqueous through the NASICON separator, and the ORR simultaneously occurs at the cathode. On charging, the Na+ ions were transported from the aqueous electrolyte into the anode chamber and reduced to metallic Na, together with the concurrent OER at the cathode side.

Question: What's the cathode?
Answer: RuO2 loaded on Ni foam
To elucidate the practical applicability, HSABs were assembled using metallic Na as the anode immersed in 1 M NaClO4 in TEGDME organic electrolyte, NASICON solid electrolyte as the separator, O2-saturated 0.1 M NaOH aqueous as the aqueous electrolyte, Pt3Ni1/NixFe LDHs, 20% Pt/C, and RuO2 loaded on Ni foam as the cathode (Fig. 1a). During the discharge process, the Na metal on the anode side is oxidized to Na+ and moves into the NaOH aqueous through the NASICON separator, and the ORR simultaneously occurs at the cathode. On charging, the Na+ ions were transported from the aqueous electrolyte into the anode chamber and reduced to metallic Na, together with the concurrent OER at the cathode side.

Question: What's the anode?
Answer: Na
To elucidate the practical applicability, HSABs were assembled using metallic Na as the anode immersed in 1 M NaClO4 in TEGDME organic electrolyte, NASICON solid electrolyte as the separator, O2-saturated 0.1 M NaOH aqueous as the aqueous electrolyte, Pt3Ni1/NixFe LDHs, 20% Pt/C, and RuO2 loaded on Ni foam as the cathode (Fig. 1a). During the discharge process, the Na metal on the anode side is oxidized to Na+ and moves into the NaOH aqueous through the NASICON separator, and the ORR simultaneously occurs at the cathode. On charging, the Na+ ions were transported from the aqueous electrolyte into the anode chamber and reduced to metallic Na, together with the concurrent OER at the cathode side.

Question: What's the electrolyte?
Answer: 1 M NaClO4 in TEGDME organic electrolyte
To elucidate the practical applicability, HSABs were assembled using metallic Na as the anode immersed in 1 M NaClO4 in TEGDME organic electrolyte, NASICON solid electrolyte as the separator, O2-saturated 0.1 M NaOH aqueous as the aqueous electrolyte, Pt3Ni1/NixFe LDHs, 20% Pt/C, and RuO2 loaded on Ni foam as the cathode (Fig. 1a). During the discharge process, the Na metal on the anode side is oxidized to Na+ and moves into the NaOH aqueous through the NASICON separator, and the ORR simultaneously occurs at the cathode. On charging, the Na+ ions were transported from the aqueous electrolyte into the anode chamber and reduced to metallic Na, together with the concurrent OER at the cathode side.

Question: What's the anode?
Answer: Na metal
To elucidate the practical applicability, HSABs were assembled using metallic Na as the anode immersed in 1 M NaClO4 in TEGDME organic electrolyte, NASICON solid electrolyte as the separator, O2-saturated 0.1 M NaOH aqueous as the aqueous electrolyte, Pt3Ni1/NixFe LDHs, 20% Pt/C, and RuO2 loaded on Ni foam as the cathode (Fig. 1a). During the discharge process, the Na metal on the anode side is oxidized to Na+ and moves into the NaOH aqueous through the NASICON separator, and the ORR simultaneously occurs at the cathode. On charging, the Na+ ions were transported from the aqueous electrolyte into the anode chamber and reduced to metallic Na, together with the concurrent OER at the cathode side.

Question: What's the electrolyte?
Answer: NASICON solid electrolyte
In the current study, we investigate composite cathodes that combine a NMC cathode (LiNi0.5Mn0.3Co0.2O2) with amorphous 75Li2S–25P2S5 (LPS) solid electrolyte. The cathode material was coated with an amorphous Li–Zr-oxide (LZO) layer to reduce the reaction between NMC and LPS and to minimize the effect of the chemical instability on the electrochemical performance. SSB cells were constructed with In metal as the anode, a composite of NMC/LPS/carbon nanofiber (CNF) in a weight ratio of 60:35:5 as the cathode, and LPS as the solid electrolyte. All the cells were cycled between 1.4 and 3.7 V vs. In (between 2 and 4.3 V vs. Li/Li+) using constant-current constant-voltage (CCCV) charging and constant-current discharging at a rate of 0.05 mA cm−2. The details of the cell fabrication have been previously reported and are provided in the ESI.†

Question: What's the cathode?
Answer: NMC
In the current study, we investigate composite cathodes that combine a NMC cathode (LiNi0.5Mn0.3Co0.2O2) with amorphous 75Li2S–25P2S5 (LPS) solid electrolyte. The cathode material was coated with an amorphous Li–Zr-oxide (LZO) layer to reduce the reaction between NMC and LPS and to minimize the effect of the chemical instability on the electrochemical performance. SSB cells were constructed with In metal as the anode, a composite of NMC/LPS/carbon nanofiber (CNF) in a weight ratio of 60:35:5 as the cathode, and LPS as the solid electrolyte. All the cells were cycled between 1.4 and 3.7 V vs. In (between 2 and 4.3 V vs. Li/Li+) using constant-current constant-voltage (CCCV) charging and constant-current discharging at a rate of 0.05 mA cm−2. The details of the cell fabrication have been previously reported and are provided in the ESI.†

Question: What's the anode?
Answer: In metal
In the current study, we investigate composite cathodes that combine a NMC cathode (LiNi0.5Mn0.3Co0.2O2) with amorphous 75Li2S–25P2S5 (LPS) solid electrolyte. The cathode material was coated with an amorphous Li–Zr-oxide (LZO) layer to reduce the reaction between NMC and LPS and to minimize the effect of the chemical instability on the electrochemical performance. SSB cells were constructed with In metal as the anode, a composite of NMC/LPS/carbon nanofiber (CNF) in a weight ratio of 60:35:5 as the cathode, and LPS as the solid electrolyte. All the cells were cycled between 1.4 and 3.7 V vs. In (between 2 and 4.3 V vs. Li/Li+) using constant-current constant-voltage (CCCV) charging and constant-current discharging at a rate of 0.05 mA cm−2. The details of the cell fabrication have been previously reported and are provided in the ESI.†

Question: What's the electrolyte?
Answer: 75Li2S–25P2S5 (LPS)
In the current study, we investigate composite cathodes that combine a NMC cathode (LiNi0.5Mn0.3Co0.2O2) with amorphous 75Li2S–25P2S5 (LPS) solid electrolyte. The cathode material was coated with an amorphous Li–Zr-oxide (LZO) layer to reduce the reaction between NMC and LPS and to minimize the effect of the chemical instability on the electrochemical performance. SSB cells were constructed with In metal as the anode, a composite of NMC/LPS/carbon nanofiber (CNF) in a weight ratio of 60:35:5 as the cathode, and LPS as the solid electrolyte. All the cells were cycled between 1.4 and 3.7 V vs. In (between 2 and 4.3 V vs. Li/Li+) using constant-current constant-voltage (CCCV) charging and constant-current discharging at a rate of 0.05 mA cm−2. The details of the cell fabrication have been previously reported and are provided in the ESI.†

Question: What's the cathode?
Answer: LiNi0.5Mn0.3Co0.2O2
The fast advancement in portable and wearable electronics has aroused growing demand for energy storage devices not only with high electrochemical performance but also having extra appealing characteristics, such as high safety, low cost, environmental friendliness, and so on. Supercapacitors are a kind of energy storage device demonstrating distinct advantages of simplicity in fabrication and high power density. However, the insufficient energy density has indeed hampered their application. In contrast, lithium-ion batteries possess a much higher energy density, but suffer considerably from cost and safety issues especially under some extreme conditions. Recently, rechargeable Zn–MnO2 batteries have attracted significant research interest due to their unique features, including high safety, light weight, nontoxicity and ease of fabrication. Solid-state rechargeable Zn–MnO2 batteries coupled with hydrogel electrolytes show excellent cycling stability, making them a promising alternative to lithium-ion batteries. Nevertheless, most electrodes for rechargeable Zn–MnO2 batteries are made from synthetic and expensive materials like graphene, carbon nanotubes, acetylene black, etc., which encounter obstacles, such as complex synthesis process, low yield, insufficient capacity, and environmental incompatibility. It is also important to note that most of the recent studies on rechargeable Zn–MnO2 batteries were focused on the optimization of electrochemically active substances, but ignored the structural design of the bulk electrode materials. As is well recognized, the hierarchical microstructure of electrodes may affect their electrochemical properties profoundly, in particular when the electrode is thick or the load of active substances is high.

Question: What's the electrolyte?
Answer: hydrogel
OECT device fabrication. OECT devices were oxygen plasma ashed before spin-coating the polymer solutions at 1000 rpm for 60 s. This was followed by baking the devices at 60 °C for 60 s before removing the sacrificial parylene layer. Following the parylene peel-off the devices were further baked at 140 °C for 30 min. A polydimethylsiloxane (PDMS) well was fabricated using Sylgard-184 base and a curing agent in a 10:1 ratio. The PDMS well contained the electrolyte with a total volume of 300 μl. TBA PF6 electrolytes and TBA PF6:DBSA mixed electrolytes (in both ACN and DCM) had a concentration of 0.1 M. The ratio of TBA PF6:DBSA was kept constant at 1:1 for all mixed electrolyte measurements.

Question: What's the electrolyte?
Answer: TBA PF6 electrolytes and TBA PF6:DBSA mixed electrolytes
As the initial SEI formed on copper modifies the nucleation and growth of lithium metal in a way that gives rise to a columnar microstructure, understanding the formation of this layer and its resulting properties is imperative. XPS results show that the initial SEI formed by galvanostatically bringing copper working electrodes to 0 V vs. Li/Li+ at 0.5 mA cm−2 in LP30 electrolyte with and without added HF are quite similar in chemical composition (Table S1†). Both SEIs contain primarily LiF, LiOH, and organic species (Fig. 4), indicating that the nanostructure of this layer rather than its chemistry is likely key to modifying lithium nucleation and growth. The thickness of this initial SEI layer is roughly 2–3 nm based both on the charge passed (∼3 nm, assuming fully dense and uniform LiF (Fig. 3a)) and the Ar ion sputter rate (∼2 nm, calibrated using SiO2, Fig. S3†). The presence of a smaller peak around 687.6 eV in the F1s spectrum for the as-received sample in Fig. 4a corresponds to PF6− and could be due to a more porous SEI that traps electrolyte. This is another indication of different SEI structures with and without an HF additive. Alternatively, this could be residue from incomplete electrolyte removal during rinsing.

Question: What's the electrolyte?
Answer: LP30
The NASICON solid electrolyte material characterization was performed through an XRD analysis using a Bruker D8 Advance X-ray diffractometer with a Cu Kα X-ray source. Measurements were performed with a 2θ range of 10°–80°. Scanning electron microscope (SEM) images were taken and an energy dispersive spectrometer (EDS) analysis of the films was performed using a Verios 460, FEI and XFlash 6130, Bruker, respectively, operated at an accelerating voltage of 10 kV.

Question: What's the electrolyte?
Answer: NASICON