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1 Supporting Information Electrochemical Synthesis of Ammonia from N 2 and H 2 O under Ambient Conditions Using Pore-Size Controlled Hollow Gold Nanocatalysts with Tunable Plasmonic Properties Mohammadreza Nazemi a,b, and Mostafa A. El-Sayed a* a Laser Dynamics Laboratory, School of Chemistry and Biochemistry, Georgia Institute of Technology, Atlanta, Georgia , United States b George W. Woodruff School of Mechanical Engineering, Georgia Institute of Technology, Atlanta, Georgia , United States melsayed@gatech.edu S1

2 Chemicals and Materials: Silver nitrate (AgNO3), poly(vinylpyrrolidone) (PVP, MW ~ 55,000), ethylene glycol (EG), sodium sulfide nonahydrate (Na2S.9H2O), potassium chloride (KCl), potassium sodium tartrate solution (C4H4KNaO6, 1.5M in H2O), nafion solution (5% wt.) were purchased from Sigma- Aldrich. Hydrogen tetrachloroaurate (III) trihydrate (ACS, 99.99% (metals basis), Au 49.0% min, HAuCl4.3H2O) was purchased from Alfa Aesar. Ammonia standard solution (1 mg L -1 ) and Nessler reagent (K2[HgI4]) were purchased from Hach Co. Indium tin oxide (ITO) coated one surface (4 8 Ω, Delta Technologies, USA), Ar (UHP, 100%, Airgas, USA), N2 (UHP, 100%, Airgas, USA), cation exchange membrane (CEM, FKB-PK-130, FuMA-Tech GmbH, Germany), anion exchange membrane (AEM, FAB-PK-130, FuMA-Tech GmbH, Germany), Platinum (100 mesh, 99.9% trace metal basis, Sigma-Aldrich, USA), Ni wire (0.5 mm, 99.9% trace metals basis, Sigma-Aldrich), and conductive silver paint (Ted Pella Inc.) were used for experiments. Working electrode preparation and electrochemical measurement: In order to prepare a working electrode (cathode), 300 µl of nanoparticles of known concentration (30 pm) and 1.5 µl of nafion solution (5% wt.) were sonicated and drop casted onto a square of indium tin oxide (ITO) (1cm 1cm) and then dried under N2 atmosphere at 75 o C for 1 h. The working electrode is attached to Ni wire with conductive silver paint and isolated from the electrolyte using epoxy. The Electrochemical measurements were carried out at 20 o C lab temperature in 0.5M LiClO4 electrolyte (ph=8, 40 ml, each side), 0.5M LiClO4+HClO4 (ph=3), and 0.1M LiOH (ph=13) using a CHI instrument potentiostat (CHI, 760D) in the three-electrode setup. Pt mesh (1cm 1cm) and Ag/AgCl reference electrodes (3M, BASi, USA) were used as counter and reference electrodes. CEM was used to separate the anodic and cathodic compartments while protons produced at the anode can transport across the membrane to the cathode side where the NRR occurs. AEM was used to enable the transport of S2

3 hydroxide (OH - ) from the cathode to the anode side in alkaline electrolysis where the cathodic and anodic reactions are as follows: N2 + 6H2O + 6e - 2NH3 + 6OH - (1) 6OH - 3/2O2 + 3H2O + 6e - (2) The overall reaction remains the same as in acidic or neutral condition: N2 + 3H2O 2NH3 + 3/2O2 (3) The measured potentials vs. Ag/AgCl are ir-compensated and converted to the reversible hydrogen electrode (RHE) scale based on the following equation: E RHE = E Ag/AgCl + 2.3RT o ph + E F Ag/AgCl (4) where ERHE is the converted potential vs. RHE, E o Ag/AgCl= at 20 o C with the slope of mv/ o C, EAg/AgCl is the experimentally measured potential against Ag/AgCl reference electrode, R is the gas constant (8.314 J mol -1 K -1 ), and T is the operating temperature (K), F is the Faraday s constant (C/eq.), and the ph of the electrolyte varies between 3, 8, and 13. The electrolyte is fed with N2 or Ar gas for 2 h before starting the measurement at the flow rate of 20 ml min -1. Ammonia quatification: The quantity of ammonia is determined via a colorimetric method using Nessler reagent. In order to obtain the calibration curve, a known volume of the standard ammonia solution (1 mg L -1 ) is added to the tube. Next, the tube is filled with the electrolyte until the total volume reaches 10 ml. Then, 1 ml of 0.2M potassium sodium tartrate in DI water is added to each of the tubes. Finally, 1 ml of Nessler reagent is added to each of the tubes and mixed thoroughly. The tubes are kept undisturbed for 20 min for color development and then the absorbance at 395 nm is measured using an Ocean optics spectrophotometer (HR4000Cg-UV-NIR). The S3

4 absorbance for the blank sample without adding standard NH3 solution is subtracted from all samples for background correction. Ammonia yield rate and Faradaic Efficiency: The ammonia yield rate (k) is calculated using the following equation: Yield rate (µg h -1 cm -2 ) = C V t A (1) where C is the ammonia concentration (mol L -1 ), V is the volume of the electrolyte (0.04 L), t is the electrolysis time, and A is the surface area of electrocatalyst. To calculate the ammonia Faradaic efficiency, the ammonia produced during the course of the experiment is divided by the total charge applied to the electrodes. Three electrons are required to produce one mole of NH3. The NH3 Faradaic efficiency is calculated according to the following equation: FE NH3 (%) = C V i t n F (2) i is the measured current (A), n is the number of electrons that is required to produce one mole of ammonia (eq.mol -1 ) which is 3, and F is the Faraday s constant (96485 C eq -1 or A.S eq -1 ). Instrumentation: TEM imaging was performed using a Hitachi HT7700 TEM with the acceleration voltage of 100kV. UV-vis spectroscopy was carried out using an Ocean optics spectrophotometer (HR4000Cg-UV-NIR) with 1 cm path length cuvettes in the wavelength range of nm. The electrochemical measurements were performed using a CHI760D electrochemical station. S4

5 Table S1: Selectivity performance of AuHNCs with various peak LSPR values toward NRR Electrocatalyst Potential (V vs. RHE) AuHNCs-635nm AuHNCs-715nm AuHNCs-795nm S5

6 A B Figure S1: UV-vis calibration curve for ammonia quantification using Nessler s method. Known concentrations of ammonium ions are added to 0.1M LiOH electrolyte and mixed thoroughly with 1 ml of 0.2M KNaC4H6O6 and 1 ml of Nessler reagent and then the absorbance at 395 nm is measured by the UV-vis spectrophotometer. The value of blank electrolyte is subtracted from all other concentrations as background. Calibration curves for 0.5M LiClO4 solution was presented in our previous study 1. S6

7 A B C D Figure S2: A) UV-Vis extinction spectra of AgNSs and AuHNSs with various peak LSPR. B), C), and D) are the TEM images of AuHNSs with the peak LSPR values at 635nm, 715nm, and 795nm, respectively. The average diameter of nanoparticles is 55 nm. S7

8 Figure S3: Chronoamperometry (CA) results of the AuHNSs with various peak LSPR values at the potential of 0.4V vs. RHE at 20 C in 0.5M LiClO4 aqueous solution. S8

9 Figure S4: Ammonia yield rate and Faradaic efficiency for AuHNSs with various peak LSPR values at the potential of 0.4V vs. RHE in 0.5M LiClO4 aqueous solution. S9

10 Figure S5: UV-vis absorbance spectra after electrochemical NRR in 0.5M LiClO4 aqueous solution using AuHNSs with various peak LSPR values at an applied potential of 0.4V vs. RHE. S10

11 Figure S6: UV-vis absorbance spectra after electrochemical NRR in various ph electrolytes using AuHNCs-715 at 0.4V vs. RHE. S11

12 TableS2: Electrochemical performance of NRR using AuHNCs-715 with various ph electrolytes at 0.4V vs. RHE. Electrolyte NH3 Yield Rate (µg cm -2 h -1 ) Average Current Density at 0.4V vs RHE (µa cm -2 ) Faradaic Efficiency (%) 0.5M LiClO M 3.10± HClO4 (ph=3) 0.5M LiClO4 (ph=8) 3.74± M LiOH (ph=13) 0.71± S12

13 A B Figure S7: The SEM images A) before and B) after the durability test. The electrode after the test was thoroughly washed with DI water and dried at room temperature before taking the measurement. References [1] Nazemi, M.; Panikkanvalappil, S.R; and El-Sayed, M.A., Enhancing the Rate of Electrochemical Nitrogen Reduction Reaction for Ammonia Synthesis under Ambient Conditions using Hollow Gold Nanocages. Nano Energy 2018, 49, S13

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