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Nature Communications logoLink to Nature Communications
. 2019 Sep 2;10:3919. doi: 10.1038/s41467-019-11903-5

Cyclic two-step electrolysis for stable electrochemical conversion of carbon dioxide to formate

Chan Woo Lee 1,2,3,#, Nam Heon Cho 1,#, Ki Tae Nam 1,✉, Yun Jeong Hwang 2,4,✉, Byoung Koun Min 2,5,✉
PMCID: PMC6718411  PMID: 31477719

Abstract

Pd metal and Pd-based alloys are ideal catalysts that allow for the electrochemical conversion of CO2 to HCOO− at almost zero-overpotential with high selectivity, but catalyst degradation caused by concurrent CO poisoning limits their practical implementation. Here, we demonstrate that cyclic two-step electrolysis, by applying the reduction and oxidation potentials alternately, achieves 100% current density stability and 97.8% selectivity toward HCOO− production for at least 45 h. The key idea for achieving the reliability is based on the selective removal of CO by controlling the parameters during the oxidation step, which utilizes the different reversibility of HCOO− and CO production reactions. Furthermore, it is found that potentiostatic electrolysis causes CO adsorption and subsequent dehydridation, which in turn lowers HCOO− selectivity. Our work provides a system-level strategy for solving the poisoning issue that is inevitable in many electrocatalytic reactions.

Subject terms: Electrocatalysis, Hydrogen fuel

Reduction of carbon dioxide is promising for the production of value-added chemicals, but electrocatalysts are hindered by carbon monoxide poisoning. Here, the authors alternate reduction and oxidation potentials to achieve stable and selective long-term electrocatalytic reduction of carbon dioxide to formate.

Introduction

Electrochemical CO2 reduction combined with renewable energy resources represents one of the promising strategies for not only reducing greenhouse gas emissions, but also storing electrical energy in a value-added chemical form1–4. Among the products, HCOO− is considered as a valuable liquid chemical for hydrogen storage because it can release H2 fuel responsibly at room temperature5,6. Pd metal is the only electrocatalyst that produces HCOO− at zero-overpotential with high selectivity7–13. It has the special character because CO2 can be activated by palladium hydride (PdHx), which is cathodically formed in an aqueous electrolyte14,15. However, a key challenge is how to minimize or prevent catalyst degradation caused by CO poisoning14. Previous approaches have focused mostly on developing catalysts that favor HCOO− production over CO adsorption16–18. These approaches were mostly based on the theoretical result that HCOO− and CO are primarily formed from different intermediates, formate (OCHO*) and carboxylate (COOH*), respectively19,20. Although the degradation rate was lowered via catalyst development, the stability issue has not been fully resolved yet.

Two-step electrolysis, applying different potentials alternately, has been exploited as an easy and scalable method for decoupling concurrent multiple reactions in electroplating and electrochemical devices21–23. For example, in electrodepositing metals into porous templates24,25, though metal deposition and ion consumption occurred simultaneously, the ion concentration can be recovered by adding another potential step. As a result, the ion depletion effect can be excluded in one cycle unit. In addition, it has already been demonstrated that a reverse bias in the solid-oxide electrochemical cell (SOC) can restore the oxygen electrode degradation22. By cycling forward and reverse bias, stable performances can be achieved. Likewise, when a perovskite solar cell operates via day/night cycling, halide defects, which are the origin of performance loss, are created during irradiation and are eliminated at night 23.

Here, we discuss the degradation mechanism using electrochemical surface analysis, and based on the understanding, we propose cyclic two-step electrolysis, applying reduction and oxidation potentials alternately, as a strategy for securing both stability and selectivity for HCOO− production. In CO2 reduction reactions on Pd-based metals, the adsorption and desorption of the CO intermediate can be reversible on the surface, whereas HCOO− formation is irreversible because HCOO− is released into the bulk electrolyte. Given that two-step electrolysis only affects reversible behaviors, the additional oxidation step can be used specifically to control the CO intermediate oxidation on the electrode. In addition to the reversibility issue, the different oxidation potentials of HCOO− and CO provide another knob for tuning the selective reaction during the reverse cycle. CO oxidation mainly occurs between 0.82 and 1.22 V vs. RHE, whereas HCOO− oxidation is blocked above 0.80 V vs. RHE. In setting the reverse potential, such a significant difference suggests that HCOO− oxidation can be prevented even at high concentration if the reverse potential exceeds 0.80 V vs. RHE. Based on these principles, two-step electrolysis can decouple the HCOO− formation from CO adsorption by selectively oxidizing CO. As a result, 100% of the initial current density is maintained even after 45 h, and a high HCOO− selectivity of 97.8% is achieved.

Results

Catalyst synthesis and electrochemical surface analysis

As a model catalyst for stable and selective HCOO− production, Pd80Ag20/C catalyst was synthesized and investigated, based on our observation that Pd80Ag20/C is more suitable in intrinsic properties than pristine Pd/C for improved reliability of HCOO− production (Supplementary Fig. 1).

For the synthesis, microwave-assisted polyol synthesis and subsequent cyclic voltammetry (CV) pretreatment were performed. In the polyol method, commercial Pd/C powder was heat-treated via microwave irradiation at approximately 200 °C with the Ag precursor. X-ray diffraction (XRD) patterns of the as-synthesized powders (Supplementary Fig. 2) showed a clear peak shift compared to that of Pd/C due to alloying with Ag. The input molar ratio of Ag/Pd was adopted as 0.67, because the largest peak shift was observed without the formation of Ag crystals (Supplementary Fig. 2). After the polyol synthesis, CV pretreatment was applied to the as-synthesized nanoparticles (NPs). Anodic CV was scanned in Ar-purged 0.1 M HClO4 solution for four cycles (Supplementary Fig. 3). For as-synthesized Pd80Ag20/C, the irreversible Ag oxidation peak positioned at approximately 1.2 V vs. RHE was diminished with increasing cycle number, whereas the redox peak associated with reversible hydrogen cycling became distinct between 0.0 and 0.4 V vs. RHE. Additionally, the initial current density of electrolysis increased with the cycle number (Supplementary Fig. 4). From transmission electron microscopy (TEM) analysis (Supplementary Fig. 5), it was confirmed that Pd80Ag20/C catalysts are carbon-supported spherical NPs with an average size of ~5 nm. The composition was analyzed with inductively coupled plasma-optical emission spectrometry (ICP-OES) and scanning transmission electron microscopy-energy dispersive X-ray spectroscopy (STEM-EDS) (Supplementary Table 1, Figs. 6 and 7).

Figure 1a shows the chronoamperometry curves of the Pd80Ag20/C catalysts measured at various potentials in a CO2-saturated 0.5 M NaHCO3/0.5 M NaClO4 electrolyte. The passed charge was fixed at 0.8 C. The Pd80Ag20/C catalyst showed a higher degradation rate of electrocatalytic current density at lower potentials. The degradation rate was measured to be 0.04, 0.08, 0.13, 0.26, 0.46 and 0.79% s−1 at −0.08, −0.18, −0.25, −0.33, −0.53, and −0.73 V vs. RHE, respectively. Basically, CO adsorption can be accelerated at more negative potentials because it is an electrochemical process, while the desorption of adsorbed CO is a chemical process, independent on potentials. Accordingly, the more negative potentials can cause the higher rate of CO poisoning, resulting in the faster degradation rate.

Fig. 1.

Fig. 1

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Relation between adsorbed/absorbed species and product selectivity. a Current density vs. time curves of Pd80Ag20/C catalysts at various potentials in a CO2-saturated electrolyte. In the electrolysis, passed charge is fixed at 0.8 C. b Cyclic voltammetry (CV) curves of Pd80Ag20/C catalysts recorded after electrolysis at various potentials. Solid and dotted lines are the first and second cycle of CV curves. In the first cycle, the anodic peaks related with H extraction (Hext) from the lattice, H desorption (Hdes) from the surface, and CO stripping (COstrip) are indicated with pink, blue, and orange triangles, respectively. c COstrip and Hext + Hdes charges measured from the CV curves. d The Faradaic efficiencies (FEs) for H2, CO, and HCOO− production measured from gas chromatograph (GC) and 1H nuclear magnetic resonance (NMR) analysis after electrolysis at various potentials in a gas-tight cell. Error bars: mean±s.d. Source data are provided as a Source Data file

To deeply understand the observed trends, adsorbed chemical species and absorbed hydrogen were investigated via anodic cyclic voltammetry (CV) after electrolysis (Fig. 1b). The first and second cycles are denoted as solid and dotted lines, respectively. The anodic scan of the first cycle showed stripping peaks of H and CO as highlighted by triangle symbols (Fig. 1b). The anodic peaks at around 0.15 and 0.31 V vs. RHE can be assigned to H extraction (Hext) from the lattice and H desorption (Hdes) from the surface, respectively26. The oxidation peaks positioned at 0.97 and 0.69 V vs. RHE correspond to the oxidation of adsorbed CO at Pd(111) terrace and stepped sites27–29. The CO oxidation was also proved by comparing the anodic CV spectra recorded after applying a cathodic potential in Ar- and CO-purged electrolytes (Supplementary Fig. 8). Additionally, with the CO oxidation, metal oxidation also occurred from 0.70 to 1.22 V vs. RHE. In the cathodic scan of the first cycle, the oxidized metal was reduced again at 0.55 V vs. RHE, and then H adsorption and absorption occurred at 0.15 and 0.00 V vs. RHE, respectively. In the second cycle, the redox reactions related with the dehydridation/hydridation and the formation of oxide and metal were observed, whereas the CO oxidation peaks disappeared.

One of the most interesting features is that CO stripping (COstrip) peaks evolves as the potential decrease, and the Hext and Hdes peaks compete with the COstrip peaks. In the CV spectra of Pd80Ag20/C (Fig. 1b), we observed that the Hext peak gradually increases from −0.08 to −0.33 V vs. RHE but decreases at more negative potentials. The Hdes peak also declined distinctly with the decrease of Hext peak. The decrease of the Hext and Hdes peaks was accompanied by the steep increase of COstrip peaks. A similar trend was also observed in the pristine Pd/C case (Supplementary Fig. 9). As the potential became more negative from −0.08 to −0.33 V vs. RHE, the Hext and Hdes peaks decreased and ultimately disappeared whereas the COstrip peaks increased dramatically. Because the anodic peaks indicate the oxidation of chemical species adsorbed and absorbed by electrolysis, these results show that lower potentials lead to the increase of CO adsorption and the decrease of H adsorption/absorption amount.

Relation between adsorbed/absorbed species and product selectivity

To determine how the surface chemical species affects CO2 reduction, we compared the amount of surface species and product selectivity as a function of potential. Figure 1c shows the COstrip and Hext + Hdes charges calculated by integrating the area under the oxidation peaks of the anodic CV spectra. The COstrip and Hext + Hdes charges reflect the amount of adsorbed CO and absorbed/adsorbed H during electrolysis, respectively. The product selectivity was investigated by a gas chromatograph (GC) and a 1H nuclear magnetic resonance (NMR) spectrometer by sampling the headspace gaseous mixtures and the electrolyte after electrolysis (Fig. 1d and Supplementary Fig. 10). The Faradaic efficiency (FE) for HCOO− accounted for 96.1% on average from −0.08 to −0.33 V vs. RHE and declined abruptly at lower potentials with the increase of H2 evolution. In contrast, CO was detected in a negligible amount with an average FE of 0.1%. Considering that the amount of CO adsorption also dramatically increased below −0.33 V vs. RHE (Fig. 1c), it can be empirically shown that there is a correlation between CO adsorption and the increase in H2 evolution. Specifically, the COstrip charges were 3.4, 4.2, 19.4 and 43.8 mC at −0.25, −0.33, −0.53 and −0.73 V vs. RHE, respectively, while the FEs for H2 production were measured to be 0.2%, 0.7%, 21.3% and 42.7% at the examined potentials. A similar trend can be also observed in the Pd/C case (Supplementary Fig. 11). The decrease in the total FE for H2, CO and HCOO− products at high overpotentials can be attributed to CO adsorption, H adsorption/absorption and non-Faradaic process (Supplementary Table 2).

Taken together, CO adsorption contributes to decreasing the amount of absorbed/adsorbed H and increasing H2 evolution, while deeper insights into CO2 reduction reactions on Pd-based catalysts can be discussed based on theoretical consideration of intermediate binding. According to a previous calculation study30, it is known that CO adsorption lowers the binding strength of the H intermediate. The weaker binding of H can increase H2 evolution and accelerate dehydridation, causing the decrease in HCOO− selectivity, which is demonstrated in this study. This phenomenon implies that intrinsically strong H binding of Pd-based metals enables high selectivity for HCOO− formation. However, it should not be overlooked that the H binding energy is also correlated with CO binding energy19. Strong H binding leads to strong CO binding. Consequently, it is challenging to completely separate the HCOO− production and CO poisoning in potentiostatic electrolysis owing to the complex interrelations.

Cyclic two-step electrolysis

We applied cyclic two-step electrolysis to completely resolve the stability issue using an extrinsic system-level control. The cyclic two-step electrolysis involves the programmed alternation of reduction and oxidation. Its special advantage is that HCOO− and CO formation can be decoupled. The decoupling principle can be understood based on empirical findings from electrochemical surface analysis. Firstly, HCOO− is released well into the bulk electrolyte while CO remains adhered to the catalyst surface (Fig. 1b, d). Due to the difference in adsorption behavior, adding an oxidation step after CO2 reduction can selectively induce the reverse reaction for CO adsorption. After the oxidation step, HCOO− becomes the sole reaction product caused by the two-step electrolysis. This result means that HCOO− production is decoupled from CO adsorption. Secondly, the HCOO− and CO oxidations occurred in different potential regimes. When the stripping analysis was performed after electrolysis for various durations at −0.18 V vs. RHE (Fig. 2a, b), the CO oxidation peaks were observed between 0.82 to 1.22 V vs. RHE, whereas the HCOO− oxidation was prevented at above 0.80 V vs. RHE. Thus, controlling the oxidation potential enables selective CO oxidation. Thirdly, the oxidation of adsorbed CO occurred preferentially before the initiation of HCOO− oxidation (Fig. 2b). This result means that controlling the oxidation period enables selective CO oxidation. Based on these principles, we designed and optimized the potential program of cyclic two-step electrolysis.

Fig. 2.

Fig. 2

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Electrochemical oxidation behavior of HCOO− and CO products. a Current density vs. time curve of Pd80Ag20/C catalysts recorded during 1 h electrolysis. Chronoamperometry was conducted at −0.18 V vs. RHE in a CO2-saturated electrolyte. The current density gradually decreases with time. b Cyclic voltammetry curves measured after electrolysis for different durations at −0.18 V vs. RHE. The anodic peaks associated with H extraction (Hext), H desorption (Hdes), HCOO− oxidation (HCOO−ox), and CO stripping (COstrip) are indicated by pink, blue, green, and orange triangles, respectively

Figure 3a shows the time-dependent profiles of current density (solid line) and H2 production FE (solid circles) recorded during cyclic two-step electrolysis and potentiostatic electrolysis on Pd80Ag20/C catalysts. The FE for gas products was measured by GC analysis under a constant gas flow, whereas the average HCOO− FE was obtained via 1H NMR analysis of the catholyte after electrolysis. In cyclic two-step electrolysis, the potential program was composed of a reduction and oxidation step per cycle as shown in Fig. 3b. In the reduction and oxidation step, −0.18 and 1.22 V vs. RHE were applied for 590 and 10 s, respectively. The redox cycle was repeated 270 times for 45 h. During the long-term experiments, the CO2-saturated electrolyte was continuously circulated using a peristaltic pump between electrolyte bottles and an electrochemical cell (Supplementary Fig. 12).

Fig. 3.

Fig. 3

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HCOO− production performance of cyclic two-step electrolysis. a Comparison between cyclic two-step electrolysis and potentiostatic electrolysis in terms of the current density and product selectivity. The blue and red lines represent the current density vs. time curves measured via potentiostatic electrolysis and cyclic two-step electrolysis, respectively. The blue and red circles represent H2 production selectivity. Both experiments were conducted in a flow cell system where CO2-saturated bicarbonate solution was continuously refreshed using a peristaltic pump. b Potential program and reaction scheme of the cyclic two-step electrolysis. In the reduction step, −0.18 V vs. RHE was applied for 590 s, whereas 1.22 V vs. RHE was applied for 10 s in the oxidation step. c Current density vs. time curves and net passed charges during cyclic two-step electrolysis. The charge used in the oxidation step accounts for 3.7% of the charge passed in the reduction step

Surprisingly, the catalytic performance remained stable for 45 h via cyclic two-step electrolysis as shown in Fig. 3a. The initial current density of the 1st cycle (11.0 mA cm−2) was identical to that of the 270th cycle (11.0 mA cm−2), indicating that the current density loss is 0.0% during the long-term experiment. In addition, H2 production was suppressed to under 1.5% throughout the experiment. Consequently, an average HCOO− FE of 97.8% was achieved. In detail, as displayed in the expanded current density profile (Fig. 3c), the initial current density of 11.0 mA cm−2 decreased to 7.8 mA cm−2 during the reduction step due to the CO accumulation. In the following oxidation step for 10 s, the cathodic current was switched to an anodic current, and the value rapidly decayed to nearly zero in a few seconds. During the anodic step, the oxidation of adsorbed CO and hydride predominantly occurred. Afterward, in the next reduction step, the current polarity was inverted again and the current density was dramatically restored to 11.4 mA cm−2. The degradation and recovery of current density were repeated in every cycle. As catalyst surface was regenerated continuously via the programmed anodic step, zero degradation of current density could be achieved regardless of electrolysis duration. In addition, as severe CO adsorption was prevented, very low selectivity for H2 production could be stably maintained. To the best of our knowledge, these catalytic performances show record-high stability in terms of current density and selectivity in comparison with the previous reports on HCOO− production using Pd-based catalysts (Supplementary Table 3)7,14,16–18,31–34. In contrast, potentiostatic electrolysis showed a current density loss as large as 63.2% in only 6 h. Simultaneously, H2 evolution selectivity abruptly started to increase after 2 h, and reached to 24.1% after 6 h. As a result, the average HCOO− FE for 6 h was measured to be 79.9%. The clear stability difference between the two experiments indicates that CO adsorption, the origin of catalyst degradation, was completely decoupled from HCOO− production in the two-step electrolysis.

The decoupling mechanism of CO adsorption can be figured out from the reaction scheme occurring in each potential step as shown in Fig. 3b. In the reduction step, the formation of HCOO− and CO proceeds concurrently on the hydride surface formed by H absorption, as identified by product and stripping analyses (Figs. 1d and 2b). Among the reduced products, CO molecules are accumulated at the catalyst surface, whereas HCOO− is released immediately and diffused into the bulk electrolyte. In the subsequent oxidation step, adsorbed CO is preferentially oxidized (Fig. 2b), whereas HCOO− oxidation is prevented. The net reaction for one cycle is only HCOO− production.

Additionally, the economic feasibility of two-step electrolysis method was evaluated by investigating the additional charge and electrical energy used in the oxidation step. In calculating the electrical energy consumption, the overpotential applied at the counter electrode was assumed to be zero for convenience. For example, the voltages of the reduction and oxidation step were set to be 0.18 + 1.23 V and 1.22 + 0.00 V, respectively. The charge consumed in the oxidation step accounted for only 3.7% of the charge passed in the reduction step as shown in Fig. 3c. In addition, the electrical energy consumed in the oxidation step was 1.9% of that in the reduction step. This proves that there is almost no difference in energy consumption between potentiostatic and cyclic two-step electrolysis methods.

Key parameters

To achieve high stability and selectivity for HCOO− production via cyclic two-step electrolysis, the adsorbed CO should be oxidized fully and selectively in the oxidation step. Current density recovery can reflect whether the adsorbed CO is fully oxidized to CO2, whereas HCOO− selectivity can reveal if the oxidation step is used only for CO oxidation. By measuring the current density vs. time curves and the average HCOO− FE during electrolysis with different oxidation potentials and periods, optimal parameters of the oxidation step were drawn. In controlling the oxidation parameters, the reduction potential and period were fixed at −0.18 V vs. RHE and 20 min, respectively.

Figure 4a shows the effect of the oxidation potential on current density recovery, where the oxidation period was fixed at 6 s. Oxidation potentials of 1.02 and 1.22 V vs. RHE were examined because CO oxidation can occur at these potentials as displayed in Fig. 2b. For the first cycle, the current densities similarly decreased with time at both oxidation potentials, whereas the current density difference became larger in the following steps. The current density recovery was calculated by dividing the initial current density of the third cycle by that of the first cycle. The current density recovery was 44.4% and 78.8% at 1.02 and 1.22 V vs. RHE, respectively, which indicated that more CO was desorbed at 1.22 V vs. RHE.

Fig. 4.

Fig. 4

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Key parameters of cyclic two-step electrolysis. a The effect of oxidation potential on current density recovery. The oxidation potential was changed with the oxidation period fixed at 6 s. b Current density vs. time curves as a function of oxidation period. The oxidation period was varied from 2 to 20 s while the oxidation potential was fixed at 1.22 V vs. RHE. In controlling the oxidation parameters, the reduction potential and period were fixed to −0.18 V vs. RHE and 20 min. c Current density vs. time curves of the oxidation step with various oxidation periods. d The dependence of the current density (jtotal) recovery and the HCOO− Faradaic efficiency (FE) on the oxidation period. The HCOO− FE was measured using 1H nuclear magnetic resonance (NMR) analysis of the liquid product after cyclic two-step electrolysis. The jtotal recovery values were calculated by dividing the initial current density of the sixth cycle by that of the first cycle in Fig. 4b. Error bars: mean±s.d. Source data are provided as a Source Data file

The current density vs. time curve was recorded as a function of oxidation period (Fig. 4b). The oxidation potential was fixed at 1.22 V vs. RHE while the oxidation period was varied from 2 to 20 s as shown in Fig. 4c. In the oxidation step, the current density initially decayed dramatically and then much more slowly after 20 s. This result indicates that capacitive and pseudo-capacitive reactions were almost terminated in 20 s. From the current density profiles, the recovery percentage was calculated by dividing the initial current density of the sixth cycle by that of the first cycle as shown in Fig. 4d. The average HCOO− FE was also estimated via 1H NMR analysis of the catholyte after electrolysis.

The oxidation period critically affected the current density recovery and the HCOO− selectivity. As the period increased from 2 to 10 s, the recovery percentage and the HCOO− FE were enhanced from 23.0% to 95.2% and from 63.7% to 96.3%, respectively. These results show not only that CO is completely eliminated in 10 s, but also that full CO elimination leads to a high HCOO− selectivity. When the period was prolonged to 20 s, the recovery percentage and the HCOO− FE was almost unchanged. By additionally considering the electrical energy consumption, we found the optimal parameters of the oxidation step for fully and selectively removing CO with a small energy cost. Additionally, applying lower reduction potentials requires additional optimization of the oxidation step because CO poisoning proceeds at a higher rate. It can be observed that current density stepwise decreases to zero in the cyclic two-step electrolysis using −0.33 V vs. RHE (Supplementary Fig. 13). In this case, increasing the oxidation period or potential can be needed for stable formate production.

Discussion

In summary, we have demonstrated that the inherent poisoning issue of Pd-based catalysts in electrochemical CO2 reduction reactions can be resolved via cyclic two-step electrolysis, an electrochemical method to apply the reduction and oxidation steps alternately. Though HCOO− production and CO adsorption simultaneously occurred in the reduction step, the CO molecules were selectively oxidized in the anodic step. The reversibility difference between the concurrent reactions played a critical role in decoupling the reactions, and could be further secured by controlling the oxidation potential and period. From the cyclic two-step electrolysis, 97.8% selectivity and 100% current density stability for 45 h were accomplished toward HCOO− production. In comparison, potentiostatic electrolysis showed that the current density and FE loss corresponded to 63.2 and 24.1%, respectively, in only 6 h. The performance degradation was caused by the increase in CO adsorption which not only blocks active sites, but also leads to dehydridation. We believe that our study can suggest an electrolysis method for solving poisoning issues in Pd-based electrochemical formate production.

Methods

Chemicals

Silver trifluoroacetate (98%) was purchased from Alfa Aesar. Commercial Pd/C (20 wt%) was purchased from Premetek. Ethylene glycol (99.5%) and methanol (99.8%) were purchased from Daejung Chemical & Metals. Carbon dioxide (99.999%) was purchased from the PSG Corporation. Sodium bicarbonate (99.5%) and sodium perchlorate monohydrate (98%) were purchased from Junsei Chemical.

Catalyst synthesis and electrode preparation

The Pd80Ag20/C catalysts were synthesized via a microwave-assisted polyol method. Firstly, 11.3 mg of silver trifluoroacetate and 40 mg of 20 wt% Pd/C (Premetek) were dissolved in 50 ml of ethylene glycol. The input molar ratio of Ag/Pd was 0.67. Then, the precursor solution was sonicated for 30 m and heated by microwave irradiation at 200 W for 6 m. The resultant powder was centrifuged and washed with methanol. The powder was dried under vacuum at room temperature overnight. Pd/C catalysts as a control sample were synthesized with the same method without the silver precursor. For electrode preparation, 6 mg of catalyst powder was dispersed in 0.5 ml of ethanol with 40 μl of the neutralized Nafion solution, which was prepared by pH adjustment of 5 wt% Nafion dispersion solution (Sigma-Aldrich) with 0.1 M NaOH aqueous solution. A 40 μL aliquot of the catalyst dispersion was drop-coated on a glassy carbon electrode (Alfa Aesar). The active area was 0.5 cm2. Before CO2 reduction measurements of the Pd/C and Pd80Ag20/C catalysts, CV was scanned in the potential range from −0.35 to 1.10 V vs. Ag/AgCl at a rate of 50 mV s−1 in Ar-purged 0.1 M HClO4 solution for four cycles.

Characterization

The TEM and STEM-EDS analyses were conducted using an FEI Talos F200X microscope. Powder XRD patterns were obtained with a D8 Advance X-ray diffractometer with Cu Kα radiation. ICP-OES measurement was performed on a Thermo iCAP 6000. For the sample preparation, 5 mg of Pd80Ag20/C powder was dissolved in 12 mL of 60% HNO3 and carbon black was separated using a filter paper (Whatman). The filtered solution was diluted with deionized water.

Product analysis and stripping experiment

Electrolyses were conducted in a two-compartment gas-tight electrochemical cell with a piece of Nafion membrane (Nafion 117). The CV-treated catalyst electrodes and a piece of platinum foil were used as the working and counter electrodes, respectively. All potentials were controlled against an Ag/AgCl reference electrode (3.0 M NaCl, BASi) using a CHI 608 C potentiostat and converted to the RHE reference scale (ERHE = EAg/AgCl + 0.210 V + 0.0591 V × pH). All potential values are given without iR correction. Before electrolysis, the catholyte, 0.5 M NaHCO3/0.5 M NaClO4, was purged with high-purity CO2 gas for at least 20 min. The electrolysis at various potentials was stopped when the passed charge was 0.8 C. After electrolysis, gas products in the headspace were extracted using a syringe (0.1 ml, Hamilton) and injected to a GC (Shimadzu) equipped with a packed Shincarbon ST 50/80 column. The gas mixtures were detected in a thermal conductivity detector (TCD) and a flame ionization detector (FID). For quantification, GC analyses were performed using standard gases with 10, 500 and 1000 ppm of H2 and CO (AirKorea Inc.). We then plotted the integrated area of H2 or CO signals with respect to the known concentrations for obtaining calibration curves (Supplementary Fig. 14). The H2 and CO concentrations in the sampled headspace gas were calculated based on the calibration curves. The concentration of produced HCOO− was estimated using a 600 MHz NMR spectrometer (Avance 600, Bruker). For 1H NMR sample preparation, the catholyte (700 μL) containing the liquid product was mixed with the D2O solution (35 μL) of 10 mM dimethyl sulfoxide (DMSO) and 50 mM phenol as internal standards. For quantitative analysis, we prepared standard solutions by mixing the electrolyte (700 μL) containing 0, 10, 30, and 50 mM HCOO− with the D2O solution (35 μL) containing 10 mM DMSO and 50 mM phenol. After 1H NMR measurements of the standards, the relative area of the HCOO− signal respect to phenol was plotted as a function of HCOO− concentration to obtain a calibration curve (Supplementary Fig. 14) as reported in a previous study35. The FE of the gas and liquid products was calculated by dividing the charge consumed to produce the specific amount of product by the total passed charge. The consumed charge was calculated by the equation: C × V × F × 2, where C is the concentration of H2 or CO or HCOO−, and F is the Faraday constant. V is the headspace volume for H2 and CO, while it is the catholyte volume for HCOO−. After electrolysis, anodic CV was scanned in the potential range from −0.65 to 0.65 V vs. Ag/AgCl at a scan rate of 10 mV s−1 in CO2-saturated 0.5 M NaHCO3/0.5 M NaClO4 for two cycles. To calculate the COstrip and Hdes charges, the area under the oxidation peaks was integrated and the charge caused by double layer charging and oxide formation was subtracted.

Cyclic two-step electrolysis

The long-term cyclic two-step electrolysis displayed in Fig. 3 was conducted in a flow cell system as shown in Supplementary Fig. 12. The catholyte and anolyte, 0.5 M NaHCO3/0.5 M NaClO4, were circulated by a peristaltic pump between the electrolyte bottles and the electrochemical cell. The electrolyte in the bottle was purged with a CO2 gas during electrolysis. The CV-treated catalyst electrodes and a piece of platinum foil were used as the working and counter electrodes, respectively. The potential program per cycle is composed of the reduction step (−0.18 V vs. RHE for 9 min 50 s) and oxidation step ( + 1.22 V vs. RHE for 10 s). For analysis of gas products, CO2 gas was supplied to the cathode compartment and delivered to a GC (Younglin 6500 GC) at a flow rate of 20 mL min−1. The gas mixtures in a capillary column (Restek RT-Msieve 5 A) were transferred and detected in a pulsed discharge detector (PDD). The measurement of FEs for gas products was performed based on the following equation: FEgas = (Ipartial/Itotal) × 100 = (V × Q × (nFp0/RT)/Itotal) × 100 where I is the current, V is the volume concentration of each gas product, Q is the gas flow rate, n is the number of electrons transferred to evolve a gas molecule, F is the Faraday constant, p0 is 1.01 bar, R is the ideal gas constant, and T is 298 K. The volume concentration was measured from the peak area of the GC spectrum, based on calibration with standard samples. The FE for HCOO− production was measured by dividing the charge required to produce the specific amount of product by the cathodic charges passed during cyclic two-step electrolysis, based on 1H NMR analysis of the resultant catholyte after electrolysis. In the experiments of controlling the oxidation potential and period, CO2 gas was continuously supplied only to electrolyte bottles at a flow rate of 20 mL min−1.

Supplementary information

Supplementary Information (1,002.1KB, pdf)
Source data (13.2KB, xlsx)

Acknowledgements

This work was supported by the KIST-SNU Joint Research Lab project (2V06170) under the KIST Institutional Program funded by the Korea government (Ministry of Science, ICT & Future Planning).

Author contributions

C.W.L. and N.H.C. contributed equally to this work. K.T.N. conceived the ideas. C.W.L. and N.H.C. performed the experiments and analysis. K.T.N., Y.J.H., and B.K.M. guided all the aspects of the research. C.W.L. and K.T.N. wrote the paper. All authors discussed the results and contributed to the paper.

Data availability

The authors declare that the main data supporting the findings of this study are available within the article and its Supplementary Information files. Extra data are available from the corresponding author upon request. The source data underlying Figs. 1d and 4d and Supplementary Figs. 1 and 11b are provided as a Source Data file.

Competing interests

The authors declare no competing interests.

Footnotes

Peer review information: Nature Communications would like to thank Tetsuya Haruyama and other, anonymous, reviewers for their contributions to the peer review of this work.

Publisher’s note: Springer Nature remains neutral with regard to jurisdictional claims in published maps and institutional affiliations.

These authors contributed equally: Chan Woo Lee, Nam Heon Cho.

Contributor Information

Ki Tae Nam, Email: nkitae@snu.ac.kr.

Yun Jeong Hwang, Email: yjhwang@kist.re.kr.

Byoung Koun Min, Email: bkmin@kist.re.kr.

Supplementary information

Supplementary Information accompanies this paper at 10.1038/s41467-019-11903-5.

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Associated Data

This section collects any data citations, data availability statements, or supplementary materials included in this article.

Supplementary Materials

Supplementary Information (1,002.1KB, pdf)
Source data (13.2KB, xlsx)

Data Availability Statement

The authors declare that the main data supporting the findings of this study are available within the article and its Supplementary Information files. Extra data are available from the corresponding author upon request. The source data underlying Figs. 1d and 4d and Supplementary Figs. 1 and 11b are provided as a Source Data file.

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