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Vieri, H.M.; Kim, M.; Badakhsh, A.; Choi, S.H. Protonic Ceramic Electrolysis Cells Design for NH3 Synthesis. Encyclopedia. Available online: https://encyclopedia.pub/entry/54656 (accessed on 04 May 2024).
Vieri HM, Kim M, Badakhsh A, Choi SH. Protonic Ceramic Electrolysis Cells Design for NH3 Synthesis. Encyclopedia. Available at: https://encyclopedia.pub/entry/54656. Accessed May 04, 2024.
Vieri, Hizkia Manuel, Moo-Chang Kim, Arash Badakhsh, Sun Hee Choi. "Protonic Ceramic Electrolysis Cells Design for NH3 Synthesis" Encyclopedia, https://encyclopedia.pub/entry/54656 (accessed May 04, 2024).
Vieri, H.M., Kim, M., Badakhsh, A., & Choi, S.H. (2024, February 02). Protonic Ceramic Electrolysis Cells Design for NH3 Synthesis. In Encyclopedia. https://encyclopedia.pub/entry/54656
Vieri, Hizkia Manuel, et al. "Protonic Ceramic Electrolysis Cells Design for NH3 Synthesis." Encyclopedia. Web. 02 February, 2024.
Protonic Ceramic Electrolysis Cells Design for NH3 Synthesis
Edit
This entry is adapted from the peer-reviewed paper 10.3390/en17020441

The application of protonic ceramic electrolysis cells (PCECs) for ammonia (NH3) synthesis has been evaluated over the past 14 years. While nitrogen (N2) is the conventional fuel on the cathode side, various fuels such as methane (CH4), hydrogen (H2), and steam (H2O) have been investigated for the oxygen evolution reaction (OER) on the anode side. Because H2 is predominantly produced through CO2-emitting methane reforming, H2O has been the conventional carbon-free option thus far. Although the potential of utilizing H2O and N2 as fuels is considerable, studies exploring this specific combination remain limited. 

electrochemical ammonia synthesis protonic ceramic electrolysis cells hydrogen catalysts nitrogen reduction reaction

1. Introduction

Hydrogen (H2) has considerable potential for energy storage. However, its low energy density poses challenges to storage and transport. One solution is to convert H2 to ammonia (NH3), where H2 that is obtained from water electrolysis (i.e., green H2) reacts with nitrogen (N2) in the air to produce NH3, which can be reversibly converted into H2 and N2 after transportation [1]. Currently, NH3 is industrially produced using the Haber–Bosch process, which requires high pressure (100–200 bar) and temperature (300–400 °C) to activate the Fe-based catalysts [2][3]. Recent advancements include the hydrogenation of N2 using Ru catalysts, which require milder reaction conditions [4].
However, the thermal approach for NH3 synthesis remains expensive, as it requires a large centralized infrastructure and is energy-intensive, consuming approximately 485 kJ mol−1 (approximately 2% of the global energy use per annum) [5]. Fertilizers Europe made conjectures about the decarbonization of the European NH3 industry [6]. They proposed that approximately 10% of H2 derived for NH3 production in 2030 could possibly originate from renewable sources. Electrochemical NH3 synthesis via N2 reduction provides a relatively high efficiency of up to 20%, environmental compatibility with renewable sources (solar, tidal, and wind), on-site H+ generation from water oxidation, and adaptable reaction control [7]. This process converts sustainable electricity from sources such as wind power into NH3 for use as a synthetic fuel or chemical feedstock [8][9].
The operating conditions are classified into three types based on the temperature, namely, low (<100 °C), intermediate (200–500 °C), and high (>400 °C) temperature. High-temperature conditions enhance the catalytic activity and substantially increase the Faradaic efficiency in NH3 synthesis. High-temperature NH3 synthesis can be performed using proton-conducting electrolytes (PCEs) or oxygen-conducting electrolytes (OCEs). OCEs, while efficient, generally present slower rates of NH3 production than PCEs [10]. This review focuses on NH3 production in protonic ceramic electrolysis cells (PCECs), which operate at high temperatures (400–600 °C). As shown in Figure 1, the PCEC combines the nitrogen reduction reaction (NRR) with other electrochemical reactions that yield protons (H+), facilitating NH3 production. Liu et al. briefly reviewed three primary PCEC configurations involving H2, CH4, and H2O as proton (H+) sources. Although H2O and N2 have considerable potential as fuels, this specific combination has not been sufficiently investigated. Despite consuming substantially more electrical energy than the other configurations, using H2O and N2 directly to produce NH3 is carbon-free and abundant in the feedstock [11]. This configuration couples the NRR with the oxygen evolution reaction (OER). High-temperature NH3 synthesis has been extensively reviewed [12][13][14][15][16]. However, reviews of the specific PCEC configurations for NH3 synthesis are limited. The unavailability of a comprehensive strategy for PCEC fabrication in a single study poses a considerable challenge for researchers aiming to develop PCECs customized for NH3 synthesis.
Energies 17 00441 g001
Figure 1. Schematic of the PCEC setup designed for NH3 synthesis, wherein H2O and N2 are transformed into NH3.
The three essential components of a PCEC are an electrolyte, an anode, and a cathode (Figure 1). The electrolyte serves as an ion conductor that separates the electrodes and facilitates ion transport. The electrochemical reactions within the PCEC are non-spontaneous, implying that they do not occur naturally; an external influence, typically electricity, is necessary to drive the reactions [17].
Anode reaction
●
At the anode, an electric current passes through water, thereby splitting water molecules into hydrogen (protons) and oxygen ions.
●
Reaction: 2H2O → O2 + 4H+ + 4e−
Electron and proton transport:
●
Electrons generated at the anode during water splitting are transported through an external electric circuit.
●
Protons generated at the anode during water splitting are transported through the electrolyte [18].
Cathode reaction
●
At the cathode, protons (H+) from the anode and nitrogen atoms react to produce NH3
●
Reaction: N2 + 3H+ + 3e− → NH3

2. PCEC Design Strategies

High-temperature cells such as solid oxide fuel cells (SOFCs) have been extensively designed [14]. However, selecting an appropriate design for each application is important because the cell performance strongly depends on the cathode, anode, and electrolyte materials. Medvedev discussed the influence of the design strategies on the performance of H2-producing PCECs [16]. However, PCEC design strategies for NH3 synthesis are limited. This section describes the fabrication and design strategies for the electrolyte and electrodes.

2.1. Electrolyte Design Strategies

The electrolyte is considered the most important component of a PCEC, particularly in electrolyte-supported systems because it occupies the largest volume. BaCeO3 and BaZrO3-based materials have been reported to be good protonic conductors [19]. Although BaCeO3 exhibits high conductivity, BaZrO3 provides better stability. Furthermore, Ce and Zr have been mixed with other dopants, such as Y and Yb, resulting in the well-known BaZr0.4Ce0.4Y0.1Yb0.1O3−δ (BZCYYB 4411) and BaZr0.1Ce0.7Y0.1Yb0.1O3−δ (BZCYYb 1711) electrolytes [20][21]. In general, a higher Ce content increases the proton conductivity, whereas a higher Zr content increases the stability [22][23]. In a PCEC, the applied electrical current serves two potential pathways: proton and electron transfers. The primary objective of a PCEC is to facilitate the movement of protons (H+) from the OER to the NRR sides, where they participate in hydrogen production. However, electron transfer, in which electrons move instead of protons, can be detrimental to the cell performance. This is because electron transfer reduces the Faradaic efficiency of the cell; particularly, a portion of the electrical energy is redirected to unintended reactions, leading to energy losses and potentially reducing the overall hydrogen production efficiency. Increasing the Ce content increases the protonic transference number and decreases the electron transference number. Therefore, BZCYYb 1711 is more suitable for PCECs than BZCYYb 4411 [24].
This discussion pertains to three distinct electrolyte forms: pellets, thin films, and columnar structures. Pellet-type electrolytes have been extensively used in fuel cells and batteries [25][26]. They are relatively easy to manufacture and integrate into PCEC stacks [27]. This method involves placing a few grams of electrolyte powder into a mold, which is typically cylindrical, and ultimately shaping it into a coin-like pellet. This conventional approach has resulted in considerable advancements in terms of electrolyte composition. The details of various pellet electrolytes developed thus far are listed in Table 1.
Table 1. Conductivities of proton-conducting electrolytes and their synthesis methods.
Electrolyte Method Conductivity (S cm−1) Thickness (mm) Reference
SrCe0.95Yb0.05O3−δ sol–gel Unknown 1.5 [28]
BaZr0.8−x−yCexNdyY0.1Yb0.1O3−δ Pechini method 500 °C: 3.77 × 10−4 0.8–1.5 [29]
BaZr0.85Y0.15O3−δ hydrothermal process 600 °C: 2.5 × 10−3 1.6 [30]
While the solid-state reaction is common for powder preparation, sol–gel or glycine nitrate processes are commonly employed to obtain finer particles and higher peak power densities [29]. The pellet electrolyte thickness is in the range of 0.8–1.6 mm (Table 1). Medvedev suggested that thin-film technology must be developed for the electrochemical synthesis of NH3 [16]. With reference to the electrolyte properties, the thickness plays a crucial role in determining both the ohmic resistance and electron transport characteristics. Thicker electrolytes increase the ohmic resistance, whereas thinner electrolytes increase contact resistance at the electrolyte/electrode interface. In conventional electrolytes, the ohmic resistance tends to increase. This limitation can be effectively addressed using thin-film electrolytes [31]. Recent advancements in thin-film electrolytes for PCECs have been comprehensively presented in Table 2.
Table 2. Conductivities of thin-film electrolytes and their deposition/synthesis methods.
Electrolyte Method Conductivity (S cm−1) Thickness (µm) Reference
BaCe0.7Zr0.1Y0.2 co-precipitation
solid-state reaction
dip-coating		 650 °C: 2.8 × 10−2 ~20 [32]
BaCe0.8Y0.2−xNdxO3−δ citrate–nitrate combustion 350 °C: 8.5 × 10−3 ~20 [33]
BaCe1−xInxO3−δ auto-combustion reaction 700 °C: 5 × 10−3 20–25 [34]
BaZr0.1Ce0.7Y0.1Yb0.1 solid-state reaction 500 °C: 1.2 × 10−2 10 [35]
BaHf0.8Yb0.2O3−δ pulsed laser deposition (PLD) 500 °C: 2.5 × 10−3 110 [35]
BaZr0.1Ce0.7Y0.1Yb0.1 solid-state reaction 500 °C: 1.3 × 10−2 ~10 [21]
BaZr0.4Ce0.4Y0.1Yb0.1 solid-state reaction 500 °C: 5.6 × 10−3 ~15 [20]
BaZr0.2Ce0.6Y0.1Yb0.1O3−δ Pechini method
inkjet printing		 600 °C: 24.39 1 [36]
BaCe0.5Zr0.35Y0.15O3−δ citric nitrate method
PLD		 Unknown 2–4 [37]
BaZr1−x−yCexYyO3 ultrafast microwave-assisted sintering
tape casting		 Unknown ~12 [38]
BaZr0.2Ce0.6Y0.2O3 solid-state reaction
spin coating		 800 °C: 1 × 10−2 ~7 [39]
BaCe0.55Zr0.3Y0.15O3−δ screen printing Unknown ~2.5 [40]
The technological advancements in thin-film electrolytes are attributed to their reduced dimensions. Various deposition techniques, such as inkjet printing, pulsed layer deposition (PLD), tape casting, spin coating, and screen printing, are involved [36][37][38][39][40]. Screen printing and spin coating are known to be simple. However, considerable material wastage occurs, with a minimum thickness of approximately 10 µm. Furthermore, PLD, which is recognized for its effectiveness, requires complex operation and energy-intensive vacuum conditions. Inkjet printing offers the advantage of producing highly uniform surfaces with a minimum thickness of just 0.83 µm [36].
BaZr0.1Ce0.7Y0.1Yb0.1 is an extensively investigated proton-conducting electrolyte, although some researchers have diverged, advocating other compositions as the most studied [21][32][34]. Some researchers have explored doping with elements such as Nd, Sc, In, and Hf, in addition to Y and Yb, to enhance the stability and sinterability of the electrolyte [21][30][31][33][35][41]. Ding et al. introduced a novel approach by ball milling, pelletizing, calcining, and crushing the pellets to produce a pure-phase powder on a relatively large scale (up to 4 kg per batch) [42]. Another approach involves combining all BZCYYb1711 nitrate precursors in deionized water, followed by the addition of a specific quantity of NaOH. NaOH reacts with nitrates and forms mixed metal hydroxides before calcination, which produce mixed metal oxides (perovskite). This mixture is washed and then subjected to a high-temperature solid-state reaction [41]. The conventional box furnace method at 1000–1500 °C with a ramp of 1–5 °C min−1 is typically used for sintering. Spark plasma and microwave sintering have been examined for rapid high-temperature results, with the aim of matching or surpassing the performance of conventional sintering [34][43].
The previous discussion encompassed two distinct electrolyte types (Figure 2), namely, the planar type (pellet and thin film), which necessitates sealing agents for the reactor connection, and the tubular configuration, which operates seamlessly without requiring sealing. Columnar electrolytes can be fabricated by templating using plaster molds or by rolling a thin-film electrolyte. Notably, columnar electrolytes have been employed in SOFCs [44][45][46]. Table 3 lists examples of columnar electrolyte utilization.
Energies 17 00441 g005
Figure 2. Illustration of (a) pellet, (b) thin-film, and (c) columnar electrolytes.
Table 3. Conductivities of columnar electrolytes and their deposition/synthesis method.
Electrolyte Method Conductivity Reference
BaZr0.4Ce0.4Y0.15Zn0.05O3 solid-state reaction Unknown [47]
BaZr0.1Ce0.7Y0.1Yb0.1 solid-state reaction Unknown [48]

2.2. Electrode Design Strategies

In contrast to thermochemical catalysts, electrocatalysts must be pretreated to ensure that they can mechanically bond to the electrolyte while remaining catalytically active. In electrolyte-supported cells, the cathode and anode are deposited on opposite sides of the cell. The difference between the anode and cathode materials makes it necessary to specify the method that should be used to deposit them onto the electrolyte.
Recently, various conventional and ambient-condition deposition methods, such as the doctor blade method, drop coating, screen printing, tape casting, and spray coating, have been used to develop electrode materials for PCECs (Table 4). Although these methods are simple, the electrode thickness is controlled only through a randomized parameter, such as printing passes or number of drops. Therefore, many researchers have recently employed PLD to produce a smooth electrode surface and ensure good interfacial contact between the electrolyte and electrode [49].
Table 4. Deposition methods and electrode thickness in key research on OER and NRR catalysts.
Cathode Deposition Method Thickness
(µm)		 Reference
La0.6Sr0.4Co0.2Fe0.8O3−δ Unknown 44 [50]
Ag - 4  
Pt - 8  
Fe doctor blade 15–25 [51]
10-Fe-BCY doctor blade 15–25  
0.5W-10Fe-BCY doctor blade 15–25  
PrBa0.5Sr0.5Co1.5Fe0.5O5+δ - 10–20 [23]
Ru–Ag/MgO Unknown - [28]
Ni-BCYR - - [52]
NdBa0.5Sr0.5Co1.5Fe0.5O5+δ (NBSCF)-BZCYYb drop coating 15 [53]
Pr2NiO4-BZCY screen printing 13 [54]
PrCo0.05Ni0.5O3−δ tape casting 29 [55]
Ba0.9Co0.7Fe0.2Nb0.1O3−δ screen printing 15 [56]
Pr0.2Ba0.2Sr0.2La0.2Ca0.2CoO3−δ spray coating 20 [57]
PrBa0.5Sr0.5Co1.5Fe0.5O5+δ PLD 20 [58]
Gd0.3Ca2.7Co3.82Cu0.18O9−δ screen printing 30 [59]

4. Current Progress

The NRR and OER have been studied extensively; the catalysts used for these reactions are summarized in Tables 5 and 6, respectively.

Table 5. Notable NRR catalysts in PCECs for NH3 synthesis.

Cathode *

Electrolyte

NH3 Production Rate [mol cm−2 s−1] × 10−9

Thickness

(µm)

Reference

La0.6Sr0.4Co0.2Fe0.8O3−δ

BaZr0.8Y0.2O3−δ

0.0850

44

[24]

Ag

BaZr0.8Y0.2O3−δ

0.0490

4

 

Pt

BaZr0.8Y0.2O3−δ

<0.0010

8

 

Fe

BaCe0.9Y0.1O3−δ

14.000

15–25

[26]

10-Fe-BCY

BaCe0.9Y0.1O3−δ

0.4200

15–25

 

0.5W-10Fe-BCY

BaCe0.9Y0.1O3−δ

0.5700

15–25

 

Ru–Ag/MgO

SrCe0.95Yb0.05O3−δ

0.0003

-

[41]

Ni-BCYR

BaCe0.9Y0.1O3−δ

0.0110

-

[63]

Based on Table 5, metallic catalysts evidently yield higher reaction rates. This could be attributed to two main factors. First, perovskite-based electrocatalysts may possibly be affected by degradation at the interface and thermal mismatch with the electrolyte, thus decreasing the performance [24]. Second, the electrochemical promotion of catalysis is more pronounced in pure metal catalysts with a higher effective double layer (S*eff) on their surfaces than in supported electrocatalysts [26]. However, pure metallic catalysts are typically expensive.

Ru is regarded as a suitable catalyst for thermochemical NH3 synthesis because of its peak position on Skulason’s volcano diagram, which shows that it requires a minimum potential for electrochemical NH3 synthesis. It has also been reported to be an ultra-efficient electrocatalyst for the NRR, with a lower reduction potential than that of Fe [71–75]. However, Ag is a more cost-effective option because of its natural abundance. Although noble-metal-based electrocatalysts exhibit favorable activity, efficiency, and selectivity, their practical application is inhibited by their high cost and scarcity [27]. Consequently, extensive research has been conducted on transition-metal-based electrocatalysts for the NRR. The NH3 synthesis rate of Pt catalysts can be primarily attributed to their strong HER activity [76,77]. At negative potentials, the surface of Pt nanoparticles tends to adsorb hydrogen atoms rather than nitrogen atoms, thus affecting the overall performance [78].

Table 6. Notable OER catalysts in PCECs for NH3 synthesis.

Anode

Electrolyte

Current Density @1.3 V and 550 °C

[A cm−2]

Thickness

(µm)

Reference

Pr0.2Ba0.2Sr0.2La0.2Ca0.2CoO3−δ

BaZr0.1Ce0.7Y0.1Yb0.1O3−δ

−0.800

20

[68]

PrBa0.5Sr0.5Co1.5Fe0.5O5+δ

BaZr0.4Ce0.4Y0.1Yb0.1O3−δ

−1.059

20

[69]

Gd0.3Ca2.7Co3.82Cu0.18O9−δ

BaZr0.1Ce0.7Y0.1Yb0.1O3−δ

−1.241

30

[70]

 

Considering NH3-producing PCECs, most studies have only focused on the NRR, whereas the OER has been overlooked. The NH3 synthesis reaction is typically performed at 475–600 °C [24]. Pei et al. briefly summarized the OER performance at a cell voltage of 1.3 V and operating temperature of 550 °C [67].

Currently, transition metals, particularly compounds based on Fe, Co, and Ni, have demonstrated remarkable catalytic activity for the OER [79]. A successful method to enhance the OER activity involves altering the surface electronic structure through the addition of supporting materials to the active metal (Fe, Co, or Ni). This strategy has attracted attention, particularly with reference to multi-metal materials such as high-entropy perovskites, because they provide numerous possibilities for modifying the characteristics and improving the catalytic performance [80].

Among multi-metal materials, Co-based double perovskite oxides are notable for their rapid ion diffusion and enhanced surface catalysis, resulting in high electrochemical performance in single cells [35,69,81]. Various studies have explored the application of OER catalysts in PCECs (Table 6). For example, Gd0.3Ca2.7Co3.82Cu0.18O9−δ exhibits the highest current density owing to various factors, including abundant oxygen vacancies in the central Co–O layer of the Ca3Co2O3 rock–salt subsystem, which alters the electronic charge carrier concentration. The needlelike grain morphology aids in the complex flow of the reaction components via triple conduction and open diffusion paths [70].

Despite the promising characteristics of Co-based double perovskite oxides, these high-entropy perovskite oxides have disadvantages such as instability, thermal mismatch, and high cost, which limit their widespread implementation [35,69,81,82]. Thermal mismatch occurs when the OER catalyst and electrolyte materials have different coefficients of thermal expansion (CTE). The CTE indicates the extent to which a material expands when exposed to changes in temperature. If the OER catalyst and electrolyte have significantly different CTE, they may expand at different rates as the temperature changes [83]. Therefore, catalysts with compatible mechanical properties need to be used.

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Subjects: Electrochemistry
Contributors MDPI registered users' name will be linked to their SciProfiles pages. To register with us, please refer to https://encyclopedia.pub/register :
Hizkia Manuel Vieri
,
Moo-Chang Kim
,
Arash Badakhsh
,
Sun Hee Choi
View Times: 105
Revisions: 6 times (View History)
Update Date: 07 Mar 2024
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