Abstract
Photocatalytic synthesis of hydrogen peroxide under mild reaction conditions is a promising technology. This article will review the recent research progress in the design of photocatalytic H2O2 synthesis systems. A comprehensive discussion of the strategies that could solve two essential issues related to H2O2 synthesis. That is, how to improve the reaction kinetics of H2O2 formation via 2e− oxygen reduction reaction and inhibit the H2O2 decomposition through a variety of surface functionalization methods. The photocatalyst design and the reaction mechanism will be especially stressed in this work which will be concluded with an outlook to show the possible ways for synthesizing high-concentration H2O2 solution in the future.
1 Introduction
H2O2 is an indispensable chemical in daily life. It has many applications in fields such as biology (Chang et al., 2021; Noh et al., 2020; Guarino et al., 2019), medicine (Andersen et al., 2006; Kozlova et al., 2015; Wang Y. et al., 2020), chemical industry (Chung et al., 2020; Zhang et al., 2021), environmental protection (Dinakar et al., 2020; Moreno, 2011). As a clean oxidant, the decomposition of H2O2 only yields H2O, which does not pose an environmental risk. Currently, the anthraquinone (AQ) method is the main method for the industrial production of H2O2 (Sterenchuk et al., 2018). The AQ method for H2O2 synthesis includes two steps: hydrogenation and oxidation (Campos-Martin et al., 2006; Halder and Lawal, 2007; Gao et al., 2020). In this method, AQ is used as an intermediate, and the hydrogenation reaction is first performed with palladium catalyst (Chen, 2008; Edwards and Hutchings, 2008; Han et al., 2015). Then, oxygen is added to oxidize the hydroanthraquinone (AQH2) back to AQ and produce H2O2 (Figure 1). However, the AQ method not only has the risk of explosion, but consumes a lot of energy and organic solvent (Chen, 2008; Jia et al., 2018). Therefore, it is crucial to develop a safe and direct method to synthesize H2O2. The methods of direct H2O2 synthesis mainly includes electrocatalysis (Apaydin et al., 2018; Du et al., 2020; Sun et al., 2020; Shu et al., 2021), photocatalysis (Chen et al., 2018; Kormann et al.), and thermal catalysis (Adams et al., 2021). The electrocatalytic H2O2 synthesis has a high yield but it needs to consume useful electricity. Thermocatalytic H2O2 synthesis from oxygen and hydrogen also faces the risk of explosion when mixing the gases. The emerging photocatalytic H2O2 synthesis only uses solar energy to drive reaction without introducing hydrogen.
FIGURE 1
Flow chart of synthesis of H2O2 by AQ method (Yang et al., 2018).
During photocatalytic H2O2 synthesis, the electron is first excited from the valence band to the conduction band of the photocatalyst. Then, it participates in oxygen reduction reactions (ORR) on the surface to generate H2O2. H2O2 synthesis via oxygen reduction can undergo two pathways. The step-by-step single-electron pathway is the first one (Eqs. 1–3), which is characterized by the presence of superoxide (HO2•) intermediate. The other is the direct two-electron (2e–) pathway (Eq. 1 and Eq. 4). Which one of these occurs can be confirmed by detecting the intermediate HO2• (Viswanathan et al., 2012; Baran et al., 2018; Fukuzumi et al., 2018; Haider et al., 2019; Anantharaj et al., 2021; Yang, 2021; Guo et al., 2022).
Photocatalytic H2O2 generation is also accompanied by a decomposition reaction, which is the root cause of poor reaction stability. The decomposition process includes photolysis and light-independent decomposition. Taking TiO2 as an example, photolysis can occur mainly in four ways (Ⅰ) photogenerated electrons reduce H2O2 to OH−and •OH; (Ⅱ) photogenerated holes oxidize hydrogen peroxide to O2 or superoxide radical •O2−; (Ⅲ) The titanium peroxide complex (Ti-OOH) formed on the surface by the interaction of TiO2 and H2O2 gradually degrades under visible light; (Ⅳ) direct decomposition of H2O2 under ultraviolet light. H2O2 can also be decomposed in ways independent of light, such as pH and temperature.
The formation and decomposition performance of hydrogen peroxide are closely related to the surface properties of semiconductor photocatalysts. First, the high selectivity of cocatalysts to 2e− ORR is needed to improve the photocatalytic H2O2 formation. Second, the functional modifier on photocatalyst can inhibit the decomposition of H2O2. These strategies indicate that surface functionalization of photocatalysts is very important. Considering these issues, we review the recent advances in the design of photocatalysts for H2O2 synthesis in this work.
2 Effect of cocatalyst on photocatalytic activity
2.1 Noble metal cocatalysts
Precious metals are widely used as cocatalysts in electrocatalysis and photocatalysis, while they also show excellent performance in ORR (Zinola et al., 1995; Chen et al., 2017a; Cai et al., 2019; Ignaczak et al., 2019; Jeon et al., 2020). Pt has good ORR performance and strong binding ability to intermediates such as O2 and OH•. When using Pt, generating H2O via 4e–ORR is favored, but it has poor selectivity for 2e–ORR (Kim J. et al., 2018; Chen J. Y. et al., 2020). Among these noble metals, Au has the best selectivity for 2e− ORR, which has achieved efficient photocatalytic H2O2 synthesis in photocatalytic reaction (Jirkovsky et al., 2010; Jirkovsky et al., 2011; Zuo et al., 2019a; Ignaczak et al., 2019; Sun et al., 2020). Zuo et al. studied the influence of a series of noble metal co-catalysts (Pd, Pt, Au, and Ag) on the performance of photocatalytic H2O2 synthesis over g-C3N4. They found that the maximum activity could be achieved when the Au loading amount is very low (0.01 wt%) on g-C3N4 (Figure 2A) (Zuo et al., 2019a). A similar study showed that Au cocatalyst has the highest activity among different precious metals modified g-C3N4 samples (Kim H. I. et al., 2018). Similar high activity was observed over Au loaded TiO2-based photocatalysts (Tsukamoto et al., 2012), (Li L. et al., 2021; Feng et al., 2021).
FIGURE 2
(A) Under visible light irradiation (λ > 420 nm), different noble metal loaded CN photocatalyzed H2O2 activity (Zuo et al., 2019a). (B) Mechanism for photocatalytic production of H2O2 on Au-Ag/TiO2 catalyst (Tsukamoto et al., 2012). (C) Photodecomposition of H2O2 under UV light with and without photocatalysts (Meng et al., 2020); (D) Energy diagrams for Au/TiO2 and Au/BiVO4, and reduction potential of O2 (Hirakawa et al., 2016).
The H2O2 yield of Au-Ag alloy cocatalyst supported on the surface of TiO2 was 2.3 times and 3.4 times higher than that of single Au or Ag cocatalyst. The reason was that the loaded Au-Ag alloy was conducive to the separation of electron holes, and the efficient photocatalytic reduction of O2 on Au atom promotes the formation of H2O2 (Figure 2B) (Tsukamoto et al., 2012). However, the activity of Au deposition on ZnO was better than that on TiO2, which is attributed to the more inert surface properties of ZnO than TiO2 when decomposing H2O2 (Figure 2C) (Meng et al., 2020).
Hirakawa et al. (Hirakawa et al., 2016) suggested that activity of Au cocatalyst is affected by the band structure of semiconductor photocatalytsts. They employed Au/BiVO4 photocatalyst to successfully produce H2O2 under visible light irradiation (λ> 420 nm). Since the conduction band potential of BiVO4 (0.02 V vs SHE) is more positive than the one-electron ORR potential (-0.13V) and more negative than the 2e− ORR (0.68 V vs SHE), the 2e− ORR can be selectively promoted while the one-electron ORR is inhibited. Compared with TiO2, BiVO4 has a narrower band gap, which indicates that BiVO4 has a better ability to utilize visible light and 2e ORR selectivity than TiO2 (Figure 2D).
2.2 Non-precious metal cocatalysts
Considering the scarcity and high cost of precious metals, developing non-precious metal co-catalysts for 2e–ORR is crucial (Zhang J. et al., 2020; Yan et al., 2020). For example, the surface of g-C3N4 was loaded with AQ as a cocatalyst. Its activity reached 361 μm/h, which was 4.4 times that of pure g-C3N4 and comparable to some precious metals. This is because, in addition to the 2e− ORR reaction catalyzed by pure g-C3N4, another H2O2 synthesis pathway via hydrogenation (AQ + 2H+ + 2e−→AQH2) and dehydrogenation (AQH2 + O2→AQ + H2O2) plays a key role in the photocatalytic reaction (Kim H. I. et al., 2018). For CoP loaded on g-C3N4, the catalytic activity of CoP/g-C3N4 (70 μM•h−1) was similar to that of Au/g-C3N4 (67.56 μM•h−1) (Zuo et al., 2019a). This can be attributed to the accelerated separation and transfer of g-C3N4 photogenerated charge by CoP (Peng et al., 2017). The method of loading quantum dots to improve visible light absorption and electron mobility is also beneficial to photocatalytic synthesis of H2O2 (Zheng et al., 2018; Zhang M. M. et al., 2020; Liu et al., 2021a). Table 1 summarizes the effects of cocatalysts on hydrogen peroxide production activity.
TABLE 1
| Photocatalyst | Catalyst mass | Incident light | Cocatalyst content | Reaction condition | H2O2 activity | Reaction mechanism∗ | References |
|---|---|---|---|---|---|---|---|
| Ag@U-g-C3N4-NS-1.0 | 0.1 g (100 ml) | 300 W Xe lamp (100 mW•cm−2) | Ag 1 wt% | pH = 3, O2, 1 mol/L HClO | 1.975 × 10–6 M•min−1 | — | Cai et al. (2019) |
| Au/C3N4-500(N2) | 1 g/L | 300 W Xe lamp (λ > 420 nm) | Au 2 wt% | pH = 3, O2, 5 vol% IPA | 1320 μmol•L−1 (4 h) | — | Chang et al. (2018) |
| Au/Bi2O3-TiO2 | 200 mg (200 ml) | 300 W Xe lamp (λ > 420 nm) | Au 0.1 wt%, Bi: Ti = 1 wt% | O2, 4 wt% C2H5OH | 11 mM (12 h) | (Ⅱ) | Feng et al. (2021) |
| Au/BiVO4 | 50 mg (30 ml) | 2 kW Xe lamp (λ > 420 nm) | Au 0.2 wt% | O2, 10 vol% EtOH | 40.2 μM (10 h) | (Ⅰ) | Hirakawa et al. (2016) |
| Au/CN | 400 mg (100 ml) | 300 W Xe lamp (λ > 420 nm) | Au 0.01 wt% | pH = 8.5, O2, 10 vol% C2H5OH | 2027 μM (30 h) | (Ⅰ) | Zuo et al. (2019a) |
| Au/β-CD-CN | 0.4 g (100 ml) | 2 kW Xe lamp (λ > 420 nm) | Au 0.05 wt% | O2, 10 vol% C2H5OH | 3000 μM (30 h) | (Ⅰ) | Zuo et al. (2020) |
| Ag/β-CD-CN | 0.4 g (100 ml) | 300 W Xe lamp (λ > 420 nm) | Ag 0.05 wt% | O2, 10 vol% C2H5OH | 1000 μM(30 h) | (Ⅰ) | Zuo et al. (2020) |
| Au/ZnO | 0.2 g (200 ml) | 300 W Xe lamp (UV-REF) | Au 0.1 wt% | O2, 4 wt% C2H5OH, 0.1M NaF | 1.5 mmol−1•h−1 | Au>0.1wt% (Ⅰ) Au<0.1wt% (Ⅱ) | Meng et al. (2020) |
| Au/SnO2-NR#TiO2 | 10 mg (10 ml) | 300 W Xe lamp (λ > 430 nm) | — | O2, 4% EtOH | 60 μM (6 h) | (Ⅰ) | Awa et al. (2020) |
| Au-Ag/TiO2 | 5 mg (5 ml) | 450 W high pressure Hg lamp (λ > 280 nm) |
Au 0.1 mol%, Ag 0.4 mol% | O2, 4 vol% C2H5OH | 3.4 m′M (12 h) | (Ⅰ) | Tsukamoto et al. (2012) |
| Au@MoS2 | 0.05 g (50 ml) | 300 W Xe lamp | Au 0.5 wt% | pH = 9, O2 | 1100 μM (12 h) | (Ⅰ) (Ⅲ) | Song et al. (2019) |
| Pt/TiO2 | 1 mg (20 ml) | 500 W Hg lamp (λ > 300 nm) | Pt 1 wt% | Ar | 5096 μmol•L−1•h−1 | 2H2O→H2+H2O2 | Wang et al. (2019b) |
| Au-(ZT)-Al | 5 cm × 5 cm | 400–650 nm | 17 wt% | pH = 7, 5 vol% C2H5OH | 0.099 μM/min | — | Willis et al. (2020) |
| Pt-KCN(5) | 0.2 g (200 ml) | 400–800 nm | Pt 1 wt% | Remove air | 620 μmol•g−1 | (Ⅱ) | Hu et al. (2020) |
| Au/F-TiO2 | 0.2 g (200 ml) | 300 W Xe lamp (λ > 420 nm) | Au 0.1wt% | O2, 4 wt% C2H5OH | 6.5 mM (12 h) | (Ⅱ) | Li et al. (2021a) |
| Cu(hfacac)2/m-BiVO4 | 80 mg (80 ml) | 300 W Xe lamp (λ > 430 nm) | 400 μM Cu(hfacac) | O2, H2O:ACN:EtOH = 86:10:4 | 120 μM (2 h) | (Ⅰ) | Teranishi et al. (2020) |
| CoP/g-C3N4 | 20 mg (50 ml) | 300 W Xe lamp (λ > 420 nm) | CoP 1.76 wt% | O2, 10 vol% C2H5OH | 140 μM (2 h) | (Ⅱ) | Peng et al. (2017) |
| AQ/C3N4 | 0.5 g/L | 100 mW•cm−2 150 W Xe lamp | AQ 10 wt% | O2, 10 vol% IPA | 361 μmol•L−1•h−1 | (Ⅱ) | Kim et al. (2018b) |
| NiS@g-C3N4-30 | 10 mg (10 ml) | 300 W Xe lamp (λ > 420 nm) | Ni 2.06 wt% | O2, 10 vol% C2H5OH | 400 μM (1 h) | (Ⅱ) | Kim et al. (2018b) |
| Ti3C2/TiO2 | 50 mg (30 ml) | 9 W white lamp (λ = 365 nm) | 10% Ti3C2 | O2, 10 vol% C2H5OH | 359.43 μmol•h−1 | (Ⅱ) | Chen et al. (2021) |
| SN-GQDs/TiO2 | 25 mg (50 ml) | 500 W Xe lamp (λ > 300 nm) | SN-GQDs 0.5 wt% | pH = 3, O2, 6 vol% IPA | 451 μM (60 min) | (Ⅱ) | Zheng et al. (2018) |
| FeOOH QDs/CQDs/g-C3N4 | 25 mg (100 ml) | 300 W Xe lamp (λ > 420 nm) | FeOOH QDs 2 wt% | 10 ml IPA | 224.24 μmol h−1 •g | (Ⅱ) | Zhang et al. (2020b) |
Activities of photocatalysts with different types of cocatalyst.
The reaction mechanism is direct two electron oxygen reduction reaction, The reaction formula is: O2 + 2e− + 2H+ → H2O2 (Ⅰ); Step by step one electron oxygen reduction reaction, the reaction formula is: O2 + e− + H+ → •OOH, •OOH + e− + H+ → H2O2 (Ⅱ); OH− + OH−→H2O2 (Ⅲ).
3 Effect of surface modification on photocatalytic activity
In addition to increasing the activity of H2O2 production by the deposition of co-catalysts, decreasing the decomposition rate via surface modification is essential to maximize the final concentration of H2O2.
3.1 Surface passivation modification
TiO2 can catalyze the decomposition of H2O2 under visible light. Ti-OOH that form on the surface due to the interaction of TiO2 and H2O2 gradually degrade under visible light. This is the main reason for the decrease of H2O2 concentration during reactions (Li et al., 2001; Teranishi et al., 2010). Surface passivation can effectively inhibit the decomposition of H2O2. It can be carried out either by metal oxide passivation or non-metal passivation. Passivation of a photocatalyst with a metal oxide leads to the formation of a heterojunction (Zeng et al., 2017; Zuo et al., 2019b; Awa et al., 2020; Feng et al., 2021). For example, the surface of anatase TiO2 and rutile TiO2 were modified with SnO2 to form SnO2-TiO2 heterojunction. Then, the surface was functionalized with gold nanoparticles, and it was found that the formation activity of H2O2 was improved. This is because the decomposition of H2O2 on the TiO2 surface is inhibited (Figure 3A) (Zuo et al., 2019b). However, the H2O2 photocatalytic synthesis reaction rate of Au modified Bi2O3-TiO2 was better than that of Au/SnO2-TiO2. This is because not only the decomposition of H2O2 is inhibited, but also the carrier recombination in Bi2O3 is inhibited (Feng et al., 2021). A similar phenomenon is found in the heterojunction formed on g-C3N4 (Chen et al., 2017b; Chen X. L. et al., 2020; Liu et al., 2021b).
FIGURE 3
(A) Schematic illustration of H2O2 synthesis and decomposition over Au/SnO2 -TiO2 (Zuo et al., 2019b). (B) Photocatalytic H2O2 production over 0.1% Au/F-TiO2 prepared with different F/Ti ratios (Li L. et al., 2021).
Non—metallic surface modification was also effective for improving photocatalytic activity (Maurino et al., 2005; Moon et al., 2014; Zhang M. M. et al., 2020; Li L. et al., 2021). For example, by hydrothermal treatment of TiO2 and NaF to obtain F-TiO2, the decomposition of H2O2 is inhibited. This was due to the fact that the F ion fixed on the TiO2 surface competes with the Ti-OOH formation, thus reducing the Ti-OOH formation. Therefore, it was no longer necessary to add NaF to the photocatalytic reaction medium (Figure 3B) (Li L. et al., 2021).
3.2 Organic molecular modification
Imine organic molecules can be used to modify the surface of g-C3N4 to inhibit the electron-hole pair recombination of g-C3N4 (Shiraishi et al., 2014a; Kofuji et al., 2016; Yang et al., 2017; Goclon and Winkler, 2018; Guo et al., 2020; Zeng et al., 2020). For example, modification of the surface of g-C3N4 with homobendiimide and bibendiimide increased the synthesis activity of H2O2 (Figures 4A–C) (Shiraishi et al., 2014a; Kofuji et al., 2016). Besides the pure g-C3N4 reaction, another H2O2 synthesis pathway (•OH +•OH→H2O2) also plays a key role in the polyimide modified g-C3N4 nanosheets (Yang et al., 2017). In another publication, it was found that the modification of g-C3N4 by β-cyclodextrin can increase its hydrophobicity and affinity for oxygen, thus increasing the yield of H2O2 (Figure 4D) (Zuo et al., 2020).
FIGURE 4
(A) Three-dimensional structure of g-C3N4/BDI. (B) Proposed Mechanism for H2O2 Formation on the Photoexcited g-C3N4/BDI Catalyst. (C) Photocurrent response of g-C3N4/BDI50 and g-C3N4/PDI51 in 0.1 M Na2SO4 solution under visible light (λ >420 nm) at a bias of 0.5 V vs. Ag/AgCl (Kofuji et al., 2016). (D) The water contact angle of Au/β-CD-CN (Zuo et al., 2020).
Metal organic frameworks (MOFs) are promising materials that can be used to modify photocatalysts. This is because metal nodes and organic linkers of MOFs can be easily modified to improve photon absorption and catalytic activity. Therefore, various modification strategies have been devised, such as double substrate metal-organic framework, metal nanoparticles and MOF composite, etc (Wang Z. et al., 2020; Duan et al., 2020; Younis et al., 2020; Fang et al., 2021). The results showed that the activity of H2O2 synthesis was improved by modification of ZIF (Chang et al., 2020) and MIL (Isaka et al., 2019) type metal-organic framework materials. It was mainly attributed to the wider bandgap energy. Titanium-zirconium MOFs were prepared and used for photocatalytic production of H2O2 in two phase system (water/benzoic acid). Ti species effectively promoted electron transfer from the photoexcited linkers of MOFs to Ti and inhibited the recombination of electron-hole pairs in the hydrophobic MOFs matrix (Chen et al., 2020c). Table 2 summarizes the effects of different surface modifications on hydrogen peroxide production activity.
TABLE 2
| Photocatalyst | Catalyst mass | Incident light | Load | Reaction condition | H2O2 activity | Function of modification | Reaction mechanism∗ | References |
|---|---|---|---|---|---|---|---|---|
| MV-MS-CN/MAFO | 0.2 g (200 ml) | 250 W high-pressure sodium lamp (400–800 nm) | nMg: nAl: nFe = 5 : 2: 1 | O2, 0.5 mol L−1 NaNO2 | 6.3 mmol L−1 (18 h) | Surface passivation modification | (Ⅰ) | Chen et al. (2017b) |
| Au/SnO2-NR#TiO2 | 10 mg (10 ml) | 300 W Xe lamp (λ > 430 nm) | — | O2, 4% EtOH | 60 μM (6 h) | Surface passivation modification | (Ⅰ) | Awa et al. (2020) |
| F/TiO2(P25) | 0.5 g/L | 40 W fluorescent lamp (λ > 360 nm) | F 1.0 × 10–2 M | pH = 3.2, Air, 1.0 × 10–2 M HCOOH | 1.3 × 10–3 mol•L−1 (100 min) | Surface passivation modification | (Ⅱ) | Maurino et al. (2005) |
| Au/SnO2-TiO2 | 0.2 g (200 ml) | 300 W Xe arc lamp | Au 0.1 wt% n Sn:nTi = 4% | O2, 4% EtOH | 9 mM (12 h) | Surface passivation modification | (Ⅱ) | Zuo et al. (2019b) |
| TiO2/rGO/WO3(TRW) | 3 mg (30 ml) | 200 W arc Mercury-Xenon research lamp |
Na2WO4 0.5 M | — | 350 μM (80 min) | Surface passivation modification | (Ⅰ) | Zeng et al. (2017) |
| rGO/TiO2/P | 0.5 g/L | λ > 320 nm | rGO 6 wt%, 0.1 M of phosphate buffer | Ph = 3, O2, 5 vol% IPA | 4.5 mM (200 min) | Surface passivation modification | — | Moon et al. (2014) |
| HTNT-CD | 20 mg (15 ml) | 350 W Xe lamp (λ > 365 nm) | CDs 2.6 wt% | Air | 3.42 mmol gcat−1 h−1 | Quantum dots | (Ⅰ) (Ⅲ) | Ma et al. (2019) |
| g-C3N4/BDI | 100 mg (30 ml) | λ > 420 nm | melem:BTCDA (mol:mol) = 1::2.5 |
O2, 10 vol% 2-PrOH | 41 μmol (48 h) | Organic molecular modification | (Ⅰ) | Kofuji et al. (2016) |
| g-C3N4/PDI | 50 mg (30 ml) | Xe lamp (λ > 420 nm) | — | O2 | 50.6 μmol (48 h) | Organic molecular modification | (Ⅱ) | Shiraishi et al. (2014a) |
| RF523 @333 K | 50 mg (30 ml) | Xe lamp (λ > 420 nm) | — | O2 | 100 μmol (24 h) | Organic molecular modification | (Ⅰ) | Shiraishi et al. (2019) |
| PCNBA0.2 | 50 mg (30 ml) | 500 W Xe lamp (λ > 420 nm) | melem:BA = 3 g: 0.2 g | O2 | >2 mg/L (1 h) | Organic molecular modification | (Ⅱ) | Teng et al. (2020) |
| rGO/Cd3 (TMT)2 | 80 mg (20 ml) | λ > 420 nm | rGO 0.1 wt% | O2, 5 vol% MeOH | 7 mmol•L−1 (24 h) | Organic molecular modification | (Ⅱ) | Xu et al. (2017) |
| PI-NCN | 50 mg (50 ml) | 300 W Xe lamp (λ > 420 nm) | PI 5 wt% | — | 120 μmol (120 min) | Organic molecular modification | (Ⅱ) (Ⅲ) | Yang et al. (2017) |
| PEI/C3N4 | 20 mg (20 ml) | arc Xenon research lamp (Newport) with AM 1.5 air filter | PEI 50% W/V | O2 | 208.1 μM (60 min) | Organic molecular modification | (Ⅱ) | Zeng et al. (2020) |
| MIL-125-R7 | 5 mg (7 ml) | λ > 420 nm | caprylic anhydride treatment | BA/H2O = 5ml/2 ml | 1500 μM (2 h) | MOF | (Ⅱ) | Isaka et al. (2019) |
| ZIF-8 | 0.05 g (100 ml) | 350 W Xenon lamp | — | O2, water | 75 μmol•L−1•h−1 | MOF | — | Chang et al. (2020) |
| OPA/Zr100-xTix-MOF | 5 mg (7 ml) | 500 W Xe lamp (λ > 420 nm) | Ti: (Ti + Zr) (mol:mol) = 7.5% |
O2, BA/H2O = 5ml/2 ml | 9.7 mmol•L−1•h−1 | MOF | (Ⅱ) | Chen et al. (2020c) |
Activities of photocatalysts with different types of surface modification.
The reaction mechanism is direct two electron oxygen reduction reaction, The reaction formula is: O2 + 2e− + 2H+ → H2O2 (Ⅰ); Step by step one electron oxygen reduction reaction, the reaction formula is: O2 + e− + H+ → •OOH, •OOH + e− + H+ → H2O2 (Ⅱ); OH− + OH−→H2O2 (Ⅲ).
4 Effect of doping on the photocatalytic activity
Doping elements can effectively reduce the band gap of photocatalysts to improve the utilization of solar light (Akpan and Hameed, 2010; Zhao et al., 2017). Studies have shown that doping can change the number of active sites, reduce the formation energy of •OOH intermediates, and promote the formation of H2O2 (Li X. et al., 2021). Therefore, incorporating metal and non-metal ions in the photocatalyst can improve the photocatalytic synthesis activity of H2O2 (Table 3).
TABLE 3
| Photocatalyst | Catalyst mass | Incident light | Load | Reaction condition | H2O2 activity | Reaction pathway∗ | References |
|---|---|---|---|---|---|---|---|
| KBH4/g-C3N4 | 50 mg (100 ml) | 300 W Xe lamp (λ > 420 nm) | KBH4 0.17 wt% | O2, 10 vol% IPA | 287 μmol h−1 | (Ⅱ) | Feng et al. (2020) |
| KPF6-CN | 0.5 g/L | 300 W Xe lamp (λ > 420 nm) | 15 mmol KPF6 | Ph = 3, O2, 10 vol% EtOH | 1.5 mM (5 h) | (Ⅰ) | Kim et al. (2018c) |
| Cv-g-C3N4 | 0.1 g (100 ml) | 300 W Xe lamp (λ > 420 nm) | — | O2 | 90 μM (60 min) | (Ⅰ) | Li et al. (2016) |
| K+-Na+/g-C3N4 | 0.2 g (200 ml) | 250 W high-pressure sodium lamp (400–800 nm) | K+ 1.3 wt%, Na+ 0.7 wt% | O2, NaNO2 (0.5 mol L−1) | 4.6 mmol L−1 (18 h) | (Ⅰ) (Ⅲ) | Qu et al. (2018) |
| Pt-KCN | 0.2 g (200 ml) | 250 W high-pressure sodium lamp (400–800 nm) | Pt 1 wt%, 5 ml KOH (0.1 mol/L) | Remove the air | 620 μmol •g−1 | (Ⅱ) | Hu et al. (2020) |
| K2HPO4/GCN | 0.1 g (100 ml) | 300 W Xe lamp (λ > 420 nm) | Urea (g): Dopant (mmol) = 10 : 10 | O2, 10 vol% EtOH | 5.05 mM (10 h) | (Ⅰ) | Tian et al. (2019) |
| OCN(24) | 0.2 g (200 ml) | 250 W high-pressure sodium lamp (400–800 nm) | — | O2, 0.5 mol L−1 NaNO2 | 3.8 mmol L−1 (12 h) | (Ⅰ) (Ⅲ) | Wang et al. (2019a) |
| Ni-FCN | 0.2 g (200 ml) | 250 W high-pressure sodium lamp (400–800 nm) | nNi/dicyandiamide = 0.006 | O2 | 7.7 mmol L−1 (12 h) | (Ⅰ) | Wu et al. (2017) |
| KPD-CN | 20 mg (40 ml) | 300 W Xe lamp (λ > 420 nm) | Urea (g): Dopant (mmol) = 4 : 7.5 | pH = 3, O2, 10 vol% EtOH | 1.5 mM (7 h) | (Ⅰ) | Moon et al. (2017) |
| rGO/TiO2/P | 0.5 g/L | λ > 320 nm | rGO 6 wt%, 0.1 M of phosphate buffer | Ph = 3, O2, 5 vol% IPA | 4.5 mM (200 min) | — | Moon et al. (2014) |
| OCN-500 | — | λ > 420 nm | — | O2, 10 vol% IPA | 730 μmol (5 h) | (Ⅰ) | Wei et al. (2018) |
| AQ/U-POCN | 10 mg (20 ml) | 300 W Xe lamp (400–780 nm) | U-POCN: AQ = 12 μM: 4 μM | Air | 75 μM h−1 | (Ⅱ) | Ye et al. (2021) |
| Br-H-GCN | 0.2 g (200 ml) | 250 W high-pressure sodium lamp (400–800 nm) | Br 0.75 wt% | O2, 0.15g EDTA | 1.99 mmol L−1 (5 h) | (Ⅰ) | Zhang et al. (2018) |
Activities of photocatalysts with different types of ion doping.
The reaction mechanism is direct two electron oxygen reduction reaction, The reaction formula is: O2 + 2e− + 2H+ → H2O2 (Ⅰ); Step by step one electron oxygen reduction reaction, the reaction formula is: O2 + e− + H+ → •OOH, •OOH + e− + H+ → H2O2 (Ⅱ); OH− + OH−→H2O2 (Ⅲ).
4.1 Metal ion incorporation
Incorporating metal ions in the photocatalyst can improve the photocatalytic synthesis activity of H2O2 (Wu et al., 2017; Kim S. et al., 2018; Qu et al., 2018; Feng et al., 2020; Hu et al., 2020). For example, incorporating g-C3N4 with K+ can be used to photocatalyze water decomposition to produce H2 and H2O2 simultaneously without any sacrificial agent (Figure 5A). K+ was coordinated into the big C-N rings by forming the N-bridge, which inhibits the crystal growth of g-C3N4, promotes the specific surface area, increases the visible light absorption. More importantly, the CB and VB can be adjusted to the best position (Figure 5B) (Hu et al., 2020). A similar phenomenon of band gap adjustment was observed in g-C3N4 co-incorporated with K+and Na+. After the band gap adjustment, not only CB electrons can reduce O2 to produce H2O2, but also VB holes can oxidize OH− to •OH for H2O2 synthesis. This made the generation mechanism of photocatalytic H2O2 change from “single channel pathway” (O2 + 2e− + 2H+ → H2O2) to “dual channel pathway” (O2 + 2e− + 2H+ → H2O2 and •OH+•OH→H2O2 reaction pathways) (Qu et al., 2018).
FIGURE 5
(A) The schematic diagram of the reactor. (B) The band position of K+/g-C3N4 (Hu et al., 2020).
4.2 Non-metal ion doping
Non-metal ion doping photocatalyst can effectively improve the synthetic activity of H2O2 (Moon et al., 2014; Wei et al., 2018; Zhang et al., 2018; Wang L. C. et al., 2019; Ye et al., 2021). For example, halogens (Cl and Br) were incorporated into g-C3N4 by hydrothermal method (Figure 6A), and it was found that g-C3N4 incorporated with Br was more conducive to H2O2 synthesis. This is mainly due to the larger specific surface area and higher charge separation rate after incorporating (Figure 6B) (Zhang et al., 2018). A similar phenomenon was observed in the co-doping of metal ions and non-metals (K and P) (Figure 6C). Compared with g-C3N4 incorporated with P (NH4H2PO4/GCN) or K+ (K2SO4/GCN), the H2O2 generation of g-C3N4 after co-incorporating was 10.98 times of the former and 5.2 times of the latter, respectively (Figure 6D) (Tian et al., 2019). Similarly, co-doping can also improve the catalytic activity of TiO2. For example, Fe and S were co-doped into TiO2 by one-step anodic oxidation, and it was found that the synthesis activity of TiO2 was improved after doping. This is mainly attributed to the fact that Fe-S co doped TiO2 had a narrower band gap than pure TiO2, resulting in a wider visible light absorption range (Momeni and Akbarnia, 2021).
FIGURE 6
(A) The SEM images of Br-H-GCN. (B) PL spectra of GCN, Cl-H-GCN and Br-H-GCN (Zhang et al., 2018). (C) TEM images of the CNKP-10 catalysts. (D) UV–vis DRS spectra of the GCN and CNKP-10 catalysts (Tian et al., 2019).
5 Effect of reaction environment on photocatalytic activity
5.1 Effects of temperature and pH
One study investigated the effect of temperature and pH on the photoactivity of H2O2 generation by using Au/TiO2 photocatalyst. The results showed that when pH value (pH = 2) or temperature (5°C) was low, it was more beneficial to improve the photoactivity. The main reason was that the thermal catalytic decomposition of H2O2 by Au/TiO2 can be effectively inhibited at low pH value or low temperature (Teranishi et al., 2016). In another study, it was found that low pH also increased the H2O2 synthesis activity of MOFs materials. At the same temperature, when the pH value of MOFs material was as low as 0.3, the formation of H2O2 was more favorable. (Isaka et al., 2019).
5.2 Effects of sacrificial agents
For the photocatalytic production of H2O2, a certain amount of sacrificial agent is usually added to act as hole scavenger and prevent the recombination of electron–hole pairs. The sacrificial agents were mainly alcohols, which provided hydrogen source for photocatalytic H2O2 generation (Kormann et al.). However, the ability of aliphatic alcohols (such as ethanol and methanol, which act as electron donors) to improve photoactivity is limited. The results showed that g-C3N4 can effectively synthesize H2O2 in deionized water containing oxygen under visible light irradiation. This was due to the efficient formation of 1, 4-endoperoxide on the surface of g-C3N4. The addition of ethanol inhibited the one-electron reduction of O2 (formation of superoxide radicals) and selectively promoted the two-electron reduction of O2. At the same time, the photodecomposition of hydrogen peroxide formed subsequently was inhibited (Shiraishi et al., 2014b). Kim et al, (2016) also investigated whether the addition of electron donors affects photocatalytic activity. The results showed that when no sacrificial agent (methanol) was added to the system, the generation activity of H2O2 was extremely low. This result confirmed that using sacrificial agents such as methanol is important. When methanol (5 vol%) was present in the system, H2O2 was generated together with formaldehyde (CH3OH + O2 → HCHO + H2O2). Meanwhile, ethanol and 2-propanol were tested further, and the results showed that these alcohols worked effectively as electron donors.
However, aliphatic alcohols (such as ethanol and methanol) as electron donors have limited improvement in photocatalytic activity for hydrogen peroxide synthesis. Therefore, some studies have tried to use aromatic alcohol (benzyl alcohol) as a sacrifice agent, compared with fatty alcohol. The results showed that, during photoreaction with aliphatic alcohol, the carbon radical was rapidly removed and leaved superoxo radical (the f→i process in Figure 7), resulting in very low for H2O2 formation. In the aqueous phase containing benzyl alcohol, the carbon free radical was stably transformed into an oxygen bridge complex (f→g→h process in Figure 7), which generates a large number of peroxides and improves the synthesis activity of H2O2. The results showed that benzyl alcohol as electron donor can improve the reactivity. (Shiraishi et al., 2013).
FIGURE 7
Proposed mechanism for photocatalytic oxidation of alcohols with O2 on the TiO2 Surface (Shiraishi et al., 2013).
Conclusions and outlook
In future, the photocatalytic H2O2 synthesis system still need to improve the reaction activity and sustainability. We should consistently increase the upper limit of H2O2 production concentration in long-term photocatalytic reaction. The kinetics of photocatalytic H2O2 decomposition should be especially concerned. It is also urgent to develop efficient non-precious cocatalysts with two-electron ORR selectivity.
The activity of H2O2 synthesis was very unsatisfactory in most pure water systems. As a compromise for adding sacrificial reagents, the photocatalytic H2O2 synthesis system could be coupled with other valuable photocatalytic selective oxidation reaction to maximize its value, such as coupling with selective oxidation or photocatalytic degradation reactions.
Statements
Author contributions
Conceptualization, XM, XX, and JZ; writing—original draft preparation, HW, and SH; writing—review and editing, XM and VR; funding acquisition, XM. HW and SH contributed equally to this work. All authors have read and agreed to the published version of the manuscript.
Funding
This work received financial support from the National Natural Science Foundation of China (51872091), the Natural Science Foundation of Hebei Province (H2022209089), Basic Scientific Research Expenses of Universities in Hebei Province (JYG2021003 and JYG 2022001), and Tangshan Talent Funding Project (A202202007).
Conflict of interest
The authors declare that the research was conducted in the absence of any commercial or financial relationships that could be construed as a potential conflict of interest.
Publisher’s note
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Summary
Keywords
photocatalysis, oxygen reduction reaction, H2O2 synthesis, cocatalyst, surface modification, ion doping
Citation
Wen H, Huang S, Meng X, Xian X, Zhao J and Roy VAL (2022) Recent progress in the design of photocatalytic H2O2 synthesis system. Front. Chem. 10:1098209. doi: 10.3389/fchem.2022.1098209
Received
14 November 2022
Accepted
12 December 2022
Published
22 December 2022
Volume
10 - 2022
Edited by
Guigao Liu, Nanjing University of Science and Technology, China
Reviewed by
Ning Zhang, Central South University, China
Haiying Jiang, Northwest University, China
Shengyao Wang, Huazhong Agricultural University, China
Updates
Copyright
© 2022 Wen, Huang, Meng, Xian, Zhao and Roy.
This is an open-access article distributed under the terms of the Creative Commons Attribution License (CC BY). The use, distribution or reproduction in other forums is permitted, provided the original author(s) and the copyright owner(s) are credited and that the original publication in this journal is cited, in accordance with accepted academic practice. No use, distribution or reproduction is permitted which does not comply with these terms.
*Correspondence: Xianguang Meng, mengxg_materchem@163.com; Xiaole Xian, xianxiaole520@126.com; Jingjing Zhao, zhaojingjing@ncst.edu.cn
This article was submitted to Catalytic Reactions and Chemistry, a section of the journal Frontiers in Chemistry
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