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Lee, H. Low-Dimensional Photocatalysts for CO2 Conversion. Encyclopedia. Available online: https://encyclopedia.pub/entry/9130 (accessed on 24 April 2024).
Lee H. Low-Dimensional Photocatalysts for CO2 Conversion. Encyclopedia. Available at: https://encyclopedia.pub/entry/9130. Accessed April 24, 2024.
Lee, Hyeonseok. "Low-Dimensional Photocatalysts for CO2 Conversion" Encyclopedia, https://encyclopedia.pub/entry/9130 (accessed April 24, 2024).
Lee, H. (2021, April 28). Low-Dimensional Photocatalysts for CO2 Conversion. In Encyclopedia. https://encyclopedia.pub/entry/9130
Lee, Hyeonseok. "Low-Dimensional Photocatalysts for CO2 Conversion." Encyclopedia. Web. 28 April, 2021.
Low-Dimensional Photocatalysts for CO2 Conversion
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This entry is adapted from the peer-reviewed paper 10.3390/catal11040418

The ongoing energy crisis and global warming caused by the massive usage of fossil fuels and emission of CO2 into atmosphere continue to motivate researchers to investigate possible solutions. The conversion of CO2 into value-added solar fuels by photocatalysts has been suggested as an intriguing solution to simultaneously mitigate global warming and provide a source of energy in an environmentally friendly manner. There has been considerable effort for nearly four decades investigating the performance of CO2 conversion by photocatalysts, much of which has focused on structure or materials modification. In particular, the application of low-dimensional structures for photocatalysts is a promising pathway. Depending on the materials and fabrication methods, low-dimensional nanomaterials can be formed in zero dimensional structures such as quantum dots, one-dimensional structures such as nanowires, nanotubes, nanobelts, and nanorods, and two-dimensional structures such as nanosheets and thin films. These nanostructures increase the effective surface area and possess unique electrical and optical properties, including the quantum confinement effect in semiconductors or the localized surface plasmon resonance effect in noble metals at the nanoscale. 

photocatalysis carbon dioxide conversion nanostructures low-dimensional photocatalysts solar fuels

1. Background

The fast-developing modern technology and explosive world population growth have resulted in a huge demand for and consumption of energy. According to an investigation from the U.S. Energy Information Administration, more than 600 quadrillion Btus of energy were spent in 2020 and it is expected that the demand will continue to skyrocket annually. To meet this huge energy demand every year, energy production has been predominately dependent on fossil fuels such as coal, oil, or natural gas. The energy production by fossil fuels is inextricably linked to the gigantic CO2 emission of more than 30 billion metric tons every year and, in turn, the accumulated CO2 in our atmosphere is deemed to be the main cause of many environmental problems such as global warming and erratic weather patterns. In this context, there is great motivation to find a way of reducing atmospheric CO2 and producing energy at the same time. For these problems, CO2 conversion by photocatalyst materials under light illumination could be an expedient solution. This is because natural sunlight provides clean, renewable, and abundant energy, and photocatalysts can be activated by light energy from the Sun, while simultaneously consuming CO2 for energy production.

In 1978, by Halmann [1], the first demonstration of the photocatalytic conversion of CO2 in aqueous solution into liquid fuels such as methanol, formic acid, and formaldehyde was achieved over p-type gallium phosphide semiconductor. The same year, the photoartificial synthesis by SrTiO3 photocatalysts for CH4 production through the gas-solid phase reaction of CO2 and H2O was reported by Hemminger [2]. In 1979, another pioneering work by Fujishima and his coworkers introduced the artificial synthesis of solar fuels from a CO2-saturated electrolyte under light illumination. In this study, liquid CO2 was converted with various semiconductor photocatalysts such as TiO2, ZnO, CdS, GaP, SiC, and WO3 to produce methane, methanol, formaldehyde and formic acid [3]. Since these historical works mentioned above, several semiconductor materials have been investigated for the conversion of CO2 into useful fuels, including graphitic carbon nitride (g-C3N4), graphene, conjugated polymers, covalent organic framework, metal organic frameworks, metal chalcogenides, metal oxides, black phosphorus, bismuth-based materials, and perovskites [4][5][6][7][8][9][10][11][12][13][14]. Moreover, a variety of strategies and approaches have been applied to improve the photocatalyst performance through elemental doping, solid solution, heterostructure, nanostrucutralization, surface engineering and modification, crystal facet engineering, cocatalysts utilization, or dimensionality tailoring [15][16][17][18][19].

Of the strategies researched to boost the efficiency of CO2 conversion, decreasing the dimensionality and constructing nanostructures of the photocatalyst have attracted a lot of attention owing to their favorable advantages in photocatalysis: first, nanostructured photocatalysts suppress the carrier recombination due to their higher crystallinity compared to non-nanostructured materials [20][21][22]; second, the implementation of low dimensionality modifies the electronic structure of bulk materials due to the quantum confinement effect in semiconductors or localized surface plasmon resonance effect in noble metals at the nanoscale; third, low-dimensional materials possess larger surface-area-to-volume ratio in comparison with bulk materials, providing more reaction sites. All three features can contribute to improved solar-driven catalytic reactions [19][23].

2. The Main Fundamentals of CO2 Photoconversion into Solar Fuels and Hydrocarbon Species

2.1. Nature of CO2

Carbon dioxide (CO2) is one of the primary greenhouse gases but, at the same time, it is the main resource for solar fuel production when coupled with proton donors such as H2O for photocatalytic CO2 conversion. Hence, understanding the nature of the gaseous CO2 molecule itself is necessary for efficient utilization of photocatalysts. CO2 is a stable linear molecule among carbon compounds because of it is in the highest oxidation state of carbon, C+4 [19]. The CO2 molecule has two C=O bonds with a dissociation energy of ~750 kJ/mol, which is quite larger than those in other chemical bonds such as C-H (~430 kJ/mol) and C-C (~336 kJ/mol). For this reason, the reduction of CO2 to produce solar fuels requires additional energy to break the C=O bond and form, for example, a C-H bond [24]. Owing to its stability and strong bonding, photocatalytic reduction of CO2 into solar fuels can be achieved primarily with the support of proton donors such as H2O or H2 [25].

2.2. CO2 Adsorption on the Surface of Photocatalysts

The adsorption and activation of CO2 on a solid surface is one of the essential steps in achieving CO2 reduction and photocatalytic performance. The adsorption mechanism of CO2 on several semiconductor photocatalysts has been investigated [26][27]. For instance, the adsorption of CO2 on TiO2 surface has been investigated by Minot and coworkers [26]. Various adsorption modes of CO2 over a rutile TiO2 surface have been studied using first-principles calculations. The oxygen atom of CO2 molecules favors the interaction with the acidic titanium cation over the surface forming a Ti–OCO bond [26]. The adsorption of CO2 on a photocatalyst surface includes the interaction between the CO2 molecule and the surface atoms of the photocatalyst. This absorption may occur with a charge transfer from the photocatalyst to the linear and stable CO2 molecule which can induce the formation of partially charged and bent adsorbate, COδ⋅−2, and this adsorbate can form three different molecular structures, as shown in Figure 1: oxygen coordination, carbon coordination, and mixed coordination [24][28][29]. The beneficial feature of COδ⋅−2, is that it has decrease in the lowest unoccupied molecular orbital (LUMO) of the CO2 energy level as linear CO2 molecule transformed into the bent structure. This would facilitate the charge transfer between a photocatalyst and COδ⋅−2, [24][28][29].

Catalysts 11 00418 g001 550

Figure 1. Schematic illustration of the different types of CO2 adsorption modes (Adapted from [24]).

In the photocatalytic reaction, the photocatalyst donates electron to the adsorbed species on the surface to initiate the reduction process of CO2 in the presence of protons. As shown in Table 1, the solar fuel production is determined by the number of electrons and protons included in the reaction [20][24]. For example, two electrons are required for CO evolution, while methane production is an eight-electron reaction. The adsorption of CO2 on the photocatalyst surface can be improved by a variety of strategies. First, decreasing the structural dimensionality of photocatalyst can improve the surface area of the photocatalyst to allow more adsorption. Second, enhanced density of active sites by incorporation of surface defects, such as oxygen and sulfur vacancies, can improve the CO2 adsorption. Third, utilization of noble metal nanoparticles can help improve the adsorption due to lowered activation energy of the CO2 reduction [24][30].

Table 1. Standard electrochemical potentials of CO2 and H2O at 25 °C and atmospheric pressure [20][24].

Reaction Eo at pH 7
(V vs. NHE)		 Solar Fuel
CO2 reduction CO2 + 2H+ + 2e− → CO + H2O −0.51 CO
CO2 + 8H+ + 8e− → CH4 + 2H2O −0.24 CH4
CO2 + 6H+ + 6e− → CH3OH + H2O −0.39 CH3OH
2CO2 + 12H+ + 12e− → C2H5OH + 3H2O −0.33 C2H5OH
CO2 + 2H+ + 2e− → HCOOH −0.58 HCOOH
CO2 + 4H+ + 4e− → HCHO + H2O −0.48 HCHO
H2O oxidation 2H2O → O2 +4H+ +0.81 O2

2.3. The Mechanism of Efficient CO2 Photoconversion

Upon absorption of light over the photocatalyst, charge carrier pairs are generated to achieve the photosynthesis of solar fuels accompanying the water splitting as shown in Table 1. To execute the conversion of CO2 into useful fuels from the thermodynamic point of view, the conduction band minimum (CBM), and the valence band maximum (VBM) of a photocatalyst should bracket the redox potential of CO2 and the oxidation potential of water, respectively, as shown in Table 1 and Figure 2. As results of the reactions, various solar fuels can be formed dependent on the number of electrons and protons in the presence of CO2 and water under the illumination.

Catalysts 11 00418 g002 550

Figure 2. The energy band structures of semiconductor photocatalysts and the corresponding redox potentials of CO2 reduction into solar fuels (Adapted from [31]).

The artificial photosynthesis of solar fuels using semiconductor photocatalysts consists of three essential steps, as described in Figure 3. Firstly, incident photons of light with energy higher than that of semiconductor band gap (Eg) induce the generation of the electron-hole pairs (Process (i)). Secondly, the photogenerated charge carriers are transferred to the photocatalyst surface (Process (ii)). Thirdly, the electrons and holes react on the surface of photocatalyst with CO2 and H2O for evolution of solar fuels (Process (iii)). For efficient photocatalytic conversion of CO2 into fuels, the ideal semiconductor photocatalyst should have optimized band gap for efficient light harvesting and photocarrier generation, facile charge separation and transportation, vigorously activated sites and high surface area for maximum adsorption of CO2 and water [30][32].

Catalysts 11 00418 g003 550

Figure 3. A schematic diagram of CO2 photocatalytic conversion process over photocatalyst. Process (i): light absorption and generation of photocarriers via a semiconductor photocatalyst. Process (ii): charge carrier separation and transfer to the surface of photocatalyst. Process (iii): reactions of CO2 and H2O with electrons and holes, respectively to produce solar fuels.

3. Strategies for Enhancement in the Light-Driven CO2 Conversion over Low-Dimensional Photocatalysts

Applying low-dimensional structure to the photocatalytic system itself is a proven way for obtaining high CO2 conversion performance. However, further improvement is available by designing the structures or modifying the photocatalytic materials so that characteristics of photocatalysts or photocatalytic system are engineered. Here, we focus on these two major strategies for further enhancement of CO2 conversion by low-dimensional photocatalysts. Table 2 summarizes the examples mentioned in this section.

Table 2. Summary of low-dimensional photocatalysts used in photocatalytic reduction of CO2 into solar fuels. NC: Nanocrystal, GQD: Graphene Quantum Dot, NF: Nanofiber, NS: Nanosheet, CNT: carbon nanotube, Mt: montmorillonite, m-CN: modified g-C3N4, NR: nanorod, NW: nanowire, CND: carbon nano dot, p-CN: protonated g-C3N4, PGCN: porous g-C3N4, TEOA: triethanolamine, bpy: bipyridine, C3N4: Melon-based polymeric carbon nitride, UTNS: ultrathin nanosheet, P-g-C3N4: Phosphorus doped g-C3N4.

Dimensionality Morphology Photocatalyst Light Source Reducing Agent Main Product Activity
[µmol∙g−1∙h−1]		 Ref.
0D QD
3–12 nm		 CsPbBr3 300 W Xe lamp H2O CO
CH4		 4.26
1.53		 [33]
QD
2.3 nm		 Cs3Bi2I9 300 W Xe lamp H2O CO 1.15 [34]
QD
2.9 nm		 Cs3Bi2Br9 300 W Xe lamp H2O CO 26.95
QD
2.4 nm		 Cs3Bi2Cl9 300 W Xe lamp H2O CO 21.01
NC
9.5 nm		 Cs2AgBiBr6 AM 1.5G Ethyl acetate CO
CH4		 2.35
1.6		 [35]
QD
9.45 nm		 FAPbBr3 300 W Xe arc lamp H2O CO
CH4		 181.25
16.9		 [36]
QD
5.86 nm		 GQD 300 W Xe lamp
420 nm cutoff filter		 H2O CH3OH 0.695 [11]
1D NR CeO2 300 W Xe lamp H2O CO 0.020 [37]
NT TiO2 300 W Xe arc lamp
320 nm < λ < 780 nm		 H2O CH4 2.128 [21]
NR TiO2 300 W Xe arc lamp
320 nm < λ < 780 nm		 H2O CH4 1.41 [21]
NT P-g-C3N4 300 W Xe lamp H2O/TEOA CO
CH4		 2.37
1.81		 [38]
NT PGCN 300 W Xe lamp H2O/MeCN /TEOA CO 103.6 [39]
NT Bi12O17Cl2 300 W Xe lamp H2O CO 48.6 [40]
NT Bi12O17Br2 300 W Xe lamp H2O CO 34.5 [41]
2D NS g-C3N4 300 W Xe arc lamp MeCN/TEOA
(4:1)		 CO
CH4		 5.407
1.549		 [42]
UTNS g-C3N4 300 W Xe lamp H2O CH4
CH3OH		 1.39
1.87		 [43]
UTNS SiC 300 W Xe lamp H2O CO
CH4		 1.29
3.11		 [44]
UTNS Bi2MoO6 300 W Xe lamp H2O CO 3.62 [45]
0D/1D QD/NW Black P/WO3 300 W Xenon arc lamp H2O CO
C2H4		 ~ 135
~ 11		 [13]
QD (10 nm)/NT WS2/Bi2S3 300 W Xe arc lamp H2O CH3OH
C2H5OH		 9.55
6.95		 [46]
QD (3.5 nm)/NW Ti3C2/Cu2O 300 W Xe lamp H2O CH3OH 78.50 [47]
0D/2D QD (1.6 nm)/NS CuO/WO3 300 W Xe lamp
λ > 400 nm		 H2O CO 1.58 [48]
ND (4.4 nm)/NS CND/p-CN Xe arc lamp H2O CO
CH4		 5.88
2.92		 [49]
QD/NS TiO2/g-C3N4 300 W Xe lamp
λ > 400 nm		 MeCN/TEOA CO 77.8 [50]
QD (5nm)/NS Au/TiO2 300 W Xe arc lamp H2O CO
CH4		 19.75
70.34		 [51]
QD (7nm) /NS CsPbBr3/Bi2WO6 300 W Xe lamp
λ > 400 nm		 H2O CO/CH4 503 µmol∙ g−1 [52]
1D/2D NF/NS TiO2/MoS2 350 W Xe lamp H2O CH4
CH3OH		 2.86
2.55		 [53]
NT/NS CNT/g-C3N4 200 W Hg and solar simulator H2O CO
CH4		 410
74		 [54]
NR/NS/NF Au/TiO2/BiVO4 300 W Xe lamp H2O CO
CH4		 2.5
7.5		 [55]
2D/2D NS/NS Ti3C2/Bi2WO6 300 W Xe lamp H2O CH4
CH3OH		 1.78
0.44		 [56]
NS/NS Bi2WO6/BiOI 500 W Xe arc lamp
λ < 400 nm		 H2O CH4 2.92 [57]
NS/NS Mt/m-CN 35 W Xenon lamp H2O/H2 CO
CH4		 505
330		 [58]
NS/NS SnS2/TiO2 300 W Xe lamp H2O CH4 23 [59]
NS/NS g-C3N4/BiVO4 300 W Xe lamp
λ ≥420 nm		 H2O CO
CH4		 5.19
4.57		 [60]
NS/NS PGCN/Bi12O17Cl2 300 W xenon lamp H2O CH4 24.4 [61]
NP-NS/NS Pd-g-C3N4 /RGOA 300 W Xe lamp H2O CH4 6.4 [62]

3.1. Construction of Junction Formed by Low-Dimensional Structures

Of the diverse strategies to promote CO2 conversion performance of photocatalysts, designing or formation of junctions in photocatalytic systems has seen some success by modifying optical and electrical properties through materials and interfaces [51]. Junctions are constructed by coupling of two or more semiconductor materials or metal materials. The formation of a junction allows valuable properties from various materials to be more available in a single system. That helps more efficient light absorption, charge separation and transfer, or more stable performance. Since the photocatalytic systems with junctions have single or multiple interfaces, the engineering of the interfacial characteristics between the materials is essential for efficient photocatalyst performance. Especially, the interface characteristics can influence on carrier behaviors through bulk or at interfaces (ex. Shockley-Read-Hall recombination).

The formation of junctions implies the presence of an internal electric field in the nanomaterial. This internal electric field can contribute to enhanced carrier behaviors such as carrier separation and transfer for the photo-induced charge carriers and to, in the end, the performance of light-driven CO2 conversion. The internal electric field can be induced by growth of a low-dimensional semiconductor on a low-dimensional semiconductor [23][63]. The combination of two or multiple low-dimensional materials could integrate the advantages of both single units and mitigate the shortcomings of single unit by the synergistic effect [64].

One of the advantages of semiconductor QDs is the quantum size effect which is responsible for the optical properties of the photocatalyst. Apart from the acceleration of charge separation and transfer process, the contact between 0D semiconductor and 1D semiconductor provides the nanocomposite with an additional properties such as excessive electroactive sites, high surface area, and homogenous dispersion [65]. 1D Bi2S3 nanotubes have outstanding ability to absorb visible and near infrared light. The tubular structure of Bi2S3 provides the photocatalytic reaction with more active sites than other morphologies [46]. The remarkable optical and electronic properties of tungsten disulfide (WS2) QDs can be realized due to the quantum confinement effect. WS2 QDs can be also dispersed uniformly on the surface of Bi2S3 forming Bi–S channels to facilitate the charge carrier separation transfer process. The designed 0D/1D nanocomposite exhibited outstanding photocatalytic reduction of CO2 into CH3OH and C2H5OH of 38.2 µmol∙g−1 and 27.8 µmol∙g−1 after 4 h radiation, respectively. The improved photoreduction performance is related to the following features. Firstly, the 0D/1D nanocomposite provided combined optical and electrical properties of both WS2 QDs and Bi2S3 nanotubes causing high visible and near infrared light absorption. Secondly, the enlarged surface area of the nanocomposite provided more active adsorptions site for CO2. Thirdly, the low resistive QDs–NTs interface due to the Bi–S bonds plays a critical role for accelerated charge carrier separation [46]. CsPbBr3 is widely used in the photocatalytic reactions but it suffers from the high rate of recombination during the interface transfer due to the strong reductive ability of electrons [52]. Hence, the suppression of undesired electron loss throughout the transfer process at the interface is critical factor for efficient utilization of CsPbBr3. Li et al. fabricated 0D/2D nanocomposite of CsPbBr3/Bi2WO6 via ultrasonic method with intimate contact at the interface to improve the charge separation and transfer. The Bi–Br bonds which is formed at the QDs–NSs interface is responsible for the strong interfacial interaction. The decoration of Bi2WO6 with CsPbBr3 QDs could enhance the CO and CH4 yield by factor of 9.5 over that of pristine CsPbBr3 [52].

The building of 1D semiconductor materials on 2D semiconductors is an efficient strategy for efficient CO2 conversion. Coupling of TiO2 nanofibers with light harvesting semiconductors such as MoS2 nanosheets is an efficient way to overcome the fast recombination of charge carriers and enhance the light absorption efficiency [53]. The electronic properties of MoS2 nanosheets can be tuned by control of the thickness. The superior conversion activity of CO2 into hydrocarbon species, that is, CH4 and CH3OH, resulted from the improved light harvesting, sufficient reactive sites for CO2 adsorption, and the intimate 1D–2D chemical contact between MoS2 and TiO2 which could be favorable for facile and efficient charge separation upon photoexcitation [53]. The increase of the contact area between the two semiconductor nanomaterials is much more favorable to enhance the photocatalytic performance over the photocatalyst. In other words, constructing the 2D/2D interface is favorable for highly separated charge carriers at the interface. Wang et al. prepared 2D/2D heterojunctions by growth of ultrathin tin disulfide (SnS2) onto TiO2 nanosheets via a hydrothermal method [59]. The production yield of CH4 over SnS2/TiO2 was much higher than that of pristine SnS2 and TiO2 nanosheets. The reason for such outstanding performance originates from the increment of the contract area between SnS2 and TiO2 nanosheets [59].

The photocatalytic systems with multiple junctions, that is, with multiple interfaces, displays excellent photocatalytic activity toward solar fuels generation compared to one with/without single junction [55][66][67]. Recently, Macyk and coworkers designed two heterointerface-based photocatalyst, TiO2/C3N4/Ti3C2, via the interfacial assembly of Ti3C2 QDs on the TiO2/C3N4 binary nanocomposite to boost the charge separation and transfer and providing strong redox ability in CO2 photoreduction reaction [67]. The as-synthesized composite exhibited enhanced light absorption, suppressed electron-hole recombination, and demonstrated stable photocurrent sensitivity. The fabricated composite could overcome the disadvantage of TiO2/C3N4 nanocomposites with a single junction by providing more efficient transport channels of electrons-hole pairs due to the strong interaction between Ti3C2 QDs and TiO2/C3N4 NS. Theoretical studies demonstrated that construction of two interfacial electric fields between TiO2/C3N4 and Ti3C2/C3N4 is due to electron transfer processes at the two interfaces. The interfacial built-in electric fields can promote the charge carrier separation and the photocatalytic reduction of CO2 into CO and CH4. Tonda et al. fabricated another multijunction system with a Bi2WO3/RGO/g-C3N4 2D/2D/2D architecture using two-step hydrothermal method for utilization in CO2 and water reduction into useful fuels [66]. This ternary heterojunction exhibited highly improved characteristics in light harvesting ability, CO2 adsorption capacity, photocurrent responses, and interfacial contact area. The photoconversion performance of CO2 over Bi2WO3/RGO/g-C3N4 was dramatically enhanced toward CH4 and CO evolution. The performance of Bi2WO3/RGO/g-C3N4 was 2.5 times higher and 3.8 times higher than those of Bi2WO3/RGO and RGO/g-C3N4, respectively [66].

3.2. Modification of Low-Dimensional Nanomaterials

Modification of nanostructured low-dimensional photocatalysts themselves are another beneficial strategy for the enhancement of photocatalytic CO2 conversion because it helps the properties of photocatalysts to be engineered. The modification can be achieved using several approaches such as introduction of surface oxygen vacancies or the formation of a porous structure.

The efficient utilization of the solar spectrum can be controlled by tuning the band structure of the semiconductor using the elemental doping [19]. Yu et al. synthesized oxygen-doped g-C3N4 nanotubes via exfoliation and a 3D g-C3N4 curling condensation method [68]. It was found that the synthesized photocatalyst consisted of curled nanosheets that had a uniform tubular structure with 20–30 nm of diameter. The oxygen atoms can substitute for the C or N atoms in g-C3N4 under high temperature oxidation conditions. The oxygen doping of 1D g-C3N4 helped the conduction band to be at a more positive potential causing a narrower band gap and efficient light harvesting. This structure exhibited a significant methanol evolution rate of 0.88 µmol∙g−1∙h−1 under visible light radiation. Wu et al. synthesized self-doped black TiO2 nanotubes arrays using a one-step aluminothermic reduction for solar-driven conversion of CO2 into CO [69]. It is found that the average diameter of the nanotubes was 75–85 nm with 5–7 nm of wall thickness. The oxygen vacancies can act as active sites for CO2 molecules for efficient photogenerated charge carrier separation. The visible light absorption of black TiO2 was largely enhanced by virtue of the oxygen vacancies. The resulted photocatalytic conversion was 185.39 µmol∙g−1∙h−1 of CO evolution rate under visible light.

The introduction of defects into semiconductors can improve the photocatalytic activity of CO2 into solar fuels ascribed to the promotion of photogenerated charge carrier separation and the extended light absorption [70]. Liu and coworkers prepared Bi12O17Cl2 nanotubes with surface oxygen defects via solvothermal method [40]. The tubular structure plays crucial role for accelerating the photogenerated charge carrier separation, while the oxygen defects on the surface act as active centers for CO2 activation. It is found that the absorption of Bi12O17Cl2 nanotubes is improved in the visible region compared to its bulk counterpart. The defective ultrathin tubular structure of Bi12O17Cl2 provides effective CO2 conversion into CO with production yield of 16.8 times higher than bulk Bi12O17Cl2. The higher photocatalytic conversion rate can be attributed to faster charge separation on the surface of Bi12O17Cl2 nanotubes.

The porosity of nanostructured semiconductors provides an additional feature to increase the surface area of photocatalysts, and subsequently is favorable for the solar-driven reduction of CO2 into valuable fuels [71]. Huang et al. used a template-free method to prepare porous g-C3N4 with increased surface area [72]. It is reported that the porous g-C3N4 nanotubes had excellent photocatalytic conversion of CO2 into CO of 40 µmol∙g−1 within 4 h illumination. The CO yield was higher than that of bulk g-C3N4 by a factor of 5.6 originated from the higher surface area of the porous tubular structure, and the improved charge carrier separation and transfer process.

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Hyeonseok Lee
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