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Article

Synthesis of g-C3N4-Decorated ZnO Porous Hollow Microspheres for Room-Temperature Detection of CH4 under UV-Light Illumination

by
Min Xiao
,
Yanwei Li
*,
Bo Zhang
,
Guang Sun
* and
Zhanying Zhang
School of Materials Science and Engineering, Cultivating Base for Key laboratory of Environment-Friendly Inorganic Materials in University of Henan Province, Henan Polytechnic University, Jiaozuo 454000, China
*
Authors to whom correspondence should be addressed.
Nanomaterials 2019, 9(11), 1507; https://doi.org/10.3390/nano9111507
Submission received: 29 August 2019 / Revised: 14 September 2019 / Accepted: 18 October 2019 / Published: 23 October 2019
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Abstract

:
UV light-assisted gas sensors based on metal oxide semiconductor (MOS) have attracted much attention in detecting flammable and explosive gases at room temperature. In this paper, graphite-based carbon nitride (g-C3N4) nanosheets-decorated ZnO porous hollow microspheres (PHMSs) with the size about 3~5 μm in diameter were successfully synthesized by annealing the solvothermally-synthesized Zn5(CO3)2(OH)6 PHMSs together with g-C3N4. The synthesized samples were characterized by XRD, SEM, TEM, FT-IR and XPS. The results indicated that the prepared g-C3N4/ZnO PHMSs were constructed by numerous loosely stacked ZnO nanoparticles of 20~30 nm in diameter. Gas sensing tests indicated that under UV light (365~385 nm) illumination, the sensors fabricated with g-C3N4/ZnO HPMSs showed an enhanced response and faster response speed than the pure ZnO counterpart at room temperature. In addition, the g-C3N4/ZnO sensor also exhibited good repeatability and long-term stability for CH4 detection.

1. Introduction

As active materials of solid-state gas sensors, metal oxide semiconductor (MOS) has been recognized a promising candidate for develop light-assisted low temperature sensor for the detection of flammable and explosive gases [1,2,3,4,5]. Methane (CH4), as a colorless and odorless fuel gas, has been widely used in various industries, as well as human daily life. However, owing to its flammable nature, the leakage of CH4 can endanger our environment by causing fire and explosion accidents. Therefore, developing safe and rapid methods for detecting CH4 is greatly desired. ZnO, as a cheap and easily available MOS material with a band gap of 3.4 eV, is a promising material for developing light-activated gas sensors that can work at a low temperature condition. Espid et al. studied the photo-responsive performance of ZnO/In2O3 sensors for detecting NO2 under UV LED irradiation at room temperature [6]. They found that the sensing process of composite materials relies on the irradiation of ultraviolet light, which can affect the response time of the sensors by changing the UV flux. Gong et al. fabricated the ZnO nanowires/optical fiber hybrid structure with responding to low concentration ethanol at ppb-level and achieved lower temperature sensing under UV light activation, the combination of UV radiation and ZnO is an effective way to develop high performance gas sensors [7]. Da Silva et al. synthesized ZnO-SnO2 heterojunctions for the room temperature photoluminescence-based ozone gas sensing, these ZnO-SnO2 heterojunctions were able to detect ozone with the concentration as low as 20 ppb [8]. The results of above reports indicate that UV irradiation is a promising way to achieve low temperature detection and improve gas sensing performance of ZnO sensors. However, there are few reports on the design and synthesis of ZnO based light-activated gas sensing materials for CH4 detection.
Two-dimensional (2D) graphite-based carbon nitride (g-C3N4) is a metal-free polymer n-type semiconductor. The unique electrical, optical, and physiochemical properties of g-C3N4 makes the g-C3N4-based material a new multifunctional platform for developing high performance MOS sensors [9,10]. Presently, g-C3N4-based gas sensors have attracted an increasing interest. Zhang et al., synthesized α-Fe2O3/g-C3N4 nanocomposites by a hydrothermal and pyrolysis method, and the α-Fe2O3/g-C3N4 sensor demonstrates a better gas sensing properties than the pure α-Fe2O3 and g-C3N4 [11]. Zhai et al. studied the UV light-assisted g-C3N4/ZnO composites for ethanol sensing characteristics at room temperature, which indicates that the content of g-C3N4 in the g-C3N4/ZnO composites has a great influence on the gas sensing performance [12]. These reports indicate that g-C3N4 can be an efficient material for improving the performance of ZnO MOS gas sensors. However, based on the excellent photocatalytic ability of g-C3N4, the g-C3N4-based materials are mostly used in energy and environmental photocatalysis applications, such as water splitting, environmental remediation and carbon dioxide reduction [13,14,15]. The design of high performance light-activated MOS gas sensors by utilizing g-C3N4 as sensitizer is still in the nascent stage.
In this paper, ZnO PHMSs decorated with g-C3N4 nanosheets were successfully prepared by annealing solvothermally-synthesized Zn5(CO3)2(OH)6 HMSs together with g-C3N4. The prepared samples were characterized with XRD, SEM, TEM, FT-IR and XPS. The results proved the successful decoration of g-C3N4 nanosheets on the porous shell of the ZnO PHMSs. The gas sensing properties of the prepared g-C3N4/ZnO composites were investigated. It was found that after decorating ZnO PHMSs with g-C3N4 nanosheets, the sensors showed a faster response speed and an enhanced response under UV-light illumination.

2. Materials and Methods

2.1. Materials

Urea (CH4N2O, 99%) and zinc acetate [Zn(CH3COO)2·2H2O, 99.0%] were purchased from Kermel (Kermel, Tianjing, China), citric acid (C6H8O7·H2O, 99.5%) and absolute ethyl alcohol (C2H6O, 99.7%) were purchased from Hongyan (Hongygan, Tianjing, China), distilled water was used throughout the experiments, all chemical reagents are analytical and are used without further purification.

2.2. Synthesis of g-C3N4/ZnO PHMSs

The synthesis of g-C3N4 is similar to our previous method [16]. 100 g urea was uniformly placed in a crucible and heated in a muffle furnace at 250 °C for 1 h in an air atmosphere at atmospheric pressure, 350 °C for 2 h, and finally 550 °C for 2 h, with a heating rate of 2 °C min−1, the yellow powder of g-C3N4 was received after cooling to room temperature.
Zn5(CO3)2(OH)6 was prepared by a solvothermal method. In a typical procedure, as illustrated in Figure 1, a mixed solution was obtained by adding 10 mL ethanol solution of urea (1.2 mol/L) and 5 mL ethanol solution of citric acid (0.12 mol/L) into 30 mL aqueous solution of Zn(CH4COO)2 (0.1 mol/L), in sequence. After stirring for 0.5 h, the mixed solution was transferred into a 50 mL Teflon-lined autoclave and maintained at 150 °C for 10 h. The precipitate was collected by centrifugation, washed with distilled water and ethanol, and dried in air at 60 °C, to obtain the Zn5(CO3)2(OH)6 precursor.
In order to synthesize g-C3N4/ZnO PHMSs, a desired amount of g-C3N4 was ground in an agate mortar and then dispersed in 20 mL of ethanol solution. After adding 250 mg of as-prepared Zn5(CO3)2(OH)6, the mixture solution was stirred at room temperature for 0.5 h and then dried at 70 °C to remove the solvent. The obtained powder mixture was then annealed at 400 °C in N2 atmosphere for 1.5 h to obtain the final g-C3N4/ZnO samples. By adjusting the using amount of g-C3N4, g-C3N4/ZnO samples with the g-C3N4 content of 3 wt.%, 5 wt.%, 8 wt.%, and 10 wt.% were prepared, which were denoted as CNZO-3, CNZO-5, CNZO-8, and CNZO-10, respectively. Pure ZnO was also prepared by directly annealing the Zn5(CO3)2(OH)6 precursor at the same condition.

2.3. Characterizations

The morphology and microstructure of prepared samples were observed by field-emission scanning electron microscopy (SEM, JEOL, JSM-6390LV, Tokyo, Japan) and transmission electron microscopy (TEM, JEOL, JEM-2100, Tokyo, Japan). The crystal phase of samples was analyzed by X-ray diffraction (XRD, Bruker/D8-Advance diffractometer, Brukerplc, Billerica, MA, USA) with Cu-Kα radiation in a scanning range of 10–80° (2θ). Surface chemical element analysis was characterized by using X-ray photoelectron spectroscopy (XPS, Thermo ESCALAB 250XI electron spectrometer, Waltham Mass, Waltham, MA, USA) with Al-Kα radiation, the C 1s peak was fixed at a binding energy of 284.6 eV. Fourier Transform Infrared Spectrometer (FT-IR, TENSOR27, Brukerplc, Billerica, MA, USA) with a resolution of 1 cm−1. The Brunauer Emmett Teller (BET) specific surface areas of the prepared samples were measured by nitrogen adsorption on a Quantachrome Autosorb-iQ sorption analyzer (Quantachrome, Boynton Beach, FL, USA).

2.4. Gas Sensor Fabrication and Analysis

The fabrication process of sensors is shown in Figure 2. In detail, a proper amount of as-prepared sample was mixed with in a few drops of deionized water to obtain slurry, which was carefully coated onto an Al2O3 ceramic substrate (13.4 × 7 mm) with interdigitated Ag-Pd electrodes and heat-treated at 60 °C for 24 h to obtain a resistance-type sensor.
The light-activated gas sensing performances of the fabricated sensors were tested on a CGS-4TPs gas sensing analysis system (Beijing Elite Tech Co., Ltd., Beijing, China), during which UV light was supplied by a UV lamp (λ = 365~385 nm, 4 W, 220 V). The vertical distance between UV lamp and sensor was 8.30 cm. In order to obtain a required concentration of target gas, a static gas distribution method was applied. The sensor response was defined as Ra/Rg, where Ra and Rg were the resistance of sensor in air and in target gas, respectively. The response and recover times were defined as the time required for the sensors’ resistance to 90% of the equilibrium state value after injecting and removing the target gas. During the gas sensing tests, the relative humidity (RH) in the test chamber was 20~25%.

3. Results and Discussion

3.1. Morphology and Structure Characterization of the Prepared Samples

Figure 3 shows the XRD patterns of the prepared samples. In Figure 3a, all diffraction peaks are accordance with the standard data of Zn5(CO3)2(OH)6 (JCPDS no. 19-1458), demonstrating the production of pure Zn5(CO3)2(OH)6 phase in the solvothermal step. After the annealing process, the Zn5(CO3)2(OH)6 precursor was completely transformed into hexagonal ZnO phase (JCPDS no. 36-1451), as shown in Figure 3b. The diffraction peaks at 2θ = 31.8°, 34.5°, 36.3°, 47.6°, 56.6°, 62.9°, 66.4°, 67.9°, 69.1°, 72.5° and 76.9° were indexed to (100), (002), (101), (102), (110), (103), (200), (112), (201), (400), and (202) planes of hexagonal wurtzite ZnO, respectively. In the XRD pattern of the prepared g-C3N4 sample, two distinct diffraction peaks at 13.6° and 27.9° were observed, which can be ascribed to the (100) and (002) planes of g-C3N4 [17,18], respectively. Besides of the peaks from ZnO, a small diffraction peak arising from g-C3N4 (2θ = 27.9°) was also observed in the CNZO-3, CNZO-5, CNZO-8 and CNZO-10 samples, indicating the successful preparation of the g-C3N4/ZnO composite after annealing the Zn5(CO3)2(OH)6 precursor together with g-C3N4. Moreover, the average crystallite sizes of the ZnO, CNZO-3, CNZO-5, CNZO-8 and CNZO-10 calculated by Scherrer’s formula were found to be 38.6, 33.7, 29.3, 22.8 and 21.5 nm, respectively. The decreased size of ZnO crystals with the increase of g-C3N4 contend indicates that the addition of g-C3N4 inhibited the further growth of ZnO crystals. No peaks from any other impurities were detected in all samples, showing the high purity of the obtained products.
Before calcination, the thermal stability of the prepared Zn5(CO3)2(OH)6 precursor was studied. In Figure 4a, the first weight loss between 75 and 281 °C on TG curve was associated with the evaporation of adsorbed water on the sample. The second weight loss at round 281 °C corresponds a weight loss of 27.2%, which is agreement with the theoretical weight loss of Zn5(CO3)2(OH)6 decomposition to produce H2O, CO2 and ZnO. Based on above results, in our experiment, the calcination temperature was set at 400 °C to ensure the complete decomposition of the Zn5(CO3)2(OH)6 precursor.
Figure 4b shows the FT-IR spectra of the prepared g-C3N4, ZnO and CNZO-8 samples. In the FT-IR spectrum of g-C3N4, the peaks at 813 and 890 cm−1 correspond to the stretching modes of triazine units [19,20], and the peaks around 1200–1650 cm−1 are attributed to the typical sp2 C=N stretching modes and the sp3 C-N stretching [21,22]. In the FT-IR spectrum of ZnO, the peaks at 433 and 499 cm−1 are ascribed to characteristic stretching of Zn–O bonds [23]. As for the composites samples of CNZO-8, besides of the characteristic peaks of Zn–O bonds, the stretching models of C-N were also detected, indicating the successful introduction of g-C3N4 in the host ZnO material.
Figure 4c,d show the N2 adsorption/desorption isotherms and pore size distribution of ZnO and CNZO-8, respectively. The nitrogen adsorption and desorption isotherms of both samples exhibit the type IV isotherm with H3 hysteresis loop. The BET surface areas of ZnO and CNZO-8 were calculated to be 95.1 and 182.1 m2/g, respectively. Obviously, after decoration with g-C3N4, the specific surface of ZnO hollow spheres was enlarged. Considering that the gas-sensing reaction is a surface-related process, the larger specific surface of g-C3N4/ZnO composite is helpful for achieving better gas sensing performance [24]. From the pore size distribution curves showed in Figure 4d, it can be seen that the dominant pore size in ZnO and CNZO-8 is around 2–6 nm.
Figure 5a,b display the typical FESEM images of the prepared g-C3N4, in which nanosheet-like g-C3N4 with the thickness about 80 nm can be clearly observed. From the low-magnification FESEM image showed in Figure 5c, one can see the prepared Zn5(CO3)2(OH)6 precursor is composed of spherical structures with the diameter about 3–5 μm. Closer observation (Figure 5d) further reveals that these microspheres are assembled from many densely stacked nanoflakes. Figure 5e,f show the FESEM images recorded from CNZO-8. It can be seen that the obtained product inherited the hollow microsphere structure from the precursor. Due to the decomposition of Zn5(CO3)2(OH)6, a loose and porous shell (about 300 nm in thickness) was formed on the ZnO hollow microspheres. In order to confirm the successful decoration of g-C3N4 nanosheets on the ZnO hollow spheres, the CNZO-8 sample was further observed by TEM. Figure 6a shows a typical TEM image recorded from the porous shell of a hollow microsphere, in which the ZnO nanoparticles (about 30–60 nm in size) covered with sheet-like g-C3N4 were clearly observed. In the HRTEM image showed in Figure 6b, clear lattice fringes were convinced. The interplanar spacing was measured to be 0.28 nm, matching well with the (100) plane of ZnO.
The chemical composition and the chemical status of the prepared pure ZnO and g-C3N4/ZnO composites were characterized by XPS. Figure 7a shows the full-range XPS survey spectra of different samples. The sharp photoelectron peaks of Zn 2p were observed in all samples. In the composite samples, N 1s peaks with a binding energy of 398.5 and 400.2 eV were observed, but being absent in the pure ZnO sample, further demonstrating the successful introduction of g-C3N4 in ZnO. Figure 7b,c show the high-resolution N 1s and C 1s spectra of CNZO-8, respectively. In Figure 7b, the peaks at 398.5 and 400.2 eV are assigned to sp2-hybridized nitrogen (C–N=C) and tertiary nitrogen (N–(C)3), respectively [25]. In Figure 7c, the C 1s peak at 284.9 and 288.2 eV can be ascribed to graphite carbon atoms and the sp2-bonded carbon (N–C=N) inside the aromatic structure [26]. The Zn 2p high-resolution spectra of ZnO and CNZO-8 (Figure 7d) can be fitted into two distinct peaks, including Zn 2p3/2 (1021.3 eV) and 2p2/1 (1044.6 eV), which are in agreement with the reported value of ZnO [27]. In the high-resolution O 1s spectra (Figure 7e), the signal of O 1s can be separated into three different peaks of lattice oxygen (OL: 530.1 ± 0.3 eV), oxygen-deficient regions (OV: 531.6 ± 0.4 eV) and chemisorbed oxygen species (OC: 532.3 ± 0.3 eV) [28]. The relative percentages of the peaks (OV) in the samples of ZnO and CNZO-8 were found to be 19.6% and 28.2%, respectively. Clearly, the OV component in the composite samples slightly increased with the increase of g-C3N4 content.

3.2. Gas Sensing Properties

The CH4 sensing properties of the sensors were tested under UV-light (365~385 nm) illumination at room temperature. Figure 8 shows the transient resistance change of the ZnO, CNZO-3, CNZO-5, CNZO-8 and CNZO-10 sensors as they were switched from air to CH4 atmosphere. It can be seen that all sensors give a decreased resistance in CH4, exhibiting a characteristic response of n-type MOS [29]. Importantly, as they were exposed to the same concentration of CH4 (2000 ppm), the five sensors showed different response-recover speeds. The measured response/recover times (Tres/Trec) were 78/90 s, 58/77 s, 45/72 s, 28/73 s and 30/70 s for ZnO, CNZO-3, CNZO-5, CNZO-8 and CNZO-10, respectively. Apparently, all the g-C3N4/ZnO sensors show faster response speed than the pure ZnO sensor. Moreover, the resistance baseline of sensors based on g-C3N4/ZnO is lower than that of the pure ZnO sensor, and decreased with increasing the amount of g-C3N4 in the composites.
The typical response curves of ZnO, CNZO-3, CNZO-5, CNZO-8 and CNZO-10 sensors at room temperature to different concentrations (500~8000 ppm) of CH4 with UV light activation are shown in Figure 9a. One can see that once exposed to different concentrations of CH4, all sensors can give a fast response before reaching their basic saturated states, and then decrease gradually as they were exposed to air again. In addition, with the increase of CH4 concentration, the response amplitudes of all sensors increased correspondingly, and the sensors based g-C3N4/ZnO can always give higher response amplitudes than the pure ZnO sensor, demonstrating the sensitization effect of g-C3N4 on ZnO. Among the five composite sensors, the CNZO-8 sensor shows the highest response amplitude, suggesting that the optimal content of g-C3N4 in the present composite system is 8 wt.%. Figure 9b shows the liner relationship between response and CH4 concentration of two different sensors. At a gas concentration of 2000 ppm, CNZO-8 sensors exhibit strong response signals (the response value is about 2 for CNZO-8 sensor). Furthermore, we can find that the sensors based on g-C3N4/ZnO have a good linear relationship in the test range (500~5000 ppm).
For practical application, good stability is an important evaluation criterion for a successful sensor. Thus, the stability of the CNZO-8 sensor was checked by testing its responses to 500, 2000, and 8000 ppm CH4. Figure 9c shows the repeatability test for the CNZO-8 sensor. Clearly, the CNZO-8 sensor accurately completed four consecutive gas response processes within 1500 s, and the response was basically stable at around 2. In general, sensors operating at a lower temperature (such as room temperature) can get a better stability because the higher operating temperature will affect the crystal structure of MOS sensor material. Moreover, to estimate the long-term stability of the CNZO-8 sensor, the CNZO-8 sensor exhibits a stable response to three concentrations of CH4 within ten weeks, in Figure 9d. It can be observed that the CNZO-8 sensor maintain its original response amplitude without significant attenuation.

3.3. Gas Sensing Mechanism

The widely accepted gas sensing mechanism of MOS sensors is based on the resistance change when the sensor was switched from air to target gas, which is closely related with gas adsorption, desorption and chemical reaction on surface of the sensing materials [30]. ZnO is a typical n-type semiconductor, and the charge carriers in its conduction band (ECB) are dominated by electrons. As shown in Figure 10a, when the ZnO sensor is irradiated with UV light, electrons in ZnO will be excited from the valence band (EVB) to the ECB when the energy of excitation source is higher than its band gap energy (Eg), leaving a hole (h+) behind. The photo-generated electrons and holes can recombine and get trapped in metastable surface states, or react with electron acceptors and donors adsorbed on the MOS surface, respectively [31]. During the gas sensing process, when the ZnO sensors are exposed to air, O2 will adsorb on the surface of ZnO and capture photo-generated electron to form photoinduced oxygen ions [O2−(hv)] [32,33], resulting in a higher sensor resistance (Ra) due to the formation of an electron depletion layer (EDL) on surface of ZnO. While, once the ZnO sensor is exposed to CH4, the redox reaction between the O2-(hv) and CH4 molecules will occur on the surface of ZnO nanoparticles, after which the trapped electrons by oxygen anions will be released back to ZnO. As a result, a lower sensor resistance (Rg) will be obtained because of the remarkably decreased EDL thickness. Since the response of the ZnO sensor to reducing gas is generally defined as Ra/Rg, the different resistance values of ZnO endows its sensing ability to CH4.
In our experiment, it was found that after decorating with g-C3N4, the ZnO sensor showed an improved response to CH4 under UV-light irradiation, which may be mainly attributed to effects of g-C3N4/ZnO heterojunction. The generation of O2− (hv) and oxygen defects will generate on the surface of heterojunction. On one hand, the formation of g-C3N4/ZnO heterojunction can promote the separation of electron-hole pair. In fact, the survival time of electron-hole pairs generated by UV-light irradiation is far shorter than the time required for migration towards the surface of the material for reacting with adsorbed oxygen ions. As a result, electron-hole recombination is a main factor that limits efficiency of the light-assisted gas sensor [34,35]. Here, the coupling effects of g-C3N4/ZnO heterostructure will take place, and some free electrons can transfer from g-C3N4 to ZnO until the two systems attain a new equilibrium Fermi energy level (EF), which will prevent the recombination of photo-generated electrons and holes, as illustrated in Figure 10b. Thus, during the gas sensing process, more photo-generated electrons will migrate to the surface of ZnO and react with oxygen molecules to form O2−(hv) [36]. As a result, a larger resistance change can be obtained when the sensor is switched from air to CH4 atmosphere, and a higher response was obtained correspondingly. Such process can be simply described as follows:
hv = h+ + e−(hv),
O2(gas) + e−(hv) = O2−(ads)(hv),
CH4 + 2O2−(ads)(hv) = CO2 + 2H2O +2e−fig
On the other hand, the formation of g-C3N4/ZnO heterojunction can result in the creation of more defects due to the mismatch of crystal lattice between ZnO and g-C3N4, such as oxygen vacancies OV. Based on the result of XPS analysis (Figure 5e), the OV content in CNZO-8 (28.2%) is found to be higher than that in pure ZnO (19.6%). Xue et al. studied the double defects (Zni and OV) of ZnO nanodishes for ethanol sensing characteristics, which explained that the mechanism of surface defects work on gas sensing performance. The sensing performance of ZnO sensor could be promoted by its rich electron donors OV, resulting in that oxygen molecules are more likely to capture electrons to form O2−(hv) on ZnO [37]. Thus, on the surface of CNZO-8, more active sites can be supplied for CH4 adsorption and O2−(hv) creation due to its higher OV content. Accordingly, when the CNZO-8 was exposed to CH4 atmosphere, more CH4 molecules will react with O2−(hv), also leading to a higher response. In addition, the higher surface area of CNZO-8 is also considered to be an important factor for its higher CH4 response. The result of N2 adsorption-desorption analysis shows that the BET surface area of CNZO-8 is 182.1 m2/g, much higher than that of pure ZnO (95.1 m2/g). Abundant previous researches have demonstrated that the higher surface area of gas sensing materials is helpful for achieving better gas sensitivity because higher surface area means that during the gas sensing process, more active sites for gas adsorption and surface reaction can be provided [38].

4. Conclusions

In summary, Zn5(CO3)2(OH)6 porous hollow microspheres (PHMSs) were successfully synthesized via a facile solvothermal method. By annealing the prepared Zn5(CO3)2(OH)6 PHMSs together with g-C3N4, g-C3N4 nanosheet-decorated ZnO PHMSs were successfully prepared. The results of gas sensing tests indicated that under UV-light irradiation, the sensor based on g-C3N4/ZnO PHMSs showed an improved CH4 sensing property than the sensor based on pure ZnO PHMSs at room temperature. The improved UV-light activated CH4 sensing properties of g-C3N4/ZnO PHMSs can be mainly attributed to the effects of g-C3N4-ZnO heterojunction, as well as the higher surface area of the composite materials. The formation of g-C3N4-ZnO heterojunction can not only promote the separation of electron-hole pair, but also lead to the creation of more surface oxygen vacancies, both of which can play an important role in enhancing the CH4 sensitivity. The present research demonstrates that decoration with g-C3N4 is a promising strategy to improve the UV-light activated CH4 sensing properties of ZnO.

Author Contributions

M.X. and G.S. conceived and designed the experiments; Y.L., B.Z. and Z.Z. performed the experiments and analyzed the data; M.X. and G.S. wrote the paper; all authors discussed the results and commented on the manuscript.

Funding

This research was funded by the National Natural Science Foundation of China (U1704255) as well as the Program for Science and Technology Innovation Talents in Universities of Henan Province (18HASTIT010).

Conflicts of Interest

The authors declare no conflict of interest.

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Figure 1. Schematic illustration of the synthesis process for g-C3N4/ZnO PHMSs.
Figure 1. Schematic illustration of the synthesis process for g-C3N4/ZnO PHMSs.
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Figure 2. Schematic illustration of the synthetic steps for gas sensor.
Figure 2. Schematic illustration of the synthetic steps for gas sensor.
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Figure 3. XRD patterns of the as-prepared (a) Zn5(CO3)2(OH)6, (b) g-C3N4, ZnO, CNZO-3, CNZO-5, CNZO-8, and CNZO-10.
Figure 3. XRD patterns of the as-prepared (a) Zn5(CO3)2(OH)6, (b) g-C3N4, ZnO, CNZO-3, CNZO-5, CNZO-8, and CNZO-10.
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Figure 4. TG-DTA curves of the Zn5(CO3)2(OH)6 precursor (a) and FT-IR spectra (b) of g-C3N4, ZnO, CNZO-3, CNZO-5 and CNZO-8, Nitrogen adsorption/desorption isotherms (c) and pore size distribution (d) of ZnO and CNZO-8.
Figure 4. TG-DTA curves of the Zn5(CO3)2(OH)6 precursor (a) and FT-IR spectra (b) of g-C3N4, ZnO, CNZO-3, CNZO-5 and CNZO-8, Nitrogen adsorption/desorption isotherms (c) and pore size distribution (d) of ZnO and CNZO-8.
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Figure 5. FESEM images of g-C3N4 (a,b), the precursor of CNZO-8 (c,d), and the CNZO-8 annealed at 400 °C (e,f).
Figure 5. FESEM images of g-C3N4 (a,b), the precursor of CNZO-8 (c,d), and the CNZO-8 annealed at 400 °C (e,f).
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Figure 6. (a) TEM and (b) HRTEM images of CNZO-8.
Figure 6. (a) TEM and (b) HRTEM images of CNZO-8.
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Figure 7. XPS survey spectra (a) of ZnO, CNZO-5, CNZO-8 and CNZO-10, XPS high-resolution spectrum and fitted curves of N 1s (b), C 1s (c) and Zn 2p (d) between ZnO and CNZO-8, O 1s (e) of ZnO, and CNZO-8.
Figure 7. XPS survey spectra (a) of ZnO, CNZO-5, CNZO-8 and CNZO-10, XPS high-resolution spectrum and fitted curves of N 1s (b), C 1s (c) and Zn 2p (d) between ZnO and CNZO-8, O 1s (e) of ZnO, and CNZO-8.
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Figure 8. UV-light activated response resistance (a–e) curves of the sensors to 2000 ppm CH4 at room temperature.
Figure 8. UV-light activated response resistance (a–e) curves of the sensors to 2000 ppm CH4 at room temperature.
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Figure 9. (a) UV light-activated dynamic response-recover curves of the g-C3N4/ZnO sensors to different concentrations of CH4 at room temperature, (b) gas responses of two sensors as a function of the ethanol concentration at room temperature, (c) repeatability measurements of the CNZO-8 sensor towards 2000 ppm CH4 at room temperature, (d) long-term stability test of CNZO-8 sensor to three concentrations of CH4 at room temperature.
Figure 9. (a) UV light-activated dynamic response-recover curves of the g-C3N4/ZnO sensors to different concentrations of CH4 at room temperature, (b) gas responses of two sensors as a function of the ethanol concentration at room temperature, (c) repeatability measurements of the CNZO-8 sensor towards 2000 ppm CH4 at room temperature, (d) long-term stability test of CNZO-8 sensor to three concentrations of CH4 at room temperature.
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Figure 10. Schematic illustration for the mechanism of photoinduced charge carrier transfers in g-C3N4/ZnO composites under UV irradiation, gas sensing mechanism of (a) ZnO and (b) g-C3N4/ZnO.
Figure 10. Schematic illustration for the mechanism of photoinduced charge carrier transfers in g-C3N4/ZnO composites under UV irradiation, gas sensing mechanism of (a) ZnO and (b) g-C3N4/ZnO.
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MDPI and ACS Style

Xiao, M.; Li, Y.; Zhang, B.; Sun, G.; Zhang, Z. Synthesis of g-C3N4-Decorated ZnO Porous Hollow Microspheres for Room-Temperature Detection of CH4 under UV-Light Illumination. Nanomaterials 2019, 9, 1507. https://doi.org/10.3390/nano9111507

AMA Style

Xiao M, Li Y, Zhang B, Sun G, Zhang Z. Synthesis of g-C3N4-Decorated ZnO Porous Hollow Microspheres for Room-Temperature Detection of CH4 under UV-Light Illumination. Nanomaterials. 2019; 9(11):1507. https://doi.org/10.3390/nano9111507

Chicago/Turabian Style

Xiao, Min, Yanwei Li, Bo Zhang, Guang Sun, and Zhanying Zhang. 2019. "Synthesis of g-C3N4-Decorated ZnO Porous Hollow Microspheres for Room-Temperature Detection of CH4 under UV-Light Illumination" Nanomaterials 9, no. 11: 1507. https://doi.org/10.3390/nano9111507

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