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Article

Solventless Mechanochemical Fabrication of ZnO–MnCO3/N-Doped Graphene Nanocomposite: Efficacious and Recoverable Catalyst for Selective Aerobic Dehydrogenation of Alcohols under Alkali-Free Conditions

by
Mujeeb Khan
1,
Syed Farooq Adil
1,*,
Mohamed E. Assal
1,
Abdulrahman I. Alharthi
2,
Mohammed Rafi Shaik
1,
Mufsir Kuniyil
1,
Abdulrahman Al-Warthan
1,
Aslam Khan
3,
Zeeshan Nawaz
4,
Hamid Shaikh
5 and
Mohammed Rafiq H. Siddiqui
1
1
Department of Chemistry, College of Science, King Saud University, P.O. Box 2455, Riyadh 11451, Saudi Arabia
2
The Department of Chemistry, College of Sciences and Humanities, Prince Sattam Bin Abdulaziz University, P.O. Box 173, Al-Kharj 11942, Saudi Arabia
3
King Abdullah Institute for Nanotechnology, King Saud University, P.O. Box 2454, Riyadh 11451, Saudi Arabia
4
SABIC Technology & Innovation, P.O. Box 5101, Riyadh 11422, Saudi Arabia
5
SABIC Polymer Research Center (SPRC), Department of Chemical Engineering, King Saud University, P.O. Box 800, Riyadh 11421, Saudi Arabia
*
Author to whom correspondence should be addressed.
Catalysts 2021, 11(7), 760; https://doi.org/10.3390/catal11070760
Submission received: 20 May 2021 / Revised: 17 June 2021 / Accepted: 17 June 2021 / Published: 23 June 2021
(This article belongs to the Special Issue Catalytic Applications of Metal or Metal Oxide Nanocomposites)
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Abstract

:
Catalytic efficacy of metal-based catalysts can be significantly enhanced by doping graphene or its derivatives in the catalytic protocol. In continuation of previous work regarding the catalytic properties of highly-reduced graphene oxide (HRG), graphene-oxide (GO) doped mixed metal oxide-based nanocomposites, herein we report a simple, straightforward and solventless mechanochemical preparation of N-doped graphene (NDG)/mixed metal oxide-based nanocomposites of ZnO–MnCO3 (i.e., ZnO–MnCO3/(X%-NDG)), wherein N-doped graphene (NDG) is employed as a dopant. The nanocomposites were prepared by physical milling of separately fabricated NDG and ZnO–MnCO3 calcined at 300 °C through eco-friendly ball mill procedure. The as-obtained samples were characterized via X-ray diffraction (XRD), Thermogravimetric analysis (TGA), Fourier-transform infrared spectroscopy (FT-IR), Raman, Field emission scanning electron microscopy (FESEM), Energy-dispersive X-ray spectroscopy (EDX) and surface area analysis techniques. To explore the effectiveness of the obtained materials, liquid-phase dehydrogenation of benzyl alcohol (BOH) to benzaldehyde (BH) was chosen as a benchmark reaction using eco-friendly oxidant (O2) without adding any harmful surfactants or additives. During the systematic investigation of reaction, it was revealed that the ZnO–MnCO3/NDG catalyst exhibited very distinct specific-activity (80 mmol/h.g) with a 100% BOH conversion and <99% selectivity towards BH in a very short time. The mechanochemically synthesized NDG-based nanocomposite showed remarkable enhancement in the catalytic performance and increased surface area compared with the catalyst without graphene (i.e., ZnO–MnCO3). Under the optimum catalytic conditions, the catalyst successfully transformed various aromatic, heterocyclic, allylic, primary, secondary and aliphatic alcohols to their respective ketones and aldehydes with high selectively and convertibility without over-oxidation to acids. In addition, the ZnO–MnCO3/NDG was also recycled up to six times with no apparent loss in its efficacy.

1. Introduction

Metal-catalyzed oxidation of alcohols to carbonyls is the most considerable fundamental functional-group reactions in organic synthetic chemistry [1,2,3]. The oxidative products are essential raw materials and precursors, which have been extensively utilized in the manufacturing of pharmaceuticals, cosmetics, fragrances, dyes, spices, plastics, flame-retardants, insecticides, and agrochemicals [4,5]. In traditional procedures, stoichiometric amounts of inorganic oxidizing agents including KMnO4, CrO3, NaClO, Na2Cr2O7, or PCC were widely used [6,7]. For the most part these oxidants are corrosive, noxious, high cost, toxic and environmentally harmful and demonstrate low selectivity [8]. From the viewpoints of green chemistry and environmental concern, considerable interest has been paid to the design and exploration of ecologically friendly and safer catalytic systems for oxidation of alcohols using greener oxidants like gaseous O2 [9]. Molecular O2 possesses various benefits: it is cheap, eco-friendly, abundantly available, and produces clean water as the sole product [10]. In this regard, noble metal catalysts like Au [11], Pd [12], Ru [13], and Pt [14] were extensively applied in the aerial oxygenation of alcohols to carbonyls. However, the high cost and scarceness of these precious metals reduces their industrial applications [15]. Consequently, exploration of plentiful and cheap catalysts like transition (non-noble) metals, such as vanadium- [16], chrome- [17], iron- [18], copper- [19], zirconium- [20], nickel- [21], rhenium- [22], and molybdenum-based catalysts have gained prominence [23] for the selective oxygenation of alcohol. In addition, numerous studies state that the effectiveness of the metal oxide-based catalysts substantially improved after compositing with other metallic NPs, due to the synergistic effects and enhanced surface area [24].
Commonly, metallic and metal oxide NPs are found to be efficacious heterogeneous catalysts for alcohol oxygenation. In addition, the activity of these catalysts could be increased by structure optimization which in-turn increases the specific surface area [25]. However, the nano-sized metal-based catalysts are usually not stable and readily agglomerate owing to huge surface energy, which consequently minimizes their activity and stability [26]. This dilemma can be reduced by suspending these materials on appropriate support which possesses high surface area and prevents particle aggregation [27]. Among various catalysts supports, carbonaceous materials, particularly graphene and its derivatives, like GO, HRG and NDG, have received increasing interest owing to their formidable potential in numerous applications, including catalysis [28]. This is because of the exceptional and unique chemical, physical, electronic, optical and magnetic properties associated with the structural integrity and large surface area of graphene derivatives [29].
Doping of nitrogen has been utilized to fine-tune the structural and electrical properties of graphene, which in-turn leads to significant change of various properties of carbonic materials. Doping creates defects on the surface of the material which offer active anchoring sites to enhance the electronic density and dispersion of catalytically active metal NPs, therefore, this modification will make carbonic materials beneficial in several disciplines [30,31]. The additional N atom on the graphene nano-layer strongly effects the growth-mechanism of NPs, controls the morphology and size of the NPs, as well as assists the uniform dispersion of nanoparticles [32]. In addition, high electro-negativity of N atom also leads to the formation of catalytically active sites, owing to which NDG-based nanocomposites have also been widely utilized as heterogeneous catalysts for plenty of organic transformations [33,34]. Apart from agglomeration of metallic nanoparticles, the inevitable aggregation of graphene nano-layers causes a decrease in its surface areas [32]. Usually, the restacking of graphene nanosheets is prohibited by the inclusion of metals or metal oxides NPs like Pt, Ag, Co3O4, and CeO2 on the graphene layer [32,35,36,37]. Indeed, theoretical and experimental studies confirmed the benefits of metals or metal oxides/NDG composites for various catalytic transformations including oxidation of alcohol [38].
Our earlier studies demonstrated the preparation of numerous metal-based nanocatalysts and their graphene nanocomposites and investigated their catalytic performances towards oxidation of alcohols [39,40,41]. In one such study, we demonstrated the promoting effect of zinc oxide NPs in the MnCO3, i.e., (1%) ZnO–MnCO3 nanocatalyst which afforded superb activity for aerial dehydrogenation of alcohols in the presence of O2. Furthermore, its HRG- and GO-doped catalysts also showed enhanced catalytic activity [40]. In continuation of this work, herein, we prepared (1%) ZnO–MnCO3/(X%-NDG) nanocomposites through a clean and simple two-step process with the co-precipitation method followed by the mechanochemical ball milling (Scheme 1), and investigated their catalytic activity towards aerial dehydrogenation of BOH as a probe reaction. The mechanochemical ball mill procedure helps to decrease the nanoparticles size as well as prohibit aggregation. The fabricated samples were characterized using appropriate microscopic and spectroscopic instruments. The prepared samples were examined for aerial dehydrogenation of a variety of alcohols to investigate the influence of NDG in the resulting nanocomposite. Notably, this is the first study of the catalytic protocol in which NDG-doped ZnO–MnCO3 is examined for the aerial dehydrogenation of alcohols to carbonyls.

2. Results and Discussion

2.1. Characterizations

XRD analysis was conducted to identify the crystallinity and phases of the as-synthesized materials. Figure 1 reveals the XRD of graphite, GO, NDG, (1%) ZnO–MnCO3, and (1%) ZnO–MnCO3/(1%-NDG). The sharp diffraction signal of graphite powder centered at 2θ = 26.5° could be ascribed to the plane (002) with d-spacing of 3.44 Å [42]. Notwithstanding, GO demonstrates a wide band at 2-theta = 11.7° which is a fingerprint band for GO structure. The absence of graphite reflection at 2-theta = 26.5° and emergence of a novel band at 2-theta = 11.7° confirms the successful oxidation of graphite to GO [43]. This 2-theta shift is because of the increase in d-spacing from 3.44 to 6.42 Å for graphite and GO, correspondingly, attributed to the existence of residual oxygenic-groups between the graphene nanolayers upon oxidation [44]. XRD diffractogram of pure NDG exhibits a broad band located at approximately 2-theta = 24.5° with plane (002) which is a fingerprint band of NDG. The absence of the diffraction band at 2-theta = 11.7° confirms the reduction of GO to NDG [45]. XRD diffractogram of undoped catalyst (1%) ZnO–MnCO3 (without NDG) matches with the rhodochrosite structure of MnCO3 (JCPDS card no. 1–0981), and the diffraction peaks marked with stars may be ascribed to the existence of ZnO [46]. For (1%) ZnO–MnCO3/(1%-NDG) diffractogram, all reflections were assigned to well-crystallized rhodochrosite MnCO3 structure (JCPDS card no. 1–0981) as well as the fingerprint diffraction band of NDG at approximately 24.5° (as indicated by arrow). Accordingly, the obtained XRD results revealed that the (1%) ZnO–MnCO3/(1%-NDG) nanocomposite was efficiently synthesized.
Thermo-gravimetric analyses (TGA) were conducted to determine the thermal property of the fabricated samples up to 800 °C. Figure 2 illustrates the comparison between the thermal stability of (1%) ZnO–MnCO3/(1%-NDG) nanocomposite and the thermal decomposition properties of its precursors include graphite, GO, NDG, and (1%) ZnO–MnCO3. The pure graphite powder is highly stable, and displays total weight loss of approximately 1% from 25 °C to 800 °C. It is observed that the pyrolysis of GO is much higher when compared to the graphite, which is ascribed to the existence of labile oxygenated groups on the surface [47]. The GO exhibits ~5% mass loss at 100 °C, attributed to the vaporization of volatile impurities and desorption of water molecules from the structure. The fundamental mass loss of ~44% was observed between 200 and 380 °C because of the thermal degradation of O-carrying groups. Eventually, the mass loss (about 10%) between 380 and 800 °C, related to the pyrolysis of graphene skeleton [48]. However, the NDG thermogram exhibits an entire weight loss of ~30%, which is ascribed to the reduction of oxygenic groups on the surface of graphene. Moreover, the thermogram of (1%) ZnO–MnCO3/(1%) NDG exhibited a total weight loss of ~19% loss with respect to the 17% weight loss showed by (1%)ZnO–MnCO3 nanocatalyst over the similar temperature range, which suggests that the doping of the NDG in the nanocomposites slightly depreciates its thermal stability.
FT-IR spectra of the nanocomposite (1%) ZnO–MnCO3/(1%-NDG) is displayed in Figure 3 and FT-IR results of GO and NDG is also presented for comparison. In pure GO, the band observed at ~3438 cm−1 is related to the vibrations of (O−H) bond or physisorbed H2O molecules [49]. The FT-IR peaks located at 1736 cm−1 and 1632 cm−1 were assigned to (C=O) vibrational modes and carbon backbone stretching vibrations from un-oxidized graphitic domains, correspondingly [50]. The other absorption peaks observed at 1396, 1227, and 1061 cm−1 are attributed to vibrations of oxygenic-groups like C–OH, C–O–C (epoxy), and C–O (alkoxy) bonds, correspondingly [51]. The characteristic peaks of oxygenic-functionalities considerably weakened and/or disappeared in the spectrum of pure NDG and (1%) ZnO–MnCO3/(1%-NDG) nanocomposite, which confirm the effective reduction of GO to NDG. With respect to NDG spectra, some characteristic absorption bands are noticed at 3430 and 1562 cm−1 which belong to N−H stretching vibrations and the peak at ~1152 cm−1 is associated with C–N [52]. The spectra of (1%) ZnO–MnCO3/(1%-NDG) exhibits a weak peak at 1634 cm−1 due to the vibrations of (C=C) bond, in addition, two strong peaks are present at 865 and 730 cm−1 and a wide band exists at 1446 cm−1, which are similar to the peaks that appeared in the IR spectrum of MnCO3 [53]. Moreover, the broad band at 3430 cm−1 is associated with vibrations of N−H and the absorption peak at 1152 cm−1 related to (C−N). Lastly, the strong band emerging at 584 cm−1 is due to the vibrations of Mn–O bond [54].
Raman spectroscopy is an advantageous tool to study the structure of graphite derivatives. Figure 4 illustrates the Raman spectrum of GO, NDG, and (1%) ZnO–MnCO3/(1%-NDG) nanocomposites. The GO spectrum displays two eminent bands, the G-band at ~1603 cm−1 owing to the E2g-phonon of the sp2 hybridization carbon atoms, and the D-band at ~1336 cm−1 related to the breathing modes of k point phonons of A1g-symmetry. The G-band is usually associated with the well-ordered structure of C–C bond stretching vibrations [55]. The D-band originates from the disorder structure, which could be due to the existence of defects like grain-boundaries, vacancies, and amorphous carbon atoms [56]. Disorder is calculated by the ratio between the intensities of D-band (ID) and G-band (IG) i.e., (ID/IG). For NDG and (1%) ZnO–MnCO3/(1%-NDG) spectra, the G-band is located at 1594 cm−1 and 1596 cm−1 as well as the D-band at 1327 and 1327 cm−1, respectively. The G-band in NDG is red shifted to a lower wavenumber because of the replacing of O atom through N-doping, which leads to the formation of pyrrolic, pyridinic, and N-graphitic instead of sp2 carbon atoms [57]. The widened D-band in GO is attributed to the decrease in size of the sp2 domains by the creation of defects, distortions, and vacancies upon oxidation. The increment of disorder ratio (ID/IG) from 1.088 (GO) to 1.324 (NDG) indicates the incorporation of heterogeneous N atoms into the graphene nanosheets. Eventually, the higher disorder (ID/IG) for (1%) ZnO–MnCO3/(1%-NDG) (1.412), compared to the pure NDG, points to the increasing of defects due to N doping [58].
The sample morphology was examined and the FESEM micrographs of pure NDG, un-doped (1%) ZnO–MnCO3 catalyst, and (1%) ZnO–MnCO3/(1%-NDG) nanocomposite is displayed in Figure 5. Figure 5a displays the layer-like structure of NDG as a continual crumpled membrane organized as sheets. The morphology of the un-doped (1%) ZnO–MnCO3 appears to be rigid and undefined (Figure 5b). Figure 5c,d displays the crumbled NDG layers scattered over a network of NPs. The ZnO–MnCO3 NPs are with clustered NDG layers over them.
The elemental mapping of (1%) ZnO–MnCO3/(1%-NDG) nanocomposite at the rectangular area displayed in Figure 6 discloses the uniform distribution of C (green), Mn (red), O (purple), N (turquoise), and Zn (yellow) atoms throughout the 4 μm sized cross-section. Furthermore, the EDX spectrum of the (1%) ZnO–MnCO3 sample confirmed the presence of carbon, oxygen, manganese, and zinc atoms, whereas as expected the EDX spectra of (1%) ZnO–MnCO3/(1%-NDG) nanocomposite revealed that the existence of carbon, oxygen, manganese, and zinc atoms along with nitrogen atom and the % of N atoms in the nanocomposite is within experimental error to the theoretical composition as demonstrated in Figure 7.
To find out the surface areas of the fabricated samples and to comprehend its linkage with the catalytic efficiency for aerobic BOH dehydrogenation, the N2 sorption mensuration was studied. Table 1 reveals that the surface area of ZnO–MnCO3 (without graphene) is about 120.3 m2/g. As anticipated, after doping the nanocomposites with graphene supports like HRG, GO, and NDG, the surface areas were considerably raised to 239.1, 244.6, and 261.4 m2/g, correspondingly.

2.2. Catalytic Evaluation Studies

The fundamental objective of this study is to oxidize a variety of alcohols to their respective carbonyl compounds with outstanding catalytic efficacy utilizing O2 as an environmental-friendly oxidizing agent under alkali-free environment. To achieve this, we utilized NDG as co-dopant for ZnO–MnCO3 nanocatalyst for aerobic dehydrogenation of BOH as a model substrate in the presence of gaseous O2, as displayed in Scheme 2. A series of catalysts were prepared by changing the wt. percentage of NDG in the catalytic system. Furthermore, various reaction variables were optimized, such as, catalyst dose, reaction time, and operation temperature, as displayed in Table 1 and Table 2 and Figure 8, Figure 9, Figure 10 and Figure 11.

2.3. Influence of Weight Percentage of NDG

Commonly, the catalytic ability of the oxidation catalyst remarkably enhanced after employing graphene as a dopant or a supporting material [59,60]. In our previous report, zinc oxide was found to be an ideal dopant for MnCO3 and (1%) ZnO–MnCO3 for aerial alcohol dehydrogenation with O2 as an eco-friendly oxidant. The amount of 0.3 g of (1%) ZnO–MnCO3 exhibited a full conversion of BOH in 25 min at 100 °C [46]. For this study, (1%) ZnO–MnCO3 was selected with a purpose of comparing the effects of additional dopants/support with the earlier catalyst. Notably, initial experiments were devoted to optimizing wt.% of NDG in the nanocomposite to promote the catalytic activity. Firstly, we investigated the efficacy of pristine N-doped graphene towards aerobic dehydrogenation of BOH with gaseous O2, and its catalytic activity is negligible. However, upon doping as-prepared metal oxide catalysts with varying wt.% of NDG, i.e., (0–7%) NDG, significant catalytic performance was observed towards BOH oxidation as shown in Table 2 and Figure 8. The catalyst without NDG, i.e., (1%) ZnO–MnCO3, yielded a ~67% conversion of BOH in 5 min. After the addition of 1 wt.% of NDG ((1%) ZnO–MnCO3/(1%-NDG)), the resulting nanocatalyst displayed enhanced catalytic efficacy. Indeed, the (1%) ZnO–MnCO3 catalyst with (1%) NDG, i.e., (1%) ZnO–MnCO3/(1%-NDG), is the best catalyst when compared to other catalysts with different wt.% of NDG. This catalyst yielded 100% conversion within a very short time (5 min) with superb specific-activity of 80 mmole/h.g. Notably, increasing the content of NDG to 3%, a small drop in BOH conversion to ~96% was observed. Similarly, upon further increase of NDG between 5% and 7%, a similar trend was observed and the conversion dropped to ~75% and ~69%, respectively, under the same conditions. It is possible that a higher percentage of NDG may block the active sites of catalyst leading to a decrease in the catalytic activity of the resulting nanocatalyst. Meanwhile, the selectivity towards BH was unaltered during all oxidation processes (>99%). A NMR spectra from one of the reactions depicting the purity of the product formed is given in Supplementary Materials Figure S1. As a result, it can be inferred that NDG played a pivotal role as a dopant in promoting the effectiveness of our catalytic-methodology for this oxidation process.

2.4. Comparison of Various Types of Graphene

Moreover, we compared the effectiveness of (1%) ZnO–MnCO3 doped with different types of graphene (i.e., GO, HRG, and NDG) for aerobic dehydrogenation of BOH to comprehend the impact of graphene on the efficacy of the catalytic protocol. The data is summed up in Table 1. Firstly, we examined the pristine MnCO3 (without ZnO NPs) for liquid-phase aerial oxidation of BOH under the above-mentioned circumstances, which only yielded 38.2% BOH conversion within 5 min; however, after doping the MnCO3 with 1 wt.% of ZnO i.e., (1%) ZnO–MnCO3, the catalytic performance remarkably increased, and gave 67.1% conversion of BOH at the same experimental conditions. Further modifications were performed by using NDG as a co-dopant, i.e., (1%) ZnO–MnCO3/(1%-NDG), which has slightly higher activity than the nanocomposites doped with GO ((1%) ZnO–MnCO3/(1%-GO)) and HRG ((1%) ZnO–MnCO3/(1%-HRG)). The NDG-doped catalyst yielded 100% conversion, whereas the (1%) ZnO–MnCO3/(1%-GO) catalyst exhibited 97.8% conversion with specific-activity of 78.2 mmole/h.g. On the other hand, HRG-doped ZnO–MnCO3 ((1%) ZnO–MnCO3/(1%-HRG)) exhibited slightly lowered activity when compared to both GO- and NDG-doped catalysts and yielded ~95%. The enhanced efficiency of the NDG-based catalyst can be attributed to the existence of the N atoms on the NDG surface, which increase the electron density of the material [61]. In addition, the existence of NDG could be responsible for extra defects in the crystalline (1%) ZnO–MnCO3 catalysts which enhance the performance of the nanocomposites. Importantly, the obtained catalytic data of the fabricated catalysts are very much consistent with the Brunauer–Emmett–Teller (BET)-surface area which plays an important role in improving catalytic activity. Interestingly, the catalytic activity after incorporating (1%) ZnO–MnCO3 with NDG, GO, and HRG, i.e., (1%) ZnO–MnCO3/(1%-NDG), (1%) ZnO–MnCO3/(1%-GO), and (1%) ZnO–MnCO3/(1%-HRG), respectively, also remarkably enhanced. Therefore, it can be said that incorporating graphene derivatives as co-dopants (i.e., NDG, GO, or HRG) had an affirmative effect on the surface area of the as-synthesized nanocomposites, which improves the effectiveness of the catalytic system. Interestingly, the (1%) ZnO–MnCO3/(1%-NDG) nanocomposite had the highest surface area and also exhibited the best alcohol conversion among all other synthesized graphene-based catalysts, while the other prepared catalysts possessed lower surface area and catalytic efficacy. The comparative graphical illustration of the surface area and its effect on the catalytic performance is given in Figure 9. Moreover, a comparative graphical illustration of percentage of benzaldehyde (BH) formed using MnCO3, ZnO (1%)-MnCO3, and their various graphene-based composites is given in Supplementary Materials Figure S2.

2.5. Influence of Temperature

In most cases, the operating temperature plays a pivotal role in catalysis and has a strong impact on the efficacy of catalysts. Subsequently, the effect of temperature on the BOH dehydrogenation was also examined by altering the temperature from RT to 100 °C using the as-prepared catalysts (MnCO3, (1%) ZnO–MnCO3 and (1%) ZnO–MnCO3/(1%-NDG)), while maintaining other catalytic variables constant; the data is presented in Figure 10. By increasing the temperature, the catalytic effectiveness also increased, and in all cases superior BH selectivity (>99%) was accomplished. It is noteworthy that the (1%) ZnO–MnCO3/(1%-NDG) catalyst afforded the highest catalytic activity, as illustrated in Figure 10, and moreover, even at RT, the catalyst displayed some conversion (34.2%). Expectedly, higher temperatures lead to higher effectiveness, whereas the optimal temperature with all studied catalysts was found to be 100 °C.

2.6. Influence of Catalyst Dosage

The catalyst quantity optimization tests were conducted by altering the catalyst amount from 0.050 to 0.30 g. Therefore, to study the impact of quantity catalyst (MnCO3, (1%) ZnO–MnCO3 and (1%) ZnO–MnCO3/(1%-NDG)), six different amounts (0.05, 0.10, 0.15, 0.20, 0.25 and 0.30 g) were used under similar conditions, and the results are presented in Figure 11. To confirm the importance of catalysts, dehydrogenation was performed in the absence of a catalyst, which did not yield any product. On the other hand, by increasing the catalyst dose from 0.050 to 0.30 g, the conversion also increased significantly, while the BH selectivity remained unchanged throughout all experiments (>99%). Even in all these experiments, (1%) ZnO–MnCO3/(1%-NDG) exhibited maximal efficiency compared to other catalysts. In this case, the percentage conversion improved considerably from 26.7% to 100% upon raising the catalyst dosage from 0.050 to 0.30 g. This can be ascribed to the increased active sites with increasing the amounts of catalysts, which leads to an accelerated oxidation rate.
To exclude the role of solvent (toluene) during oxidation, a blank experiment was performed under optimized conditions without the substrate (BOH) using (1%) ZnO–MnCO3/(1%-NDG) catalyst. No product was obtained, which confirms that the BH is produced only because of the catalytic dehydrogenation of BOH and not toluene. Additionally, to comprehend the significance of the oxidizing agent (O2) for this transformation, the experiment was preformed over the (1%) ZnO–MnCO3/(1%-NDG) employing air instead of bubbling gaseous O2. Using the optimal catalytic conditions, the prepared catalyst exhibited only 25.6% alcohol conversion, which is much lower than 100% conversion obtained when this transformation was performed utilizing gaseous O2.

2.7. Recycling Tests

Catalyst reutilization has the utmost significance from both an industrial and environmental perspective. Thus, the durability of (1%) ZnO–MnCO3/(1%-NDG) nanocomposite over several usage cycles for aerobic dehydrogenation of BOH with gaseous O2 was inspected under optimal catalytic circumstances. After carrying out the first experiment, the catalyst was separated by centrifugation. The resulting material was washed with toluene several times and then dried at 105 °C for 3 h. The recovered catalyst was then recycled for this transformation under identical conditions and the conversion of BOH was evaluated using GC. Repeated experiments revealed that the catalyst could be successfully utilized up to six times without compromising its effectiveness. As illustrated in Figure 12, the BOH conversion merely reduced from 100% to ~90% after six runs. The slight reduction in BOH conversion could be due to the slight weight loss of the synthesized sample during the filtration method [62]. In addition, throughout these reactions, the selectivity towards aldehyde stayed the same (>99%). Therefore, all these results indicate that the (1%) ZnO–MnCO3/(1%-NDG) has a superb stability as well as reproducibility, which is potentially useful for industrial applications.
Moreover, the catalytic activities of nanocatalysts studied herein towards the oxidation of alcohols were compared with similar types of catalytic systems containing GO, HRG, and NDG reported in the literature; the comparison is outlined in Table 3. Compared to the listed catalysts, the (1%) ZnO–MnCO3/(1%-NDG) demonstrated superior catalytic properties for BOH dehydrogenation with respect to conversion, time, specific-activity, and selectivity. The studied catalyst exhibits 100% transformation of BOH and >99% BH selectivity in a short time with high specific activity, while the other graphene-containing catalysts yielded less conversion, lower specific-activity, and required longer time to complete the reaction. This is possibly ascribed to the presence of a high number of vacancies, distortions, and defects in the NDG, which plays an essential role in improving effectiveness. Xie et al. [63] synthesized Au nanoparticles immobilized in N-doped graphene (AuNPs/NDG) nanocomposite and employed it as an oxidation catalyst for dehydrogenation of BOH. The nanocomposite afforded 67% conversion and 40% selectivity of BH as well as 0.4 mmole/h.g specific-activity within 6 h. Hu and his group [64] reported aerial dehydrogenation of BOH over MnO2/GO nanocomposite with air as an ecofriendly oxidant with 96.8% conversion of BOH, 100% selectivity of BH, and calculated specific-activity of 1.6 mmole/h.g within 3 h at 110 °C.

2.8. Substrate Scope

Encouraged by the aforementioned observations, we expanded the applicability of the fabricated (1%) ZnO–MnCO3/(1%-NDG) catalyst for liquid-phase selective dehydrogenation of several kinds of alcohols like primary, secondary, aromatic, aliphatic, allylic, and heterocyclic (Table 4). As demonstrated in Table 4, whole primary benzylic alcohols smoothly oxidize to the respective aldehydes with full conversion in a short time under optimum conditions with no further oxidation to carboxylic acids. Additionally, superb selectivity to corresponding aldehydes or ketones (>99%) was obtained for all alcohols used in this investigation and no other products were detected. The electronic properties of groups attached to the aromatic alcohols showed a significant influence on the effectiveness due to their capability to give electrons to the benzene ring [65]. It is noteworthy that the electron donating groups have a slightly positive impact on efficacy compared with electron withdrawing substituents; for example, the substituted benzylic alcohol with electron releasing groups like 4-methoxy-benzyl alcohol, was wholly transformed to 4-methoxy-benzaldehyde in 6 min, whereas, 4-trifluoromethyl-benzyl alcohol, that contains an electron withdrawing group, required a longer period (15 min). In addition, aromatic alcohols with substituents at para-position were fully transformed after comparatively shorter periods with respect to the ortho- and meta-positions. This may be due to the minimum steric resistance in para-position compared to ortho- and meta-positions [66].
In this context, para-methyl-benzyl alcohol was fully oxidized to para-methyl-benzaldehyde in merely 7 min, whilst ortho- and meta-methyl-benzyl alcohol required relatively longer times such as 15 and 9 min, respectively, for complete conversion. Notably, the steric effect also considerably impacted the rate of oxidation as bulky substrates (2,3,4,5,6-Pentaflouro, 2,4-Dichloro, and 2,3,4-Trimethoxy) attached to an aromatic ring inhibited the efficacy of the oxidation transformation, possibly due to the steric-resistance [71]. Allylic alcohols like cinnamic alcohol also smoothly oxidized to cinnamic aldehyde with 100% conversion and selectivity in 12 min. In addition, a heterocyclic alcohol like furfuryl alcohol was selectively converted to furfural in 28 min, with complete conversion. Furthermore, the present catalysts were also found to be efficient in the dehydrogenation of secondary aromatic alcohols, in which 100% conversion and selectivity towards corresponding ketones was accomplished. Styrallyl alcohol was completely oxidized into acetophenone in just 7 min, while 1-(4-chlorophenyl)ethanol also showed 100% conversion in a relatively longer reaction time (12 min), probably owing to 1-(4-chlorophenyl)ethanol containing an electron withdrawing group that inhibits the benzene ring by minimizing electron density.
Predominantly, by comparing with the dehydrogenation of benzylic alcohols, the aliphatic counterparts are much more difficult under identical conditions [76]. In this regard, the oxidation of cyclohexylmethanol, citronellol, and 1-octanol to their respective aliphatic aldehydes occurs over longer times. Similarly, the dehydrogenation of secondary aliphatic alcohols to aliphatic ketones exhibits lower reactivity with respect to secondary benzylic alcohols. Notably, a longer reaction time could be attributed to the difficulty of dehydrogenation of aliphatic alcohols compared to their aromatic counterparts. Total conversion of styrallyl alcohol occurred in 7 min, whereas the full conversion of 2-octanol occurred in 140 min. In conclusion, the effectiveness of this catalytic system is significantly affected by the steric and electronic effects.

3. Experimental Part

3.1. Preparation of GO and NDG

GO was fabricated from graphite using Hummers oxidation route [77], thereafter, GO was reduced and doped by using NH4OH and NH2NH2·H2O to obtain N-doped graphene for which the experimental details are mentioned in the Supplementary File.

3.2. Preparation of (1%)ZnO–MnCO3/(X%-NDG)

Briefly, ZnO NPs–MnCO3 were synthesized by coprecipitation procedure by mixing stoichiometric concentrations of Zn(NO3)2 and Mn(NO3)2 solutions in a round-bottomed flask and the mixture was continuously stirred at 96 °C. The solution of NaHCO3 (0.50 M) was added drop-wise to the solution until the pH reached ~9, then the addition was stopped and the reaction mixture was stirred at the same temperature for 4 h. Vigorous stirring was continued overnight at RT. The resulting solution was filtered and then dried at 65 °C overnight. The resultant powder sample was calcined at 300 °C in a muffle-furnace and ZnO NPs–MnCO3 was obtained. Subsequently, the synthesized NDG was dried in a furnace at 65 °C and firstly ground in a planetary ball mill. Then varied weight percentages of NDG were mixed with (1%) ZnO–MnCO3 in a planetary ball mill to get (1%) ZnO–MnCO3 doped (X%-NDG) nanocomposites (i.e., (1%) ZnO–MnCO3/(X%-NDG)). The details related to the planetary ball mill method are given in the Supplementary Information.

3.3. Characterizations

The synthesized samples were characterized utilizing several techniques. Specifics about instruments are described in the Supplementary File.

3.4. Catalytic Evaluation Tests

The typical process for aerobic base-free dehydrogenation of alcohols is mentioned in the Supplementary Information.

4. Conclusions

Herein, ZnO nanoparticles doped MnCO3 co-doped with nitrogen-doped graphene (NDG) nanocomposites were prepared via a co-precipitation procedure followed by a mechanochemical procedure. The fabricated nanocomposites were employed for aerial alkali-free dehydrogenation of BOH with gaseous O2 as an environmentally friendly oxidant. The efficacies of (1%) ZnO–MnCO3 doped with different graphene derivatives (NDG, GO, and HRG) were compared for this transformation to understand the role of different graphene derivatives in this catalytic system. The results disclosed that the (1%) ZnO–MnCO3/NDG has higher catalytic activity than undoped catalyst (1%) ZnO–MnCO3, (1%) ZnO–MnCO3/GO, and (1%) ZnO–MnCO3/HRG. The higher effectiveness of (1%) ZnO–MnCO3/(1%-NDG) could be ascribed to the presence of NDG, which influences the interactions between N-atoms on the surface of NDG and (1%) ZnO–MnCO3 NPs. Furthermore, the presence of graphene layers develops numerous defects and distortions in structure, which facilitate the adsorption of aromatic reactants at catalytically active sites which promote the interactions between NDG surface and acidic substrates, leading to enhanced catalytic activities. The best results were achieved in the case of (1%) ZnO–MnCO3/(1%-NDG) catalyst which led to a 100% BOH conversion and >99% product selectivity in quite a short time. The catalyst also delivered excellent specific activity (80 mmole/h.g) when compared to published studies. Notably, the dehydrogenation of aromatic alcohols is much easier than aliphatic ones, presumably because of the strong π–π stacking interactions between aromatic substrates and graphene sheets. The (1%) ZnO–MnCO3/(1%-NDG) catalyst can be reused efficiently without compromising its activity up to six times. The main features of the studied catalytic system are: (a) simple workup, (b) easily available precursors, (c) low cost and green oxidant, (d) no external additives or nitrogenous alkalis, (e) mild reaction conditions, (f) inexpensive recyclable catalyst, (g) highly efficient in case of both conversion and selectivity, (h) shorter reaction time, and (i) effective for all kinds of alcohols.

Supplementary Materials

The following are available online at https://www.mdpi.com/article/10.3390/catal11070760/s1. Figure S1. 1HNMR spectra for the product (benzaldehyde) obtained after selective oxidation of benzyl alcohol; Figure S2. Comparative graphical illustration of percentage of benzaldehyde (BH) formed using MnCO3, ZnO(1%)-MnCO3 and their various graphene based composites within 5 minutes.

Author Contributions

M.K. (Mujeb Khan): formal analysis; investigation; writing—review and editing; S.F.A.: conceptualization; investigation; methodology; writing—original draft; writing—review and editing; M.E.A.: formal analysis; investigation; writing—original draft; A.I.A.: formal analysis; M.R.S.: formal analysis; investigation; M.K. (Mufsir Kuniyil): formal analysis; investigation; A.A.-W.: supervision; A.K.: formal analysis; Z.N.: formal analysis; H.S.: formal analysis; M.R.H.S.: supervision. All authors have read and agreed to the published version of the manuscript.

Funding

The authors extend their appreciation to the Deanship of Scientific Research at King Saud University for funding this work through Research Group No. RG-1436-032.

Data Availability Statement

The data contained within the article and supplementary file.

Acknowledgments

The authors extend their appreciation to the Deanship of Scientific Research at King Saud University for funding this work through Research Group No. RG-1436-032.

Conflicts of Interest

The authors declare no conflict of interest.

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Catalysts 11 00760 sch001 550
Scheme 1. Synthesis of (1%) ZnO–MnCO3/(X%-NDG) nanocomposites through mechanochemical ball milling technique.
Scheme 1. Synthesis of (1%) ZnO–MnCO3/(X%-NDG) nanocomposites through mechanochemical ball milling technique.
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Figure 1. XRD analysis of (a) graphite, (b) GO, (c) NDG, (d) un-doped (1%) ZnO–MnCO3 catalyst, and (e) (1%)ZnO–MnCO3/(1%-NDG) samples.
Figure 1. XRD analysis of (a) graphite, (b) GO, (c) NDG, (d) un-doped (1%) ZnO–MnCO3 catalyst, and (e) (1%)ZnO–MnCO3/(1%-NDG) samples.
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Figure 2. TGA thermogram of (a) graphite, (b) GO, (c) NDG, (d) un-doped (1%) ZnO–MnCO3 catalyst, and (e) (1%)ZnO–MnCO3/(1%-NDG) nanocomposite.
Figure 2. TGA thermogram of (a) graphite, (b) GO, (c) NDG, (d) un-doped (1%) ZnO–MnCO3 catalyst, and (e) (1%)ZnO–MnCO3/(1%-NDG) nanocomposite.
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Figure 3. FT-IR results of (a) GO, (b) NDG, and (c) (1%)ZnO–MnCO3/(1%-NDG).
Figure 3. FT-IR results of (a) GO, (b) NDG, and (c) (1%)ZnO–MnCO3/(1%-NDG).
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Figure 4. Raman analysis of (a) GO, (b) NDG, and (c) (1%) ZnO–MnCO3/(1%-NDG).
Figure 4. Raman analysis of (a) GO, (b) NDG, and (c) (1%) ZnO–MnCO3/(1%-NDG).
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Catalysts 11 00760 g005 550
Figure 5. FESEM images of (a) NDG sample, (b) (1%) ZnO–MnCO3 sample, and (c,d) (1%)ZnO–MnCO3/(1%-NDG) sample showing presence of NDG sheets.
Figure 5. FESEM images of (a) NDG sample, (b) (1%) ZnO–MnCO3 sample, and (c,d) (1%)ZnO–MnCO3/(1%-NDG) sample showing presence of NDG sheets.
Catalysts 11 00760 g005
Catalysts 11 00760 g006 550
Figure 6. Elemental mapping of (1%) ZnO–MnCO3/(1%-NDG) nanocomposite.
Figure 6. Elemental mapping of (1%) ZnO–MnCO3/(1%-NDG) nanocomposite.
Catalysts 11 00760 g006
Catalysts 11 00760 g007 550
Figure 7. (a) EDX spectra of (1%) ZnO–MnCO3 sample, (a1) quantitative analysis of (1%)ZnO–MnCO3 sample, (b) EDX spectra of (1%)ZnO–MnCO3/(1%-NDG) sample, (b1) quantitative analysis of (1%)ZnO–MnCO3/(1%-NDG) sample.
Figure 7. (a) EDX spectra of (1%) ZnO–MnCO3 sample, (a1) quantitative analysis of (1%)ZnO–MnCO3 sample, (b) EDX spectra of (1%)ZnO–MnCO3/(1%-NDG) sample, (b1) quantitative analysis of (1%)ZnO–MnCO3/(1%-NDG) sample.
Catalysts 11 00760 g007
Catalysts 11 00760 sch002 550
Scheme 2. Scheme diagram of BOH dehydrogenation in presence of gaseous O2 catalyzed by the synthesized nanocomposite.
Scheme 2. Scheme diagram of BOH dehydrogenation in presence of gaseous O2 catalyzed by the synthesized nanocomposite.
Catalysts 11 00760 sch002
Catalysts 11 00760 g008 550
Figure 8. Graphical illustration of BOH dehydrogenation using (a) (1%) ZnO–MnCO3, (b) (1%) ZnO–MnCO3/(1%-NDG), (c) (1%) ZnO–MnCO3/(3%-NDG), (d) (1%) ZnO–MnCO3/(5%-NDG), and (e) (1%) ZnO–MnCO3/(7%-NDG) nanocomposites.
Figure 8. Graphical illustration of BOH dehydrogenation using (a) (1%) ZnO–MnCO3, (b) (1%) ZnO–MnCO3/(1%-NDG), (c) (1%) ZnO–MnCO3/(3%-NDG), (d) (1%) ZnO–MnCO3/(5%-NDG), and (e) (1%) ZnO–MnCO3/(7%-NDG) nanocomposites.
Catalysts 11 00760 g008
Catalysts 11 00760 g009 550
Figure 9. Comparative illustration of effect of various graphene-based dopants in the catalytic system on its catalytic efficiency.
Figure 9. Comparative illustration of effect of various graphene-based dopants in the catalytic system on its catalytic efficiency.
Catalysts 11 00760 g009
Catalysts 11 00760 g010 550
Figure 10. Impact of operation temperature on BOH dehydrogenation using (a) MnCO3, (b) (1%)ZnO–MnCO3, and (c) (1%)ZnO–MnCO3/(1%-NDG).
Figure 10. Impact of operation temperature on BOH dehydrogenation using (a) MnCO3, (b) (1%)ZnO–MnCO3, and (c) (1%)ZnO–MnCO3/(1%-NDG).
Catalysts 11 00760 g010
Catalysts 11 00760 g011 550
Figure 11. Influence of varying catalyst quantity on BOH oxidation in the presence of (a) MnCO3, (b) (1%) ZnO–MnCO3, and (c) (1%) ZnO–MnCO3/(1%-NDG) catalysts.
Figure 11. Influence of varying catalyst quantity on BOH oxidation in the presence of (a) MnCO3, (b) (1%) ZnO–MnCO3, and (c) (1%) ZnO–MnCO3/(1%-NDG) catalysts.
Catalysts 11 00760 g011
Catalysts 11 00760 g012 550
Figure 12. Reusability data of (1%) ZnO–MnCO3/(1%-NDG) catalyst for aerial dehydrogenation of BOH. Conditions: BOH (2.0 mmole), toluene (15 mL), O2 flow rate (20 mL/min), catalyst amount (0.30 g), operation temperature (100 °C), and time (5 min).
Figure 12. Reusability data of (1%) ZnO–MnCO3/(1%-NDG) catalyst for aerial dehydrogenation of BOH. Conditions: BOH (2.0 mmole), toluene (15 mL), O2 flow rate (20 mL/min), catalyst amount (0.30 g), operation temperature (100 °C), and time (5 min).
Catalysts 11 00760 g012
Table
Table 1. Catalytic dehydrogenation of BOH using different prepared catalysts.
Table 1. Catalytic dehydrogenation of BOH using different prepared catalysts.
E.CatalystSurface Area (m2/g)Conv. (%)Selectivity (%)Specific-Activity (mmole/h.g)
1MnCO370.538.2>9930.6
2(1%) ZnO–MnCO3120.367.1>9953.7
3(1%) ZnO–MnCO3/(1%-NDG)261.4100.0>9980.0
4(1%) ZnO–MnCO3/(1%-GO)244.697.8>9978.2
5(1%) ZnO–MnCO3/(1%-HRG)239.194.9>9975.9
Conditions: BOH (2.0 mmole), toluene (15 mL), O2 flow rate (20 mL/min), catalyst amount (0.30 g), operation temperature (100 °C), and time (5 min).
Table
Table 2. Catalytic efficacies of several prepared catalysts.
Table 2. Catalytic efficacies of several prepared catalysts.
E.CatalystConv. (%)Select. (%)Specific-Activity (mmole/h.g)
1NDG2.4>991.9
2(1%) ZnO–MnCO367.1>9953.7
3(1%) ZnO–MnCO3/(1%-NDG)100.0>9980.0
4(1%) ZnO–MnCO3/(3%-NDG)92.6>9974.1
5(1%) ZnO–MnCO3/(5%-NDG)75.5>9960.4
6(1%) ZnO–MnCO3/(7%-NDG)69.3>9955.4
Conditions: BOH (2.0 mmole), toluene (15 mL), O2 flow rate (20 mL/min), catalyst amount (0.30 g), operation temperature (100 °C), and time (5 min).
Table
Table 3. Comparison of the (1%) ZnO–MnCO3/(1%-NDG) catalyst for aerial oxidation of BOH with already published catalytic systems containing graphene.
Table 3. Comparison of the (1%) ZnO–MnCO3/(1%-NDG) catalyst for aerial oxidation of BOH with already published catalytic systems containing graphene.
CatalystTemp. (°C)Conv. (%)Select. (%)Time (h)Sp. Activity (mmole/h.g)Ref.
(1%) ZnO–MnCO3/NDG100100<990.0880.0This study
(1%) ZnO–MnCO3/GO10097.8<990.0878.2[40]
(1%) ZnO–MnCO3/HRG10094.9<990.0875.9[39]
AuNPs/NDG70674060.4[63]
MnO2/GO11096.810031.6[64]
CoOx/RGO-HP11096<99614.8[67]
(1%) RGO–MnCoO14078100212.6[68]
Fe3O4–Pt/rGO8033.6100342.0[69]
Co/NDG10089.597.384.5[70]
PW@IL-GO1009491512.5[71]
MnO2–Ag2O/HRG100100<990.611.4[72]
GO-1008010010051.1[73]
Pd NPs/GO1103634.161.0[74]
Cu NPs@rGO80<9998.6168.3[75]
4%Ru(CO)/NDG9046<99246.4[61]
Table
Table 4. Aerobic base-free dehydrogenation of various alcohols over (1%) ZnO–MnCO3/(1%-NDG) nanocomposite using gaseous O2.
Table 4. Aerobic base-free dehydrogenation of various alcohols over (1%) ZnO–MnCO3/(1%-NDG) nanocomposite using gaseous O2.
E.AlcoholsCarbonyl CompoundsTime (minutes)Conv. (%)/Select. (%)
1 Catalysts 11 00760 i001 Catalysts 11 00760 i0025100/>99
2 Catalysts 11 00760 i003 Catalysts 11 00760 i0046100/>99
3 Catalysts 11 00760 i005 Catalysts 11 00760 i0067100/>99
4 Catalysts 11 00760 i007 Catalysts 11 00760 i0089100/>99
5 Catalysts 11 00760 i009 Catalysts 11 00760 i0109100/>99
6 Catalysts 11 00760 i011 Catalysts 11 00760 i01210100/>99
7 Catalysts 11 00760 i013 Catalysts 11 00760 i01412100/>99
8 Catalysts 11 00760 i015 Catalysts 11 00760 i01615100/>99
9 Catalysts 11 00760 i017 Catalysts 11 00760 i01813100/>99
10 Catalysts 11 00760 i019 Catalysts 11 00760 i02015100/>99
11 Catalysts 11 00760 i021 Catalysts 11 00760 i02218100/>99
12 Catalysts 11 00760 i023 Catalysts 11 00760 i02418100/>99
13 Catalysts 11 00760 i025 Catalysts 11 00760 i02622100/>99
14 Catalysts 11 00760 i027 Catalysts 11 00760 i02822100/>99
15 Catalysts 11 00760 i029 Catalysts 11 00760 i03025100/>99
16 Catalysts 11 00760 i031 Catalysts 11 00760 i03230100/>99
17 Catalysts 11 00760 i033 Catalysts 11 00760 i03412100/>99
18 Catalysts 11 00760 i035 Catalysts 11 00760 i03628100/>99
19 Catalysts 11 00760 i037 Catalysts 11 00760 i0387100/>99
20 Catalysts 11 00760 i039 Catalysts 11 00760 i0409100/>99
21 Catalysts 11 00760 i041 Catalysts 11 00760 i04212100/>99
22 Catalysts 11 00760 i043 Catalysts 11 00760 i04415100/>99
23 Catalysts 11 00760 i045 Catalysts 11 00760 i04625100/>99
24 Catalysts 11 00760 i047 Catalysts 11 00760 i04840100/>99
25 Catalysts 11 00760 i049 Catalysts 11 00760 i050125100/>99
26 Catalysts 11 00760 i051 Catalysts 11 00760 i052135100/>99
27 Catalysts 11 00760 i053 Catalysts 11 00760 i05445100/>99
28 Catalysts 11 00760 i055 Catalysts 11 00760 i056140100/>99
Conditions: Substrate (2.0 mmole), (1%) ZnO–MnCO3/(1%-NDG) catalyst annealed at 300 °C (0.30 g), toluene (10 mL), O2 flow rate (20 mL/min), operation temperature (100 °C), and time (5 min).
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Khan, M.; Adil, S.F.; Assal, M.E.; Alharthi, A.I.; Shaik, M.R.; Kuniyil, M.; Al-Warthan, A.; Khan, A.; Nawaz, Z.; Shaikh, H.; et al. Solventless Mechanochemical Fabrication of ZnO–MnCO3/N-Doped Graphene Nanocomposite: Efficacious and Recoverable Catalyst for Selective Aerobic Dehydrogenation of Alcohols under Alkali-Free Conditions. Catalysts 2021, 11, 760. https://doi.org/10.3390/catal11070760

AMA Style

Khan M, Adil SF, Assal ME, Alharthi AI, Shaik MR, Kuniyil M, Al-Warthan A, Khan A, Nawaz Z, Shaikh H, et al. Solventless Mechanochemical Fabrication of ZnO–MnCO3/N-Doped Graphene Nanocomposite: Efficacious and Recoverable Catalyst for Selective Aerobic Dehydrogenation of Alcohols under Alkali-Free Conditions. Catalysts. 2021; 11(7):760. https://doi.org/10.3390/catal11070760

Chicago/Turabian Style

Khan, Mujeeb, Syed Farooq Adil, Mohamed E. Assal, Abdulrahman I. Alharthi, Mohammed Rafi Shaik, Mufsir Kuniyil, Abdulrahman Al-Warthan, Aslam Khan, Zeeshan Nawaz, Hamid Shaikh, and et al. 2021. "Solventless Mechanochemical Fabrication of ZnO–MnCO3/N-Doped Graphene Nanocomposite: Efficacious and Recoverable Catalyst for Selective Aerobic Dehydrogenation of Alcohols under Alkali-Free Conditions" Catalysts 11, no. 7: 760. https://doi.org/10.3390/catal11070760

APA Style

Khan, M., Adil, S. F., Assal, M. E., Alharthi, A. I., Shaik, M. R., Kuniyil, M., Al-Warthan, A., Khan, A., Nawaz, Z., Shaikh, H., & Siddiqui, M. R. H. (2021). Solventless Mechanochemical Fabrication of ZnO–MnCO3/N-Doped Graphene Nanocomposite: Efficacious and Recoverable Catalyst for Selective Aerobic Dehydrogenation of Alcohols under Alkali-Free Conditions. Catalysts, 11(7), 760. https://doi.org/10.3390/catal11070760

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