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Synthesis and characterization of Ag@Ni co-axial nanocables and their fluorescent and catalytic properties

  • Sadia Sharif EMAIL logo , Taiba Ahmed , Zahoor Ahmad EMAIL logo , Muhammad Aziz Choudhary and Muhammad Arshad
Published/Copyright: May 20, 2024
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Science and Engineering of Composite Materials
From the journal Science and Engineering of Composite Materials Volume 31 Issue 1

Abstract

We report here a convenient, rapid one-pot synthesis of new metal–metal core–shell nanocomposites comprising silver nanowires (AgNWs) coated with nickel. The resulting AgNWs and nickel-coated silver nanocables average 60–80 nm in diameter were prepared by the polyol synthetic route. This method employed ethylene glycol as a reducing agent and polyvinylpyrrolidone as a capping agent. These nanomaterials are designated as AgNWs (0.1 M) and Ag@Ni (0.2 M), Ag@Ni (0.3 M), Ag@Ni (0.4 M), and Ag@Ni (0.5 M) nanocables based on the nickel content and were characterized by scanning electron microscopy (SEM) with energy dispersive X-ray spectroscopy (EDX), X-ray diffraction (XRD), UV–Visible (UV–Vis) spectroscopy, and photoluminescence (PL) spectroscopy. The morphology of each nanowire and nanocable was clarified using SEM, while EDX quantified the presence of Ni. XRD patterns confirmed the face-centered cubic structure of the nanomaterials. The Debye–Scherrer formula was applied to establish different characteristics such as crystallite size and lattice constant. Surface plasmon resonance was measured using UV−Vis spectroscopy and fluorescence of each product was determined by PL spectroscopy, respectively. Both the AgNWs and Ag@Ni nanocables catalyze the reduction of p-nitrophenol to p-aminophenol by sodium borohydride.

Graphical abstract

Keywords: AgNWs, Ag@Ni nanocomposites; polyol method, catalytic reduction; fluorescence

1 Introduction

The synthesis of metal–metal nanocomposites with improved properties for various applications is important in material science and nanotechnology [1,2]. Heteronuclear core–shell metallic nanostructures have gained much importance because of their value in the fields of optics, medicine, catalysis, energy conversion, and storage [3–6]. In such materials, the core has major functional properties, and the surrounding shell protects and stabilizes the inner core. Since the properties of nanostructures greatly depend upon their shape, size, and composition, these structures exhibit significantly superior and enhanced characteristics relative to their single-component counterparts [7–9]. Metal-based nanoparticles (NPs) have intrigued scientists for more than a century and almost any metal can be converted into nanostructures such as copper (Cu), silver (Ag), aluminium (Al), gold (Au), cobalt (Co), cadmium (Cd), lead (Pb), iron (Fe), zinc (Zn), and nickel (Ni) [10]. The capping agents of such nanocomposites facilitate the effective catalysis of stereoselective and stereospecific processes due to steric hindrances from specific crystal planes [11].

McKiernan et al. synthesized core/shell Ag@Ni nanowires via two-step solution-based method and studied their electric and magnetic properties. They observed a decrease in electric conductivity of Ag nanowires with a coating of nickel because of electron transfer from the silver core to the nickel. The Ag@Ni core/sheath nanocomposites show potential applications in areas such as medical, spintronics, displays and electronics [12–14]. Zhang et al. prepared an efficient electrocatalyst for hydrogen evolution by coating AgNWs with nickel [15]. Recently, hydrothermal [16], laser ablation [17], galvanic replacement [18], and sonochemical [19] methods have been used to synthesize bimetallic core/shell nanostructures to improve coating quality. The microwave polyol method was used by Tsuji et al. for the synthesis of Ag@Ni core/shell NPs [20]. Superparamagnetic core/shell Ag@Ni NPs and Ag@Pd NPs were fabricated by using the one-pot synthetic method. The as-synthesized product was used as a catalyst for the hydrolysis of NaBH4 to generate hydrogen (H2) gas. In addition, better catalysts have been fabricated by coating metal oxide layers on metal cores. The resulting core/shell NPs exhibit enhanced catalytic performance compared to conventional supported catalysts [21,22]. We note that sodium borohydride can be problematical in the synthesis of bimetallic nanostructured catalysts because it can reduce some metal ions at room temperature during synthesis, and this frequently leads to irregular particle sizes.

Nickel catalyzes many reactions including oxidative coupling of inert chemicals and hydrogenation of vegetable oils [23,24]. Bimetallic Ag@Ni/C particles are effective cathodic catalysts in alkaline fuel cells due to their low working temperature and low corrosivity. In addition, nickel and nickel dispersion coatings are used in a multitude of applications where corrosion and wear resistance are challenges. Such dispersion films combine the ductility of the metal matrix with the hardness of incorporated non-metallic particles, such as alumina, titania, or silicon carbide [25]. Coatings of nickel, tin, and chromium are cathodic coatings as these are higher than steel in the galvanic series. These coatings provide a physical barrier between metal and the environment [26]. Also, nano-sized nickel catalysts are used for Stille coupling reactions in water. Nickel NPs, like those of other catalytic transition metals, benefit from large surface-to-volume ratios, which result in greater efficiency compared to bulk materials [27]. Nickel NPs can be used for the conversion of p-nitrophenol (p-NP) to p-aminophenol (p-AP) through catalytic hydrogenation. Despite these extensive catalytic applications of nickel, improvements are still needed in performance and catalyst cost [28]. The main objective of this work is to study the morphology of Ni sheath on the surface of nanostructure and investigate the catalytic and fluorescent properties of as synthesized material.

This study reports easily prepared Ag@Ni co-axial nanocable catalysts for the selective conversion of p-NP to p-AP by sodium borohydride which is more effective than many reported catalysts for this process [29]. This hybrid nanomaterial has been characterized by multiple physical techniques and its catalytic activity studied in detail.

2 Experimental

This section describes the material used in the study and the process used in the synthesis of nanocomposites.

2.1 Materials

Analytical grade reagents and chemicals were used in this work. Nickel acetate (Degussa) and silver nitrate AgNO3 99.0% (Analytical reagent) were used as precursors. Ethylene glycol (EG) (C2H6O2) 99% (Sigma Aldrich) was employed as solvent and reductant, and polyvinylpyrrolidone (PVP, K-90 from Daejung Reagent Chemicals-Korea) was used as a capping agent. p-NP (UNI-CHEM), acetone (Ridel-de-Haen), sodium borohydride (NaBH4), and absolute ethanol (CH3CH2OH) from Merck were used as received.

2.2 Methods

This section presents a discussion of the specific steps used in the literature review and collection of data for the study.

2.2.1 Synthesis of AgNWs

AgNWs (0.1 M) were synthesized using the polyol method. In a typical synthesis, 10 mL of EG was pre-heated for 30 min at 160°C. Then, 60 µL aliquots of an EG solution of NaCl (0.0087 g in 5 mL) were added to 10 mL of pre-heated EG. To this resulting solution was added slowly and dropwise EG solutions of silver nitrate (5 mL, 0.085 g, 0.5 mmol) and PVP (5 mL, 0.055 g, 0.5 mmol). After these additions, the resulting solution was yellowish brown which turned grey after a few minutes. The temperature of the reaction mixture dropped to 140°C during the addition. It was then maintained for 1 h at 160°C, acetone was added, and the resulting mixture was centrifuged at 3,000 rpm for 15 min. The compacted solid product was suspended in ethanol and centrifuged, sequentially, several times to afford the gray-colored AgNWs.

2.2.2 Synthesis of Ag@Ni nanocables

The Ag@Ni nanostructures were synthesized by preheating 10 mL of EG at 160°C under continuous stirring for 1 h. The EG solutions of silver nitrate (AgNO3; 0.085 g, 0.5 mmol) and PVP (0.055 g, 0.5 mmol) were added dropwise to the preheated EG. The addition of the AgNO3 solution resulted in the formation of seeds, which was followed by the formation of NWs. The silver nanostructures with varying amounts of nickel coating were prepared using varying concentrations of nickel acetate (0.2, 0.3, 0.4, and 0.5 M solutions in EG). Here, a 2 mL solution of 0.2 M (0.09 g) nickel acetate was added to the above reaction after 30 min. Each reaction was stirred for 1 h to ensure completion. For the synthesis of Ag@Ni (0.3 M), Ag@Ni (0.4 M), and Ag@Ni (0.5 M), a similar method was applied. Finally, the reaction was cooled to room temperature, washed with ethanol, and centrifuged at 6,000 rpm to remove any small particles and un-passivated PVP. Each sample was dispersed in ethanol and designated as Ag@Ni (0.2 M), Ag@Ni (0.3 M), Ag@Ni (0.4 M), and Ag@Ni (0.5 M).

2.3 Catalytic properties of AgNWs and Ag@Ni nanocables

The catalytic reduction of p-NP to p-AP by NaBH4 was studied in the presence of the nickel nanocatalyst in aqueous media. For this purpose, p-NP (0.0069 g, 0.05 mmol) and NaBH4 (0.007 g, 0.2 mmol) were prepared, separately, in 5.0 mL of distilled water. A molar 1:4 ratio of substrate:reagent was used. The catalyst, AgNWs (0.1 M), was added to the solution of p-NP, and the resulting mixture was sonicated for 30 min at room temperature. The reaction was started by the addition of the aqueous NaBH4 solution as shown in Scheme 1. The catalytic conversion was followed by the consumption of p-NP monitored at 400 nm. The same procedure was used to study the catalytic behavior of Ni-coated AgNWs using 0.025 g of AgNWs (0.1 M), Ag@Ni (0.2 M), Ag@Ni (0.3 M), and Ag@Ni (0.4 M).

Scheme 1 Reaction scheme for the reduction of p-NP to p-AP.
Scheme 1

Reaction scheme for the reduction of p-NP to p-AP.

2.4 Characterization of Ag@Ni nanocables

The following methods were used to establish the structure and morphology of the as-prepared samples. A TESCAN MIRA3 XMU scanning electron microscope coupled with energy dispersive X-ray spectroscopy (EDX) provided both morphologies and elemental compositions, while X-ray diffraction (XRD) (Bruker D-8 discoverer X-ray diffractometer) gave the structural information. UV–Visible (UV–Vis) spectroscopy (SHIMADZU UV 1800 Spectrophotometer) and photoluminescence (PL) spectroscopy (SHIMADZU RF-6000 Spectro Fluorometer) were used to quantify surface plasmon resonance (SPR) and fluorescent properties of the nanostructures.

3 Results and discussion

3.1 Scanning electron microscopy (SEM) and EDX characterization

The SEM micrographs of the pure AgNWs and Ag@Ni nanocables are shown in Figure 1a–e. Figure 1a indicates the AgNWs diameters between 60 and 80 nm and lengths on μm scale. Such dimensions are consistent with reported data [30]. The images indicate that the as-synthesized wires have smooth surfaces at the 500-nm scale. Furthermore, the new structures appear in different morphologies including spheres, cubes, and rod-like NPs (Figure 1a–e). The SEM images of Ag@Ni (0.2 M), Ag@Ni (0.3 M), Ag@Ni (0.4 M), and Ag@Ni (0.5 M) are shown in Figure 1b–e. Figure 1b shows the presence of rod-like NPs which co-exist with the AgNWs. Additionally, there are small deposits of spherical NPs around the AgNWs. In these domains, the Ag support is in its initial growth mode. Thus, Figure 1a and b shows that different metal precursors result in highly varied morphologies under otherwise identical conditions. Such results help to understand the impact of the cations and the PVP capping agents used in the synthesis, the reducing ability of the metal precursors, and the potential of multi-metal nuclei to develop stable dimensions. Figure 1c shows NWs along with some NPs. The diameter of the AgNWs is 55–60 nm, but these are interspersed with some ultra-long, thin (30 nm in diameter) AgNWs. The observed diameter of the former in Figure 1d is 57–65 nm, with the presence of ultrathin wires around 31 nm diameter, along with NPs with geometry spherical and cubic shapes. The cubic NPs are also within the 70–75 nm size range. The NWs are still the dominant structures in this case. The small spherical NPs in Figure 1e disappeared upon increasing the concentration of nickel. The diameter of the wires also increased up to 80 nm with the coating of nickel because the tiny nickel NPs are uniformly deposited on their surface.

Figure 1 SEM images of (a) AgNWs (0.1 M) and nanocables (b) Ag@Ni (0.2 M), (c) Ag@Ni (0.3 M), (d) Ag@Ni (0.4 M), and (e) Ag@Ni (0.5 M): (f) EDX pattern and (f1) Line mapping of Ag@Ni (0.2 M).
Figure 1

SEM images of (a) AgNWs (0.1 M) and nanocables (b) Ag@Ni (0.2 M), (c) Ag@Ni (0.3 M), (d) Ag@Ni (0.4 M), and (e) Ag@Ni (0.5 M): (f) EDX pattern and (f1) Line mapping of Ag@Ni (0.2 M).

The images depicted on the SEM were also analyzed using EDX to assess the elemental compositions. The EDX pattern shows the weight percentage of Ag and Ni in the nanocables. Silver is the dominant element in all cases. The existence of Si in the EDX is due to the glass substrate, the reduced silver, Ag(i), and oxygen result from the surface oxidation of these structures. Ag:Ni weight percentage for the nanocables displayed in Figure 1b–e is 3.04:0.44, 7.26:0.46, 18.31:2.40, and 44.55:2.54.

3.2 XRD analysis

XRD was used to study the degree of crystallinity of the AgNWs and Ag@Ni nanocables in Figure 2a–e. According to Figure 2a, four distinct diffraction peaks at 2θ = 38.2°, 44.6°, 65°, and 77.4° have been assigned as planes (111), (200), (220), and (311), respectively. It is worth noting that the peak at 38.02° exhibits relatively high intensity, indicating the anisotropic growth of the (111) phase of Ag during synthesis. An additional peak appeared at 77.4° when data were recorded in the scan range of 10–80° which corresponds to the (311) plane of fcc Ag. The strong and narrow peaks show a highly crystalline nature. The characteristic peak of Ni which was supposed to be at 52° did not appear due to the low concentration of nickel. This shows that the silver phase is dominant in both AgNWs and Ag@Ni nanocables. While Figure 2b and c further shows anisotropic behavior, a peak at 20° derives from PVP, which is present due to its affinity with particles in the sample. Typically, residual polymer shows up in many just-synthesized nanocomposites and is generally seen in the PXRD data as is the case here. The remaining four distinct diffraction peaks of Ag in Figure 2b and c are also in Figure 2a. Subsequently, mass transport on the growing end of the NWs decreased, allowing ample time for existing structures to rearrange to the more stable phase.

Figure 2 XRD pattern of (a) AgNWs (0.1 M), (b) Ag@Ni (0.2 M), (c) Ag@Ni (0.2 M), (d) Ag@Ni (0.4 M), and (e) Ag@Ni (0.5 M).
Figure 2

XRD pattern of (a) AgNWs (0.1 M), (b) Ag@Ni (0.2 M), (c) Ag@Ni (0.2 M), (d) Ag@Ni (0.4 M), and (e) Ag@Ni (0.5 M).

We have also found that the use of NaCl in the polyol reduction reactions, in which Cl− ions are released, results in an improved yield of AgNWs [31]. The crystallite sizes of the as-synthesized samples were calculated from the full-width at half maximum (FWHM) of the Bragg reflections using the Debye–Scherrer equation:

(1) D = K λ / β cos θ ,

where D represents the crystallite size (nm), K is the dimensionless shape factor called the Scherrer constant having a value of about 0.94 which can vary with the actual shape of the crystallite, λ is the wavelength of the X-ray source, typically 0.15418 nm, β represents the FWHM intensity in radians, and θ is the Bragg angle or peak position of main crystal plane. The crystallite size is calculated for the samples in Figure 2a–e: 36, 35, 33, 32, and 30 nm by choosing the (111) plane of Ag and showing that the sizes decrease with increasing Ni percent. The lattice spacing was determined using the Bragg equation:

(2) n λ = 2 d sin θ ,

where d represents the lattice spacing, n is the order of diffraction, λ is the X-ray wavelength, and θ is the peak position angle. By choosing the (111) plane of Ag, the lattice spacings were determined to be 2.354, 2.356, 2.358, 2.36, and 2.36 Å. This reduction in spacing results from the Ni atoms having a smaller radius (124 pm) than Ag atoms (144 pm) in the silver lattice. The decrease in crystallite size with increasing Ni content and the presence of single fcc structure peaks are evidence that there is atomic level alloying of the two metal atoms. It is worth noting that the peak at 38.02° is relatively intense, indicating anisotropic growth of Ag at (111) phase and coaxial growth of Ni in the same phase.

3.3 UV–Vis spectroscopy

SPRs were determined for each sample from the λ max values in the UV–Vis spectra. Figure 3 shows the SPR and the morphological evolution of AgNWs and the nickel-coated AgNWs. The SPR peaks appeared at different wavelengths proving to be dependent on the shapes and sizes of the metal nanostructures [32]. Metal surfaces exhibit plasma-like properties that result from free electrons and positively charged nuclei in the surface layers. SPR occurs near the AgNW surface, as electrons are excited to the conduction band. The SPR peaks give rise to intense colors. Figure 3 shows the spectra of AgNWs (0.1 M), Ag@Ni (0.2 M), Ag@Ni (0.3 M), Ag@Ni (0.4 M), and Ag@Ni (0.5 M). The two relatively sharp SPR peaks at 356 and 386 nm result from the transverse mode of the AgNWs. The shoulder peak at 356 nm and the peak at 386 nm are attributed to the out-of-plane quadropole resonance and the out-of-plane dipole resonance of the AgNWs, respectively [33,34]. The broad peak at 386 nm for Ag@Ni nanostructures indicates the presence of NWs as well as particles. The transverse SPR of AgNWs (0.1 M) at 356 nm has been suppressed, a result consistent with nickel deposited on the surface of wires. A slight red shift is also observed in the case of Ag@Ni (0.2 M), Ag@Ni (0.3 M), Ag@Ni (0.4 M), and Ag@Ni (0.5 M). The band gap of the AgNWs is calculated using the equation:

(3) E g = h c / λ ,

where E g is the band gap, h and c are constants, and λ is an absorption wavelength. The calculated band gaps for samples illustrated in Figure 3 are 3.24, 3.07, 3.06, 3.04, and 2.99 eV. The existence of a band gap in Ag nanostructures clearly demonstrates that the ψ function of the electron is restricted in the nanodomain and allowed in the microdomain for the conduction of electrons.

Figure 3 UV–Vis spectra of AgNWs (0.1 M) and the Ag@Ni (0.2 M), Ag@Ni (0.3 M), Ag@Ni (0.4 M), and Ag@Ni (0.5 M) nanocables.
Figure 3

UV–Vis spectra of AgNWs (0.1 M) and the Ag@Ni (0.2 M), Ag@Ni (0.3 M), Ag@Ni (0.4 M), and Ag@Ni (0.5 M) nanocables.

3.4 PL spectroscopy

Metal nanostructures exhibit good light-harvesting behavior because their fluorescence is not limited to a single wavelength. Both fluorescence and absorptions in metal nanostructures are broad. These optical characteristics frequently render metal nanostructures suitable candidates for photovoltaic applications [35]. Figure 4a–c shows the PL spectra of AgNWs (0.1 M), Ag@Ni (0.2 M), Ag@Ni (0.3 M), Ag@Ni (0.4 M), and Ag@Ni (0.5 M) at different excitation wavelengths. In Figure 4b, the different excitation wavelengths of 356, 361, 364, 365, and 368 nm were used for each sample and the respective emissions were recorded. All the samples gave an emission of around 500 nm, but the intensity of the emitted light was reduced upon coating AgNWs with nickel. The same phenomenon is the case in Figure 4c where excitation wavelengths of 386–430 nm were used for AgNWs and Ag@Ni nanostructures AgNWs (0.1 M), Ag@Ni (0.2 M), Ag@Ni (0.3 M), Ag@Ni (0.4 M), and Ag@Ni (0.5 M), respectively, and emissions were recorded between 500 and 600 nm. The fluorescence of Ag is more evident in the AgNWs (0.1 M) sample and more intense compared to the other samples. High enhancement of fluorescence emission, improved fluorophore photostability, and significant reduction of fluorescence lifetime were derived from the high aspect ratio of the AgNWs. The data showed that the Ag emission spectra follow the relationship in the equation:

(4) n λ excitation = 2 n λ emission ,

Figure 4 PL spectra (a–c) of AgNWs (0.1 M) and nanocables Ag@Ni (0.2 M), Ag@Ni (0.3 M), Ag@Ni (0.4 M), and Ag@Ni (0.5 M) at different wavelengths.
Figure 4

PL spectra (a–c) of AgNWs (0.1 M) and nanocables Ag@Ni (0.2 M), Ag@Ni (0.3 M), Ag@Ni (0.4 M), and Ag@Ni (0.5 M) at different wavelengths.

which reflect the non-linear second-order optical properties of confirmed metal nanostructures. These, in turn, result from electric-dipole interaction with radiation of strong intensity.

3.5 Catalytic activity of the AgNWs and Ag@Ni nanocables

The nickel is used in a variety of catalytic reactions, such as alcohol oxidation and the hydrogenation of unsaturated olefins. It is also an important catalyst precursor for ethylene homopolymerization and the alternating copolymerization of ethylene with carbon monoxide [36]. For the reduction of carbonyl, imine, nitrile, and alkyne groups, NaBH4 is commonly used, but it is the least effective for the reduction of nitro residues. Therefore, many researchers use different nanocatalysts to improve nitro-to-amino reduction selectivity. Recently, nano-Ag has been successfully employed for the reduction of nitro groups by NaBH4 [37]. The yellow-colored aqueous mixture of p-NP and sodium borohydride shows an absorption maximum at 400 nm due to the formation of p-nitrophenolate ions. Reduction does not proceed in the absence of catalyst and the absorption peak remains unchanged over time. However, after the addition of catalyst, a change in the absorption pattern is observed. The yellow solution becomes colorless at the end of reaction, indicating the reduction of p-NP to p-AP. AgNWs (0.1 M), Ag@Ni (0.2 M), Ag@Ni (0.3 M), and Ag@Ni (0.4) converted the phenolate ions into p-AP in 48, 40, 36, and 26 min, respectively. The speed of reduction correlates with the thickness of the Ni layer and higher Ni content in the Ag/Ni nanocomposite. The main peak of the nitrophenolate at 400 nm decreases with time; whereas, a second peak at 300 nm, of the aminophenol product, increases slowly. Finally, the isobestic point is clearly observed in all the Ag@Ni nanocomposites around 314 nm. Figure 5 shows the successive UV–Vis absorption spectra of the reduction of p-NP by NaBH4 in the presence of AgNWs or Ag@Ni nanocable catalysts. The kinetic reaction rate order was calculated from the change in concentration of the substrate A (phenolate ions) as shown in Figure 6. The plot of 1/[A] versus time reveals second-order kinetics.

Figure 5 Catalytic activities of (a) AgNWs (0.1 M), (b) Ag@Ni (0.2 M), (c) Ag@Ni (0.3 M), and (d) Ag@Ni (0.4 M) for reduction of p-NP to p-AP by NaBH4.
Figure 5

Catalytic activities of (a) AgNWs (0.1 M), (b) Ag@Ni (0.2 M), (c) Ag@Ni (0.3 M), and (d) Ag@Ni (0.4 M) for reduction of p-NP to p-AP by NaBH4.

Figure 6 Plot of 1/[A] versus time for reduction of p-NP to p-AP by NaBH4 in aqueous solution, showing good second-order kinetics.
Figure 6

Plot of 1/[A] versus time for reduction of p-NP to p-AP by NaBH4 in aqueous solution, showing good second-order kinetics.

4 Conclusions

This study reports a new and facile approach to fabricate metal@metal nanocomposites containing Ag and Ni. Using the polyol method, Ag@Ni nanocables with different concentrations of Ni were successfully synthesized. The product of the syntheses was confirmed, using UV–Vis spectroscopy, SEM coupled with EDX, and XRD. SEM image shows that with changing the metal concentration, the morphology is changed. The suppression of transverse SPR of AgNWs at 356 nm confirmed that the AgNW surfaces were coated with nickel. XRD showed the characteristic sharp peaks of silver. The Ag-based nanomaterials exhibited good light harvesting properties, which were assessed through PL spectroscopy. Ni-containing nanocomposites catalyzed the facile and selective reduction of p-NP to p-AP by sodium borohydride. The time required for the reduction decreased with increasing nickel content in the silver-nickel NWs (Table 1). This comparison clearly shows that the silver@nickel nanocables are more efficient catalysts for p-NP reduction than Ag nanowires. In addition, the new nanocomposites generally enhance the ability of NaBH4 to reduce nitro groups. These silver nickel nanocomposites may well have enhanced rates and selectivities in other Ni-based catalytic reductions. The nanocomposite formed has extensive potential for use in many sectors across the medical, electronic, and environmental fields.

Table 1

Comparison of catalyst quantity and time of reduction of p-NP

Sr. no Name of sample Reduction time (min) Slope (k) (M−1 s−1)
1 AgNWs 48 0.0050
2 Ag@Ni (0.2 M) 40 0.0052
3 Ag@Ni (0.3 M) 36 0.0186
4 Ag@Ni (0.4 M) 26 1.03295

Acknowledgments

The ORICMUST and HEC (Project Number: 7183) Pakistan are gratefully acknowledged for the financial support to the study.

  1. Funding information: The study was funded by The ORICMUST and HEC (Project Number: 7183).

  2. Author contributions: All authors have accepted responsibility for the entire content of this manuscript and consented to its submission to the journal, reviewed all the results, and approved the final version of the manuscript. SS: investigation, supervision, writing – original draft. TA: investigation, validation. ZA: conceptualization, visualization, writing – original draft, writing – review & editing. MAC: conceptualization, supervision, funding acquisition. MA: methodology, software.

  3. Conflict of interest: Authors state no conflict of interest.

  4. Data availability statement: The authors confirm that the data supporting the findings of this study are available within the article or its supplementary materials can be shared upon request.

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Received: 2023-12-07
Revised: 2024-03-25
Accepted: 2024-04-11
Published Online: 2024-05-20

© 2024 the author(s), published by De Gruyter

This work is licensed under the Creative Commons Attribution 4.0 International License.

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https://doi.org/10.1515/secm-2024-0010
Keywords for this article
AgNWs, Ag@Ni nanocomposites; polyol method, catalytic reduction; fluorescence
Creative Commons
BY 4.0

Articles in the same Issue

  1. Regular Articles
  2. Research on damage evolution mechanisms under compressive and tensile tests of plain weave SiCf/SiC composites using in situ X-ray CT
  3. Structural optimization of trays in bolt support systems
  4. Continuum percolation of the realistic nonuniform ITZs in 3D polyphase concrete systems involving the aggregate shape and size differentiation
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