# Adsorption of Molecular Gases on Silver/Carbon Nanotube Composites at Low Temperatures and Low Pressures

Authors: M. Barberio; P. Barone; F. Stranges; R. A. Romano; F. Xu; A. Bonanno
Journal: Journal of Chemistry
 (2014)

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## Abstract

We present an experimental study adsorption of molecular gases (N2, H2, O2, CH4, C2H4, and C2H6)  on multiwalled carbon nanotubes (MWCNTs) and MWCNT doped with Ag at low temperatures (35 K) and pressures (10−6 Torr) using the temperature programmed desorption technique. Our results show that the desorption kinetics is of the first order; furthermore comparative measurements indicate that Ag/MWCNTs have an adsorption capacity higher than that of a pure sample suggesting that these composites are good candidates as gas cryosorbers for applications in cryopumps or sensor of latest generation.


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## Body

## 1. Introduction

In last decades, carbon nanotubes have been intensively studied because of their importance as building blocks in nanotechnology [1–3]. In particular, gas adsorption on carbon nanotubes and nanotubes bundles is an important issue for both fundamental research in nanotubes and their technical applications [4–6]. Considerable experimental and theoretical efforts have been dedicated to hydrogen storage in nanotube based materials [4–6], but the changes in electronic properties of carbon nanotubes upon exposure to gases as O2, NO2, NH3, or CH4 are also object of several studies for application to sensor.Recently we proposed to use multiwalled carbon nanotubes (MWCNTs) as hydrogen cryosorber in cryopumps and accelerators of latest generation [7]. We have demonstrated that MWCNT has, in conditions of very low temperature and pressure, an adsorption capacity about two orders of magnitude higher than that of activated carbon (charcoal) [7].A means to achieve a high uptake of gas on a surface is to vary the porosity and the specific area of the adsorption surfaces, so that trapping and condensation of molecules inside the pores increase. Carbon nanotubes are good candidates for gas storage because of their high specific surface area and large volume of pores. Therefore it can be interesting to study the doping effects of nanoparticles on specific surface of carbon nanotubes. In fact, metallic nanoparticles possess a large surface area which makes them highly reactive in interactions with gas molecules. So, the insertion of metallic nanoparticles in nanotube networks can lead to the formation of composites with very great surface area. Recently we introduced a simple method to obtain composites based on carbon nanotubes doped with Ag nanoparticles [8]. We obtained that the Ag doping produces strong changes in electronic and optical properties of carbon nanotubes at very low nanoparticle concentration [8]. In this work we investigate the possibility to use these new materials as gas cryosorbers and demonstrate that the Ag doping improves the adsorption without changing the physical properties of chemical bonds between gas and surfaces. We report data of adsorption for different gases (N2, H2, O2, CH4, C2H4, and C2H6) at very low temperature and pressure and compare the results with those obtained from pure MWCNT and pure copper surfaces.The composites were produced by mixing commercial MWCNT and Ag nanoparticles obtained by laser ablation (LA). The produced nanoparticles were monitored by optical absorption measurements and SEM images, while the composites were characterized by X-ray photoelectron spectroscopy (XPS) and SEM images. The gas adsorption was studied by temperature programmed desorption (TPD) technique.


## 2. Experiments

### 2.1. Materials

The MWCNT powder used in this study was purchased from “Nanostructured & Amorphous Materials, Inc.,” with a nominal purity greater than 95%. The samples are characterized (SEM analysis in Figure1(a)) by the presence of CNT bundles with an average diameter of 30 nm and 5–20 μm in length.Figure 1
SEM images of Ag/CNT sample: (a) BSE image and (b) corresponding SE image of sample produced by process A. (c) BSE and (d) SE details on silver microparticles; (e-f) SE images of a silver microparticle completely covered by CNT.The powder of silver microparticles is obtained by laser ablation process on silver bar (nominal purity of 99.99% purchased from Goodfellow) which leads to formation of spherical and spheroid particles with dimensions of about 600–500 nm. Laser ablation was performed on silver bar placed vertically in a glass vessel filled with a 20 mL of acetone. We carried out the LA process with the first harmonic (1064 nm) of a Quanta-Giant series 710 Nd:YAG laser operating at 10 Hz (laser power is fixed at 600 mJ/pulse). Upon irradiation of the laser beam, the solution, initially transparent, gradually turns brownish-yellow indicating the formation of Ag nanoparticles in solution [9]. After the LA, the solution is sonicated to prevent the self-aggregation of microparticles suspended in acetone and the formation of macroclusters. SEM images of Ag particles obtained by the analysis in backscattered electron mode (BSE) (Figure 1(b)) show the formation of spherical silver particles with dimensions ranging from 100 to 500 nm. Shape and dimensions of silver nanoparticles were monitored during LA process by measuring the optical absorbance of the solution [9]. The process was stopped when the optimal conditions of shape and dimensions were reached.Silver/carbon nanotubes composite structures were prepared using a simple chemical mixing method as indicated in Yao et al. [10, 11] and improved in several of our works to obtain CNT based heterostructures [10, and references therein]. This method is a sequence of mixing, evaporation, and drying processes. In the first step, carbon nanotubes and the acetone solution containing silver particles are dispersed in dichlorobenzene (C6H4Cl2) as solvent and then sonicated for 1 h. After sonication the suspension containing CNTs and silver is deposited on a copper plate (1 cm × 2 cm), previously sonicated in acetone, and then heated at 180°C in air on a hot plate for 15 minutes to allow solvent evaporation and a fairly accurate cleanness of carbon nanotubes. In effect the carbon nanotubes cleanness, as demonstrated in our previous works [10], is effective only after some heating cycles at high temperature in ultra-high vacuum systems. Using one heating cycle in air at low temperature allows removing only the amorphous carbon, but not the oxygen. The BSE-SEM images of the composites show spherical silver microparticles with dimensions of about 100–500 nm randomly dispersed on MWCNT bulk (Figure 1(c)). Images at higher zoom level obtained in secondary electron mode (SE-SEM) indicate that each nanoparticle is inserted in MWCNT bulk and wrapped by carbon nanotubes (Figures 1(d), 1(e), and 1(f)).


### 2.2. Methods

The transmitted spectrum was obtained by a Horiba VS-140 VIS-NIR spectrometer working in the 350–1200 nm range. A white led has been used as light source to enlighten the solution Ag-acetone (the vessel glass surface containing the solution is completely transparent to white light). Transmittance(t(λ)) and absorbance (a(λ)) as function of wavelength are obtained with the Beer-Lambert law:
(1)t(λ)=It(λ)Is(λ),a(λ)=-ln(t(λ)), where It(λ) is the transmitted light and Is(λ) is the source light.The transmitted spectrum was monitored during the whole laser ablation process, taking spectra at regular intervals of 5 seconds. At timet, the absorbance intensity A(t) of each spectral transition was obtained by numerical integration over λ, assuming a Gaussian distribution of the spectral bands (Figure 2).Figure 2
Absorbance spectra taken at regular interval of 50 seconds. Right inset: Gaussian analysis of the spectrum acquired after 500 s as an example of data treatment. Left inset: total optical absorbance versus LA irradiation time.XPS measurements were conducted in a UHV chamber equipped for standard surface analysis with a pressure in the range of 10−9 Torr. Nonmonochromatic Mg-Kα X-ray (hν=1253.64 eV) was used as excitation source. The XPS spectra were calibrated with the C 1s peak of a pure carbon sample (energy position 284.6 eV). All XPS spectra have been corrected for the analyzer transmission factor and background subtraction obtained by using the straight line subtraction mode. Moreover the XPS data were fitted assuming a Gaussian distribution.The thermal programmed desorption (TPD) experiments were conducted in a UHV chamber (base pressure in the low 10−9 Torr range) evacuated with a dry turbo pump (more information about experimental setup is in [7, 12, 13]). The gas (N2, H2, O2, CH4, C2H4, and C2H6 with purity of 99.999%) was introduced in the chamber through a precision leak valve while keeping the sample at an adsorption temperature of Tad=35 K and at a fixed pressure of 1×10-6 Torr (measured at room temperature and corrected for the ion gauge sensitivity factor), for a chosen time interval. The samples (3 mg for each sample) were deposited directly onto the copper head (6 cm2) of a cold finger with closed He cycling and dried. A quite uniform thin film was obtained and its adhesion to the copper surface remained stable during all the measurements. The sample temperature was monitored with an Au=0 : 7% Fe-chromel thermocouple. Thermal desorption was achieved by heating the head of the cold finger with a linear ramp (10 K/min) and the desorbed gas was measured with a quadrupole mass analyzer. No appreciable gas contamination signals were detected neither in the adsorption nor in the desorption processes. Complete reversibility of charging and discharging cycles was routinely verified and a total reproducibility was observed. The desorption rate was obtained by multiplying the detected gas partial pressure (the integral intensity of a quadrupole mass spectrum centered at specific gas atomic mass and composed of some 50 data points) by the vacuum system pumping speed (l/s technical data). The total amount of desorbed gas then could be evaluated from the integration of the desorption rate-time curves with an estimated error of about 5%.


## 2.1. Materials

The MWCNT powder used in this study was purchased from “Nanostructured & Amorphous Materials, Inc.,” with a nominal purity greater than 95%. The samples are characterized (SEM analysis in Figure1(a)) by the presence of CNT bundles with an average diameter of 30 nm and 5–20 μm in length.Figure 1
SEM images of Ag/CNT sample: (a) BSE image and (b) corresponding SE image of sample produced by process A. (c) BSE and (d) SE details on silver microparticles; (e-f) SE images of a silver microparticle completely covered by CNT.The powder of silver microparticles is obtained by laser ablation process on silver bar (nominal purity of 99.99% purchased from Goodfellow) which leads to formation of spherical and spheroid particles with dimensions of about 600–500 nm. Laser ablation was performed on silver bar placed vertically in a glass vessel filled with a 20 mL of acetone. We carried out the LA process with the first harmonic (1064 nm) of a Quanta-Giant series 710 Nd:YAG laser operating at 10 Hz (laser power is fixed at 600 mJ/pulse). Upon irradiation of the laser beam, the solution, initially transparent, gradually turns brownish-yellow indicating the formation of Ag nanoparticles in solution [9]. After the LA, the solution is sonicated to prevent the self-aggregation of microparticles suspended in acetone and the formation of macroclusters. SEM images of Ag particles obtained by the analysis in backscattered electron mode (BSE) (Figure 1(b)) show the formation of spherical silver particles with dimensions ranging from 100 to 500 nm. Shape and dimensions of silver nanoparticles were monitored during LA process by measuring the optical absorbance of the solution [9]. The process was stopped when the optimal conditions of shape and dimensions were reached.Silver/carbon nanotubes composite structures were prepared using a simple chemical mixing method as indicated in Yao et al. [10, 11] and improved in several of our works to obtain CNT based heterostructures [10, and references therein]. This method is a sequence of mixing, evaporation, and drying processes. In the first step, carbon nanotubes and the acetone solution containing silver particles are dispersed in dichlorobenzene (C6H4Cl2) as solvent and then sonicated for 1 h. After sonication the suspension containing CNTs and silver is deposited on a copper plate (1 cm × 2 cm), previously sonicated in acetone, and then heated at 180°C in air on a hot plate for 15 minutes to allow solvent evaporation and a fairly accurate cleanness of carbon nanotubes. In effect the carbon nanotubes cleanness, as demonstrated in our previous works [10], is effective only after some heating cycles at high temperature in ultra-high vacuum systems. Using one heating cycle in air at low temperature allows removing only the amorphous carbon, but not the oxygen. The BSE-SEM images of the composites show spherical silver microparticles with dimensions of about 100–500 nm randomly dispersed on MWCNT bulk (Figure 1(c)). Images at higher zoom level obtained in secondary electron mode (SE-SEM) indicate that each nanoparticle is inserted in MWCNT bulk and wrapped by carbon nanotubes (Figures 1(d), 1(e), and 1(f)).


## 2.2. Methods

The transmitted spectrum was obtained by a Horiba VS-140 VIS-NIR spectrometer working in the 350–1200 nm range. A white led has been used as light source to enlighten the solution Ag-acetone (the vessel glass surface containing the solution is completely transparent to white light). Transmittance(t(λ)) and absorbance (a(λ)) as function of wavelength are obtained with the Beer-Lambert law:
(1)t(λ)=It(λ)Is(λ),a(λ)=-ln(t(λ)), where It(λ) is the transmitted light and Is(λ) is the source light.The transmitted spectrum was monitored during the whole laser ablation process, taking spectra at regular intervals of 5 seconds. At timet, the absorbance intensity A(t) of each spectral transition was obtained by numerical integration over λ, assuming a Gaussian distribution of the spectral bands (Figure 2).Figure 2
Absorbance spectra taken at regular interval of 50 seconds. Right inset: Gaussian analysis of the spectrum acquired after 500 s as an example of data treatment. Left inset: total optical absorbance versus LA irradiation time.XPS measurements were conducted in a UHV chamber equipped for standard surface analysis with a pressure in the range of 10−9 Torr. Nonmonochromatic Mg-Kα X-ray (hν=1253.64 eV) was used as excitation source. The XPS spectra were calibrated with the C 1s peak of a pure carbon sample (energy position 284.6 eV). All XPS spectra have been corrected for the analyzer transmission factor and background subtraction obtained by using the straight line subtraction mode. Moreover the XPS data were fitted assuming a Gaussian distribution.The thermal programmed desorption (TPD) experiments were conducted in a UHV chamber (base pressure in the low 10−9 Torr range) evacuated with a dry turbo pump (more information about experimental setup is in [7, 12, 13]). The gas (N2, H2, O2, CH4, C2H4, and C2H6 with purity of 99.999%) was introduced in the chamber through a precision leak valve while keeping the sample at an adsorption temperature of Tad=35 K and at a fixed pressure of 1×10-6 Torr (measured at room temperature and corrected for the ion gauge sensitivity factor), for a chosen time interval. The samples (3 mg for each sample) were deposited directly onto the copper head (6 cm2) of a cold finger with closed He cycling and dried. A quite uniform thin film was obtained and its adhesion to the copper surface remained stable during all the measurements. The sample temperature was monitored with an Au=0 : 7% Fe-chromel thermocouple. Thermal desorption was achieved by heating the head of the cold finger with a linear ramp (10 K/min) and the desorbed gas was measured with a quadrupole mass analyzer. No appreciable gas contamination signals were detected neither in the adsorption nor in the desorption processes. Complete reversibility of charging and discharging cycles was routinely verified and a total reproducibility was observed. The desorption rate was obtained by multiplying the detected gas partial pressure (the integral intensity of a quadrupole mass spectrum centered at specific gas atomic mass and composed of some 50 data points) by the vacuum system pumping speed (l/s technical data). The total amount of desorbed gas then could be evaluated from the integration of the desorption rate-time curves with an estimated error of about 5%.


## 3. Results and Discussion

Conventionally metal nanoparticles are characterized by their extinction spectra (absorption and/or scattering spectra) [9]. The peaks observed in absorption or in scattering spectra of particles, during the light excitation, are due to resonant wavelengths of plasmon eigenmodes (called dipole plasmon resonance) of the particles as demonstrated in [9]. Secondary oscillations, called quadrupole plasmon resonances, appear at lower energy for larger particles [9, and references therein]. The plasmon oscillation frequency is determined by four factors: the density of electrons, the effective electron masses, and size and shape of charge distribution (i.e., by shape and size of nanoparticles) [9].We collected, for 500 seconds, the absorbance spectrum of acetone-nanoparticles solution during LA at regular time intervals of 5 seconds, monitoring the changes in its intensity and line shape. Figure2 shows, as example of typical measured, the absorbance spectra at intervals of 50 seconds. We observe that during the first 50 seconds the spectra exhibit two bands centered at about 460 nm and 930 nm with a full width at half maximum (FWHM) of 30 nm and 60 nm, respectively. After the first 100 seconds, a third band appears at about 520 nm while after 200 s a band at 620 nm emerges (see the right inset in Figure 2 for Gaussian analysis of spectrum taken at 500 s). All the four bands can be associated with oscillation of surface plasmon in spherical or spheroid nanoparticles. Kelly et al. in their theoretical work [9] calculated the plasmon absorption wavelength for both spherical and spheroid nanoparticles as function of particles dimensions. They demonstrated that spherical particles present two absorption bands centered at about 350 nm (dipole resonance) and at 440–460 nm (quadrupole resonance) for particles with dimensions of 60 nm. These positions change strongly with particles dimensions and shape. If the sphere diameter increases, the bands are red-shifted and can reach the NIR region if the particles are large spheroids.So, our absorption spectra (with three resonance bands) can be interpreted as superposition of signals from particles of different sizes in solution. In the first 50 seconds, LA produces spherical particles which generate the resonance at 460 nm. The dimensions of these particles, from the comparison with numerical data in [9], range between 60 and 70 nm. Moreover in the first phases a little amount of spheroid particles is also present (resonance at 930 nm). After the first 50 seconds the particle concentration in solutions increases and several nanoparticles aggregate to form spherical particles with larger dimensions causing the 520 and 620 band appearance. As the LA time increases, several particles aggregate forming larger spheres, while spheroid particles increase their concentration without changing size. SEM images in Figure 1(b) show spherical particles obtained after 500 s of LA, confirming the interpretation of our absorption spectra. The particle deposited after a LA time of 500 s is mainly spherical with a diameter of about 100–500 nm. In our deposited samples only a little amount of spheroid particles is observed as evidenced by the small increases of the 930 nm band. Moreover the total optical absorbance obtained as time integration of absorbance spectra (see left inset in Figure 2) increases with LA irradiation time, indicating the increases of silver nanoparticle amount in solution.XPS survey spectrum in Figure3 shows the presence in our Ag/CNT composites of carbon, oxygen and silver without signs of impurities caused by the growth processes. The C 1s line (inset in Figure 3) is asymmetric and cannot be reproduced by one single Gaussian. Our fit indicates the presence of three well-distinguished peaks at 284.3 (main structure of C 1s), 285.6 eV (C–O chemical bonds), and 308 eV that are typical of carbon structures. In particular the broad structure at 302 eV is due to plasma loss with both π and σ characters [14]. The O 1s lines present a main structure at roughly 532 eV; this structure is often assigned to oxygen bonded to C indicating a single C–O bonding [14]. The presence of C–O chemical bonds in the spectra is due to oxygen adsorbed in carbon nanotubes before the mixing with silver particles. The Ag 3d lines are not structured and do not present a shift with respect to lines taken from a pure silver surface. This excludes the formation of chemical bonds between CNT or oxygen and Ag.Figure 3
XPS survey spectrum taken from Ag/CNT composites. Inset: Gaussian analysis of C 1s line.The element percentage in composites, calculated by XPS data, indicates a very little presence of silver on the surface (about 0.1%). Besides this low doping, microporosity measurements indicate a strong increases of specific surface area of Ag/CNT with respect to pure MWCNT. In fact the specific surface for pure MWCNT is of 174 m2/g while for Ag/CNT composites are 2394 m²/g. Moreover the sample roughness, measured under AFM condition, increases of about 16% in sample with silver nanoparticles (70.8 nm for pure MWCNT and 83.3 nm for Ag/CNT composites).So, XPS and microporosity results indicate that Ag doping of CNT is a simple physisorption without any signs of chemical bonds; the only effect of doping is changing the porosity of surface. These results are also confirmed by the increases in desorption for all tested gases on Ag/CNT composites.In Figure4(a) we illustrate some representative TPD traces for different gases at dose 1000 L (the adsorption temperature is for all gases fixed at Tad=35K). The position of the desorption temperature changes with gas species indicating a different adsorption energy for different gases; in fact, it is known that the binding energy of a molecule on a surface varies with the adsorbate/surface combination [15].Temperature programmed desorption traces of molecular gases adsorbed on Ag/MWCNT composites at a dose of 1000 L (a). TPD traces of adsorbed C2H6 at different doses as example for all gases (b).
(a)
(b)Moreover Figure4(b) shows, as example for all gas, the changes in adsorption, varying the exposure dose (1 L = 10−6 Torr sec and the sample heating rate was fixed at 1 K = min) of C2H6; the behavior of all gases on both pure MWCNT and Ag/MWCNT is identical.These TPD traces are quite similar to each other and the temperature position of the spectrum maxima remains unchanged as the gas dose adsorption increases, clearly indicating a first-order desorption mechanism. This indicates interaction only between gas molecules and substrates, without gas-gas interplay on the sample surface. The position of the maximum in the desorption spectrum, indicated in Table1, is identical (in the limit of experimental error), for each gas, on both samples and on cold head copper surface. This indicates that the absorption energy is unchanged for different materials; consequently in all cases the gases are physisorbed on surfaces without formation of chemical bonds with the substrate. Moreover the desorption temperature, as demonstrated in our previous work [7], is associated with the absorption energies which are less than those required for chemisorption processes (>50 kJ/mol).Table 1
Desorption temperatures (K).
C2H4
C2H6
CH4
H2
N2
O2
Copper
65.07
70.22
48.5
42.7
44.4
45.27
MWCNT
65.25
69.39
47.58
41.7
43.9
43.1
Ag/MWCNT
64.41
70.4
48.67
41.6
44
43/50The only exception is the behavior of oxygen that (as visible from data in Table1) shows a desorption temperature of about 43 K on all surface and a second desorption at about 50 K on Ag/MWCNT composites. We attribute this behavior to great interaction between silver nanoparticles and oxygen. In our recent work [8] we demonstrate that silver nanoparticles exposed to atmospheric oxygen interact with oxygen to form silver oxide also in this case the exposure to O2 leads, as well as the oxygen absorption on surface, to the formation of silver oxide on Ag/MWCNT (as indicated by the Ag 3d XPS lines). So, the physisorbed oxygen is desorbed at 45 K (as on MWCNT or copper) while the chemisorbed oxygen is desorbed at higher temperature of 50 K.The total molecular gas content, as determined from integration of the desorbed gas TPD trace curves, is plotted, for all gases and for all analyzed surfaces, in Figure5 as a function of gas doses. It is interesting to note that it increases with doses for all surfaces, and for many of investigated gases the adsorption on Ag/MWCNT composites is greater than that on pure MWCNT, confirming the increases on specific area by doping with Ag nanoparticles. Only for H2 and CH4 the adsorption is comparable in pure and doped samples. Experiments on the absorption temperature of both these gases on carbon nanotubes and copper surfaces [7, 13] demonstrated that the adsorption is maximum at about 10–12 K and decreases strongly with temperature. So we can hypothesize that the adsorption temperature in this work is too high for H2 and CH4 adsorption also for Ag doped CNT.Molecular gases adsorbed on MWCNT, Ag/MWCNT, and copper cold head surface as a function of gases dose.
(a)
(b)
(c)
(d)
(e)
(f)


## 4. Conclusions

In this work we present a study of gas adsorption on Ag doped MWCNT. The Ag/MWCNT composites show an increase in specific area of about 15 times as compared with a pure MWCNT surface, even with a very low Ag doping (0.1%). The adsorption rate, which increases for many investigated gases (N2, O2, C2H4, and C2H6), shows in all cases a first-order adsorption process. The desorption temperatures, and then the absorption energies, are unchanged between pure MWCNT and Ag/MWCNT composites, clearly indicating that the absorption is on both samples a physisorption process without formation of chemical bonds between gases and substrate. The only exception is O2, since the silver nanoparticles are most reactive to oxygen and the O2 absorption leads to the formation of silver oxide on composite surfaces and to the appearance of a second peak, at higher energy, in the TPD spectrum.



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*Source: 816193-2014-01-09.xml*