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Photocatalytic Removal of Carcinogenic Reactive Red S3B Dye by using
ZnO and Cu doped ZnO Nanoparticles Synthesized by Polyol Method: A
Kinetic Study.Humaira Rashid Khan, a Ghulam Murtaza, b Muhammad Aziz Choudhary, a Zahoor Ahmed a
Mohammad Azad Malik c*
a Department of Chemistry, Mirpur University of science and Technology (MUST), Mirpur, AJ&K-
10250, Pakistanb School of Chemistry, The University of Manchester, Manchester, Oxford Road, M13 9PL, UKc School of Materials, The University of Manchester, Manchester, Oxford Road, M13 9PL, UK
Corresponding author Email: [email protected]
Abstract
Zinc oxide (ZnO) nanoparticles were synthesised from zinc acetate as a precursor and PVP as
a capping agent by polyol method. The as prepared ZnO nanoparticles were doped with
0.01M solution of copper acetate in PVP. Both ZnO and Cu-doped ZnO nanoparticles were
characterized by UV-Vis spectroscopy, X-rays diffraction (XRD), scanning electron
microscopy (SEM), photoluminescence (PL) and energy dispersion X-rays (EDX)
spectroscopy.
The sunlight irradiated photocatalytic degradation of Reactive Red S3B was carried out using
both ZnO and Cu doped ZnO nanoparticles. Both ZnO and Cu-doped ZnO decolourize the
respective dyes but Cu-doped ZnO nanoparticles were clearly more powerful catalyst than
ZnO. The kinetics of the photocatalytic degradation was also studied. It was found that the
degradation of Reactive Red S3B followed the pseudo first-order kinetics. These
photocatalysts are efficient and environment-friendly and can be highly useful for the
wastewater treatment contaminated with these carcinogenic synthetic dyes.
Key Words:
ZnO, Cu-Doped ZnO, Polyol method, Photo-catalysis, Reactive red S3B,
Introduction
Materials industry is one of the most essential industries that consumes large amount of water
and creates a lot of wastes containing numerous coloured substances.1 Dyeing and finishing
processes are the main source of pollution in wastewater.2 Synthetic dyes are extensively
utilized as a part of these procedures; in this way, their release into normal water causes
serious environmental issues.3
A large number of these dyes are carcinogenic, unsafe to human health and because of their
complex structures and synthetic nature, they are exceptionally stable and it is hard to
decolourize them by biological treatment approaches.4 At the point when the biological
treatment strategies can't treat polluted and harmful water, advanced oxidation processes
(AOPs) are one of the promising techniques to treat the polluted water. The principal
advantages of this process are its cost-effectiveness, the non-selective oxidation of substrates,
the possibility of using solar light and the fact that the catalyst is easy to obtain. Moreover,
the reactions can be carried out at room temperature and at atmospheric pressure under sun
light. Photodegradation of wastewater pollutants using solar light can make it an
economically feasible process in particular for large-scale aqueous-phase applications.5 In
AOP, the hydroxyl radicals (.OH) which are exceptionally stable and non-particular chemical
oxidants are produced in solution, and these are used for the oxidation of the natural effluents
to water and carbon dioxide.6
Various wide band gap semiconductors, for example, ZnS 7, SnO2 8, ZnO 9 and TiO2 10-11 have
been used as photocatalysts for this purpose. Usually, the mostly used catalyst has been TiO2
due to its activity below 390 nm, however in the last few years ZnO has attracted more
attention because of its high photocatalytic activity, cheap, and easily synthesised.11,12 ZnO
nanoparticles have been synthesized by hydrothermal13, co-precipitation14-15, sol-gel16,
evaporative decomposition of solution and gas-phase synthesis with various reagents.17 There
are only few reports in which poly (vinyl pyrrolidone) (PVP) was utilized as a capping agent
to prepare ZnO nanoparticles in various techniques.18-19 The polyol method is an
extraordinary type of solvothermal synthesis of ZnO which utilizes different diols as a
reaction medium. In addition to reaction medium it works as a stabilizing agent and confines
the particle growth. 20 The polyol method has the advantage of producing nanoparticles with
an organophilic surface layer that can be used as nanocomposites without any extra surface
modification. Polyvinylpyrrolidone (PVP), is an amorphous thermoplastic material with ideal
mechanical and handling properties, it replaces inorganic glass in numerous applications.21
ZnO nanoparticles in pure and doped forms have been utilized for removal of dyes such as
methyl blue (MB) 22, methyl orange (MO) 23 and Rhodamine 6G by photo-catalytic method. 24-27
The semiconductor ZnO is vastly used in photocatalysis in the disinfection and
detoxification of the environment due to its special physicochemical properties. However, its
large exciton binding energy (60 meV) and the wide bandgap (3.37 eV) restricts the response
to visible portion of solar radiation highlighting an important challenge. Another challenge to
be dealt with is the fast recombination of photo-generated electron–hole pairs. Therefore,
many reports were presented to increase the sensitivity of ZnO towards visible portion of
solar spectrum and decrease the rate of electron/hole recombination. ZnO doped with
transition metals improve the absorption of visible radiation from solar light. Also the doping
improves the separation of hole-electron pair resulting in higher photodegradation activity.28
The use of ZnO has some evident disadvantages including high recombination of
photo-generated electron-hole, the constricted light responsive range, and photo corrosion.
These restrictions have been overcome by different methods, for example, doping of ZnO and
coupling of semiconductor oxides.29-31 ZnO nanoparticles doped with Cu were found to be
more photochemically active due to their higher substrate and reagent binding ability. These
doped nanoparticles found their applications in reducing a large number of cancer-causing
dyes32 especially in print industrial effluents which are too carcinogenic, and toxic for aquatic
life.
Herein we report the synthesis of ZnO and Cu-doped ZnO nanoparticles by polyol method,
their full characterization and their use as photo-catalyst for the removal of carcinogenic dye
Reactive Red S3B (Figure 1).
Experimental
Materials
Copper nitrate trihydrate Cu(NO3)2.3H2O,Mw = 241.6 (Merck), zinc acetate dihydrate
Zn(CH3COO)2.2H2O, Mw = 219.5 (Merck), Poly (vinylpyrrolidone) PVP (Daejung Reagent
Chemicals-Korea), Ethylene glycol (EG) 99% (Daejung), and reactive red S3B used for
photocatalytic degradation was taken from native fabric dye industries and was used without
additional purification.
Apparatus
SHIMADZU UV 1800 Spectrophotometer was used to measure the UV-Vis absorption
spectra. The structures of the nanoparticles were characterized by FESEM TESCAN
MIRA3XMU Scanning Electron Microscope (SEM) together with EDX (JEOL, USA). The
crystal structures of as synthesized nanoparticles were studied by D8 ADVANCE XRD
(Bruker, Germany). The photocatalytic activities of pure and Cu-doped ZnO nanoparticles
were revealed against the removal of typical dye i.e.; reactive red solution in the presence and
absence of 1mL H2O2 and 0.1g nanocatalyst at ambient temperature after specific intervals.
Synthesis of nanoparticles
A characteristic polyol reduction method was used to synthesize ZnO nanoparticles. In this
method ethylene glycol was used as a solvent and reducing agent and PVP assumed the part
of capping agent. 20 mL of EG was preheated at 170 oC for half an hour with a steady
stirring in a 250 mL round bottom flask. After attaining the constant temperature, 15 mL
solution of PVP was added to the flask followed by the dropwise addition of Zn (acac) 2 with
constant stirring. The concentration of both the solutions was 0.1 M. The whole reaction
mixture was heated for four hours at 170 oC. After the complete of the reaction, the white
suspension was obtained, which was allowed to cool at room temperature and washed with
distilled water and ethanol to remove the unreacted reagents. The similar procedure was
repeated for the doping of copper by adding 2 mL of 0.01 M copper nitrate solution to dop
the ZnO nanoparticles.
Photocatalytic Activity Estimation
Aqueous solution of Reactive Red S3B was selected to check the photocatalytic activity of
pure ZnO and Cu-ZnO nanoparticles at ambient temperature.
In photocatalytic experiment, 0.10 g of ZnO or Cu doped ZnO was dispersed in 50 ppm
Reactive red S3B solution. The suspension was carefully mixed by magnetic stirring for 15
minutes to establish the adsorption-desorption equilibrium among the nanocatalyst, the dye
and water. This mixture was then subjected to visible light radiation. After every 10 minutes,
3 mL aliquot was taken out from the reaction mixture and was centrifuged for 10 min at 1000
rpm to separate the catalyst. The progress of the reaction was checked by calculating the
absorbance (A) of the purified filtrate solution at 542 nm (λmax) using UV-Vis
spectrophotometer (Shimadzu UV 2550). The photocatalytic degradation efficiency (%) was
estimated by using the following formula:
Decolorization Efficiency (%) = Co−Ct
Co x 100 (1)
Where C0 is the initial concentration of dye and Ct is the concentration of dye after photo
irradiation at different time intervals (expressed in mol/L).
Result and Discussion
In order to determine the transient energy levels of pure and Cu-doped ZnO nanoparticles
UV-Vis spectroscopy was carried out. Figure 2 shows an absorbance peak for ZnO
nanoparticle at 360 nm and for Cu-doped ZnO nanoparticles at 390 nm respectively. The 390
nm peak clearly shows the shift due to Cu-doping of ZnO. There was no evidence of the
presence of any Cu or CuO due the absence of any peak at 350 nm.33 The absence of any
metallic copper shows that copper is doped in the ZnO rather than an impurity.
Tauc relationship was applied to calculate the direct band gap of pure and Cu-doped ZnO
nanoparticles. With respect to the absorption spectra measured, (ᾳhυ)2 against hυ curves of
ZnO nanoparticles are revealed in Figure 3 (a, b). The values of band gap at about 3.03 and
2.7 eV were calculated for both ZnO and Cu-doped ZnO respectively. The doping of Cu in
ZnO showed a significant decrease in the band gap i.e. from 3.03 to 2.7 eV. The decrease in
band gap was also the strong mixing of p-d orbitals of O and Cu.
The photoluminescence (PL) spectra of ZnO and Cu-ZnO nanoparticles are presented in
figure 4. The intensity of the peaks is directly proportional to the rate of electron-hole
recombination. The ZnO exhibited UV emission peak at 349 and a broad emission band at
700 nm while the Cu doped ZnO showed emission peak at 379 nm and broad emission band
at 760 nm respectively which is a significant change. The UV emission is usually attributed
to the near-band-edge emissions of ZnO. The broad emission bands at about 700 nm and 760
nm are mostly attributed to the radiative recombination of a photo-generated hole with an
electron occupying the oxygen vacancy.34
Figure (5) shows an XRD pattern of ZnO and Cu-ZnO nanoparticles. The XRD
pattern of ZnO shows the reflection peaks at 2θ values of 31.82°, 34.33° ,36.49° and 47.56°
which correspond to (100), (002), (101) and (102) planes. These value match to the standard
value reported in the literature (ICPDS card No.36-1451). There was no noticeable shift in
the peaks when copper was doped in zinc oxide nanoparticles. A very intensity peak was
observed for copper in the copper doped zinc oxide which indicates that not all copper was
gone inside the crystal lattice of zinc oxide. The size of crystallites was determined by using
Debye’s Scherer’s formula.
Average crystallite size (D) = 0.9 λβcosθ (2)
Where λ is wavelength of X-ray used (0.15418nm), β is FWHM (101) plane and θ is the
diffraction angle. It is clear from the figure 4 that the average particle size was reduced from
11.51 to 6.36 nm. The broadening of the peaks in the XRD pattern of Cu-ZnO show the
smaller size of the nanoparticles in Cu-ZnO.35
Scanning electron microscopy shows the size, shape and general morphology of the
nanoparticles. The SEM images of ZnO (Figure 6a, b) nanoparticles show the spherical
shape of the crystallites with varying size. There are few larger particles with a diameter of
approx. 1µm dispersed in smaller spherical particles with diameter of around 200 nm. Figure
5 (a) and (b) show images with different magnifications. The SEM images of Cu-doped ZnO
(Figure 5c, d) show the non-uniform size distribution. Most of the smaller spherical particles
form clusters of different sizes and shapes which range from 1µm to 300 nm. Clear can be
observed by the ZnO and Cu.ZnO images e.g. there are no large size spherical particles
observed in Cu.ZnO as shown by ZnO images.
The elemental analysis of ZnO and Cu.ZnO nanoparticles were studied with EDX (Table 1).
EDX of ZnO showed the atomic ration of Zn and O as 55.64:44.36 which is close to 1:1 ratio
as expected despite the difficulty of measuring the oxygen with high accuracy. Cu.ZnO
sample showed the presence of 0.94 atomic percentage of Cu in ZnO which correspond to the
amount added i.e., 10% Cu in ZnO
Photodegradation studies
The UV/Vis spectra of Reactive red S 3B dye is represented in figure 7a. The degradation of
this dye was studied under four different experimental conditions viz. solar energy /ZnO,
solar energy /ZnO/H2O2, solar energy/Cu.ZnO and Dark/ZnO. The removal rate was
monitored by the change in intensity of UV/Vis peak at 542 nm for Reactive red S 3B dye.
Figure 6a shows the UV/Vis spectra of Reactive red S 3B dye solution. Initially the reaction
was started by illuminating the dye solution to sun light without the presence of any catalyst.
The UV/Vis measurements showed that the peak intensity decreased by 6.47% (Figure 7 b).
The adsorption of the dye over the photocatalyst was monitored under the four different
conditions mentioned earlier (solar energy /ZnO, solar energy /ZnO/H2O2, solar
energy/Cu.ZnO and Dark/ZnO) at fixed amount of dye solution (50 mg/L) and photocatalyst
loaded (0.1 g/L). The dye was exposed to daylight at a 10 minutes interval for 120 minutes to
check the degradation effect. It was observed that the absorption peak decreases slowly with
the decrease in the dye concentration and is shown in figure 7 (c, d, e, f). The gradual change
in absorption peak showed that the organic compound has been decomposed in the solution.
The percentage removal rate of the dye at different conditions are presented in the Figure 8.
The degradation efficiency is increased as the catalyst load was increased upto 0.1 g/L and
afterward it decreases gradually. The decrease in the rate of degradation with increase of
catalysts above 0.10 g/L may be because of the scattering of light and low penetration of light
through the dye solution. With a higher catalyst concentration, the activated molecules start
colliding with the ground state molecules and become deactivated, resulting in lowering the
rate of reaction. The percentage degradation of the dye using ZnO, Cu.ZnO, H2O2/ZnO in the
presence of light and ZnO in the dark was 79.68%, 88.98%, 79.04% and 26.24% respectively
and is shown in the figure 8.
Figure 9 shows the concentrations of the dye left after reacting with the photocatalysts.
Initially the concentration of pure dye was exposed to the sunlight without adding any
catalyst. It shows that there was no change in the absorption of the dye solution. So it was
labelled as the pure dye solution without any environmental effects. Similarly, when ZnO
was added to the dye but placed in the dark there was only 26.24% degradation of the dye.
However, when the dye solution was treated with H2O2, ZnO and Cu-doped nanoparticles
under sun light then a significant degradation was observed. It is cleared from the graph that
the rate of degradation was almost same (79.68%, 79.04%) with ZnO/H2O2 and ZnO exposed
to the light for 120 min. But the doped nanoparticles (Cu-ZnO) showed the most degradation
(88.98%) of the dye.
The kinetics of degradation of dye was roughly calculated. The kinetic model of the pseudo-
first-order model were applied to analyse the kinetics rate in the photodegradation process of
reactive red S3B onto ZnO and Cu.ZnO nanoparticles and are generally stated by the
following equation.
ln (CtCo
¿ = kt
Where k is the rate constant (min−1) and Ct and Co are the concentrations (mg/L) of dye at
various time intervals and initially used, respectively. The graph between ln (Ct/C0) and time
of reaction t gives a straight line which shows that the reaction follows a pseudo-first-order
kinetics behaviour.36-37 The results are shown in Figure 10.
The value of correlation coefficient (R2) was 0.9945, which specifies that the
photodegradation of dye satisfies the kinetic model. The rate constants of the dye in the
presence of ZnO, Cu.ZnO, in the dark and with H2O2/ZnO were 0.78, 0.68, 0.27 and 1.45
min−1, respectively. The ZnO (in the pure and doped forms) used in the photocatalytic
treatment was washed with distilled water and ethanol many times, dried at 70 °C in an oven
and it was reused further in the next photocatalytic experiments. It was observed that renewed
nanocatalysts have nearly the same efficiency for the dye degradation and can be used for
further photocatalytic decolourization of given dye solution.
Conclusion
Wurtzite ZnO and Cu-doped ZnO nanoparticles have been synthesized by polyol method
which is simple and easily scalable. These polyol nanoparticles are stable for periods of
several months at room temperature. Both ZnO and Cu-doped ZnO showed a good
photocatalytic activity against Reactive Red S3B, a carcinogenic dye. These non-toxic
nanoparticles are useful photocatalyst for the industrial effluents containing these types of
dyes and for the degradation of many other carcinogenic dyes which were used in print and
textile industry. We believe that the polyol method used to synthesise these materials is
highly effective to produce high quality products. The work on the degradation of other dyes
is under investigation and will be published elsewhere.
Acknowledgement
The author appreciatively acknowledges the financial support from the Higher Education
Commission (HEC) Pakistan and Office of Research Innovation and Commercialization
(ORIC), MUST, for the arrangement of funds required for the chemicals and samples
characterizations.
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Figures
Fig.1 Structure of Reactive red S3B
Fig. 2 UV-Visible spectra of ZnO and Cu-doped ZnO nanoparticles
IRVisibleUV
Fig. 3 Tauc plots showing the band gaps of (a) ZnO (b) Cu-Doped ZnO nanoparticles
(b)(a)
Fig.4 PL spectra of ZnO and Cu-ZnO nanoparticles
Fig.5 p-XRD pattern for (a) ZnO (b) Cu-ZnO nanoparticles
Fig. 6 SEM images of (a, b) ZnO and (c, d) copper doped ZnO nanoparticles at different magnifications.
(d)
1 µm
(c)
5 µm
(a)
5 µm 1 µm
(b)
(c)
(b)
(d)
(a)
(a)
Fig.7 UV-Vis absorbance spectra of (a) RR S3B solution (b) RRS3B solution exposure to
sun light without adding catalyst (c) In Dark, (d) RRS3B solution in the presence of ZnO (e)
RR S3B solution in the presence of Cu-ZnO, (f) RR S3B solution in presence of H2O2/ZnO.
(f)
(c)
(e)
(d)
(b)(a)
Fig. 8 Percentage degradation of (a) RR S3B solution in presence of H2O2/ZnO, (b) RR S3B
solution in the presence of Cu-ZnO, (c) RRS3B solution in the presence of ZnO, (d) RR S3B
dye in the presence of dark.
Fig. 9 Effect of catalysts on photocatalytic degradation of (a) RRS3B dye solution, (b) RR S3B solution in the dark, (c) RRS3B solution in the presence of ZnO, (d) RR S3B solution in presence of H2O2/ZnO, (e) ) RR S3B solution in the presence of Cu-ZnO (Conditions: Initial Dye concentration = 50 ppm, Catalyst Loaded = 0.1 g/L).
Fig. 10 Photocatalytic degradation kinetic curves for photocatalytic degradation of (a) RR S3B dye in the presence of dark, (b) RRS3B solution in the presence of ZnO, (c) RR S3B solution in the presence of Cu-ZnO, (d) RR S3B solution in presence of H 2O2/ZnO. (50 ppm initial concentration of solution, 0.1 g/L catalysts)
Table 1. EDX data for ZnO and Cu.ZnO nanoparticles
Materials Elements Weight% Atomic%
ZnO
O 23.49 55.64
Zn 76.51 44.36
Cu.ZnO
O 19.53 49.77
Zn 79.00 49.29
Cu 1.47 0.94