Low-cost flow photoreactor for degradation of Reactive Black 5 dye by UV/H₂O₂, Fenton and photo-Fenton processes: a performance comparison

Fotorreator contínuo de baixo custo para degradação do corante Reactive Black 5 pelos processos UV/H₂O₂, Fenton e foto-Fenton: uma comparação de performances

Abstract

In this work, a flow photoreactor was designed and set up using low-cost and recyclable parts to develop chemical treatments based on advanced oxidation processes (AOP) of highly colored textile wastewater. To evaluate this sustainable system´s efficiency, we investigated and compared the performance of three types of destructive methods (UV/H₂O₂, Fenton, and photo-Fenton) on the decolorization of aqueous solutions of Reactive Black 5 dye (RB5). We also analyzed the effect of the oxidant and dye concentrations on the rate of color removal in each one of the three methods. The results showed that, regardless of the initial operating conditions, the photo-Fenton process achieved the highest degradation rates, particularly when the highest ratio between the oxidant and dye concentrations was used ([H₂O₂]: [RB5] = 24.5 mg L^-1: 25 mg L^-1), leading to complete color removal within only 10 minutes of reaction. With the same initial condition, the Fenton and UV/H₂O₂ processes were also capable of removing the color entirely, even though they demanded more extended runs of 25 min. and 45 min., respectively. The effect of pH on the decolorization by the photo-Fenton process was also investigated, showing the same high performance at pHs 3 and 4. The degradation profile achieved by the photo-Fenton treatment was appropriately fitted by a pseudo-first-order kinetic. The non-expensive photoreactor proved to be quite useful for the degradation of the RB5, mainly when this azo dye underwent the photo-Fenton process.

Keywords:
advanced oxidation process; color removal; Reactive Black 5 dye; textile pollutants

Resumo

Neste trabalho, um fotorreator contínuo foi projetado e montado, usando peças recicláveis e de baixo custo, para desenvolver tratamentos químicos, baseados em processos oxidativos avançados (AOP), de efluentes têxteis altamente coloridos por azo-compostos. A fim de avaliar a eficiência deste sistema reacional sustentável, foi investigada a performance de três tratamentos destrutivos (UV/H₂O₂, Fenton e foto-Fenton) sobre a remoção de cor de soluções aquosas do corante denominado Reactive Black 5 (RB5). O efeito da concentração de oxidante (H₂O₂) e da carga inicial de corante sobre a taxa de remoção de cor foi também analisado. Os resultados mostraram que, independentemente das condições operacionais iniciais, o processo foto-Fenton alcançou as taxas mais elevadas de degradação, especialmente quando a maior razão entre as concentrações do oxidante e do corante foi empregada ([H₂O₂]: [RB5] = 24.5 mg L^-1: 25 mg L^-1), com a completa remoção de cor em apenas 10 minutos de experimento. Usando-se as mesmas condições iniciais, os processos Fenton e UV/H₂O₂ foram também capazes de descolorir completamente o poluente têxtil, entretanto precisando de 25 minutos e 45 minutos de reação, respectivamente. O efeito do pH sobre a descoloração pelo processo foto-Fenton foi também investigado, mostrando a mesma elevada performance nos pHs 3 e 4. O perfil de degradação obtido no tratamento foto-Fenton foi devidamente modelado pela cinética de pseudo-primeira ordem. O fotorreator contínuo de baixo custo mostrou-se bastante útil na degradação do corante RB5, principalmente quando o processo foto-Fenton foi empregado.

Palavras-chave:
corante Reactive Black 5; poluentes têxteis; processos oxidativos avançados; remoção de cor

1. INTRODUCTION

The textile industry is one of the essential socio-economic activities in Brazil. According to the Brazilian Association of the Textile Industry and Confection (ABIT), this type of sector accounts for more than 1 million tons of fabric annually, making this industrial segment stand out as the second-most important in respect of job generation nationwide.

Although this activity significantly contributes to wealth creation and social inclusion, inevitably, environmental impacts may be caused, especially when there is inappropriate disposal of the effluents from the fabric dyeing process. These effluents typically have a high organic load of synthetic dyes, particularly azo dyes, which combine high toxicity with low biodegradability (Bali and Karagözoglu, 2007; Liu et al., 2011; Silva et al., 2009). Azo dyes are molecules bearing the functional group diazenyl (R - N = N - R´), where R and R´ usually are aromatic groups, which makes them a highly conjugated and stable system. Figure 1 shows the structure of azo dye Reactive Black 5 (RB5 dye) studied in the present work.

Figure 1.
Structural formula of the Reactive Black 5 dye (RB5).

Therefore, to reduce potential impacts in the environment, the development and application of efficient techniques are crucial for removal or degradation of that type of dye from textile industry effluents.

Countless published studies have demonstrated promising aspects of advanced oxidation processes (AOP) for the degradation of organics pollutants (Fragoso et al., 2009; Guimarães et al., 2012; Vedrenne et al., 2012; Basturk et al., 2015; Abhilasha et al., 2016; Leite et al., 2016; Starling et al., 2017; Manaa et al., 2019; Mittersteiner et al., 2020). In that technique, the organic molecule undergoes successive oxidative breakings through a chain reaction initiated with highly reactive radicals, particularly the hydroxyl (·OH) and hydroperoxyl (·OOH). These radicals are promoted by the direct action of solar light or artificial source of UV radiation on the hydrogen peroxide (H₂O₂), a process known as UV-induced peroxidation (UV/H₂O₂). Another way to induce those radicals is to use iron ions (Fe²⁺, Fe³⁺) as initiating species, a process, in this case, known as Fenton. The following equations describe an overview of the reactions mentioned (Hsueh et al., 2005; Ioannou et al., 2015; Mofrad et al., 2015; Pouran et al., 2015; Gutierrez-Mata et al., 2017; Vorontsov, 2019).

H₂O₂ photolysis (Equation 1):

${\mathrm{H}}_2{\mathrm{O}}_2+\mathrm{h}\mathrm{\nu }\to \mathrm{}·\mathrm{O}\mathrm{H}\mathrm{}+\mathrm{}·\mathrm{O}\mathrm{H}$ (1)

Fenton Equations 2 and 3:

$\mathrm{F}{\mathrm{e}}^{2+}\mathrm{}+\mathrm{}{\mathrm{H}}_2{\mathrm{O}}_2\mathrm{}\to \mathrm{}\mathrm{F}{\mathrm{e}}^{3+}\mathrm{}+\mathrm{}\mathrm{O}{\mathrm{H}}^{-}+\mathrm{}·\mathrm{O}\mathrm{H}\mathrm{}\mathrm{}\mathrm{}\mathrm{}\mathrm{}\mathrm{}\mathrm{}\mathrm{}\mathrm{}{\mathrm{}\mathrm{k}}_1\mathrm{}=\mathrm{}76\mathrm{}\mathrm{M}{\mathrm{s}}^{-1}$ (2)

$\mathrm{F}{\mathrm{e}}^{3+}\mathrm{}+\mathrm{}{\mathrm{H}}_2{\mathrm{O}}_2\mathrm{}\to \mathrm{}\mathrm{F}{\mathrm{e}}^{2+}\mathrm{}+\mathrm{}·\mathrm{O}\mathrm{O}\mathrm{H}\mathrm{}+\mathrm{}{\mathrm{H}}^{+}\mathrm{}\mathrm{}\mathrm{}\mathrm{}\mathrm{}\mathrm{}\mathrm{}\mathrm{}\mathrm{}\mathrm{}\mathrm{}{\mathrm{k}}_2\mathrm{}=\mathrm{}0.001-0.01\mathrm{}\mathrm{M}{\mathrm{s}}^{-1}$ (3)

Upon comparing the reaction rate constants (k₁, k₂), it becomes evident that the Fe²⁺ ion is remarkably more active than the Fe³⁺ ion, as a radical promoter of the oxidation process, a fact that unexpectedly brings about a technical drawback. As can be seen in Equation 3, the Fe²⁺ ion is regenerated from the reduction of Fe³⁺ ion. Unfortunately, since k ₂ << k _1, the regeneration of the most active iron ion is much slower than its consumption rate, leading to a gradual reduction in the Fenton process efficiency over time. Additionally, the pH increase (Equation 2), along with the Fe³⁺ accumulation, might lead to coagulated ferric complexes (Neyens and Baeyens, 2003), which requires na extra solid-liquid separation step or a pH adjustment to the efluente treatment process.

Combination of UV irradiation and the Fenton process (photo-Fenton) is considered a promising alternative to the drawbacks aforementioned, since the radiation allows the direct photolysis of the H₂O₂, as well as na increase in the Fe²⁺ regeneration rates, according to Equation 4, enhancing the overall production rate of hydroxyl radicals.

$\mathrm{F}{\mathrm{e}}^{3+}\mathrm{}+\mathrm{}{\mathrm{H}}_2\mathrm{O}\mathrm{}+\mathrm{}\mathrm{h}\mathrm{\nu }\mathrm{}\to \mathrm{}\mathrm{F}{\mathrm{e}}^{2+}\mathrm{}+\mathrm{}·\mathrm{O}\mathrm{H}\mathrm{}+\mathrm{}{H}^{+}$ (4)

The high reactivity of the radicals from H₂O₂, especially the hydroxyl (·OH), turn them into non-selective and strong oxidants (Gligorovski et al., 2015; Miao et al., 2018), which considerably broadens the application spectrum of the Fenton process and photo-Fenton process. Thus, they are capable of efficiently degrading countless types of organic pollutants, such as pharmaceutical residues (Trovó et al., 2012; Dúran et al., 2013; Ahmed and Chiron, 2014), agricultural defensives (Farré et al., 2006; Zhang and Pagilla, 2010; Monteagudo et al., 2011) and the azo dyes themselves (Barka et al., 2010; Sun et al., 2013; Yu et al., 2010; Mehrdad et al., 2011; Khataee et al., 2016; Leite et al., 2016; Guo et al., 2018; Rubeena et al., 2018). Several of those applications highlight the photo-Fenton capability to obtain high mineralization rates of pollutants, according to Equation 5 (Sun et al., 2009; Idel-aouad et al., 2011; Guimarães et al., 2012; Monteagudo et al., 2014). This vital outcome significantly reduces the environmental impacts from the effluents with a high organic load.

$\mathrm{R}-\mathrm{H}\mathrm{}(\mathrm{o}\mathrm{r}\mathrm{g}.)\mathrm{}+\mathrm{}·\mathrm{O}\mathrm{H}\mathrm{}\to \mathrm{}{\mathrm{H}}_2\mathrm{O}\mathrm{}+·\mathrm{R}\mathrm{}\to \mathrm{}\mathrm{f}\mathrm{u}\mathrm{r}\mathrm{t}\mathrm{h}\mathrm{e}\mathrm{r}\mathrm{}\mathrm{o}\mathrm{x}\mathrm{i}\mathrm{d}\mathrm{a}\mathrm{t}\mathrm{i}\mathrm{o}\mathrm{n}\mathrm{}\to \mathrm{}\mathrm{C}{\mathrm{O}}_2\mathrm{}+\mathrm{}{\mathrm{H}}_2\mathrm{O}\mathrm{}+\mathrm{}\mathrm{m}\mathrm{i}\mathrm{n}\mathrm{e}\mathrm{r}\mathrm{a}\mathrm{l}\mathrm{i}\mathrm{z}\mathrm{a}\mathrm{t}\mathrm{i}\mathrm{o}\mathrm{n}\mathrm{}\mathrm{p}\mathrm{r}\mathrm{o}\mathrm{d}\mathrm{u}\mathrm{c}\mathrm{t}\mathrm{s}$ (5)

As the Fenton process is usually performed in mild conditions and needs simple and low-cost chemicals, it can lead to economically feasible industrial applications. According to the work of Starling et al. (2017), the processing cost is estimated somewhere between US$ 0.90 and 2.20 per cubic meter of treated effluent, including the energy costs.

However, it is essential to consider the usually high initial costs with the project and assembly of the reactor. In a global scenario of financial limitations, the first step to achieving an industrial system of effluent treatment that is technically and economically feasible consists of building a versatile and low-cost lab-scale apparatus to research the operating conditions that optimize the pollutant degradation.

In most reported studies, the AOP experiments have been developed in batch systems, usually by adapting glass beakers or Erlenmeyer flasks as reactors (Farré et al., 2006; Bali et al., 2007; Fragoso et al., 2009; Silva et al., 2009; Guimarães et al., 2012; Módenes et al., 2012; Khataee et al., 2016; Starling et al., 2017; Guo et al., 2018; Rubeena et al., 2018; Manaa et al., 2019; Mittersteiner et al., 2020;). Although this alternative is capable of providing essential data for the optimization of operating conditions, the batch reactor is rare when it comes to industrial applications, where processes with flowing streams are much more common. Thus, the advantage of employing a flow photo-reactor in lab experiments is undeniable, even with refluxing streams, since it allows not only an assessment on variables that directly affect the reaction rates but also the hydrodynamic conditions, which can speed up an industrial scale-up.

Hence, primarily focusing on a sustainable and cost-effective approach, the present study had as a first step the design and setup of a continuous annular photo-reactor, employing recyclable materials and adapting low-cost parts, available on the local market. With this reactional apparatus, experiments with three types of advanced oxidation process (UV/H₂O₂, Fenton and photo-Fenton) were carried out in order to compare their effectiveness of decolorizing RB5 dye solutions. Additionally, the chemical kinetics was studied, assessing the effect of the oxidant dosage and dye concentration on degradation rates.

2. MATERIAL AND METHODS

2.1. Chemicals

Reactive Black 5 (RB5, color index 20505, CAS number 17095-24-8) was used in this study as the model of azo textile dye without any further purification process. Its molecular formula is C₂₆H₂₁O₁₉N₅S₆Na₄, a molecular weight of 991,82 g mol^-1, maximum absorbance wavelength of 597 nm, and water solubility of 200 g L^-1 at 20^°C.

To make the Fenton´s reagent, hydrogen peroxide (H₂O₂, 30% m/m) was used as oxidant agent, purchased from Êxodo Científica (Brazil), and, as the source of ferrous ions (Fe²⁺), ferrous sulfate heptahydrate (FeSO₄.7H₂O, purity 99%) was acquired from Vetec (Brazil). For any pH adjustments, sulfuric acid (H₂SO₄) and sodium hydroxide (NaOH) was used as needed.

2.2. Photoreactor Setup

The experimental apparatus was almost entirely designed and constructed in our lab and basically consisted of an annular flow photoreactor (Figure 2, left). This reactor was set up by mounting a UV-C germicidal Hg-lamp (power 30 W) in the center of a cylindrical glass tube 1 m long, a configuration that left a total working volume of 334 mL. The glass tube was externally wrapped with an aluminum foil to prevent the technicians from being exposed to the harmful UV irradiation.

The bottom of two recyclable PET bottles (volume of 2 L each) was transversally cut off to turn them into reservoirs (Figure 2, right), one for the aqueous dye solution and the other one for cooling water. The cooling system is composed of two Liebig condensers with a series connection, working as heat exchangers to maintain temperature during the reaction.

Figure 2.
Annular flow photoreactor with the aluminum foil (left) and reservoirs for the dye solution and cooling water (right).

Two windshield washer pumps were purchased from a local auto parts store and adapted to the reservoir outlets to pump the dye solution through the photoreactor and the cooling water through the heat exchangers. A digital power supply (MedTec, Model PS-4000) was used to set the voltage and current appropriately to operate the pumps at a constant volumetric flow rate of 1.5 10^-5 m³ s^-1.

2.3. Advanced oxidation experiments: efficiency analysis

Before the AOP experiments themselves, various standard RB5 solutions (2 ,4, 10, 20, 50, 80, 100 and 150 mg L^-1) were prepared to build the calibration curve that depicts the relationship between the dye concentration and maximum absorbance of its chromophore group, which occurs at the wavelength of 547 nm. A UV-visible spectrophotometer (THERMOSCIENTIFIC, Model EVO 60) was used to measure the absorbances.

To evaluate the effectiveness of the photoreactor towards the color removal of the azo dye RB5, several assays of three types of homogeneous advanced oxidation process were performed: UV-induced peroxidation, Fenton and photo-Fenton process. Photolysis experiments without any oxidant agent were carried out as well.

For all the assays aforementioned, dye solutions 50 mg L^-1 were prepared by dissolving the RB5 in distilled water. The effect on the color removal of two different concentrations of the hydrogen peroxide (2.45 mg L^-1 and 24.50 mg L^-1) was analyzed. For the Fenton and photo-Fenton experiments, the ferrous sulfate heptahydrate 15.00 mg L^-1 was dissolved in the dye samples. Their pH was adjusted to 3, by using a solution of H₂SO₄ 0.50 mol L^-1 previously prepared, in order to avoid the coagulation of ferric ions (Fe³⁺) with the hydroxyl ions (Pignatello et al., 2006).

The UV-induced peroxidation (UV/H₂O₂) was performed at neutral pH. Each one of AOP runs was performed in the photoreactor, keeping the volumetric flow rate at 1.50 10^-5 m³ s^-1, with the UV-C lamp turned on, except for the Fenton process. Afterwards, all the samples were taken to the UV-visible spectrophotometer to read the absorbance at the characteristic wavelength (547 nm), then the final concentrations were obtained by using the calibration curve.

The efficiency of each treatment on color removal was calculated as follows (Equation 6), where C ₀ and C denote, respectively, the initial azo dye concentration and its concentration at a given time.

$Efficiency\left(\%\right)=\frac{(C_0-C)}{C_0}x100$ (6)

The AOP at the highest ratio [oxidant]:[RB5] that led to the most efficient color removal was chosen to investigate the residual hydrogen peroxide, by using permanganate titration in acidic medium (Tzanov et al., 2002). Moreover, the acidity effect on the dye degradation profile was evaluated at two different pHs, one slightly lower (pH=2) and the other higher (pH=4) than the value set for all experiments.

2.4. Kinetics analysis of AOPs

The kinetic profiles of the color removal were obtained for the Fenton, photo-Fenton, and UV/H₂O₂ processes, performing experiments with the following initial azo dye concentrations: 25, 50 and 100 mg L^-1.

For each run, the effluent reservoir was loaded with 1 L of the dye solution and enough oxidant solution to provide 24.5 mg of H₂O₂ ([H₂O₂] = 0.720 mM). Moreover, 15 mg FeSO₄.7H₂O was dissolved for the Fenton and photo-Fenton assays, corresponding to a concentration of 0.054 mM for the ferrous ion (Fe²⁺). The UV lamp and pumps were turned on simultaneously, allowing the dye solution to be exposed to the UV irradiation, except for the Fenton process, which takes place in a completely dark environment. During the reaction, effluent aliquots were collected from the reservoir, at predefined time intervals, then their absorbances were immediately measured by the UV-vis spectrophotometer.

The pseudo-first-order and pseudo-second-order kinetic models (Equations 7 and 8) were employed to check, through linear regression, which one better fits the actual degradation profiles of the dye over the reaction time. In Equations 7 and 8,C ₀ ,Candkdenote the initial concentration of the dye, its concentration at a given timet, and the apparent rate constant, respectively.

$Ln\left(\frac{C_0}{C}\right)=kt(pseudo-first-ordermodel)$ (7)

$\frac{1}{C}-\frac{1}{C_0}=kt(pseudo-second-ordermodel)$ (8)

3. RESULTS AND DISCUSSIONS

In this study, a low-cost annular photoreactor was built to develop and study several degradation processes of the RB5 azo dye. The efficiencies of four techniques were investigated (UV photolysis, UV/H₂O₂, Fenton, and photo-Fenton), using three initial concentrations of dye (25, 50, 100 mg L^-1). Two different dosages of H₂O₂ were used (2.45 mg L^-1 and 24.5 mg L^-1) to investigate the oxidant effect on the advanced oxidation processes. The kinetic modeling of the RB5 decolorization by Fenton and photo-Fenton treatments was also studied and reported.

3.1. Efficiency comparison between UV/H₂O₂ and photolysis

First, to bring up an overview on the role played by the presence of the oxidant on the degradation of the dye, the efficiency of the lone action of the UV irradiation (photolysis) was compared to the combination of UV with H₂O₂ (UV-induced peroxidation), performing the experiments with a specific set of initial concentrations ([RB5] = 50 mg L^-1, [H₂O₂] = 24.5 mg L^-1) at neutral pH.

As can be seen in Figure 3, after a long 90-min. run, the dye degradation by photolysis was quite low, roughly 22%, an expected result (Lizama et al., 2002; Elmorsi et al., 2010), since no oxidant nor catalyst was employed. The degradation rate notably improves with the H₂O₂, as this oxidant generates highly reactive radicals (·OH) under the action of UV photons. As a result, those species promote fast successive bond breakings, generating other intermediate radicals through a complex mechanism that can lead to the mineralization of most organic fragments (Shu and Chang, 2005; Elmorsi et al., 2010). Figure 3 shows the complete removal of the dye color by the UV/H₂O₂ process after the same 90-min. run. Although this time interval seems long, it is important to highlight that the UV/H₂O₂ process required approximately 30 min. to bleach more than 90% of the dye.

Figure 3.
Color removal of the RB5 dye by the UV photolysis and UV/H₂O₂. Initial concentrations: [RB5] = 50 mg L^-1, [H₂O₂] = 24.5 mg L^-1.

3.2. Efficiency of the advanced oxidation processes

The results of the three advanced oxidation processes on the decolorization of RB5 are depicted in Figure 4. The effect of the initial concentrations of dye and oxidant dosages on the degradation profile can also be analyzed. Upon a quick comparison between the three processes, it becomes evident, as expected, that the photo-Fenton turns out to be the most efficient and fastest on the color removal of RB5 in all initial operating conditions employed in this study.

The lowest oxidant dosage (2.45 mg L^-1) appears inadequate to bleach the dye dissolved completely in the studied solutions (25, 50, 100 mg L^-1). In this case, naturally, the best result occurs with the highest ratio [H₂O₂]:[RB5], where a maximum degradation of 79% is reached by the Fenton and photo-Fenton treatments, and 63% by UV/H₂O₂ process (Figure 4 (a)).

By observing all the graphics in Figure 4, the slope of the curves clearly demonstrates that the higher [H₂O₂]:[RB5] ratio, the higher degradation rate of the azo dye, regardless of the type of treatment used. The best scenario for the dye degradation emerges, as shown in Figure 5 (b), when the highest oxidant dosage (24.5 mg L^-1) and lowest dye concentration (25 mg L^-1) are used. With this initial set of concentrations, the most efficient treatment, photo-Fenton, was capable of a complete color removal after only 10 min. The dark Fenton and UV/H₂O₂ treatments were less efficient, requiring approximately 25-min. and 45-min. run, respectively, to bleach the solution entirely. Furthermore, higher dye loads make its degradation even lower, an outcome that can be explained by the shallow penetration of the UV photons into the solution with high intense color (Behnajady et al., 2004).

In each one of the graphics (Figure 4), a comparison between the three treatments demonstrated that the degradation promoted by the UV/H₂O₂ is clearly slower than the one achieved by the Fenton and photo-Fenton processes, which suggests that the ferrous ions play an essential role in the generation of H₂O₂-derived radicals. As expected, the highest degradation rate of the azo dye occurs when the ferrous ions are combined with the UV irradiation, since it increases the generation of those radicals (Neamtu et al., 2003).

Figure 4.
Decolorization profile of the RB5 dye by UV/H₂O₂, Fenton and photo-Fenton treatments with respect to initial dye concentration and oxidant dosage.

For comparison purposes, Table 1 presents an overview of the AOP performances on the dye color removal at some reaction times, using the highest oxidant dosage ([H₂O₂] = 24.5 mg L^-1).

Figure 5.
Kinetic profile of the RB5 degradation by the photo-Fenton treatment ([H₂O₂] = 24.5 mg L^-1, [RB5] = 25 mg L^-1). Pseudo-first-order fitting (left) and Pseudo-second-order fitting (right).

Table 1.
RB5 color removal by the UV/H₂O₂, Fenton and photo-Fenton processes using the initial oxidant dosage of 24.5 mg L^-1.

[RB5] (mg L-1)	Dye color removal (%)
	Reaction time (min)	UV/H2O2	Fenton process	Photo-Fenton process
25	5	47.2	92.2	98.7
	10	76.6	97.8	100
	30	98.8	99.8	100
50	5	39.4	81.1	92.4
	10	63.0	91.2
	30	92.5	98.0	99.2
100	5	30.5	68.8	77.2
	10	49.6	79.9	87.0
	30	83.0	90.4	92.7

The results described in some similar previous studies found in the literature can corroborate the promising aspects of the continuous photo-reactor developed in the presented work. For instance, Silva et al. (2009) carried out several photo-Fenton experiments to degrade the RB5 in a batch reactor, testing out, among other operational conditions, three different reaction times (40 min., 50 min., 60 min.). In the shortest run (40 min.), complete dye removal was only reached when the concentration ratio was [H₂O₂]:[RB5] = 150 mg L^-1:100 mg L^-1, slightly higher than the best concentration set used in our work ([H₂O₂]:[RB5] = 24.5 mg L^-1:25 mg L^-1). In another AOP work, now using a flow photo-reactor, Leite et al. (2016) developed studies of degradation of the dispersed red 1 (DR1) dye, also by the UV-Fenton process. In this work, a 45-min. run was required to reduce the dye concentration from 23 mg L^-1 to 0.4 mg L^-1 (98.2% removal) with a high oxidant concentration of 170 mg L^-1. In the Miao et al. (2018) study, a heterogeneous photo-Fenton system, with α-FeOOH as the catalyst, was used to study Orange II dye color removal. With the initial concentrations of the oxidant and dye set at 340 mg L^-1 and 70 mg L^-1, respectively, color removal of 99.7% was obtained in 30-min. reaction. In comparison to the instances above and other previous works (Barka et al., 2010; Belayachi et al., 2019), the results presented in Table 1 demonstrate more rapid dye degradation rates, particularly by the photo-Fenton process, despite using a lower ratio [oxidant]:[dye] than the ones set in those works. This comparison suggests that the continuous photo-reactor, set-up and used in our work, notably allowed an improvement in color removal efficiency and, thus, this low-cost apparatus can be considered as a promising alternative towards a feasible treatment of textile pollutants.

The results of the residual hydrogen peroxide for the best treatment (photo-Fenton) and ratio [H₂O₂]:[RB5] = 24.5 mg L^-1:25 mg L^-1 are presented in Table 2.

Table 2.
Residual hydrogen peroxide for the photo-Fenton process with ratio [H₂O₂]:[RB5] = 24.5 mg L^-1:25 mg L^-1.

Reaction time (min.)	[H2O2] (mg L-1)	Residual percentage
0	24.5	100.0
45	3.4	13.9
90	2.0	8.2

The residual concentration of hydrogen peroxide, higher than 10%, even after 45 min. of photo-Fenton reaction, indicates that a much lower oxidant dosage would have been needed if the only goal of the treatment was the RB5 color removal. Actually, it is well known that the color of a dye emerges from a structure based on the resonance of highly conjugated π-electrons, and, therefore, a simple cleavage of the azo bonds (- N = N -), turning the RB5 into smaller fragments, would cease this extended resonance and accomplish the effluent decolorization. However, besides the color removal, other issues are likewise crucial for appropriate effluent treatment, such as the aromatic chemicals´ degradation. The slight drop of the hydrogen peroxide concentration, from 3.4 mg L^-1 to 2.0 mg L^-1, between 45 min. and 90 min. of reaction, significantly later than the complete color removal (10 min.), demonstrates few oxidable organic compounds remained in the system after 45 min. However, further analysis should be essential to corroborate this outcome, such as total organic chemical (TOC) analysis.

3.3. Kinetic modelling

Graphics of- ln(C ₀ /C)and1/Cversus time were plotted, and their linearization coefficients (R ² ) were calculated to compare the ability of pseudo-first-order and pseudo-second-order kinetic models in fitting the experimental results of dye degradation. The most efficient operating condition, which was the photo-Fenton process with the highest ratio [H₂O₂]/[RB5] ([H₂O₂] = 24.5 mg L^-1; [RB5] = 25 mg L^-1), was chosen to analyze the kinetic modelling of the degradation profile. The temperature was kept constant at 20^oC.

As shown in Figure 5, the pseudo-first-order kinetic fits the RB5 degradation appropriately, which can be confirmed by its high linearization coefficient (R² = 0.98). The rate constant and half-life are shown in the Table 3 for this pseudo-first-order degradation. The same conclusion is reported by several other studies in the literature (Shuai et al., 2018; Manaa et al., 2019). On the other hand, the pseudo-second-order kinetic is remarkably inadequate to fit the experimental results (R² = 0.54).

Table 3.
Kinetic parameters of the pseudo-first-order modelling for the dye degradation by the photo-Fenton treatment ([H₂O₂] = 24.5 mg L^-1; [RB5] = 25 mg L^-1).

Parameter	Value
Rate constant (k)	0.76 min-1
Half-life (t1/2)	0.91 min

3.4. Effect of the initial pH

Three different acidic pHs (2, 3, and 4) were chosen to investigate its effect on color removal of the photo-Fenton treatment. Higher pHs can bring about the complexation of insoluble ferric hydroxides, which hinders the crucial reaction between ferrous ions (Fe²⁺) and H₂O₂. As a result, the concentration of hydroxyl radicals is reduced (Sun et al., 2009). Furthermore, this coagulation is likely to clog the pumps, which decreases the flow rate and eventually damages them. Figure 6 depicts the decolorization efficiency at 3 min., 5 min., and 10 min. of reaction for the three chosen pHs. All the experiments were carried out with the highest ratio [oxidant]:[RB5].

Figure 6.
Effect of initial pH on the color removal of RB5 by photo-Fenton process. [H₂O₂]:[RB5] = 24.5 mg L^-1: 25 mg L^-1.

The results showed that pH had an insignificant effect on the time required for complete color removal of RB5, which was nearly 10 min. of reaction in the three acidic conditions. The only notable effect of the pH on the decolorization arose within the first 3-min. reaction when the most acidic condition (pH=2) led to 86% efficiency. In contrast, the pHs of 3 and 4 led to higher decolorization degrees, 95% and 96%, respectively. After 5-min. reaction, the decolorization efficiency reached 94% in the most acidic condition, in this case slightly closer to the results at the other studied pHs (99%). Based on similar reported studies (Sun et al., 2009; Elmorsi et al., 2010; Liu et al., 2011), the pH that maximizes the degradation rates ranges between 3 and 4. Moreover, those studies demonstrated the dye degradation appears to slow at very low pHs. According to Xu et al. (2004), pH < 2.5 increases the concentration of the ferrous hexaaqua complex, [Fe(H₂O)₆]²⁺, which is less active than the [Fe(OH)(H₂O)₅]⁺ complex towards the hydroxyl radicals generation. Therefore, the overall oxidation is retarded.

3.5. EE/O analysis

In order to estimate the cost-effectiveness with electricity of our oxidative system towards RB5 color removal, the electrical energy per order (EE/O) was calculated for the UV/H₂O₂ and photo-Fenton processes, and the results are presented in Table 4. EE/O is defined as the electric energy required to degrade one order of magnitude of the textile pollutant in one cubic meter of effluent, and it can be calculated according to the following Equation 9 (Nikravesh et al., 2020).

$\frac{EE}{O}=\frac{P.t.1000}{60.V.log\left(\frac{C_0}{C}\right)}$ (9)

Where P is the power (kW) of UV lamp, V is the volume (L) of effluent, t is reaction time (min), C ₀ and C are initial and final concentrations of RB5.

Table 4.
EE/O for RB5 color removal by the UV/H₂O₂ and photo-Fenton processes ([H₂O₂] = 24.5 mg L^-1).

	EE/O (kWh m-3order-1)
[RB5] (mg L-1)	UV/H2O2	Photo-Fenton
25	7.5	1.0
50	13.5	2.0
100	21.0	7.5

As expected, the photo-Fenton process with the highest ratio [oxidant]:[RB5] stands out as the most effective treatment in the matter of energy cost, with the lowest EE/O of 1.0 kWh m^-3 order^-1. Additionally, Table 4 corroborates the crucial role played by ferrous ions on the degradation rates, since without them, in the UV/H₂O₂ treatment, the cost with electricity might be 7.5 times higher to achieve the same degradation degree, depending on the initial concentrations.

The EE/O was not reported for the experiments with the lowest oxidant dosage ([H₂O₂] = 2.45 mg L^-1), because with this initial condition, the processes were unable to reach 90% color removal within the total reaction time, as can be observed in Figure 4.

4. CONCLUSIONS

The presented work aimed to design and build a sustainable experimental apparatus for performing advanced oxidation processes (AOPs), adapting low-cost parts and recyclable materials. Several experiments were performed with this annular flow photo-reactor for color removal of dye RB5, using three types of AOP, namely UV-induced peroxidation, Fenton, and photo-Fenton process. The effect of the dye load and oxidant (H₂O₂) concentration on the degradation efficiency was evaluated. As expected, the combination of Fe²⁺ ions and UV photons to generate more hydroxyl radicals made the photo-Fenton process the most effective treatment, regardless of the set of initial concentrations. For instance, for the highest ratio [H₂O₂]:[RB5] (24.5 mg L^-1: 25 mg L^-1), the photo-Fenton was capable of bleaching entirely the dye solution within only 10 minutes, whereas the Fenton and UV/H₂O₂ processes required 25 min. and 45 min., respectively.

The pH study showed that the high decolorization efficiency by the photo-Fenton process was not impacted by switching the pH from 3 to 4. The most acidic condition (pH=2) slightly slowed down the degradation rate, although it can be considered high, with 86% of color removal achieved within only a 3 min. reaction. Naturally, from a cost-wise point of view, the pH of 4 should be chosen for further studies with photo-Fenton treatment, since closer pHs to neutral conditions allows lower acid-base consumption for appropriate treatment and disposal of the effluent.

It is crucial to point out that the lower the ratio [H₂O₂]:[RB5], the lower the degradation efficiency in all types of AOPs evaluated in this work. For the lowest ratio ([H₂O₂]:[RB5] = 2.45 mg L^-1: 100 mg L^-1), none of the treatments were capable of complete color removal. Even the photo-Fenton process only led to a degradation of roughly 47% after 45 minutes.

As long as the adequate oxidant concentration is set for a given pollutant load, those results demonstrated that the non-expensive photo-reactor, built in this work, proved to be a propitious system for textile effluent treatments. Especially when the photo-Fenton process is employed, notable decolorization rates were accomplished.

5. ACKNOWLEDGEMENTS

The authors would like to thank the Federal Institute for Education, Science and Technology (IFPE), Brazil, for financial support of this research.

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Publication Dates

• Publication in this collection
  31 May 2021
• Date of issue
  2021

History

• Received
  15 Dec 2020
• Accepted
  12 Apr 2021