# Efficiency Improvement of a Capacitive Deionization (CDI) System by Modifying 3D SWCNT/RVC Electrodes Using Microwave-Irradiated Graphene Oxide (mwGO) for Effective Desalination

Authors: Ali Aldalbahi; Mostafizur Rahaman; Mohammed Almoiqli; Al Yahya Meriey; Govindasami Periyasami
Journal: Journal of Nanomaterials
 (2020)

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## Abstract

This work is aimed at improving the electrosorption capacity of carbon nanotube/reticulated vitreous carbon- (CNT/RVC-) based 3D electrodes and decreasing the duration of electrosorption-desorption cycles by facilitating the ions’ adsorption and desorption on the electrode surface. This was achieved by preparing composites of microwave-irradiated graphene oxide (mwGO) with CNT. All composite materials were coated on RVC by the dip-coating method. The highest loading level was 50 mg. This is because it exhibited the maximum electrosorption capacity when tested in terms of geometric volume. The results showed that the 9-CNT/mwGO/RVC electrode exhibited 100% capacitive deionization (CDI) cyclic stability within its 1st five cycles. Moreover, 27.78% time was saved for one adsorption-desorption cycle using this electrode compared to the CNT/RVC electrode. In addition, the ion removal capacity of NaCl by the 9-CNT/mwGO/RVC electrode with respect to the mass of the electrode (3.82 mg/g) has increased by 18.27% compared to the CNT/RVC electrode (3.23 mg/g) when measured at the optimum conditions. In a complete desalination process, the water production per day for the 9-CNT/mwGO/RVC electrode was increased by 67.78% compared to the CNT/RVC electrode when measured within the same CDI cell using NaCl solution of concentration less than 1 mg/L. When considered volume of 1 m3, this optimum 9-CNT/mwGO/RVC electrode produces water 29,958 L per day. The highest electrosorption capacity, when measured experimentally at 500 mg/L NaCl feed concentration, was 10.84 mg/g for this optimum electrode, whereas Langmuir isotherm gave the theoretically calculated highest value as 16.59 mg/g. The results for the 9-CNT/mwGO/RVC composite electrode demonstrate that it can be an important electrode material for desalination in CDI technology.


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## Body

## 1. Introduction

The electrosorption capacity and stability of an electrode depend on its pore structure, surface area, and electrical conductivity of electrode [1–6]. These play a significant role in the improvement of electrical double-layer capacitance in a capacitive deionization (CDI) system. This could occur by a uniform distribution of macropores that provide better electrochemical accessibility and facilitates rapid and easy ion transport. Nowadays, carbon materials like carbon nanofiber (CNF), carbon nanotubes (CNTs), graphene, and reticulated vitreous carbon (RVC) are used as electrode materials in a CDI system [7–10]. Wang et al. have shown that the electrical conductivity of electrode materials plays a great role in the performance of a CDI system [6]. They prepared a monolithic composite electrode using reduced graphene oxide (rGO) and activated carbon nanofiber (aCNF) through an ultrasound-assisted electrospinning technique. The electrosorption capacity of desalination was recorded for the NaCl solution as 9.2 mg/g, which was governed by the formation of an electrical double layer and can be further improved by increasing the electrical conductivity of the electrode.CNTs were accidentally discovered in 1991 by a Japanese scientist, Iijima, using an arc-discharge process [11]. Individual CNT can be either conducting or semiconducting, depending on the CNT structure [12]. Several physical properties of CNTs are of particular importance for the CDI application that is electrical conductivity, thermal conductivity, surface area, and mechanical strength. CNTs are one of the strongest materials in the world with elastic modulus reaching to 1 terapascal (TPa) and strength between 50 and 100 gigapascal (GPa) [13]. These extraordinary mechanical properties make them theoretically at least 100 times stronger and 5 times lighter than an equivalent weight of the strongest steel. CNTs have also demonstrated high thermal conductivity compared to other high thermally conductive materials such as copper [14]. Kwon and Kim predicted that the thermal conductivity can reach up to 6600 W/mK [15]. CNT shells can be either metallic or semiconducting in nature, depending on their chirality and their conformation. The CNTs could replace copper wire for electricity transport because its electrical conductivity is higher than copper [16]. The above characteristics make CNTs an ideal case for real-world applications including electrical field emission, conductive and mechanically reinforced plastics, energy storage, field-effect transistors, flexible transparent electrodes, solar cells, medical applications, water desalination, and capacitive deionization [12, 17–27]. The application of CNT membranes has impacted in the area of water technology development with their ultrahigh water flux and low biofouling potential.Graphene has recently been attracted huge attention among the scientific communities because of its unique characteristics like large theoretical specific surface area (2630 m2/g), high intrinsic mobility (200,000 cm2/vs) [28, 29], high tensile modulus (1 TPa) [30], good thermal conductivity (∼5000 W/mK) [31], high optical transmittance (97.7%), and high electrical conductivity [32, 33]. Various applications of graphene have been reported such as a catalytic electrode in fuel cell [34], transparent electrode in solar cell [35], supercapacitors [36], electrode in sensors [37], and transistors [38].The most common approach to graphite exfoliation is the use of strong oxidizing agents to produce graphene oxide. The first production of graphene oxide was demonstrated by Oxford chemist Brodie in 1859, who added a portion of potassium chlorate (KClO3) to a slurry of graphite in fuming nitric acid (HNO3) [39]. Later in 1898, Staudenmaier improved Brodie’s technique by using concentrated sulphuric acid (H2SO4) as well as fuming nitric acid and adding the potassium chlorate solution after certain intervals of time during the course of reaction [40]. This small change in the procedure made the production of highly oxidized GO within roughly a week. In the 1950s, Hummers and Offeman reported a method, which is most commonly used today with its minor modification for GO production that could be done within roughly 2 h and at lower temperatures [41]. In this approach, the graphite is oxidized by treating with a mixture of potassium permanganate (KMnO4) and sodium nitrate (NaNO3) in concentrated H2SO4. Hydrogen peroxide (H2O2) is then added to decompose excess permanganate ions, which can act as contaminants in the form of manganese ions Mn4+ [42, 43]. It should be noted that all previous procedures produce hazards due to the formation of toxic NO2, N2O4, and/or ClO2 gas. Luo et al. demonstrated that the preexfoliation of graphite via microwave heating helped to remove intercalated species and improved oxygen absorption in subsequent Hummers processing [44]. In 2010, Marcano et al. [45] described an alternative approach to produce graphene oxide that has significant advantages over the Hummers method, with the improved efficiency of the oxidation process and no toxic gas produced during the chemical reactions. The protocol for running this reaction was the exclusion of using sodium nitrate (NaNO3), increasing the amount of potassium permanganate (KMnO4) and performing the reaction at 9 : 1 mixture of H2SO4/H3PO4. Microwave irradiation is also a powerful technique to reduce graphite oxide for getting reduced graphene oxide (rGO). Hu et al. have studied the effect of microwave irradiation on graphite oxide (GO) [46]. They have reported that the increase in oxygen content in GO decreases the activity of radiation absorption because of the reduction of the size of π-π bonding. Hence, the reduction of GO to rGO becomes less effective. The reduction of GO starts from the unoxidized part of GO. As a result, graphene was more sensitive to microwave radiation compared to GO. It was observed that a small amount addition of graphene with GO leads to greater absorption of radiation and increases the deoxygenation process. In another study, microwave-irradiated graphene aerogel was prepared from GO, which was very low in density and highly compressible in nature [47].Graphene has become one of the most attractive subjects due to its several breakthroughs in fundamental research and some promising practical applications [42, 48–55]. The interlayer spacing in a graphene oxide electrode (more than 0.625 nm) allows the hydrated Na+ ion, which has a radius of 0.358 nm, to enter into the electrodes [45]. The abovementioned attractive properties of graphene make it feasible as electrode materials for the CDI system. Li et al. have pioneered the application of graphene as an electrosorption electrode material for the CDI system in 2009 [56]. The graphene was fabricated by the modified Hummers method followed by a hydrazine reduction process and was employed as the electrode for an electrosorption application. Batch-mode electrosorption experiments with good repeatability in NaCl solutions were conducted where high ion removal efficiency was achieved at high applied voltage 2.0 V and volume flow rate 40 mL/min. The result showed that the graphene exhibited high specific electrosorption capacities of 1.85 mg/g and 22.04 mg/g using feed concentrations of 22.5 mg/L and 490 mg/L, respectively. In 2012, Li et al. have used reduced graphene oxide (rGO) nanoflakes to enhance the specific capacitance of activated carbon (AC) [57] and carbon nanotubes (CNTs) [58]. It was synthesized using 10 wt% graphene by a facile chemical synthesis method. The best electrochemical performance of this composite electrode gave a specific capacitance of 311 F/g, which is much higher than the CNT electrode (202 F/g) in the 1 M NaCl solution at a scan rate of 10 mV/s. The electrosorption capacity of composite and CNT electrodes using the 25 mg/L NaCl solution was nearly the same: 0.88 and 0.87 mg/g, respectively. The conditions used were 1.6 V and 25 mL/min volume flow rate, but the time of electrode saturation in a single adsorption cycle decreased to half in the composite electrode compared to the CNT electrode, which took around 1 hour. In 2013, Wimalasiri and Zou made graphene electrodes for CDI using the modified Hummers method as stated by Marcano et al. [45] and then 9 wt% of SWCNT was combined with GO nanosheets, not only to increase the interlayer distance but also to contribute to the overall surface area and conductivity of the active material [59]. The specific surface area of graphene and the CNT/rGO composite was 362 and 391 m2/g, respectively, and the mean pore diameter of graphene increased from 4.38 nm to 5.0 nm of the CNT/rGO composite. Moreover, the specific capacitance of the CNT/GO composite was increased from 140 F/g to 220 F/g for the graphene electrode when measured at a 5 mV/s scan rate using the 1 M NaCl solution. Furthermore, the electrosorption capacity of the CNT/rGO composite was 26.42 mg/g, which was comparatively higher than graphene (22.27 mg/g) when measured using the NaCl solution at the initial concentration 780 mg/L, volume flow rate 25 mL/min, and cell voltage 2.0 V. In addition, the CNT/rGO composite-based electrodes demonstrated considerably faster salt adsorption and desorption cycles within an average of 62 min compared to graphene-based electrodes, which required 112 min, for a single adsorption and desorption cycle.In this study, our aim is to prepare 3D electrode materials based on acid-functionalized single-walled carbon nanotubes (a-SWCNT) and mwGO using RVC as a substrate and check their performance in a CDI system using a feed stream flowing directly through the electrodes. The performance of the electrodes was tested at different working conditions like flow rate and bias potential, which were optimized. Furthermore, the electrosorption isotherms like Langmuir and Freundlich models were investigated to describe how ions interact with electrodes. The performance of electrodes was evaluated through the electrosorption dynamic study. All the characteristics are very important to develop electrode materials for using effectively in desalination technology.


## 2. Materials, Methods, and Characterizations

### 2.1. Materials

The commercial SWCNT (Hipco-CCNI/Lot # p1001) and graphite powder were supplied by Carbon Nanotechnologies, Inc. (Houston, TX) and Bay Carbon, Inc., respectively, and those were used as received. The chemicals DMF, HNO3 (70%), KMnO4, C2H5OH, and NaCl were procured from Sigma-Aldrich. In addition, the chemicals like H2SO4 (98%, w/v), H2O2 (30% aqueous), and HCl (36%, w/v) were purchased from Univar. All these chemicals were analytical reagent (AR) grade and were also used as received. The RVC (compressed 60 ppi (pores per inch)) was procured from ERG Materials and Aerospace Engineering Limited. The membrane filters (0.2 μm pore size GTTP) were supplied by Millipore. Milli-Q water, having electrical resistivity 18.2 mΩ/cm, was used in all preparation methods.


### 2.2. Methods

In this study, the SWCNT was functionalized by treating with nitric acid (a-SWCNT) and graphene oxide (GO) was synthesized by the modified Hummers method as described by Marcano et al. [45]. The GO was exfoliated and reduced by the microwave irradiation (mwGO) technique [60]. Both the mwGO and a-SWCNT were dispersed in DMF and then mixed together to prepare the a-SWCNT/mwGO composite coating solutions at different weight ratios. The a-SWCNT, mwGO, and prepared a-SWCNT/mwGO composites were dip coated on an optimized RVC substrate to prepare different electrodes. Pretreatment of RVC was done with nitric acid to remove any traces of impurity from its surface before dip coating. The details of these processes are given in the Supplementary section from S1 to S8.


### 2.3. Characterizations

The electrochemical characterizations of base materials and their composite electrodes were performed by cyclic voltammetry (CV). The measurement was done using the three-electrode system setup. The a-SWCNT/RVC, mwGO/RVC, or a-SWCNT/mwGO/RVC acted as the working electrode (WE) in the 1 M NaCl aqueous solution over the voltage range -0.2-1.0 V; RVC electrode and Ag/AgCl (3 M NaCl) acted as the counter electrode (CE) and reference electrode (RE), respectively. For the CDI characterization, Pt electrode was used as a CE to avoid any chance of limiting the performance of the other composite electrodes. The measurement was performed at the scan rate of 5, 10, 20, 50, 100, and 200 mV/s. A platinum wire was used to make contact between WE and CE.The desalination experiments were performed within a flow-through electrode system using a capacitive deionization (CDI) cell. In this measurement, the total volume and concentration of the NaCl solution were 70 mL and 75 mg/L, respectively. The distance between electrodes was 5 mm, and the solution temperature was maintained at 293 K. The total desalination processes, which involve the measuring of the amount of ion removal from the NaCl aqueous solution, the construction of a capacitive deionization (CDI) cell, measuring the effect of flow rate and voltage on ion removal efficiency, and the calculation of electrosorption capacity, are described within supplementary sectionsS9-S12.


## 2.1. Materials

The commercial SWCNT (Hipco-CCNI/Lot # p1001) and graphite powder were supplied by Carbon Nanotechnologies, Inc. (Houston, TX) and Bay Carbon, Inc., respectively, and those were used as received. The chemicals DMF, HNO3 (70%), KMnO4, C2H5OH, and NaCl were procured from Sigma-Aldrich. In addition, the chemicals like H2SO4 (98%, w/v), H2O2 (30% aqueous), and HCl (36%, w/v) were purchased from Univar. All these chemicals were analytical reagent (AR) grade and were also used as received. The RVC (compressed 60 ppi (pores per inch)) was procured from ERG Materials and Aerospace Engineering Limited. The membrane filters (0.2 μm pore size GTTP) were supplied by Millipore. Milli-Q water, having electrical resistivity 18.2 mΩ/cm, was used in all preparation methods.


## 2.2. Methods

In this study, the SWCNT was functionalized by treating with nitric acid (a-SWCNT) and graphene oxide (GO) was synthesized by the modified Hummers method as described by Marcano et al. [45]. The GO was exfoliated and reduced by the microwave irradiation (mwGO) technique [60]. Both the mwGO and a-SWCNT were dispersed in DMF and then mixed together to prepare the a-SWCNT/mwGO composite coating solutions at different weight ratios. The a-SWCNT, mwGO, and prepared a-SWCNT/mwGO composites were dip coated on an optimized RVC substrate to prepare different electrodes. Pretreatment of RVC was done with nitric acid to remove any traces of impurity from its surface before dip coating. The details of these processes are given in the Supplementary section from S1 to S8.


## 2.3. Characterizations

The electrochemical characterizations of base materials and their composite electrodes were performed by cyclic voltammetry (CV). The measurement was done using the three-electrode system setup. The a-SWCNT/RVC, mwGO/RVC, or a-SWCNT/mwGO/RVC acted as the working electrode (WE) in the 1 M NaCl aqueous solution over the voltage range -0.2-1.0 V; RVC electrode and Ag/AgCl (3 M NaCl) acted as the counter electrode (CE) and reference electrode (RE), respectively. For the CDI characterization, Pt electrode was used as a CE to avoid any chance of limiting the performance of the other composite electrodes. The measurement was performed at the scan rate of 5, 10, 20, 50, 100, and 200 mV/s. A platinum wire was used to make contact between WE and CE.The desalination experiments were performed within a flow-through electrode system using a capacitive deionization (CDI) cell. In this measurement, the total volume and concentration of the NaCl solution were 70 mL and 75 mg/L, respectively. The distance between electrodes was 5 mm, and the solution temperature was maintained at 293 K. The total desalination processes, which involve the measuring of the amount of ion removal from the NaCl aqueous solution, the construction of a capacitive deionization (CDI) cell, measuring the effect of flow rate and voltage on ion removal efficiency, and the calculation of electrosorption capacity, are described within supplementary sectionsS9-S12.


## 3. Results and Discussion

### 3.1. Adsorption Performance of the 9-CNT/mwGO-Coated RVC Electrode

The adsorption performance test was carried out at the optimum applied voltage 1.5 V (in this study, the ferricyanide solution was used to test the 3 electrode system. We observed the oxidation peak shift to 0.59 V, where the ideal oxidation peak was 0.29 V. Hence, the maximum/optimum applied voltage for our CDI system was 1.5 V.) and optimum flow rate 50 mL/min, as reported in our previous study for the CNT/RVC electrode [61, 62]. These conditions were used in further studies to compare the desalination performance of a range of electrodes with different amounts of 9-CNT/mwGO composite materials coated on the RVC electrode. All experiments were performed by keeping the total volume of the NaCl solution at 70 mL and the initial feed concentration at 75 mg/L (143 μS/cm). Figure 1(a) shows the CDI process for all loading level composites at the geometric volume 2.16 cm3 of the RVC electrode: 10, 30, and 50 mg loadings. There is a drop in the conductivity of the test saline solution with increasing amounts of material on the electrode because ions were attracted by the oppositely charged electrodes when an electric field was applied [63]. A better electrosorption performance was achieved at 50 mg coated RVC electrode where the conductivity was significantly dropped by approximately 5.21 μS/cm in the electrosorption process. Figure 1(b) shows the electrosorption of various 9-CNT/mwGO/RVC electrodes in terms of the mass of 9-CNT/mwGO and the volume of electrode (calculated as per supplementary section S12). It is evident from the figure that the electrosorption capacity was decreased with the increase in weight of composite material. It is clear that when the RVC electrode was loaded with 10 mg of composite, the electrosorption capacity was 9.91 mg/g and when the same electrode was loaded with 50 mg of composite, the electrosorption capacity became 3.82 mg/g. On the contrary, the electrosorption capacity of electrodes in terms of geometric volume was increased with the increase in amount of composite material. The calculation showed that when the RVC electrode was separately loaded with 10 mg and 50 mg of composites, the electrosorption capacities were 0.05 mg/cm3 and 0.09 mg/cm3, respectively. This result leads to the generalization that the electrosorption capacity increases with increasing amounts of material on the electrode.Figure 1
(a) Adsorption behaviour and (b) the electrosorption capacity in terms of the mass of composite material loading and the geometric volume of the electrode of various 9-CNT/mwGO/RVC electrodes. Loadings (mg): 10, 30, and 50.
(a)(b)


### 3.2. Optimization of Conditions for Ion Removal Efficiency

This study is based on the 50 mg 9-CNT/mwGO composite-coated RVC electrode because it showed the highest electrosorption capacity in terms of geometric volume. The optimization was carried out for electrical voltage and flow rate. The investigated cell voltages were 1.3 V and 1.5 V, and the flow rates were 25 mL/min, 50 mL/min, and 75 mL/min as shown in Figures2(a) and 2(b). Cell voltages above 1.5 V were not investigated because saving energy is one of our targets. Figure 2(a) represents the variation solution conductivity with respect to time at two different voltages. It was observed that with the increase in applied voltage, the ion removal amount was also increased. Hence, higher ion removal was achieved at 1.5 V. Figure 2(b) shows that the highest variation in solution conductivity was observed at a 50 mL/min flow rate, which indicated the highest electrosorption capacity. This is because a low pump rate would result in an obvious coion effect, which will suppress the electrosorption process, while a high pump rate will introduce a high pump force that is greater than that of electrosorption force and therefore decrease the electrosorption amount [64]. Thus, the optimized cell voltage and flow rate for the CDI process were found to be 1.5 V and 50 mL/min, respectively.Figure 2
Conductivity variations of the NaCl solution with various (a) applied voltages and (b) applied flow rates, with respect to operating time, using the 9-CNT/mwGO/RVC electrode loaded with 50 mg composite material.
(a)(b)


### 3.3. Capacitive Deionization (CDI) System

#### 3.3.1. Adsorption/Desorption Performance of the CNT/mwGO/RVC Electrodes

The CDI system was investigated with respect to the influence of increasing ratios of mwGO in the CNT/mwGO composite material-coated RVC electrodes on the ion removal performance. The ratio levels were 10 : 0, 9 : 1, 8 : 2, and 7 : 3 CNT : mwGO, respectively, and the mass of materials coated on all RVC electrodes was 50 mg. All experiments were performed with the same previous conditions at 1.5 V and 50 mL/min flow rate with 6 min adsorption processes. Figure3(a) shows the CDI process for all composite-coated RVC electrodes. As expected, once the electrical voltage was applied, the solution conductivity dramatically decreased for all electrodes because ions were attracted by opposite charges on the electrodes [63]. Then, the conductivity would gradually approach a constant minimum level, indicating that saturation was achieved [58]. During the discharging of the CDI system under 0 V of applied voltage, the solution conductivity was returned to approximate its initial value (143 μS/cm), meaning that the ions were released from the double layer region back into the solution because of the disappearance of electrostatic forces. It is clear that the highest drop in conductivity was around 5.2 μS/cm using the 9-CNT/mwGO/RVC electrode. The second-largest drop in conductivity was around 4.8 μS/cm using the 8-CNT/mwGO/RVC electrode. The drop in conductivity for the CNT/RVC electrode was higher than that of the 7-CNT/mwGO/RVC electrode. It is notable that the 9-CNT/mwGO/RVC electrode’s saturation was achieved after 5 min, whereas the CNT/RVC electrode saturation was achieved after 6 min. It is also interesting to note that the regeneration by discharging the CDI cells was completed, at 0 V, after 13 min for the electrode with the least amount of the mwGO ratio in the sample that is 9-CNT/mwGO/RVC. However, for the CNT/RVC electrode, the required time for one electrosorption-desorption process was 18 min. Hence, there was 27.78% saving of time in one desalination cycle for the 9-CNT/mwGO/RVC electrode compared to the CNT/RVC electrode [61]. Moreover, the electrosorption capacities in terms of mass of electrode for 9-CNT/mwGO/RVC and CNT/RVC electrodes were 3.82 mg/g and 3.23 mg/g, respectively. Thus, there was an 18.27% increment in the electrosorption removal performance for the 9-CNT/mwGO/RVC electrode compared to the CNT/RVC electrode. This improvement in electrosorption amount in the 9-CNT/mwGO/RVC electrode can be attributed to many complicated factors: these included the increasing specific surface area, specific capacitance, more accessible interlayer, pore microstructure, and pore size distribution which can play important roles in affecting the electrosorption capacity [58, 59, 65].Figure 3
(a) Adsorption and release behaviour and (b) the electrosorption capacity in terms of mass of CNT/mwGO and the geometric volume of electrode of various ratios 10, 9, 8, and 7 CNT in CNT/mwGO/RVC electrodes.
(a)(b)Figure3(b) shows the electrosorption performances of all electrodes which were measured from the data in Figure 3(a). The variation of the solution conductivity was monitored instantly by a multifunction conductivity meter. Accordingly, the correlation of conductivity (μS/cm) with concentration (mg/L) was calibrated prior to experiments (shown in supplementary section S9). Furthermore, the 8-CNT/mwGO/RVC electrode also afforded better CDI system performance than the a-SWCNT/RVC electrode, as evidenced by time saving of the 11.11% and 8.98% better electrosorption removal of NaCl. Table 1 also represents the detailed electrosorption in terms of mass, area, and volume for each composite electrode (calculated as per supplementary section S12). It is clear that the electrosorption behaviours of all composite electrodes in terms of area and in terms of volume followed the electrosorption behaviours of composite electrodes in terms of mass of electrode because all the parameters were held constant: mass of material, electrode area, and volume. These results suggested that the CDI process, using the 9-CNT/mwGO/RVC electrode, was promising as an effective technology for desalination.Table 1
Electrosorption of NaCl by the CNT/mwGO/RVC electrodes with various ratios of CNT and time of one desalination cycle (∗comparing with the CNT/RVC electrode).
Ratio of a-SWCNT in electrodesElectrosorption∗Enhancement percentage in electrosorptionTime of one desalination cyclemg/gmg/cm2mg/cm3%min73.018.4E−030.071783.529.9E−030.098.981693.821.1E−020.1018.2713103.239.4E−030.0818


#### 3.3.2. Electrosorption Dynamics

The performance of electrode adsorptions is evaluated by dynamics study, which describes the solute uptake rate, and evidently, this rate controls the residence time of adsorptive uptake at the solid-solution interface [66, 67]. However, this section will investigate the controlling mechanism of electrosorption and the constants of sorption of pseudo-first-order kinetics as proposed by Lagergren [68], where the conformity between experimental data and the model’s predicted values is expressed by the correlation coefficients (r2, values close or equal to 1). The electrosorption dynamic and pseudo-first-order dynamic models for the NaCl adsorption onto CNT/RVC, 9-CNT/mwGO/RVC, 8-CNT/mwGO/RVC, and 7-CNT/mwGO/RVC electrodes at voltage 1.5 V, flow rate 50 mL/min, and constant temperature 298 K are presented in Figure 4. The composite electrodes (except 9-CNT/mwGO/RVC) exhibited steady increment in electrosorption within the first minute, then it became dynamic adsorption, and after three minutes, the electrode gradually approached saturation as shown in Figures 4(a), 4(b), and 4(d). The time required to reach the adsorption equilibrium was 6 minutes. However, the electrosorption of NaCl onto the 9-CNT/mwGO/RVC electrode was very rapid within the first half minute. This could be because the external surface area of bundled CNT in this electrode is higher than other electrodes, thus increasing the possibility of ions to reach the surface easily. After that, the electrosorption of NaCl onto this electrode becomes dynamic adsorption for four minutes and then followed by the electrode saturation as shown in Figure 4(c). The time required to reach adsorption equilibrium was 5 minutes, which may be due to the higher rate of diffusion of ions onto the electrode particle surface.Figure 4
(a–d) Electrosorption and (e–h) pseudo-first-order adsorption kinetics of the NaCl electrosorption onto CNT/RVC, 9-CNT/mwGO/RVC, 8-CNT/mwGO/RVC, and 7-CNT/mwGO/RVC electrodes, respectively, at 1.5 V and 50 mL/min flow rate. Results have been derived from Figure 5.15 (a) (adsorption process).The pseudo-first-order kinetics for all electrodes was studied within the first four minutes as shown in Figures4(e)–4(g) and 4(d), respectively. To evaluate the kinetics of the electrosorption process, the pseudo-first-order model was tested to interpret the experimental data. The pseudo-first-order equation has been expressed in Supplementary section S13. The slopes and intercepts of plots of log (qe–qt) versus t were used to determine the first-order rate constant k1. In all electrodes, methods that are based on the linearization of the models and correlation coefficients (r2) of around 0.99 confirm that all electrodes followed pseudo-first-order dynamics. Similar trends were reported in the literature for the adsorption of NaCl ions from aqueous solutions by other adsorbents [56, 64, 69–73]. A comparison of the rate constant k1 with the correlation coefficients is shown in Table 2. The rate constant (k1) of the pseudo-first-order kinetics was 0.816, 0.525, 0.555, and 0.639 min-1 for CNT/RVC, 9-CNT/mwGO/RVC, 8-CNT/mwGO/RVC, and 7-CNT/mwGO/RVC electrodes, respectively. Hence, it is clear that there is an inverse relationship between the rate constant and electrosorption; when the electrosorption capacity is increased, the rate constant is decreased. Also, the theoretical qe values found from the pseudo-first-order kinetics model gave reasonable values (3.19, 3.66, 3.45, and 2.75 mg/g for CNT/RVC, 9-CNT/mwGO/RVC, 8-CNT/mwGO/RVC, and 7-CNT/mwGO/RVC electrodes, respectively).Table 2
The comparison between the adsorption rate constant (k1) and correlation coefficients of pseudo-first-order kinetics and the estimated theoretical and experimental (qe) maximum electrosorption with the pseudo-first-order model.
a-SWCNT : mwGOR2K1 (min-1)Theoreticalqe (mg/g)Experimentalqe (mg/g)7 : 30.9900.6392.753.018 : 20.9870.5553.453.529 : 10.9920.5253.663.8210 : 00.9940.8163.193.23


#### 3.3.3. CDI Cycling Stability

The regeneration of electrodes plays a significant role in their commercialization for using in CDI systems. To test reversibility, the 9-CNT/mwGO/RVC electrode was selected because it had the highest electrosorption capacity among all the electrodes. Several charging and discharging cycles for this electrode are presented in Figure5. The figure clearly shows that no oxidation and reduction reactions occur in electrosorption. This indicates that the consumption of current is mainly because of charging the electrode where the ions are electroadsorbed from the bulk solution [74], and there is complete formation of electrical double layer at the electrode and electrolyte interface [75]. Moreover, the conductivity changes are reproducible for the first five cycles of electrosorption and desorption, confirming that the CDI could be regenerated very well without any driving energy and secondary pollution, which is critical for large-scale applications. It is observed from the figure that the regeneration test can be performed in a short period of time because the same pattern is noticed when considered for four repeated electrosorption-desorption cycles; each cycle takes 13 min that is 6 min of ion adsorption and 7 min release of ions. Initially, for the first five cycles, the electrode showed very high recycling stability (100%) because of no decay of the electrosorption capacity. This type of high cycling stability behaviour of the CNT/GO electrode in a CDI system is reported in other research as well as when tested for four cycles [58]. It is observed from the figure that during 41-45 cycles, the amplitude of conductivity is less compared to the first five cycles. This indicates that the electrosorption capacity during higher cycles becomes worse, and there is the degradation of the CDI performance.Figure 5
Multiple electrosorption-desorption cycles of the 75 mg/L NaCl solution for the 9-CNT/mwGO/RVC electrode measured at 50 mL/min flow rate through electrode upon polarization and depolarization at 1.5 V and 0 V, respectively.


#### 3.3.4. Electrosorption Isotherm

The electrosorption isotherm is generally used to describe how ions interact with carbon electrodes. The Langmuir and Freundlich isotherms are the two most common isotherms, and they were employed for simulating the ion adsorption on the 9-CNT/mwGO/RVC electrode. The electrosorption isotherms of NaCl onto the 9-CNT/mwGO/RVC electrode were evaluated, and their results were compared with the results of the CNT/RVC electrode. This experiment was performed using the different concentrations of NaCl as presented in Figure6. It is observed from the figure that the trend of the electrosorption capacity behaviour of both electrodes is the same and differs only in their magnitude. For both electrodes, the removal of NaCl has increased with the increase in concentration. This can be attributed to the enhancement of ions’ mass transfer rate inside the microporous electrodes [71, 76, 77]. The figure shows that the electrosorption capacity of 9-CNT/mwGO/RVC and CNT/RVC electrodes is 10.84 and 8.89 mg/g, respectively, at 500 mg/L feed concentration. This implies that combining mwGO with CNT materials has increased the number of adsorption sites in the 9-CNT/mwGO/RVC electrode under an electric field. Langmuir and Freundlich isotherms (shown in Supplementary section S14) were used to fit the experimental data for electrosorption of Na+ and Cl- onto the electrodes. The Langmuir isotherm is applicable to localized adsorbed ions with a limited adsorption amount [78], and the Freundlich isotherm is suitable for the description of ion adsorption with a wide variety of adsorption strength [79].Figure 6
The electrosorption isotherms for 9-CNT/mwGO/RVC and CNT/RVC electrodes at 1.5 V and 50 mL/min flow rate using different initial concentrations of the NaCl solutions.Table3 shows the comparison between Langmuir and Freundlich isotherms for the NaCl electrosorption using both electrodes. It is revealed that the electrosorption isotherm of both electrodes obeys both models, when considering the R2 values (better than 99.9% confidence level). The regression coefficients for CNT/RVC were 0.997 and 0.989 and for the 9-CNT/mwGO/RVC electrode were 0.995 and 0.981 for the Langmuir and Freundlich isotherms, respectively. These results suggest that the monolayer adsorption is the primary adsorption mechanism during the electrosorption process [70, 72]. The KL values of both electrodes are 0.01, and the KF values of CNT/RVC and 9-CNT/mwGO/RVC electrodes are 0.28 and 0.32, respectively. Normally, a higher value of n between 1 and 10 represents more beneficial adsorption [64], and the volume of n for both electrodes was around 1.74. Hence, the electrodes with a high value of n exhibit a high potential for electrosorption capability. In this type of system, the adsorbed layer is extremely thin, and the amount adsorbed is only a fraction of the monolayer capacity. Therefore, the electrosorption for both electrodes is followed by the monolayer adsorption [56]. Additionally, as a standard procedure, in order to calculate the maximum electrosorption amount of electrodes, the term qm in the Langmuir equation has been considered as the maximum adsorption capacity. The results show that the qm has improved with the increase in bias concentration. The qm measured at polarization of 1.5 V and a flow rate of 50 mL/min was 13.08 and 16.59 mg/g using CNT/RVC and 9-CNT/mwGO/RVC electrodes, respectively. Hence, it can be suggested that the maximum adsorption capacity qm for NaCl on the 9-CNT/mwGO/RVC electrode has improved compared to the CNT/RVC electrode. When considering a concentration of 500 mg/L NaCl, the qm at equilibrium for the CNT/RVC electrode is much higher compared to multiwalled carbon nanotubes (MWCNTs) [72] and activated carbon (AC) [80], which were 3.10 mg/g and 9.72 mg/g, respectively. This is because the surface area and average pore size in the CNT/RVC electrode are larger, where the surface area in MWCNTs and AC electrodes was 153 and 1153 m2/g [72, 80], respectively. In addition, the qm of the CNT/RVC electrode is very close to the qm of composite made from carbon nanotubes and carbon nanofiber (CNTs-CNFs) electrode, which was 13.35 mg/g [71]. The maximum electrosorption capacity results of 9-CNT/mwGO/RVC and CNT/RVC electrodes are lower than the graphene electrode, which was 21.04 mg/g [56]. This graphene electrode mainly consists of mesopores with an average pore diameter of about 7.42 nm, which is greatly beneficial to a capacitive deionization system.Table 3
The parameters of Langmuir and Freundlich isotherms for the NaCl electrosorption using the 9-CNT/mwGO/RVC and CNT/RVC electrodes.
IsothermParameterValue9-CNT/mwGO/RVCValue∗CNT/RVCLangmuirqm (mg/g)16.5913.08KL (L/mg)0.010.01R20.9950.997FreundlichKF (L/mg)0.320.28n1.741.74R20.9810.989∗These results were calculated in article [61].


#### 3.3.5. Water Production by a CDI System

The water production experiment and calculation were carried out at the NaCl feed solution concentration 75 mg/L. It has been shown earlier that 1 g of the 9:CNT/mwGO composite and CNT coated on 43.20 cm3 RVC electrode adsorbed 3.82 mg and 3.23 mg NaCl during 13 mins and 18 mins, respectively. Hence, the solution concentration was reduced from 75 mg/L to 71.18 mg/L and 71.77 mg/L for 9:CNT/mwGO/RVC and CNT/RVC electrodes, respectively, after 1 desalination cycle. Moreover, it has also been shown that the electrosorption capacity varied with the increase in solution concentration and exhibits a linear relationship below the concentration of 100 mg/L (Figure 6). The abovementioned claim has been confirmed by their linear fit as shown in Figure 7(a) where plots for 9:CNT/mwGO/RVC and CNT/RVC composite electrodes are based on Equations (1) and (2), respectively.Figure 7
(a) The variation of electrosorption with respect to feed concentration and (b) the variation of feed concentration with respect to desalination cycles.
(a)(b)For the 9:CNT/mwGO/RVC composite electrode,(1)Electrosorptionmg/g=0.050∗concentration.For the CNT/RVC composite electrode,(2)Electrosorptionmg/g=0.042∗concentration.From these equations, the variation of concentration can be known after each desalination cycle. Figure7(b) represents the variation of concentration with respect to the desalination cycle. The reading was noted till the concentration was reached less than 1 mg/L using 1 g of the CNT/mwGO composite or CNT coated on a 43.20 cm3 RVC electrode. It is observed from the figure that the CNT/RVC electrode when used in a CDI system required 103 desalination cycles for reducing solution concentration from 75 mg/L to 1 mg/L. As each desalination cycle for this electrode takes 18 mins, hence, the total time required is 1854 mins (18min×103 cycles) for the production of 1 L of water that contains the NaCl concentration of less than 1 mg/L. Thus, the desalinated water produced per day is 0.78 L using 1 g of CNT coated on a 43.20 cm3 RVC electrode, or 17,855 L using 1 m3 of the same composite electrode. On the other hand, by using the 9-CNT/mwGO/RVC electrode in a CDI system, it is required 85 desalination cycles for the reduction of the same amount of solution concentration. This indicates that this electrode takes time for about 1105 mins (13min×85 cycles) to produce 1 L desalinated water where it contains the same NaCl concentration. Thus, the water produced per day is 1.30 L using 1 g of 9-CNT/mwGO coated on a 43.20 cm3 RVC electrode or 29,958 L using 1 m3 of the same composite electrode. Hence, it can be inferred that the 9-CNT/mwGO/RVC composite electrode produced 67.78% more desalinated water per day compared to the CNT/RVC composite electrode when used in the same CDI system.


## 3.1. Adsorption Performance of the 9-CNT/mwGO-Coated RVC Electrode

The adsorption performance test was carried out at the optimum applied voltage 1.5 V (in this study, the ferricyanide solution was used to test the 3 electrode system. We observed the oxidation peak shift to 0.59 V, where the ideal oxidation peak was 0.29 V. Hence, the maximum/optimum applied voltage for our CDI system was 1.5 V.) and optimum flow rate 50 mL/min, as reported in our previous study for the CNT/RVC electrode [61, 62]. These conditions were used in further studies to compare the desalination performance of a range of electrodes with different amounts of 9-CNT/mwGO composite materials coated on the RVC electrode. All experiments were performed by keeping the total volume of the NaCl solution at 70 mL and the initial feed concentration at 75 mg/L (143 μS/cm). Figure 1(a) shows the CDI process for all loading level composites at the geometric volume 2.16 cm3 of the RVC electrode: 10, 30, and 50 mg loadings. There is a drop in the conductivity of the test saline solution with increasing amounts of material on the electrode because ions were attracted by the oppositely charged electrodes when an electric field was applied [63]. A better electrosorption performance was achieved at 50 mg coated RVC electrode where the conductivity was significantly dropped by approximately 5.21 μS/cm in the electrosorption process. Figure 1(b) shows the electrosorption of various 9-CNT/mwGO/RVC electrodes in terms of the mass of 9-CNT/mwGO and the volume of electrode (calculated as per supplementary section S12). It is evident from the figure that the electrosorption capacity was decreased with the increase in weight of composite material. It is clear that when the RVC electrode was loaded with 10 mg of composite, the electrosorption capacity was 9.91 mg/g and when the same electrode was loaded with 50 mg of composite, the electrosorption capacity became 3.82 mg/g. On the contrary, the electrosorption capacity of electrodes in terms of geometric volume was increased with the increase in amount of composite material. The calculation showed that when the RVC electrode was separately loaded with 10 mg and 50 mg of composites, the electrosorption capacities were 0.05 mg/cm3 and 0.09 mg/cm3, respectively. This result leads to the generalization that the electrosorption capacity increases with increasing amounts of material on the electrode.Figure 1
(a) Adsorption behaviour and (b) the electrosorption capacity in terms of the mass of composite material loading and the geometric volume of the electrode of various 9-CNT/mwGO/RVC electrodes. Loadings (mg): 10, 30, and 50.
(a)(b)


## 3.2. Optimization of Conditions for Ion Removal Efficiency

This study is based on the 50 mg 9-CNT/mwGO composite-coated RVC electrode because it showed the highest electrosorption capacity in terms of geometric volume. The optimization was carried out for electrical voltage and flow rate. The investigated cell voltages were 1.3 V and 1.5 V, and the flow rates were 25 mL/min, 50 mL/min, and 75 mL/min as shown in Figures2(a) and 2(b). Cell voltages above 1.5 V were not investigated because saving energy is one of our targets. Figure 2(a) represents the variation solution conductivity with respect to time at two different voltages. It was observed that with the increase in applied voltage, the ion removal amount was also increased. Hence, higher ion removal was achieved at 1.5 V. Figure 2(b) shows that the highest variation in solution conductivity was observed at a 50 mL/min flow rate, which indicated the highest electrosorption capacity. This is because a low pump rate would result in an obvious coion effect, which will suppress the electrosorption process, while a high pump rate will introduce a high pump force that is greater than that of electrosorption force and therefore decrease the electrosorption amount [64]. Thus, the optimized cell voltage and flow rate for the CDI process were found to be 1.5 V and 50 mL/min, respectively.Figure 2
Conductivity variations of the NaCl solution with various (a) applied voltages and (b) applied flow rates, with respect to operating time, using the 9-CNT/mwGO/RVC electrode loaded with 50 mg composite material.
(a)(b)


## 3.3. Capacitive Deionization (CDI) System

### 3.3.1. Adsorption/Desorption Performance of the CNT/mwGO/RVC Electrodes

The CDI system was investigated with respect to the influence of increasing ratios of mwGO in the CNT/mwGO composite material-coated RVC electrodes on the ion removal performance. The ratio levels were 10 : 0, 9 : 1, 8 : 2, and 7 : 3 CNT : mwGO, respectively, and the mass of materials coated on all RVC electrodes was 50 mg. All experiments were performed with the same previous conditions at 1.5 V and 50 mL/min flow rate with 6 min adsorption processes. Figure3(a) shows the CDI process for all composite-coated RVC electrodes. As expected, once the electrical voltage was applied, the solution conductivity dramatically decreased for all electrodes because ions were attracted by opposite charges on the electrodes [63]. Then, the conductivity would gradually approach a constant minimum level, indicating that saturation was achieved [58]. During the discharging of the CDI system under 0 V of applied voltage, the solution conductivity was returned to approximate its initial value (143 μS/cm), meaning that the ions were released from the double layer region back into the solution because of the disappearance of electrostatic forces. It is clear that the highest drop in conductivity was around 5.2 μS/cm using the 9-CNT/mwGO/RVC electrode. The second-largest drop in conductivity was around 4.8 μS/cm using the 8-CNT/mwGO/RVC electrode. The drop in conductivity for the CNT/RVC electrode was higher than that of the 7-CNT/mwGO/RVC electrode. It is notable that the 9-CNT/mwGO/RVC electrode’s saturation was achieved after 5 min, whereas the CNT/RVC electrode saturation was achieved after 6 min. It is also interesting to note that the regeneration by discharging the CDI cells was completed, at 0 V, after 13 min for the electrode with the least amount of the mwGO ratio in the sample that is 9-CNT/mwGO/RVC. However, for the CNT/RVC electrode, the required time for one electrosorption-desorption process was 18 min. Hence, there was 27.78% saving of time in one desalination cycle for the 9-CNT/mwGO/RVC electrode compared to the CNT/RVC electrode [61]. Moreover, the electrosorption capacities in terms of mass of electrode for 9-CNT/mwGO/RVC and CNT/RVC electrodes were 3.82 mg/g and 3.23 mg/g, respectively. Thus, there was an 18.27% increment in the electrosorption removal performance for the 9-CNT/mwGO/RVC electrode compared to the CNT/RVC electrode. This improvement in electrosorption amount in the 9-CNT/mwGO/RVC electrode can be attributed to many complicated factors: these included the increasing specific surface area, specific capacitance, more accessible interlayer, pore microstructure, and pore size distribution which can play important roles in affecting the electrosorption capacity [58, 59, 65].Figure 3
(a) Adsorption and release behaviour and (b) the electrosorption capacity in terms of mass of CNT/mwGO and the geometric volume of electrode of various ratios 10, 9, 8, and 7 CNT in CNT/mwGO/RVC electrodes.
(a)(b)Figure3(b) shows the electrosorption performances of all electrodes which were measured from the data in Figure 3(a). The variation of the solution conductivity was monitored instantly by a multifunction conductivity meter. Accordingly, the correlation of conductivity (μS/cm) with concentration (mg/L) was calibrated prior to experiments (shown in supplementary section S9). Furthermore, the 8-CNT/mwGO/RVC electrode also afforded better CDI system performance than the a-SWCNT/RVC electrode, as evidenced by time saving of the 11.11% and 8.98% better electrosorption removal of NaCl. Table 1 also represents the detailed electrosorption in terms of mass, area, and volume for each composite electrode (calculated as per supplementary section S12). It is clear that the electrosorption behaviours of all composite electrodes in terms of area and in terms of volume followed the electrosorption behaviours of composite electrodes in terms of mass of electrode because all the parameters were held constant: mass of material, electrode area, and volume. These results suggested that the CDI process, using the 9-CNT/mwGO/RVC electrode, was promising as an effective technology for desalination.Table 1
Electrosorption of NaCl by the CNT/mwGO/RVC electrodes with various ratios of CNT and time of one desalination cycle (∗comparing with the CNT/RVC electrode).
Ratio of a-SWCNT in electrodesElectrosorption∗Enhancement percentage in electrosorptionTime of one desalination cyclemg/gmg/cm2mg/cm3%min73.018.4E−030.071783.529.9E−030.098.981693.821.1E−020.1018.2713103.239.4E−030.0818


### 3.3.2. Electrosorption Dynamics

The performance of electrode adsorptions is evaluated by dynamics study, which describes the solute uptake rate, and evidently, this rate controls the residence time of adsorptive uptake at the solid-solution interface [66, 67]. However, this section will investigate the controlling mechanism of electrosorption and the constants of sorption of pseudo-first-order kinetics as proposed by Lagergren [68], where the conformity between experimental data and the model’s predicted values is expressed by the correlation coefficients (r2, values close or equal to 1). The electrosorption dynamic and pseudo-first-order dynamic models for the NaCl adsorption onto CNT/RVC, 9-CNT/mwGO/RVC, 8-CNT/mwGO/RVC, and 7-CNT/mwGO/RVC electrodes at voltage 1.5 V, flow rate 50 mL/min, and constant temperature 298 K are presented in Figure 4. The composite electrodes (except 9-CNT/mwGO/RVC) exhibited steady increment in electrosorption within the first minute, then it became dynamic adsorption, and after three minutes, the electrode gradually approached saturation as shown in Figures 4(a), 4(b), and 4(d). The time required to reach the adsorption equilibrium was 6 minutes. However, the electrosorption of NaCl onto the 9-CNT/mwGO/RVC electrode was very rapid within the first half minute. This could be because the external surface area of bundled CNT in this electrode is higher than other electrodes, thus increasing the possibility of ions to reach the surface easily. After that, the electrosorption of NaCl onto this electrode becomes dynamic adsorption for four minutes and then followed by the electrode saturation as shown in Figure 4(c). The time required to reach adsorption equilibrium was 5 minutes, which may be due to the higher rate of diffusion of ions onto the electrode particle surface.Figure 4
(a–d) Electrosorption and (e–h) pseudo-first-order adsorption kinetics of the NaCl electrosorption onto CNT/RVC, 9-CNT/mwGO/RVC, 8-CNT/mwGO/RVC, and 7-CNT/mwGO/RVC electrodes, respectively, at 1.5 V and 50 mL/min flow rate. Results have been derived from Figure 5.15 (a) (adsorption process).The pseudo-first-order kinetics for all electrodes was studied within the first four minutes as shown in Figures4(e)–4(g) and 4(d), respectively. To evaluate the kinetics of the electrosorption process, the pseudo-first-order model was tested to interpret the experimental data. The pseudo-first-order equation has been expressed in Supplementary section S13. The slopes and intercepts of plots of log (qe–qt) versus t were used to determine the first-order rate constant k1. In all electrodes, methods that are based on the linearization of the models and correlation coefficients (r2) of around 0.99 confirm that all electrodes followed pseudo-first-order dynamics. Similar trends were reported in the literature for the adsorption of NaCl ions from aqueous solutions by other adsorbents [56, 64, 69–73]. A comparison of the rate constant k1 with the correlation coefficients is shown in Table 2. The rate constant (k1) of the pseudo-first-order kinetics was 0.816, 0.525, 0.555, and 0.639 min-1 for CNT/RVC, 9-CNT/mwGO/RVC, 8-CNT/mwGO/RVC, and 7-CNT/mwGO/RVC electrodes, respectively. Hence, it is clear that there is an inverse relationship between the rate constant and electrosorption; when the electrosorption capacity is increased, the rate constant is decreased. Also, the theoretical qe values found from the pseudo-first-order kinetics model gave reasonable values (3.19, 3.66, 3.45, and 2.75 mg/g for CNT/RVC, 9-CNT/mwGO/RVC, 8-CNT/mwGO/RVC, and 7-CNT/mwGO/RVC electrodes, respectively).Table 2
The comparison between the adsorption rate constant (k1) and correlation coefficients of pseudo-first-order kinetics and the estimated theoretical and experimental (qe) maximum electrosorption with the pseudo-first-order model.
a-SWCNT : mwGOR2K1 (min-1)Theoreticalqe (mg/g)Experimentalqe (mg/g)7 : 30.9900.6392.753.018 : 20.9870.5553.453.529 : 10.9920.5253.663.8210 : 00.9940.8163.193.23


### 3.3.3. CDI Cycling Stability

The regeneration of electrodes plays a significant role in their commercialization for using in CDI systems. To test reversibility, the 9-CNT/mwGO/RVC electrode was selected because it had the highest electrosorption capacity among all the electrodes. Several charging and discharging cycles for this electrode are presented in Figure5. The figure clearly shows that no oxidation and reduction reactions occur in electrosorption. This indicates that the consumption of current is mainly because of charging the electrode where the ions are electroadsorbed from the bulk solution [74], and there is complete formation of electrical double layer at the electrode and electrolyte interface [75]. Moreover, the conductivity changes are reproducible for the first five cycles of electrosorption and desorption, confirming that the CDI could be regenerated very well without any driving energy and secondary pollution, which is critical for large-scale applications. It is observed from the figure that the regeneration test can be performed in a short period of time because the same pattern is noticed when considered for four repeated electrosorption-desorption cycles; each cycle takes 13 min that is 6 min of ion adsorption and 7 min release of ions. Initially, for the first five cycles, the electrode showed very high recycling stability (100%) because of no decay of the electrosorption capacity. This type of high cycling stability behaviour of the CNT/GO electrode in a CDI system is reported in other research as well as when tested for four cycles [58]. It is observed from the figure that during 41-45 cycles, the amplitude of conductivity is less compared to the first five cycles. This indicates that the electrosorption capacity during higher cycles becomes worse, and there is the degradation of the CDI performance.Figure 5
Multiple electrosorption-desorption cycles of the 75 mg/L NaCl solution for the 9-CNT/mwGO/RVC electrode measured at 50 mL/min flow rate through electrode upon polarization and depolarization at 1.5 V and 0 V, respectively.


### 3.3.4. Electrosorption Isotherm

The electrosorption isotherm is generally used to describe how ions interact with carbon electrodes. The Langmuir and Freundlich isotherms are the two most common isotherms, and they were employed for simulating the ion adsorption on the 9-CNT/mwGO/RVC electrode. The electrosorption isotherms of NaCl onto the 9-CNT/mwGO/RVC electrode were evaluated, and their results were compared with the results of the CNT/RVC electrode. This experiment was performed using the different concentrations of NaCl as presented in Figure6. It is observed from the figure that the trend of the electrosorption capacity behaviour of both electrodes is the same and differs only in their magnitude. For both electrodes, the removal of NaCl has increased with the increase in concentration. This can be attributed to the enhancement of ions’ mass transfer rate inside the microporous electrodes [71, 76, 77]. The figure shows that the electrosorption capacity of 9-CNT/mwGO/RVC and CNT/RVC electrodes is 10.84 and 8.89 mg/g, respectively, at 500 mg/L feed concentration. This implies that combining mwGO with CNT materials has increased the number of adsorption sites in the 9-CNT/mwGO/RVC electrode under an electric field. Langmuir and Freundlich isotherms (shown in Supplementary section S14) were used to fit the experimental data for electrosorption of Na+ and Cl- onto the electrodes. The Langmuir isotherm is applicable to localized adsorbed ions with a limited adsorption amount [78], and the Freundlich isotherm is suitable for the description of ion adsorption with a wide variety of adsorption strength [79].Figure 6
The electrosorption isotherms for 9-CNT/mwGO/RVC and CNT/RVC electrodes at 1.5 V and 50 mL/min flow rate using different initial concentrations of the NaCl solutions.Table3 shows the comparison between Langmuir and Freundlich isotherms for the NaCl electrosorption using both electrodes. It is revealed that the electrosorption isotherm of both electrodes obeys both models, when considering the R2 values (better than 99.9% confidence level). The regression coefficients for CNT/RVC were 0.997 and 0.989 and for the 9-CNT/mwGO/RVC electrode were 0.995 and 0.981 for the Langmuir and Freundlich isotherms, respectively. These results suggest that the monolayer adsorption is the primary adsorption mechanism during the electrosorption process [70, 72]. The KL values of both electrodes are 0.01, and the KF values of CNT/RVC and 9-CNT/mwGO/RVC electrodes are 0.28 and 0.32, respectively. Normally, a higher value of n between 1 and 10 represents more beneficial adsorption [64], and the volume of n for both electrodes was around 1.74. Hence, the electrodes with a high value of n exhibit a high potential for electrosorption capability. In this type of system, the adsorbed layer is extremely thin, and the amount adsorbed is only a fraction of the monolayer capacity. Therefore, the electrosorption for both electrodes is followed by the monolayer adsorption [56]. Additionally, as a standard procedure, in order to calculate the maximum electrosorption amount of electrodes, the term qm in the Langmuir equation has been considered as the maximum adsorption capacity. The results show that the qm has improved with the increase in bias concentration. The qm measured at polarization of 1.5 V and a flow rate of 50 mL/min was 13.08 and 16.59 mg/g using CNT/RVC and 9-CNT/mwGO/RVC electrodes, respectively. Hence, it can be suggested that the maximum adsorption capacity qm for NaCl on the 9-CNT/mwGO/RVC electrode has improved compared to the CNT/RVC electrode. When considering a concentration of 500 mg/L NaCl, the qm at equilibrium for the CNT/RVC electrode is much higher compared to multiwalled carbon nanotubes (MWCNTs) [72] and activated carbon (AC) [80], which were 3.10 mg/g and 9.72 mg/g, respectively. This is because the surface area and average pore size in the CNT/RVC electrode are larger, where the surface area in MWCNTs and AC electrodes was 153 and 1153 m2/g [72, 80], respectively. In addition, the qm of the CNT/RVC electrode is very close to the qm of composite made from carbon nanotubes and carbon nanofiber (CNTs-CNFs) electrode, which was 13.35 mg/g [71]. The maximum electrosorption capacity results of 9-CNT/mwGO/RVC and CNT/RVC electrodes are lower than the graphene electrode, which was 21.04 mg/g [56]. This graphene electrode mainly consists of mesopores with an average pore diameter of about 7.42 nm, which is greatly beneficial to a capacitive deionization system.Table 3
The parameters of Langmuir and Freundlich isotherms for the NaCl electrosorption using the 9-CNT/mwGO/RVC and CNT/RVC electrodes.
IsothermParameterValue9-CNT/mwGO/RVCValue∗CNT/RVCLangmuirqm (mg/g)16.5913.08KL (L/mg)0.010.01R20.9950.997FreundlichKF (L/mg)0.320.28n1.741.74R20.9810.989∗These results were calculated in article [61].


### 3.3.5. Water Production by a CDI System

The water production experiment and calculation were carried out at the NaCl feed solution concentration 75 mg/L. It has been shown earlier that 1 g of the 9:CNT/mwGO composite and CNT coated on 43.20 cm3 RVC electrode adsorbed 3.82 mg and 3.23 mg NaCl during 13 mins and 18 mins, respectively. Hence, the solution concentration was reduced from 75 mg/L to 71.18 mg/L and 71.77 mg/L for 9:CNT/mwGO/RVC and CNT/RVC electrodes, respectively, after 1 desalination cycle. Moreover, it has also been shown that the electrosorption capacity varied with the increase in solution concentration and exhibits a linear relationship below the concentration of 100 mg/L (Figure 6). The abovementioned claim has been confirmed by their linear fit as shown in Figure 7(a) where plots for 9:CNT/mwGO/RVC and CNT/RVC composite electrodes are based on Equations (1) and (2), respectively.Figure 7
(a) The variation of electrosorption with respect to feed concentration and (b) the variation of feed concentration with respect to desalination cycles.
(a)(b)For the 9:CNT/mwGO/RVC composite electrode,(1)Electrosorptionmg/g=0.050∗concentration.For the CNT/RVC composite electrode,(2)Electrosorptionmg/g=0.042∗concentration.From these equations, the variation of concentration can be known after each desalination cycle. Figure7(b) represents the variation of concentration with respect to the desalination cycle. The reading was noted till the concentration was reached less than 1 mg/L using 1 g of the CNT/mwGO composite or CNT coated on a 43.20 cm3 RVC electrode. It is observed from the figure that the CNT/RVC electrode when used in a CDI system required 103 desalination cycles for reducing solution concentration from 75 mg/L to 1 mg/L. As each desalination cycle for this electrode takes 18 mins, hence, the total time required is 1854 mins (18min×103 cycles) for the production of 1 L of water that contains the NaCl concentration of less than 1 mg/L. Thus, the desalinated water produced per day is 0.78 L using 1 g of CNT coated on a 43.20 cm3 RVC electrode, or 17,855 L using 1 m3 of the same composite electrode. On the other hand, by using the 9-CNT/mwGO/RVC electrode in a CDI system, it is required 85 desalination cycles for the reduction of the same amount of solution concentration. This indicates that this electrode takes time for about 1105 mins (13min×85 cycles) to produce 1 L desalinated water where it contains the same NaCl concentration. Thus, the water produced per day is 1.30 L using 1 g of 9-CNT/mwGO coated on a 43.20 cm3 RVC electrode or 29,958 L using 1 m3 of the same composite electrode. Hence, it can be inferred that the 9-CNT/mwGO/RVC composite electrode produced 67.78% more desalinated water per day compared to the CNT/RVC composite electrode when used in the same CDI system.


## 3.3.1. Adsorption/Desorption Performance of the CNT/mwGO/RVC Electrodes

The CDI system was investigated with respect to the influence of increasing ratios of mwGO in the CNT/mwGO composite material-coated RVC electrodes on the ion removal performance. The ratio levels were 10 : 0, 9 : 1, 8 : 2, and 7 : 3 CNT : mwGO, respectively, and the mass of materials coated on all RVC electrodes was 50 mg. All experiments were performed with the same previous conditions at 1.5 V and 50 mL/min flow rate with 6 min adsorption processes. Figure3(a) shows the CDI process for all composite-coated RVC electrodes. As expected, once the electrical voltage was applied, the solution conductivity dramatically decreased for all electrodes because ions were attracted by opposite charges on the electrodes [63]. Then, the conductivity would gradually approach a constant minimum level, indicating that saturation was achieved [58]. During the discharging of the CDI system under 0 V of applied voltage, the solution conductivity was returned to approximate its initial value (143 μS/cm), meaning that the ions were released from the double layer region back into the solution because of the disappearance of electrostatic forces. It is clear that the highest drop in conductivity was around 5.2 μS/cm using the 9-CNT/mwGO/RVC electrode. The second-largest drop in conductivity was around 4.8 μS/cm using the 8-CNT/mwGO/RVC electrode. The drop in conductivity for the CNT/RVC electrode was higher than that of the 7-CNT/mwGO/RVC electrode. It is notable that the 9-CNT/mwGO/RVC electrode’s saturation was achieved after 5 min, whereas the CNT/RVC electrode saturation was achieved after 6 min. It is also interesting to note that the regeneration by discharging the CDI cells was completed, at 0 V, after 13 min for the electrode with the least amount of the mwGO ratio in the sample that is 9-CNT/mwGO/RVC. However, for the CNT/RVC electrode, the required time for one electrosorption-desorption process was 18 min. Hence, there was 27.78% saving of time in one desalination cycle for the 9-CNT/mwGO/RVC electrode compared to the CNT/RVC electrode [61]. Moreover, the electrosorption capacities in terms of mass of electrode for 9-CNT/mwGO/RVC and CNT/RVC electrodes were 3.82 mg/g and 3.23 mg/g, respectively. Thus, there was an 18.27% increment in the electrosorption removal performance for the 9-CNT/mwGO/RVC electrode compared to the CNT/RVC electrode. This improvement in electrosorption amount in the 9-CNT/mwGO/RVC electrode can be attributed to many complicated factors: these included the increasing specific surface area, specific capacitance, more accessible interlayer, pore microstructure, and pore size distribution which can play important roles in affecting the electrosorption capacity [58, 59, 65].Figure 3
(a) Adsorption and release behaviour and (b) the electrosorption capacity in terms of mass of CNT/mwGO and the geometric volume of electrode of various ratios 10, 9, 8, and 7 CNT in CNT/mwGO/RVC electrodes.
(a)(b)Figure3(b) shows the electrosorption performances of all electrodes which were measured from the data in Figure 3(a). The variation of the solution conductivity was monitored instantly by a multifunction conductivity meter. Accordingly, the correlation of conductivity (μS/cm) with concentration (mg/L) was calibrated prior to experiments (shown in supplementary section S9). Furthermore, the 8-CNT/mwGO/RVC electrode also afforded better CDI system performance than the a-SWCNT/RVC electrode, as evidenced by time saving of the 11.11% and 8.98% better electrosorption removal of NaCl. Table 1 also represents the detailed electrosorption in terms of mass, area, and volume for each composite electrode (calculated as per supplementary section S12). It is clear that the electrosorption behaviours of all composite electrodes in terms of area and in terms of volume followed the electrosorption behaviours of composite electrodes in terms of mass of electrode because all the parameters were held constant: mass of material, electrode area, and volume. These results suggested that the CDI process, using the 9-CNT/mwGO/RVC electrode, was promising as an effective technology for desalination.Table 1
Electrosorption of NaCl by the CNT/mwGO/RVC electrodes with various ratios of CNT and time of one desalination cycle (∗comparing with the CNT/RVC electrode).
Ratio of a-SWCNT in electrodesElectrosorption∗Enhancement percentage in electrosorptionTime of one desalination cyclemg/gmg/cm2mg/cm3%min73.018.4E−030.071783.529.9E−030.098.981693.821.1E−020.1018.2713103.239.4E−030.0818


## 3.3.2. Electrosorption Dynamics

The performance of electrode adsorptions is evaluated by dynamics study, which describes the solute uptake rate, and evidently, this rate controls the residence time of adsorptive uptake at the solid-solution interface [66, 67]. However, this section will investigate the controlling mechanism of electrosorption and the constants of sorption of pseudo-first-order kinetics as proposed by Lagergren [68], where the conformity between experimental data and the model’s predicted values is expressed by the correlation coefficients (r2, values close or equal to 1). The electrosorption dynamic and pseudo-first-order dynamic models for the NaCl adsorption onto CNT/RVC, 9-CNT/mwGO/RVC, 8-CNT/mwGO/RVC, and 7-CNT/mwGO/RVC electrodes at voltage 1.5 V, flow rate 50 mL/min, and constant temperature 298 K are presented in Figure 4. The composite electrodes (except 9-CNT/mwGO/RVC) exhibited steady increment in electrosorption within the first minute, then it became dynamic adsorption, and after three minutes, the electrode gradually approached saturation as shown in Figures 4(a), 4(b), and 4(d). The time required to reach the adsorption equilibrium was 6 minutes. However, the electrosorption of NaCl onto the 9-CNT/mwGO/RVC electrode was very rapid within the first half minute. This could be because the external surface area of bundled CNT in this electrode is higher than other electrodes, thus increasing the possibility of ions to reach the surface easily. After that, the electrosorption of NaCl onto this electrode becomes dynamic adsorption for four minutes and then followed by the electrode saturation as shown in Figure 4(c). The time required to reach adsorption equilibrium was 5 minutes, which may be due to the higher rate of diffusion of ions onto the electrode particle surface.Figure 4
(a–d) Electrosorption and (e–h) pseudo-first-order adsorption kinetics of the NaCl electrosorption onto CNT/RVC, 9-CNT/mwGO/RVC, 8-CNT/mwGO/RVC, and 7-CNT/mwGO/RVC electrodes, respectively, at 1.5 V and 50 mL/min flow rate. Results have been derived from Figure 5.15 (a) (adsorption process).The pseudo-first-order kinetics for all electrodes was studied within the first four minutes as shown in Figures4(e)–4(g) and 4(d), respectively. To evaluate the kinetics of the electrosorption process, the pseudo-first-order model was tested to interpret the experimental data. The pseudo-first-order equation has been expressed in Supplementary section S13. The slopes and intercepts of plots of log (qe–qt) versus t were used to determine the first-order rate constant k1. In all electrodes, methods that are based on the linearization of the models and correlation coefficients (r2) of around 0.99 confirm that all electrodes followed pseudo-first-order dynamics. Similar trends were reported in the literature for the adsorption of NaCl ions from aqueous solutions by other adsorbents [56, 64, 69–73]. A comparison of the rate constant k1 with the correlation coefficients is shown in Table 2. The rate constant (k1) of the pseudo-first-order kinetics was 0.816, 0.525, 0.555, and 0.639 min-1 for CNT/RVC, 9-CNT/mwGO/RVC, 8-CNT/mwGO/RVC, and 7-CNT/mwGO/RVC electrodes, respectively. Hence, it is clear that there is an inverse relationship between the rate constant and electrosorption; when the electrosorption capacity is increased, the rate constant is decreased. Also, the theoretical qe values found from the pseudo-first-order kinetics model gave reasonable values (3.19, 3.66, 3.45, and 2.75 mg/g for CNT/RVC, 9-CNT/mwGO/RVC, 8-CNT/mwGO/RVC, and 7-CNT/mwGO/RVC electrodes, respectively).Table 2
The comparison between the adsorption rate constant (k1) and correlation coefficients of pseudo-first-order kinetics and the estimated theoretical and experimental (qe) maximum electrosorption with the pseudo-first-order model.
a-SWCNT : mwGOR2K1 (min-1)Theoreticalqe (mg/g)Experimentalqe (mg/g)7 : 30.9900.6392.753.018 : 20.9870.5553.453.529 : 10.9920.5253.663.8210 : 00.9940.8163.193.23


## 3.3.3. CDI Cycling Stability

The regeneration of electrodes plays a significant role in their commercialization for using in CDI systems. To test reversibility, the 9-CNT/mwGO/RVC electrode was selected because it had the highest electrosorption capacity among all the electrodes. Several charging and discharging cycles for this electrode are presented in Figure5. The figure clearly shows that no oxidation and reduction reactions occur in electrosorption. This indicates that the consumption of current is mainly because of charging the electrode where the ions are electroadsorbed from the bulk solution [74], and there is complete formation of electrical double layer at the electrode and electrolyte interface [75]. Moreover, the conductivity changes are reproducible for the first five cycles of electrosorption and desorption, confirming that the CDI could be regenerated very well without any driving energy and secondary pollution, which is critical for large-scale applications. It is observed from the figure that the regeneration test can be performed in a short period of time because the same pattern is noticed when considered for four repeated electrosorption-desorption cycles; each cycle takes 13 min that is 6 min of ion adsorption and 7 min release of ions. Initially, for the first five cycles, the electrode showed very high recycling stability (100%) because of no decay of the electrosorption capacity. This type of high cycling stability behaviour of the CNT/GO electrode in a CDI system is reported in other research as well as when tested for four cycles [58]. It is observed from the figure that during 41-45 cycles, the amplitude of conductivity is less compared to the first five cycles. This indicates that the electrosorption capacity during higher cycles becomes worse, and there is the degradation of the CDI performance.Figure 5
Multiple electrosorption-desorption cycles of the 75 mg/L NaCl solution for the 9-CNT/mwGO/RVC electrode measured at 50 mL/min flow rate through electrode upon polarization and depolarization at 1.5 V and 0 V, respectively.


## 3.3.4. Electrosorption Isotherm

The electrosorption isotherm is generally used to describe how ions interact with carbon electrodes. The Langmuir and Freundlich isotherms are the two most common isotherms, and they were employed for simulating the ion adsorption on the 9-CNT/mwGO/RVC electrode. The electrosorption isotherms of NaCl onto the 9-CNT/mwGO/RVC electrode were evaluated, and their results were compared with the results of the CNT/RVC electrode. This experiment was performed using the different concentrations of NaCl as presented in Figure6. It is observed from the figure that the trend of the electrosorption capacity behaviour of both electrodes is the same and differs only in their magnitude. For both electrodes, the removal of NaCl has increased with the increase in concentration. This can be attributed to the enhancement of ions’ mass transfer rate inside the microporous electrodes [71, 76, 77]. The figure shows that the electrosorption capacity of 9-CNT/mwGO/RVC and CNT/RVC electrodes is 10.84 and 8.89 mg/g, respectively, at 500 mg/L feed concentration. This implies that combining mwGO with CNT materials has increased the number of adsorption sites in the 9-CNT/mwGO/RVC electrode under an electric field. Langmuir and Freundlich isotherms (shown in Supplementary section S14) were used to fit the experimental data for electrosorption of Na+ and Cl- onto the electrodes. The Langmuir isotherm is applicable to localized adsorbed ions with a limited adsorption amount [78], and the Freundlich isotherm is suitable for the description of ion adsorption with a wide variety of adsorption strength [79].Figure 6
The electrosorption isotherms for 9-CNT/mwGO/RVC and CNT/RVC electrodes at 1.5 V and 50 mL/min flow rate using different initial concentrations of the NaCl solutions.Table3 shows the comparison between Langmuir and Freundlich isotherms for the NaCl electrosorption using both electrodes. It is revealed that the electrosorption isotherm of both electrodes obeys both models, when considering the R2 values (better than 99.9% confidence level). The regression coefficients for CNT/RVC were 0.997 and 0.989 and for the 9-CNT/mwGO/RVC electrode were 0.995 and 0.981 for the Langmuir and Freundlich isotherms, respectively. These results suggest that the monolayer adsorption is the primary adsorption mechanism during the electrosorption process [70, 72]. The KL values of both electrodes are 0.01, and the KF values of CNT/RVC and 9-CNT/mwGO/RVC electrodes are 0.28 and 0.32, respectively. Normally, a higher value of n between 1 and 10 represents more beneficial adsorption [64], and the volume of n for both electrodes was around 1.74. Hence, the electrodes with a high value of n exhibit a high potential for electrosorption capability. In this type of system, the adsorbed layer is extremely thin, and the amount adsorbed is only a fraction of the monolayer capacity. Therefore, the electrosorption for both electrodes is followed by the monolayer adsorption [56]. Additionally, as a standard procedure, in order to calculate the maximum electrosorption amount of electrodes, the term qm in the Langmuir equation has been considered as the maximum adsorption capacity. The results show that the qm has improved with the increase in bias concentration. The qm measured at polarization of 1.5 V and a flow rate of 50 mL/min was 13.08 and 16.59 mg/g using CNT/RVC and 9-CNT/mwGO/RVC electrodes, respectively. Hence, it can be suggested that the maximum adsorption capacity qm for NaCl on the 9-CNT/mwGO/RVC electrode has improved compared to the CNT/RVC electrode. When considering a concentration of 500 mg/L NaCl, the qm at equilibrium for the CNT/RVC electrode is much higher compared to multiwalled carbon nanotubes (MWCNTs) [72] and activated carbon (AC) [80], which were 3.10 mg/g and 9.72 mg/g, respectively. This is because the surface area and average pore size in the CNT/RVC electrode are larger, where the surface area in MWCNTs and AC electrodes was 153 and 1153 m2/g [72, 80], respectively. In addition, the qm of the CNT/RVC electrode is very close to the qm of composite made from carbon nanotubes and carbon nanofiber (CNTs-CNFs) electrode, which was 13.35 mg/g [71]. The maximum electrosorption capacity results of 9-CNT/mwGO/RVC and CNT/RVC electrodes are lower than the graphene electrode, which was 21.04 mg/g [56]. This graphene electrode mainly consists of mesopores with an average pore diameter of about 7.42 nm, which is greatly beneficial to a capacitive deionization system.Table 3
The parameters of Langmuir and Freundlich isotherms for the NaCl electrosorption using the 9-CNT/mwGO/RVC and CNT/RVC electrodes.
IsothermParameterValue9-CNT/mwGO/RVCValue∗CNT/RVCLangmuirqm (mg/g)16.5913.08KL (L/mg)0.010.01R20.9950.997FreundlichKF (L/mg)0.320.28n1.741.74R20.9810.989∗These results were calculated in article [61].


## 3.3.5. Water Production by a CDI System

The water production experiment and calculation were carried out at the NaCl feed solution concentration 75 mg/L. It has been shown earlier that 1 g of the 9:CNT/mwGO composite and CNT coated on 43.20 cm3 RVC electrode adsorbed 3.82 mg and 3.23 mg NaCl during 13 mins and 18 mins, respectively. Hence, the solution concentration was reduced from 75 mg/L to 71.18 mg/L and 71.77 mg/L for 9:CNT/mwGO/RVC and CNT/RVC electrodes, respectively, after 1 desalination cycle. Moreover, it has also been shown that the electrosorption capacity varied with the increase in solution concentration and exhibits a linear relationship below the concentration of 100 mg/L (Figure 6). The abovementioned claim has been confirmed by their linear fit as shown in Figure 7(a) where plots for 9:CNT/mwGO/RVC and CNT/RVC composite electrodes are based on Equations (1) and (2), respectively.Figure 7
(a) The variation of electrosorption with respect to feed concentration and (b) the variation of feed concentration with respect to desalination cycles.
(a)(b)For the 9:CNT/mwGO/RVC composite electrode,(1)Electrosorptionmg/g=0.050∗concentration.For the CNT/RVC composite electrode,(2)Electrosorptionmg/g=0.042∗concentration.From these equations, the variation of concentration can be known after each desalination cycle. Figure7(b) represents the variation of concentration with respect to the desalination cycle. The reading was noted till the concentration was reached less than 1 mg/L using 1 g of the CNT/mwGO composite or CNT coated on a 43.20 cm3 RVC electrode. It is observed from the figure that the CNT/RVC electrode when used in a CDI system required 103 desalination cycles for reducing solution concentration from 75 mg/L to 1 mg/L. As each desalination cycle for this electrode takes 18 mins, hence, the total time required is 1854 mins (18min×103 cycles) for the production of 1 L of water that contains the NaCl concentration of less than 1 mg/L. Thus, the desalinated water produced per day is 0.78 L using 1 g of CNT coated on a 43.20 cm3 RVC electrode, or 17,855 L using 1 m3 of the same composite electrode. On the other hand, by using the 9-CNT/mwGO/RVC electrode in a CDI system, it is required 85 desalination cycles for the reduction of the same amount of solution concentration. This indicates that this electrode takes time for about 1105 mins (13min×85 cycles) to produce 1 L desalinated water where it contains the same NaCl concentration. Thus, the water produced per day is 1.30 L using 1 g of 9-CNT/mwGO coated on a 43.20 cm3 RVC electrode or 29,958 L using 1 m3 of the same composite electrode. Hence, it can be inferred that the 9-CNT/mwGO/RVC composite electrode produced 67.78% more desalinated water per day compared to the CNT/RVC composite electrode when used in the same CDI system.


## 4. Conclusions

The CNT/mwGO composites at their different ratios were successfully coated on the RVC electrode to prepare 3D electrodes and used in the CDI cell. The results showed that the optimal electrode had very high CDI cyclic stability, maintaining an electrochemical cycling stability of 100% when measured up to five cycles. Moreover, the time saving of one electrosorption-desorption cycle with the 9-CNT/mwGO/RVC electrode was 27.78%, compared with the CNT/RVC electrode, which required 18 min. In addition, the electrosorption removal of NaCl by the 9-CNT/mwGO/RVC electrode in terms of mass of the electrode (3.82 mg/g) increased 18.27% compared to the CNT/RVC electrode (3.23 mg/g) when measured at the optimum condition. The optimum electrode, 9-CNT/mwGO/RVC composite, showed a 67.78% increment per day in the desalinated water production compared to the CNT/RVC electrode at their same testing condition. The optimum electrode performed the highest 29,958 L production of water per day when using an electrode size of 1 m3. Moreover, the highest electrosorption capacity has resulted from the same electrode that is 10.84 mg/g at the solution feed concentration 500 mg/L, whereas the theoretically calculated value through the Langmuir isotherm showed the maximum electrosorption capacity value of 16.59 mg/g. The results for the 9-CNT/mwGO/RVC composite electrode demonstrate that it can be a promising electrode material in CDI technology.



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*Source: 5165281-2020-09-07.xml*