Environ Eng Res > Volume 25(1); 2020 > Article
Singh, Srivastava, Goyal, and Mall: Breakthrough modeling of furfural sorption behavior in a bagasse fly ash packed bed

### Abstract

Adsorptive breakthrough modelling is essential for design of a sorption packed bed. In this work, breakthrough modelling of the furfural uptake in bagasse fly ash (BFA) packed bed has been performed. Effect of various parameters like bed height (Z = 15–60 cm), flow rate (Q = 0.02–0.04 L/min) and initial furfural concentration (Co = 50-200 mg/L) on the breakthrough curve of furfural sorption in a BFA packed bed have been studied. Enhanced breakthrough performance was observed for the higher value of Z, and lower values of Co and Q. For Co = 100 mg/L, packed bed operated at Q = 0.03 L/min and Z = 60 cm was found to have lowest adsorbent utilization rate of 5.61 g/L with highest breakthrough volume of 14.67 L. Bed depth service time and Thomas models well represented the experimental data points under all experimental conditions. It can be concluded that BFA can be utilized efficiently in continuous system for the removal of furfural. Overall, more than 99% of furfural was adsorbed in BFA packed bed at experimental conditions.

### 1. Introduction

Various solvents are used in the petroleum refinery to meet the increasing demand of high quality fuels. Furfural is one of the popular solvents used in lube extraction unit in petroleum refineries. Besides this, usage or production of furfural is being practiced during various processes in numerous industries such as paper and pulp industry, pharmaceutical industry, petroleum refining, petrochemical and food industries [1, 2]. It finds its application as weed killer, flavoring agent, fungicide, and also as an intermediate in chemical reactions [3]. During these processes, furfural gets discharged into wastewater streams. Furfural is highly toxic in nature, and its presence in water makes it unusable. Further inebriating effects include ecstasy, giddiness, headache, queasiness, and eventual fainting and death due to breath loss. Prolonged skin exposure to furfural can cause skin allergy as well as an abnormal vulnerability to sunburn. Thus, to make it safe to use for domestic and industrial purpose, a thriving interest is seen nowadays for furfural removal from wastewater.
The work presented here aims to report the performance of BFA packed bed for furfural adsorptive removal from its aqueous solution. The effects of bed height (Z), flow rate (Q) and initial furfural concentration (Co) on the breakthrough point are also presented. Results of studies on testing of various models to predict the breakthrough curves are also presented.

### 2. Materials and Methods

BFA, used as an adsorbent in the present study, was obtained from a nearby sugar mill. It was used as such without any kind of pre-treatment. Exhaustive physico-chemical traits of the BFA are already presented the literature [1113]. The average particle size of BFA was 167.35 μm. Proximate analysis manifested the presence of 7.6% moisture, 17.4% volatile matter, 26.4% ash and 49.6% fixed carbon in BFA. Bulk density of BFA was determined as 133.3 kg/m3. The d-spacing values provided by the XRD spectra of BFA reflected the presence of alumina (Al2O3), silica (SiO2), CaO, CaSiO3, and Ca8Si5O18. The pore surface area of BFA was found to be 171 m2/g, whereas BJH adsorption/desorption surface area of pores was 54.2/49.9 m2/g. The average pore diameter of BFA was found to be 23.9 Å whereas the BJH adsorption/desorption average pore diameter was 39.4 Å/33.9 Å.

The concentration of furfural was determined by using UV-spectrophotometer (HACH, DR/5,000). Maximum absorbance for this was obtained at a wavelength (λmax) of 277 nm and the same was used to plot a model graph to relate absorbance and furfural concentration in the solution. The graph showed linear limit up to maximum furfural concentration of 10 mg/L. Therefore, for reliable determination of the furfural in samples, dilution was done using distilled/milliQ water, for the samples having a concentration higher than 10 mg/L of furfural so as to lower the concentration of furfural below 10 mg/L [1].

### 2.3. Column Studies

Schematic representation of experimental set up is given in Fig. 1. A thermostatic heating device was used in the chamber in which the column assembly was kept so as to control the temperature and maintained at 303 ± 1 K. A plexiglas column having inside diameter (D) of 2.54 cm and length 90 cm was used for the experimental studies. The feed port for the column was provided at the bottom center of the column. Glass beads of 0.2–0.3 cm diameter were used to fill the lower portion of the column up to a height of 1.5 cm. This was done to distribute the solution uniformly across the whole cross section of the column. Varying heights (Z = 15, 30, 45 and 60 cm) were chosen from the bottom to pack BFA in the column. Aqueous solution of furfural was pumped (upward flow) to bed using a peristaltic pump (Miclins PP20). The Co and Q were varied in the range of 50–200 mg/L and 0.02–0.04 L/min, respectively. pH of the furfural solution in all experiments was 5.5.
To achieve 100% wettability of packing inside the bed, an upward flow was adopted in the study presented. If done otherwise, it necessitated the use of specifically modelled distributors of liquid such that complete distribution of liquid is achieved inside bed [14]. Often, the holdup decreases as the liquid flow rate falls and the disturbance it causes in distribution of liquid poses great threat to the process efficacy [15, 16].

### 2.4. Theory: Behavior of Packed-bed Sorption Columns

A typical experimental breakthrough curve is shown in Fig. 2(a). It was found that the furfural adsorbed on BFA was initially rapid such that the bulk solution released from the bed was having zero furfural in it. But the BFA started to satiate gradually as the furfural containing feed is fed for further time, and as a result, the amount of furfural in the bulk solution at outlet started to increase until the bed fully gets satiated. During actual operation, process is suspended as the amount of furfural in outlet solution increases up to a specified limit, known as breakthrough concentration, after which it is not suggested to proceed with the process. In the present study, the operation is continued till the bed reaches its satiation point. During estimation of typical variables of the system, breakthrough amount of furfural CBP (10% of Co) was set, and the time corresponding to this concentration was considered as breakthrough time (tBP).
The idea of the mass transfer zone (MTZ) was initially introduced in fixed bed columns’ operation to understand the evolution patterns of the various parameters and to plan an efficient model for better performance during sorption in a fixed bed column [17, 18]. Significant sorption at any adsorbate inside the bed occurs in this MTZ [19]. Fractional capacity (F), the height of MTZ (HZ) and the speed of the MTZ along the bed height (UZ) determine the characteristics of the MTZ. They help us understand the way the adsorption process inside the bed advances. Various parameters of system can be expressed directly or indirectly using these parameters that control the overall sorption inside the bed. F is the term obtained when the proportional amount of adsorbent actually involved in sorption is divided by the total amount of adsorbent utilized for MTZ. In other words, it can be stated as the ratio of actual amount of adsorbate removed from the solution to the ideal extent of adsorbate removal by the adsorbent within the MTZ [1719]. F is given as:
##### (1)
$F=AZAmx=∫VBPVE(Co-C)dVCo(VE-VBP)=∫tBPtE(1-(C/Co))dt(tE-tBP)$
where, VE is the bulk amount of effluent treated at the point of exhaustion time (tE) with immediate concentration (CE) equivalent to 90% of the amount in effluent (Co) at the start of process. Based on the fashion in which the bed is operating, this amount in effluent in selected randomly while keeping the process as economized as possible. VBP is the bulk amount of effluent treated at point of breakthrough time (tBP) with immediate concentration (CBP) which is lower than 10% of the amount present at the start of the process.
HZ is the area where practically all sorption takes place. It plays a significant role in evaluating the removal rate of adsorbate by the BFA, and guides regarding the diffusion resistances present during the process. The lower the resistance offered by the system, more the kinetics of uptake of adsorbate paces and shorter is the height of MTZ at any given instant. Thus, it proves to be a significant variable in figuratively estimating the overall kinetics of the uptake during the process. HZ is formulated as:
##### (2)
$HZ=Z(tE-tBP)tBP+F(tE-tBP)$
UZ is basically used to evaluate the behavior of sorption in a fixed bed with continuous flow when a state of equilibrium is reached. It is basically an output function corresponding to the adsorbent’s uptake potential, and thus, allows estimating the bed saturation rate. Being directly proportional to HZ, it shows that as the HZ decreases, uptake rate of adsorbate increases, and the fixed bed satiates at a much faster rate [1719]. UZ is given as:
##### (3)
$UZ=HZtZ=ZtBP+F(tE-tBP)$
In order to find the efficacy of overall bed, we need to find number of unit transfer equivalents (NZ) [17]. It is given as:
##### (4)
$NZ=HBPHZ=tBP+F(tE-tBP)(tE-tBP)$
For a rapid uptake of adsorbate by adsorbent, lesser is HZ and higher is NZ. Other than this, during a dynamic uptake process, larger values of NZ is avoided in order to avoid the rapid satiation of bed.

### 3.1. Effect of Initial Furfural Concentration

The influence of Co on breakthrough curves is shown by data points in Fig. 2(a) and the results are tabulated in Table 1. It is evident from the figure that t0.1 decreased with an increase in the Co. At lower Co, curves were sparser and breakthrough occurred sluggishly. As the value of Co increased, the slope of breakthrough increased [20]. These results establish that any alteration in concentration gradient also alters the bed usage rate and the breakthrough time [21]. This occurs because large number of sorption sites gets occupied with an increase in Co. As the value of Co increases, mass transfer driving force is seen to over-power the resistance offered by solution [22, 23]. This phenomenon helps the bed to increase its fractional capacity (F). Also, along with the increase in furfural loading rate, which further causes the shortening of the sorption zone length (HZ) due to the increase in kinetics of process [17, 24]. As NZ varies inversely to HZ, a rise in its value is seen on the onset of increase in Co. Also, due to rapid satiation of sorption sites, UZ is seen to increase progressively with the increase in Co [18, 25].
The effect of Co on F, HZ, UZ and NZ is shown in Fig. 3(a) and (b). The value of F (as per expectation) can be seen increasing from the graph as Co increases, until a maximum capacity limit of 0.435 for Co (= 100 mg/L) is achieved. After this, Co doesn’t affect much on F as the bed has already reached its maximum fractional capacity due to increase in Co keeping every other parameters constant. In accordance to the increasing F, HZ can be seen decreasing to the point when Co reaches 100 mg/L making HZ minimum at 20 cm. Further this point, HZ again starts to increase as the bed reaches its limit of sorption capacity for the MTZ at any given instant. NZ rises to a maximum value of 3 at Co (= 100 mg/L) and further decreases as we increase Co. A fashion of rise and decline NZ is due to the decrease of MTZ height during the first phase when Co varies from 50–100 mg/L and then, increase in MTZ height after further increasing Co, respectively [19, 26]. Also, UZ is increasing as we move from (50–200) mg/L. UZ is basically related directly with the satiation of column and increasing Co ensured a rapid sorption.

### 3.2. Effect of Flow Rate

The breakthrough curves obtained for three Q (= 0.02, 0.03 and 0.04 L/min) at constant Z (= 60 cm) and Co (= 100 mg/L) were investigated. The experimental breakthrough times deduced from Fig. 2(b) are shown in Table 1. The value of t0.1 decreased as the value of Q increased. Inclusive of this, decreasing Q also resulted in the widening of breakthrough curve, which resulted in further increase in the difference between the breakthrough time and the saturation time. As anticipated, steeper curves with short mass transfer zone are seen due to reduction in breakthrough and exhaustion times, whenever there is a rise in Q [2628].
The effect of Q on F, HZ, UZ and NZ is shown in Fig. 3(c) and (d). At lower Q (0.02 and 0.03 L/min), resistance for transfer of furfural from solution to adsorbent is less, thus, the removal of adsorbate is faster. Therefore, HZ and UZ are less at lower Q (0.02 and 0.03 L/min) as compared to at higher Q (0.04 L/min). At lower Q (0.02 and 0.03 L/min), shorter HZ increases the value of NZ, therefore, the exhaustion of bed is better (i.e., better occupation of sites). This leads to increase in F. At higher Q (0.04 L/min), very less time is available for the volume element of solution to contact with the fixed bed which is inadequate to achieve equilibrium [19, 25]. This further leads to low sorption of adsorbate from the solution being fed at high Q.
The value of F is higher at Q = 0.03 L/min as compared to that at Q = 0.02 L/min. Generally, when Q is lowered, the liquid holdup gets decreased too and liquid maldistribution thus caused may show its impact on the efficacy of the bed [16]. At smaller liquid holdup, it is possible that some amount of the adsorbent may not get properly wet with the solution, and thus, don’t participate in the sorption process and stay unutilized. Also, this improper circulation of solution may cause liquid to flow through a favorable channel in the bed and leave the rest of bed untouched [29]. The lower value of F at Q = 0.02 L/min may be attributed to channeling. As per the recent developments, it is seen that larger values of Q > 0.03 L/min are generally not preferred as it leads to rapid arrival of breakthrough and lesser sharp-edged.

### 3.3. Effect of Bed Height

The breakthrough curves for furfural sorption (shown in Fig. 2(c) by data points) were investigated at four different Z (= 15, 30, 45 and 60 cm) at a constant Q = 0.02 L/min and Co = 100 mg/L. It can be seen that the tBP was lower for the lower values of Z, and increased with increase in Z due to the increase of the available surface area and binding sites for the furfural sorption. The breakthrough curves got flattened with an increase in Z. This is due to the widened mass transfer zone that cause breakthrough curve to be less steep. The breakthrough curves for the lowest Z showed a very little “tail” approaching saturation time because of the lesser amount of the BFA present inside the bed. As the value of Z is increased, a steep S shape breakthrough curve was seen [26, 28]. Due to intra-particle diffusion or non-idealities in flow at higher Z, breakthrough curves showed a broad tailing edge [30]. These results clearly reflect that the bed having greater value of Z was more difficult to completely exhaust as compared to bed having low value of Z [22, 25, 31, 32].

### 3.4. Empty Bed Contact Time and Adsorbent Usage Rate

Empty bed contact time (EBCT) can be calculated using the following equation:
##### (5)
$EBCT=VCQ=ACZQ$
The performance of an adsorbent packed bed is formulated in reference to the adsorbent usage rate (Ur). Ur is stated as the mass of adsorbent used per liter of solution treated [33].
##### (6)
$Ur=mCVBP=VcρVCNBP=ρNBP$
where, VC is the volume of the BFA in the packed-bed (L), AC is the cross-sectional area of the packed-bed (cm2), mC is the mass of the BFA in the packed-bed (g), VBP the volume of treated effluent discharged till breakthrough (L), ρ is the apparent density of the BFA (g/cm3) and NBP is the bed volumes of the effluent to breakthrough.
Choosing 10% breakthrough point as the end point, the values of EBCT and Ur were evaluated and the results are given in Table 1. As per the definitions, lower values of Ur and higher values of NBP are desirable. Obtained results show that Ur generally increased and NBP generally decreased with an increase in Z, Co and Q. Adsorbent mass has a negative effect on NBP and Ur. Higher values of Ur and lower values of NBP were found at higher Z. In spite of more binding sites available for sorption at higher Z, not all of them were accessible to the furfural molecules. This was due to operational problems such as axial dispersion, channeling and bed compaction [34, 35]. This behavior has been reported earlier as well [36]. For Co as variable parameter, it is obvious that higher amount of furfural at higher Co will exhaust the bed early and Ur values would be higher which is undesirable. The amount of furfural molecules that enter the packed-bed increase the adsorption rate, causing higher values of Ur and lower values of NBP. Similar results were found by other authors as well [36, 37]. With an increase in Q from 0.02 L/min to 0.03 L/min, positive effect (lower values of Ur and higher values of NBP) was observed. This was because of the decrease in film which offers mass transfer resistance around BFA particles [38]. However, further increase in Q to 0.04 L/min decreased the performance (higher values of Ur and lower values of NBP) because of the inadequate residence time of the liquid phase in the packed-bed and availability of less time for furfural diffusion into the pores of the BFA [39, 40].

### 3.5. Breakthrough Modeling

During sorption operation in any packed bed, the main motive is to minimize the concentration in the effluent so that it does not go beyond critical limited of CBP. During start, when the BFA is fresh and unsaturated, the actual effluent concentration does not exceed CBP. As pumping of furfural solution is continued through the bed, the BFA uptake capacity starts to decrease and the effluent concentration increasingly approaches CBP i.e., the breakthrough point is attained. Different models are utilized by researchers in the literature for the estimation of breakthrough time. In this current work, bed depth service time (BDST) and Thomas models have been utilized for the estimation of the breakthrough time for furfural sorption onto BFA. Srivastava et al. [33] have shared in the literature the theory linked to these models.
Earlier work on the BDST model was done by Bohart and Adams [41], who formulated a correlation between Z and breakthrough time (tBP). The description of initial phase of breakthrough curve is done generally using Bohart-Adams model [42]. As for the rest of the typical operational variables of the system, they can be evaluated from the plot of C/Co against t for a set value of Z and Q [25, 41]. Hutchins [43] linearized this model as follows:
##### (7)
$t=NoCoUZ-1kBColn (CoC-1)$
where, C is the desired concentration of the furfural at time t (mg/L), kB is the furfural sorption rate constant in the packed-bed (L/min mg), No is the adsorptive or saturation capacity of the BFA packed-bed (mg/L) and U is the linear flow velocity of the feed (cm/min). Here, the slope of the plot (No/CoU) represents the adsorptive capacity of the system whereas the intercept (I) gives the value of rate constant kB as per the following given equation [42]:
##### (8)
$I=-1kBColn (CoC-1)$
At halfway in breakthrough curve, when Co/C = 2 and t = t0.5, and therefore, the equation reduces as:
##### (9)
$t0.5=NoCoUZ$
Thus, it infers a linear plot of time passing through the origin for t0.5 against Z at 50% breakthrough, allowing No to be calculated. The dynamic behavior of the packed-bed sorption was predicted by BDST model given above and Thomas model given in subsequent paragraph. Coefficient of determination (R2) and Marquardt’s percent standard deviation (MPSD) were used to estimate the error between the experimental and calculated values of C/Co [33]:
##### (10)
$MPSD=1001N-P∑i=1n((C/C0)exp-(C/C0)cal(C/C0)exp)i2$
where, N represents the number of data points and P represents the number of parameters. The deviation between the experimental and calculated tBP was calculated by using the following equation:
##### (11)
$ɛ=100(tBP,exp-tBP,caltBP,exp)$
The plot of t0.5 and t0.1 obtained at constant Q = 0.02 L/min and Co = 100 mg/L are against four different Z (15, 30, 45 and 60 cm) is shown in Fig. 4. It gives a linear relationship. As stated, 50% breakthrough curve between t and Z should have been a linear plot passing through the origin, however, despite being linear it does not pass through origin. This indicates that a much more complex mechanism is involved in furfural uptake using BFA and that more than one rate-limiting step exists during the process [44]. No and k as calculated from the slope and the intercept of t0.1 versus Z plot are found to be 3,338 mg/L and 0.000562 L/mg min, respectively. No values showed deviation of 3.88% when compared with estimated using 10% breakthrough and 50% breakthrough plot. Fig. 2 shows the experimental and theoretical breakthrough curves predicted by BDST model at various experimental conditions. It shows a very good fit to the data up to 50% sorption of furfural. This suggests that the BDST model is valid for the relative concentration region up to 0.5. The values of No and kB as calculated from Eq. (7) are tabulated in Table 2. It is seen that the value of kB generally increases with an increase in Z and decrease in Q.
Thomas model [45] is based on the second order reaction kinetics. The linear form of the Thomas model is given as [18, 25, 46]:
##### (12)
$ln(CoC-1)=kTqomQ-kTCoQVeff$
where, kT is the Thomas rate constant (L/min mg), qo the maximum sorption capacity of the BFAe (mg/g), mC is the mass of the BFA in the column (g), and Veff is the throughput volume (L) [47]. The kT and qo can be determined from the intercept and the slope of the plot of ln[(Co/C)−1] against t at a given Q. Thomas model was applied to the data at C/Co ratios higher than 0.08 and lower than 0.99 with respect to Z, Co and Q [4850]. kT and qo values are shown in Table 3. Values of R2 were found to be > 0.9063. Sahu et al. [1] found that the sorption kinetics of furfural onto BFA was represented by second order kinetics. Therefore, Thomas model was expected to well-represent the breakthrough curves [26]. Fig. 5 shows the experimental and theoretical breakthrough curves obtained at different Z, Co and Q for the Thomas model. Fig. 5 and the data in Table 3 indicate that the t0.1 values as estimated using the Thomas model were very similar to those obtained from experimental results.
Comparison of the kinetic rate constants, kB and kT (L/mg min), obtained by modeling the experimental breakthrough curves with the Bohart-Adams and Thomas models shows some difference in values among them, however, they were of the same order of magnitude in general. No in Bohart-Adams model represents saturation capacity of the adsorbent bed whereas qo in the Thomas model represents the maximum adsorption capacity of the BFA. Values of No and qo generally decreased with an increase in Z. This is because of inaccessibility of all active sites despite the increase in active sites at higher Z value which can be attributed to problems such as axial dispersion, channeling and bed compaction [34, 35]. An increase in the value of No and qo was observed with an increase in Co and Q up to certain limit. Higher load of furfural in the BFA bed at higher Co and Q increased the driving force which increased the No and qo [51, 52]. Also, the reduction mass transfer resistance because of the decrease in the size of laminar boundary layer/film around BFA particles at higher Co and Q increased the No and qo values [38]. The obtained breakthrough curves for furfural removal by BFA fitted better by Bohart-Adams model. This illustrates that the furfural and the functional groups on the surface of BFA interacted via hydrogen bonding, dipole-dipole and hydrophobic interactions among furfural and these interaction played significant role in the adsorption process [53]. Since, Thomas model is not able to better-predict the breakthrough curves than Adams-Bohart model. Hence, the external and internal diffusions seem to be the limiting steps during the sorption process [52].

### 4. Conclusions

Sorption of furfural from aqueous solution onto BFA was studied using packed column at 303 K in a continuous fashion. Improvement in bed performance was observed with an increase in Z and decrease in Q and Co. For Co = 100 mg/L, packed bed operated at Q = 0.03 L/min and Z = 60 cm was found to have lowest adsorbent utilization rate (Ur) of 5.61 g/L with highest breakthrough volume (VBP) of 14.67 L. Adam-Bohart model well predicted the breakthrough curve up to 50% breakthrough at all Z, Co and Q. Adsorptive capacity of BFA as calculated from C/Co BDST model for 10% breakthrough plot was 3,338 mg/L. Thomas model was also applied at C/Co higher than 0.08 and lower than 0.99 for the prediction of breakthrough curves. Thomas model was found to be appropriate to explain the dynamic behavior of overall column or a section of the column in association to all Z, Co and Q.

#### Nomenclature

NBP

bed volumes to breakthrough

NZ

number of unit transfer equivalents

P

number of parameters

Q

volumetric flow rate (L/min)

qo

maximum solid-phase concentration of the solute (mg/g)

t

contact time (min)

tBP

breakthrough time (min)

t0.1

time for 10% adsorbate breakthrough (min)

t0.5

time for 50% adsorbate breakthrough (min)

tE

exhaustion time (min)

U

linear flow velocity of the feed to the bed (m/min)

Ur

UZ

velocity of the MTZ along the bed height (m/min)

VBP

volume of solution treated at breakthrough (L)

VC

volume of the sorbent in the bed (L)

Veff

throughput volume (L)

VE

bulk amount of effluent treated at the point of exhaustion time (L)

Z

height of the sorbent bed in the column (cm)

ɛ

percent deviation between the experimental and theoretical time for the breakthrough

ρ

apparent density of adsorbent in column (g/cm3)

### References

1. Sahu AK, Mall ID, Srivastava VCStudies on the adsorption of furfural from aqueous solution onto low-cost bagasse fly ash. Chem Eng Commun. 2008;195:316–335.

2. Sahu AK, Mall ID, Srivastava VCAdsorption of furfural from aqueous solution onto activated carbon: Kinetic, equilibrium and thermodynamic study. Sep Sci Technol. 2008;43:1239–1259.

3. Steyermark AKirk-Othmer encyclopedia of chemical technology. 14:3rd edMicrochemical Journal. New Jersey: John Wiley & Sons, Inc; 1984.

4. Pitter PDetermination of biological degradability of organic substances. Water Res. 1976;10:231–235.

5. Rivard CJ, Grohmann KDegradation of furfural (2-furaldehyde) to methane and carbon dioxide by anaerobic consortium. Appl Biochem Biotechnol. 1991;28:285–295.

6. Borghei SM, Hosseini SNComparison of furfural degradation by different photooxidation methods. Chem Eng J. 2008;139:482–488.

7. Gupta P, Nanoti A, Garg MO, Goswami ANThe removal of furfural from water by adsorption with polymeric resins. Sep Sci Technol. 2001;36:2835–2844.

8. Lucas S, Cocero MJ, Zetzl C, Brunner GAdsorption isotherms for ethylacetate and furfural on activated carbon from supercritical carbon dioxide. Fluid Phase Equilibria. 2004;219:171–179.

9. Mall ID, Srivastava VC, Kumar GVA, Mishra IMCharacterization and utilization of mesoporous fertilizer plant waste carbon for adsorptive removal of dyes from aqueous solution. Colloids Surf A: Physicochem Eng Asp. 2006;278:175–187.

10. Mane V, Mall ID, Srivastava VCKinetic and equilibrium isotherm studies for the adsorptive removal of brilliant green dye from aqueous solution by rise husk ash. J Environ Manage. 2007;84:390–400.

11. Srivastava VC, Mall ID, Mishra IMTreatment of pulp and paper mill wastewaters with poly aluminium chloride and bagasse fly ash. Colloids Surf A: Physicochem Eng Asp. 2005;260:17–28.

12. Srivastava VC, Mall ID, Mishra IMModelling individual and competitive adsorption of cadmium(II) and zinc(II) metal ions from aqueous solution onto bagasse fly ash. Sep Sci Technol. 2006;41:2685–2710.

13. Srivastava VC, Mall ID, Mishra IMAdsorption thermodynamics and isosteric heat of adsorption of toxic metal ions onto bagasse fly ash (BFA) and rice husk ash (RHA). Chem Eng J. 2007;132:267–278.

14. Treybal REMass-transfer operations. 3rd edMcGraw-Hill International Editions; 1981.

15. Inglezakis VJ, Hadjiandreou KJ, Loizidou MD, Grigoropoulou HPPretreatment of natural clinoptilolite in a laboratory-scale ion exchange packed bed. Water Res. 2001;35:2161–2166.

16. Milan Z, Sanchez E, Weiland P, et alAmmonia removal from anaerobically treated piggery manure by ion exchange in columns packed with homoionic zeolite. Chem Eng J. 1997;66:65–71.

17. Namane A, Hellal AThe dynamic adsorption characteristics of phenol by granular activated carbon. J Hazard Mater. 2006;137:618–625.

18. Gilca E, Maicaneanu A, Ilea PKinetics analysis of zinc sorption in fixed bed column using a strongly basic anionic exchange resin. Water Sci Technol. 2015;71:1646–1653.

19. Yazid H, Amour L, Terkmani A, Maachi RBiosorption of lead from aqueous solution by biologically activated date pedicels: Batch and column study. Desalin Water Treat. 2013;51:1690–1699.

20. Sulaymon AH, Yousif SA, Al-Faize MMCompetitive biosorption of lead, mercury, chromium and arsenic ions onto activated sludge in fixed bed adsorber. J Taiwan Inst Chem Eng. 2014;45:325–337.

21. Goel J, Kadirvelu K, Rajagopal C, Garg VKRemoval of lead(II) by adsorption using treated granular activated carbon: Batch and column studies. J Hazard Mater. 2005;125:211–220.

22. Thanhmingliana , Lalhriatpuia C, Tiwari D, Lee SMEfficient removal of 17β-estradiol using hybrid clay materials: Batch and column studies. Environ Eng Res. 2016;21:203–210.

23. Vera LM, Bermejo D, Uguña MF, Garcia N, Flores M, González EFixed bed column modeling of lead(II) and cadmium(II) ions biosorption on sugarcane bagasse. Environ Eng Res. 2018;24:31–37.

24. Han R, Ding D, Xu Y, et alUse of rice husk for the adsorption of congo red from aqueous solution in column mode. Bioresour Technol. 2002;99:2938–2946.

25. Gobi K, Mashitah MD, Vadivelu VMUtilising waste activated sludge from a palm oil mill effluent treatment plant to remove methylene blue in continuous column studies. Int J Environ Eng. 2012;4:253–268.

26. Sadaf S, Bhatti HNBatch and fixed bed column studies for the removal of Indosol Yellow BG dye by peanut husk. J Taiwan Inst Chem Eng. 2014;45:541–553.

27. Lodeiro P, Cordero B, Grille Z, Herrero R, Sde VPhysicochemical studies of cadmium(II) biosorption by the invasive alga in Europe. Sargassum muticum Biotechnol Bioeng. 2004;88:237–247.

28. Lee I, Park JA, Kang JK, et alBatch and flow-through column studies for Cr(VI) sorption to activated carbon fiber. Environ Eng Res. 2014;19:157–163.

29. Inglezakis VJ, Lemonidou M, Grigoropoulou HPLiquid holdup and dispersion in zeolite packed beds. Chem Eng Sci. 2001;56:5049–5057.

30. Cooney DOAdsorption design for wastewater treatment. Boca Raton, FL: Lewis Publishers; 1999.

31. Netpradit S, Thiravetyan P, Towprayoon SEvaluation of metal hydroxide sludge for reactive dye adsorption in a fixed bed column system. Water Res. 2004;38:71–78.

32. Zulfadhly Z, Mashitah MD, Bhatia SHeavy metals removal in fixed bed column by macro fungus Pycnoporus sanguineus . Environ Pollut. 2001;112:463–470.

33. Srivastava VC, Prasad B, Mishra IM, Mall ID, Swamy MMPrediction of breakthrough curves for sorptive removal of phenol by bagasse fly ash packed bed. Ind Eng Chem Res. 2008;47:1603–1613.

34. McCabe WL, Smith JC, Harriott PUnit operations of chemical engineering. 5th edSingapore: McGraw-Hill International Editions; 1993.

35. de Franco MAE, de Carvalho CB, Bonetto MM, Soares RP, Feris LARemoval of amoxicillin from water by adsorption onto activated carbon in batch process and fixed bed column: Kinetics, isotherms, experimental design and breakthrough curves modelling. J Clean Prod. 2017;161:947–956.

36. de Franco MAE, de Carvalho CB, Bonetto MM, Soares RP, Feris LADiclofenac removal from water by adsorption using activated carbon in batch mode and fixed-bed column: Isotherms, thermodynamic study and breakthrough curves modeling. J Clean Prod. 2018;181:145–154.

37. Sotelo JL, Ovejero G, Rodríguez A, Alvarez S, Galan J, García JCompetitive adsorption studies of caffeine and diclofenac aqueous solutions by activated carbon. Chem Eng J. 2014;240:443–453.

38. Mthombeni NH, Mbakop S, Ray SC, Leswifi T, Ochieng Aoyi, Onyango MSHighly efficient removal of chromium(VI) through adsorption and reduction: A column dynamic study using magnetized natural zeolite polypyrrole composite. J Environ Chem Eng. 2018;6:4008–4017.

39. Lin S, Song Z, Che G, et alAdsorption behavior of metal-organic frameworks for methylene blue from aqueous solution. Micro Meso Mater. 2014;193:27–34.

40. Hayati B, Maleki A, Najafi F, et alHeavy metal adsorption using PAMAM/CNT nanocomposite from aqueous solution in batch and continuous fixed bed systems. Chem Eng J. 2018;346:258–270.

41. Bohart G, Adams EQSome aspects of the behavior of charcoal with respect to chlorine. J Am Chem Soc. 1920;42:523–544.

42. Hadi M, Samarghandi MR, McKay GSimplified fixed bed design models for the adsorption of acid dyes on novel pine cone derived activated carbon. Water Air Soil Pollut. 2011;218:197–212.

43. Hutchins RANew method simplifies design of activated-carbon system. Chem Eng. 1973;80:133–138.

44. Sharma DC, Foster CFColumn studies into the adsorption of chromium(VI) using sphagnum moss peat. Bioresour Technol. 1995;52:261–267.

45. Thomas HCHeterogeneous ion exchange in a flowing system. J Am Chem Soc. 1944;66:1664–1666.

46. Zeinali F, Ghoreyshi AA, Najafpour GRemoval of toluene and dichloromethane from aqueous phase by granular activated carbon (GAC). Chem Eng Commun. 2012;199:203–220.

47. Dorado AD, Gamisans X, Valderrama C, Sole M, Lao CCr(III) removal from aqueous solutions: A straightforward model approaching of the adsorption in a fixed-bed column. J Environ Sci Health A Toxic Hazard Subst Environ Eng. 2014;49:179–186.

48. Aksu Z, Gonen FBiosorption of phenol by immobilized activated sludge in a continuous packed bed: Prediction of breakthrough curves. Process Biochem. 2004;39:599–613.

49. Ghali AE, Baouabb MHV, Roudeslia MSPreparation, characterization and application of a [copper(II)/ethylenediamine-cotton] complex for the removal of AB25 from aqueous solution in a laboratory scale column. Chem Eng J. 2011;174:18–26.

50. Singh S, Srivastava VC, Mall IDFixed-bed study for adsorptive removal of furfural by activated carbon. Colloids Surf A: Physicochem Eng Asp. 2009;332:50–56.

51. Xu X, Gao B, Tan X, et alNitrate adsorption by stratified wheat straw resin in lab-scale columns. Chem Eng J. 2013;226:1–6.

52. Gouran-Orimi R, Mirzayi B, Nematollahzadeh A, Tardast ACompetitive adsorption of nitrate in fixed-bed column packed with bio-inspired polydopamine coated zeolite. J Environ Chem Eng. 2018;6:2232–2240.

53. Niasar HS, Das Sreejon, Xu C, Ray MBContinuous column adsorption of naphthenic acids from synthetic and real oil sands process-affected water (OSPW) using carbon-based adsorbents. Chemosphere. 2019;214:511–518.

##### Fig. 1
Schematic diagram of experimental set up. (1) Reservoir tank with aqueous solution of furfural, (2) peristaltic pump, (3) supporting flange, (4) glass beads, (5) column, (6) filter media, (7) effluent storage.
##### Fig. 2
Comparison of experimental and theoretical breakthrough curves for furfural sorption on BFA packed bed using the Bohart Adams model. Experimental values are shown by data points, and model predictions are represented by lines. (a) At varied Co: Q = 0.02 L/min, Z = 60 cm. (b) At varied Q: C0 = 100 mg/L, Z = 60 cm. (c) At varied Z: Co = 100 mg/L, Q = 0.02 L/min.
##### Fig. 3
The effect of initial furfural concentration (Co), flow rate (Q) and bed height (Z) on fractional capacity (F), the height of mass transfer zone, MTZ (Hz) and the rate of the movement of the MTZ (UZ), and number of mass transfer units (Nz).
##### Fig. 4
BDST plot of breakthrough time versus bed height for furfural sorption onto BFA packed bed.
##### Fig. 5
Comparison of experimental and theoretical breakthrough curves for furfural sorption on BFA packed bed using the Thomas model. Experimental values are shown by data points, and model predictions are represented by lines (a) At varied Co: Q = 0.02 L/min, Z = 60 cm. (b) At varied Q: C0 = 100 mg/L, Z = 60 cm. (c) At varied Z: Co = 100 mg/L, Q = 0.02 L/min.
##### Table 1
BFA Packed Bed Performance for Furfural Sorption
Co (mg/L) Q (L/min) Z (cm) EBCT (min) tBP (min) VBP (L) NBP Ur (g/L)
100 0.02 15 3.80 193.35 3.87 50.86 5.32
100 0.02 30 7.60 248.80 4.98 32.72 8.27
100 0.02 45 11.40 426.31 8.53 37.38 7.24
100 0.02 60 15.21 557.30 11.16 36.65 7.38
50 0.02 60 15.21 700.10 14.01 46.04 5.88
100 0.02 60 15.21 557.30 11.15 36.65 7.38
200 0.02 60 15.21 227.61 4.55 14.97 18.07
100 0.02 60 15.21 557.30 11.15 36.65 7.38
100 0.03 60 10.14 488.70 14.67 48.21 5.61
100 0.04 60 7.61 200.16 8.01 26.33 10.28
##### Table 2
Co (mg/L) Q (L/min) Z (cm) kB × 105 (L/mg min) No (mg/L) tBP,exp (min) tBP,cal (min) ɛ R2 MPSD
100 0.02 15 26.97 7,775 193 210 8.68 0.9501 60.75
100 0.02 30 24.65 4,704 248 264 6.16 0.9419 71.09
100 0.02 45 37.70 4,369 426 437 2.50 0.9813 80.12
100 0.02 60 37.94 4,341 557 599 7.50 0.9133 92.92
50 0.02 60 24.38 3,069 700 744 6.32 0.8883 436.43
100 0.02 60 37.94 4,341 557 599 7.53 0.9133 429.62
200 0.02 60 13.17 4,444 227 250 10.00 0.9647 326.99
100 0.02 60 37.94 4,341 557 599 7.53 0.9133 438.67
100 0.03 60 19.42 6,408 488 531 8.65 0.9748 377.64
100 0.04 60 17.94 4,455 200 210 5.06 0.9531 570.54
##### Table 3
Parameters Estimated Using Thomas Model
Co (mg/L) Q (L/min) Z (cm) kT × 105 (L/mg min) qo (mg/g) tBP,exp (min) tBP,cal (min) ɛ R2 MPSD
100 0.02 15 48.22 3.59 193 205 6.09 0.9892 69.45
100 0.02 30 30.97 2.34 248 255 2.60 0.9895 68.56
100 0.02 45 27.82 2.38 426 418 1.77 0.9721 94.85
100 0.02 60 21.89 2.47 557 588 5.47 0.9370 152.35
50 0.02 60 14.05 1.72 700 646 7.72 0.9063 684.01
100 0.02 60 21.89 2.47 557 588 5.47 0.9370 427.13
200 0.02 60 11.38 2.34 227 230 0.96 0.9801 359.89
100 0.02 60 21.89 2.46 557 588 5.47 0.9370 436.13
100 0.03 60 23.27 3.28 488 515 5.30 0.9871 356.57
100 0.04 60 20.33 2.19 200 197 1.54 −0.9856 680.92
TOOLS
Full text via DOI
E-Mail
Print
Share:
METRICS
 0 Crossref
 0 Scopus
 450 View