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© 2019 JETIR February 2019, Volume 6, Issue 2 www.jetir.org (ISSN-2349-5162)
JETIRAB06067 Journal of Emerging Technologies and Innovative Research (JETIR) www.jetir.org 381
RHODAMINE 6G REMOVAL USING PROSOPIS SPICIGERA L. WOOD(PSLW)CARBON-IRON
OXIDE COMPOSITE
[1]R. Dhana Ramalakshmi,[2] V. Jeyabal,[3]M. Murugan
[1]Reg.No: 12583, Department of Chemistry, Rani Anna Government College for Women, Tirunelveli-627008,Research centre (St. Xavier's College, Tirunelveli-627002), affiliation of Manonmaniam
Sundaranar University, Abishekapatti, Tirunelveli-627012, Tamil Nadu, India. [2]Associate professor, Department of Chemistry, St. Xavier's College, Palayamkottai,Tirunelveli-
627002, Tamil Nadu, India. [3]Associate professor, Department of Chemistry, Sri K.G.S. Arts College, Srivaikuntam-628619,
Thoothukudi, Tamil Nadu, India. mail:[1][email protected], [2][email protected], [3][email protected]
Abstract:
Rhodamine 6G, a cationic dye is used to dyeing silk, cotton, wool, baste fiber, paper, leather, and
plastic. It is toxic and carcinogenic in nature. Hence it is essential to remove Rhodamine 6G from dyeing
industrial discharge and contaminated drinking water resources. In this present work, a waste plant
material Prosopis spicigera L.wood is carbonised (by natural process) and its composite with iron oxide,
is used for the removal of Rhodamine 6G from aqueous solutions by batch and column methods. The
PSLW carbon-iron oxide compositeis characterized by FTIR for functional group, scanning electron
microscope for surface morphology and potentiometric titration for pHzpc. Batch experiments have
been carried out to investigate the influence of sorption parameters such as initial dye concentration,
pH, contact time, in the presence of other ions and temperature on the removal of Rhodamine 6G. The
batch experiments were carried out at pH 6.0. The adsorption equilibrium fits Langmuir isotherm. The
kinetic data follows pseudo second order model. The thermodynamic study indicated that the
adsorption of dye is spontaneous and endothermic in nature. In order to apply this process to industrial
and domestic applications, column analysis was performed. Column data was analysed using Thomas
model.
Keywords: Adsorption, Kinetics, PSLW carbon, Langmuir Isotherm, Rhodamine 6G,Thomas model. Introduction
Dyes are colored compounds which are widely used in textiles, printing, cosmetics, plastics,
rubber and leather industries. These industrial effluents contain a large amount of colored wastewater
and pollute the environment. The usage of natural dye which is isolated from natural materials is limited.
The discovery of synthetic dyes and its wide range of uses such as fastness and brightness produce a
massive industrial effluents[1]. However, synthetic dyes have toxic behavior and adverse effect.
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The presence of dyes or their degradation products in water even at low concentration can cause
human health disorders like nausea, haemorrhage, ulceration of the skin, damage kidneys,
reproductive system, liver,brain and central nervous system[2]. It is difficult to remove these dyes using
conventional water treatment method because they are designed to have high water solubility [3]. Many
physical, chemical and biological methods are available for the removal of dye from aqueous system.
Among various physical methods, adsorption is one of the best method to successively remove them.
In sorption technique, adsorbents have a prominent role. The common adsorbents like activated
carbon, peat, wood, fly ash, coal and silica are used. Activated carbons are most widely used to remove
pollutants from aqueous solutions due to their high surface area, adsorption capacity and easily
availability. The adsorption capacity of activated carbon stillcan be increased by modifying the surface
of carbon. One such process is composite formation with iron metal oxides. The magnetic particle
technology have received more attention to solve the environmental problems[4]. Compared to other
adsorbents, the magnetic composites are good adsorbents because of their large surface area, high
adsorption capacity and after adsorption, it can be easily separated from the medium by a simple
magnetic process. In our present study, a low-cost adsorbent i.e., Prosopis spicigera L. wood (PSLW)
carbon and its iron oxide composite which is used for Rhodamine 6G removal. The effect of pH, contact
time, initial concentration, adsorbent dosage, presence of other ions and temperature of Rhodamine
6G solution on PSLW carbon-iron oxide composite were examined. The equilibrium and kinetic data of
the adsorption process were then analyzed to study the adsorption isotherms, kinetics and
thermodynamic parameters.
MATERIALS AND METHODS
Materials
PSLW plant material used in the present work was collected from the dry land area of
Palayamkottai in Tirunelveli district, Tamilnadu state, India. The branch and roots of the plant were cut
into pieces and piled up on a firing hearth. Before firing, the heaped wood pieces were enclosed by
fresh plantain pith and the whole mass was covered and plastered with layers of wet clay. This
arrangement prevented the direct entry of air into wood pieces and hence prohibited burning of wood
and its becoming ash. After 48 h of continuous firing and subsequent natural cooling, the activated
carbon was obtained. After removing the non-carbonaceous materials the carbon was isolated,
crushed and sieved to 75 micron particles. The composite adsorbent was prepared using the slightly
modified literature procedure [5],[6]. 20 g of PSLW carbon was suspended in 400 mlof FeCl3(7.8 g, 28
mmol) and FeSO4 (3.9 g, 14 mmol) at 70℃. The above solution was stirred well using a magnetic stirrer
for 3 hours. Sodium hydroxide solution (100 ml, 5 mol/L) was added dropwise to precipitate the iron
oxides. Again the stirring was continued for another two hours at 70℃. Later the solid material was
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separated, washed with de-ionised water until the washings became neutral. Further the washings
were tested for iron with 1:10 phenonthroline for reddish color or precipitates. The final productwas
dried in an air oven at 100℃ for 8 hours and finally stored in air tight containers.
Characterisation of the adsorbent
The standard procedure [7], [8] was adopted to study the characteristics of PSLW carbon-iron
oxide composites.Surface functional groups and surface morphology of these adsorbent have been
analysed using FT-IR (JASCO FT/IR-4700 type A) and SEMrespectively. The morphological studies
SEM was performed on Jeol, JSM 6390, Oxford instruments, UK. Potentiometric titration with
acid/alkali was made to determine the zero point charge [9].
Batch Adsorption studies
The stock solution was prepared by dissolving 1 g of Rh 6G in 1000 mL of distilled water. The
stock solution was diluted with distilled water for further experimental studies. A digital pH meter with
glass electrode model (Roy instruments RI 501) was used for the measurement of pH of the dye
solution. The initial pH of the solution was varied (1-10) using 0.1 M NaOH or 0.1 M H2SO4 solutions.
Batch adsorption studies were carried out in 10 ml of dye solution. After adsorption, the solution was
centrifuged and absorbance was measured at 524 nm using UV–Visible spectrophotometer. The batch
experiments were studied to determine the effect of pH (1-10), initial concentration (10, 15 and 20
mg/L), contact time (5-150 min), in the presence of other ions (chloride, carbonate, nitrate and sulphate
ions) and temperature (20–50°C).
The amount of adsorbate adsorbed at equilibrium, qe (mg/g) was calculated as:
WVCCq ee (1)
Where, Co and Ce (mg/L) are the initial and equilibrium concentration of adsorbate respectively. V is
the volume of the solution (L) and W is the mass of adsorbent (g).
Column study
In column study, 5 g of PSLW carbon-iron oxide composite was packed in a glass column (2.5
cm diameter and 48 cm height) for a bed height of 3.5 cm. The dye solution was dropped into the
column at a rate of 2 mL/min from a separatory funnel fixed at a height of 1 meter. Effluents were
collected at regular intervals and analysed.
Results and Discussion
Characterisation of adsorbent
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The FTIR spectrum of PSLW carbon and its iron composite (Fig. 2) show that both of their
surface have very few bands with very weak intensities. This indicates the presence of meagre amount
of acidic and basic groups on their surface. Further the composite formation has little interaction with
the surface functional groups. SEM study is used to understand the changes of morphological features
during adsorption process. The comparative study of SEM images of free PSLW carbon and PSLW
carbon-iron composite (Fig. 3) reveals that the PSLW carbon powder has irregularly shaped particles
with porous structure whose size is further reduced in the composites. Further a coating of white
patches of iron oxide is seen on the surface of the PSLW carbon.
Fig. 1 structure of Rhodamine 6GFig.2 The FTIR spectrum of (a) pure PSLW carbon
(b) PSLW carbon-iron oxide composite (c) Rh 6G loaded carbon
4000 3600 3200 2800 2400 2000 1600 1200 800 400
(c)
(b)
(a)
Tran
sm
itta
nce (
%)
Wave number (cm-1)
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Fig.3 SEM images of (a) pure PSLW carbon (b) PSLW carbon-iron oxide composite (c) Rh 6G loaded
carbon
Effect of pH
The adsorbate and the surface charge of the adsorbent in aqueous solution are pH dependent,
which makes pH be one of the most important factors affecting dye
Fig. 4 Effect of pH Fig. 5 Effect of initial concentrations and contact time
adsorption ontothe adsorbent [10].Fig.4 shows, the removal of dye which increases with increase in
pH and maximum sorption is noted above pH = 8.0. The maximum adsorption above pH = 8.0 may be
due to electrostatic attraction between adsorbent and dye molecule [11], [12].The pHzpc of the
composite is 8.22 and it reveals that the surface of the adsorbent is positively charged. Therefore the
adsorption of Rhodamine 6G cationic dye on the PSLW carbon-iron oxide composite above pH=8.0
may be due to electrostatic interaction. But the desorption study with 0.1 N NaOH shows 90.5 % of the
Rhodamine 6G dye is desorped. Therefore the adsorption may involve weak interaction between the
dye molecule and the composite. This is evident from the IR spectral study. In the IR spectrum there
is no shift in the stretching frequencies of the PSLW carbon composite (Fig. 2c) and the spectrum is
only due to the adsorbed Rhodamine 6G molecule. Further SEM analysis after adsorption of
Rhodamine 6G onto the composite (Fig. 3c) shows the presence of aggregated larger size particles
0 2 4 6 8 10
0
2
4
6
8
10
12
14
16
Adsorbent dose 0.5 g/L
Concentration 50 mg/L
pH 1-10
Am
ount
adso
rbed
(m
g/g
)
pH
0 20 40 60 80 100 120 140 160
0
4
8
12
16
20
3
2
1
Adsorbent dose 0.5 g/L
pH 6
Concentration of Rh 6G
1. 10 mg/L
2. 15 mg/L
3. 20 mg/L
q (
mg/g
)
Time (min)
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with filled pores. This indicates the asorption of Rhodamine 6G molecule onto the composites. But as
an optium pH=6.0 is maintained throughout the adsorption study to apply this process to treat polluted
drinking water.
Effect of initial concentration and contact time
Fig.5shows the effect of initial concentration and contact time. The sorption process increases
with increase in contact time and attains equilibrium in 150 minutes. The maximum adsorption capacity
at three differentconcentrations of 10, 15 and 20 mg/Lare found to be 11.6, 16.4 and 18.3 mg/g
respectively for an adsorbent dose 0.5 g/L.
Effect of Temperature
Fig.6 depicts that the adsorption capacity of adsorbentincreases with increase in temperature
due to increase in dye mobility that may occur at high temperature between the adsorbent and the
adsorbate [13]. This indicates that the adsorption of dye is an endothermic process [14].
Fig. 6 Effect of temperature
Adsorption of dye in the presence of other ions
Adsorption capacity of PSLW carbon-iron oxide composite of the dye was examined in the
presence of mixture of chloride, carbonate, nitrate and sulphate ions of concentration 0.001 M each.
The adsorption capacity increases with time and equilibrium is reached at 60 min which is similar to
that of adsorption of dye in the absence of above ions. But the adsorption capacity decreases and this
may be due to competition between the ions and dye molecules for the same number of adsorption
sites.
Thermodynamic behavior
0 30 60 90 120 150
0
4
8
12
16
4
3
2
1
Adsorbent dose 0.5 g/L
pH 6
Concentration of Rh 6G 10 mg/L
1. 20
o C
2. 30o C
3. 40o C
4. 50o C
q (
mg
/g)
Time (min)
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The thermodynamic parameters, standard free energy (∆G°), standard enthalpy (∆H°)and
standard entropy (∆S°) were calculated using equations (2), (3)and (4).
kRTG ln (2)
RTHRSk ln (3)
STHG (4) where, T is
the temperature (K), R is the gas constant (8.314 J/mol k) and K is the equilibrium constant. A plot of
ln k versus l/T gives a straight line with slope ∆H°and intercept ∆S°.The values of the thermodynamic
parameters are listed in table I. The negative value of ∆G° which indicates the adsorption of dye on
PSLW carbon-iron oxide composite is a spontaneous process. The positive value of ∆H° shows the
adsorption process is endothermic. This reveals that the adsorption capacity increases with increase
in temperature. The ∆S° value increases with temperature, which indicates the randomness of
adsorption of dye on adsorbent surface. From thermodynamic parameters, the adsorption process is
spontaneous and endothermic [15], [16]. Thus, temperature plays a vital role in adsorption of dye on
PSLW carbon-iron oxide composite.
I. Thermodynamic parameters: Adsorbent dose 0.5 g/L
Isotherm Analysis
Adsorption isotherm is used to predict the mechanism of sorption process. The adsorption
capacity of the adsorbent was examined by Langmuir[17] and Freundlich[18] models. Langmuir and
Freundlich models are expressed by equations (5)and (6)
QCbQqC ee 1 (5)
ef CnKq log1loglog (6)
Temperature
(K)
- ∆G°
(KJ/mol)
∆H°
(KJ/mol)
∆S°
(KJ/mol K)
293
120.34
512.14
2.16
303
313
115.88
164.46
2.07
2.16
323 172.40 2.12
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where Ce is the equilibrium concentration of the adsorbate (mg/L), q is the amount of dye adsorbed at
equilibrium (mg/g), Qo and b are the Langmuir constants which represents the maximum monolayer
adsorption capacity and energy of adsorption respectively.Kf and 1/n are Freundlich constants related
to adsorption capacity and adsorption intensity respectively. Fig. 7 shows the linear plot Ce/q versus
Ceat different initial concentration and temperature. The slope and intercept of the plot gives the values
of Qo and b respectively. The adsorption process follows Langmuir isotherm and not Freundlich
isotherm.
Fig.7 Langmuir plot ofRh 6G adsorption at different concentrations and temperatures
The essential characteristics of the Langmuir isotherm can be described by the dimensionless
separation factor RL[19] calculated using equation (7).
bCRL 11 …. (7)
The values of Qo, b and RL are tabulated in table II. The observed values of RL lie between zero to one,
which establish the fact that the adsorption process is favorable under the studied conditions.
II. Langmuir isotherm constants: Adsorbent dose 0.5 g/L
Co
(mg/L)
Temp
(°C)
Langmuir isotherm constants
Qo
(mg/g)
B
(L/mg)
RL
10 30 3.2952 0.2517 0.2843
15 30 5.8213 0.1826 0.2674
20 30 5.9319 1.1650 0.0412
10 20 4.4436 0.3425 0.2259
10 30 3.0463 0.3623 0.2163
0 3 6 9 12
0.0
0.3
0.6
0.9
1.2
3
2
1
Adsorbent dose 0.5 g/L
pH 6
Concentration of Rh 6G
1. 10 mg/L
2. 15 mg/L
3. 20 mg/L
Ce/q
(g/L
)
Ce ( mg/L)
4.0 4.5 5.0 5.5 6.0 6.5 7.0 7.5
0.0
0.2
0.4
0.6
0.8
1.0
Adsorbent dose 0.5 g/L
pH 6
Concentration of Rh 6G 10 mg/L
1. 20o C
2. 30o C
3. 40o C
4. 50o C
4
3
2
1
Ce/q
(g/L
)
Ce (mg/L)
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10 40 5.5816 0.3761 0.2100
10 50 4.8655 0.3311 0.2019
Adsorption kinetics
The kinetics of dye adsorption on PSLW carbon-iron oxide composite was analyzedby pseudo-
first order [20]or pseudo- second order [21], [22] kinetic models,given by equations (8) and (9).
tKqqq ee 1lnln (8)
eet qtqKqt 2
21 (9)
Where, qeandqt is the amount of adsorbate, adsorbed at equilibrium (mg/g) and at particular time
intervals respectively. K1 and K2 are the rate constants. A plot of ln (qe-q) versus t gives a straight line
slope of k1 and intercept of ln qe. The rate constants (K1 and K2) and calculated equilibrium capacity
(qe cal) of pseudo first order and second order models were determined from the slope and intercept
of linear plotsof pseudo first order and second order models at different concentration and temperature.
Fig. 8 shows that the linear plot of pseudo first order and second order models at different concentration
and temperature. The summary of kinetic parameters listed in table. III
Fig.8 Pseudo- second order plot of Rh 6G adsorption at different concentrations and temperatures
III. Pseudo first order and second order constants at different concentrations and temperatures:
Adsorbent dose 0.5 g/L
Co Temp Pseudo first order constants Pseudo second order constants
0 20 40 60 80 100 120 140 160
0
2
4
6
8
10
12
14
Adsorbent dose 0.5 g/L
pH 6
Concentration of Rh 6G
1. 10 mg/L
2. 15 mg/L
3. 20 mg/L
t/q
t
Time (min)
0 20 40 60 80 100 120 140 160
0
2
4
6
8
10
12
14
43
2 1
1. 20o C
2. 30o C
3. 40o C
4. 50o C
Adsorbent dose 0.5 g/L
pH 6
Concentration of Rh 6G 10 mg/L
t/q
t
Time (min)
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(mg/L) (°C) qe(exp)
(mg/g)
K1
(min-1)
qe(cal)
(mg/g)
R2
K2(g/mg/m
in)
qe (cal)
(mg/g)
R2
10 30 11.6102 0.0091 1.6352 0.9616 0.01215 11.6265 0.9936
15 30 16.4832 0.0076 1.5503 0.8162 0.01777 16.4554 0.9983
20 30 18.3052 0.0077 1.0077 0.9671 0.02883 18.4060 0.9994
10 20 12.373 0.0921 1.9771 0.8543 0.00757 12.7064 0.9755
10 30 11.6102 0.1068 1.9176 0.9735 0.01215 11.6265 0.9936
10 40 13.1357 0.0108 1.7545 0.9953 0.01174 13.1961 0.9954
10 50 13.8985 0.01370 2.0713 0.9857 0.00852 14.1242 0.9926
From the experimental data, it is clearly seen that the adsorption of dye follows pseudo second order
kinetics. The comparision between qe(cal) and qe (exp) value and the closeness of R2 towards unity is
closer for pseudo second order kinetics than pseudo first order kinetics. Thus, the adsorption process
follows pseudo second order kinetics.
Pore diffusion
The intra particle diffusion method is used to study the mechanism of Rh 6G dye adsorption.
The plot of q versus t½ gives the information about the mechanism and the slope is the intra particle
diffusion constant (ki). The ki values are listed in table. IV for different concentration and temperature.
The ki value increases with increase in concentration and temperature and it indicates the increase in
boundary layer thickness and it leads to decrease in external mass transfer and increase the internal
mass transfer [23].
IV. The intra particle diffusion constant:Adsorbent dose 0.5 g/L
Co (mg/L) T °C Intra particle diffusion
(ki) (mg/g/min1/2)
10 30 2.2701
15 30 3.7976
20 30 4.5772
10 20 1.5636
10 30 1.7036
10 40 1.8595
10 50 1.9532
Column Study
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The columnstudy provides the practical application of this process to industries. The observed
data fit to the linearised form of the Thomas model [24], [25] and are given in equation (10).
QVKCQMKqCC e 1log (10)
where, Co and Ce are the influent and effluent dyes concentrations (mg/L) respectively. K stands for
the Thomas rate constant (mL/min/mg), qo is the maximum solid phase concentration of solute (mg/g),
M is the mass of the adsorbent (g), and V is the throughput volume (ml/min). The linear plot of log
(Co/Ce-1) against V gives the value of K (slope) and qo (intercept).The column study was performed by
10 mg/L dye solution. The concentration of dye is gradually increases with bed volume. The value of
rate constant K (1.712 mL/min/mg) and the solute concentration qo (1.95 mg/g) are useful for designing
columns on large scale.
Conclusion
The present study describes the effective removal of Rh 6G dye from aqueous solution using
low-cost PSLW carbon-iron oxide composite as an adsorbent. Batch studies exhibits the adsorption
process follows Langmuir adsorption. The thermodynamic parameters show the adsorption process is
spontaneous, favorable and endothermic nature. The effective removal of dye can be obtained even
at high temperature. The kinetic data indicates the removal of dye follows the pseudo-second order
kinetics. In column study, Thomas model is used to assign the dye removal in industrial scale. From
the above results, it is concluded that the effective removal of Rh 6G from industrial effluents can be
achieved using PSLW carbon-iron oxide composite.
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