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Investigation of Cu-S intermediate species during electrochemical dissolutionand bioleaching of chalcopyrite concentrate
Weimin Zeng, Guanzhou Qiu, Miao Chen
PII: S0304-386X(13)00046-7DOI: doi: 10.1016/j.hydromet.2013.02.009Reference: HYDROM 3683
To appear in: Hydrometallurgy
Received date: 21 November 2012Revised date: 31 January 2013Accepted date: 11 February 2013
Please cite this article as: Zeng, Weimin, Qiu, Guanzhou, Chen, Miao, Investigationof Cu-S intermediate species during electrochemical dissolution and bioleaching of chal-copyrite concentrate, Hydrometallurgy (2013), doi: 10.1016/j.hydromet.2013.02.009
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Investigation of Cu-S intermediate species during electrochemical
dissolution and bioleaching of chalcopyrite concentrate
Weimin Zeng a, b, c
, Guanzhou Qiu a, b*
, Miao Chen c*
a School of Minerals Processing and Bioengineering, Central South University, Changsha, China
b Key Laboratory of Biometallurgy, Ministry of Education, Changsha, China
c CSIRO Process Science and Engineering, Clayton, Victoria, 3169, Australia
Abstract: the electrochemistry behaviour of chalcopyrite electrodes was investigated by
cyclic voltammetry. The results showed that the Cu-S intermediate species during
electrochemical dissolution of chalcopyrite was mainly as Cu2S, CuxS (1<x<2) and CuS. The
formation process of these species was analysed. It was shown that the oxidation of
chalcopyrite can only produce CuS, but CuxS and Cu2S were mainly formed due to the
reduction reaction of copper ion and sulphur. Furthermore, it was found that the addition of
copper ion could greatly affect the formation of Cu-S intermediate species. Therefore, during
bioleaching of chalcopyrite, the effect of different concentration of copper ion on the
bioleaching process was investigated. The results revealed that when the copper concentration
was low, it was hard to form Cu-S species in the ore residue. However, as the increase of
copper concentration, the formation of Cu-S intermediate species also increase and could be
detected by X-ray diffraction.
Keywords: Bioleaching, chalcopyrite; Cu-S intermediate species; moderate thermophiles
1. Introduction
Chalcopyrite is the most important copper sulphide due to it takes about 70% of
copper resource in the world (Dutrizac 1978). As it has higher lattice energy than
other copper sulfides, the bioleaching of chalcopyrite by mesophilic microorganisms
would lead to slow kinetics and poor extraction and its industrial application is still a
major challenge in the biohydrometallurgy field (Rawlings 2002). Since the end of
last century, more and more researchers in hydrometallurgy field focus on the use of
moderate thermophiles during bioleaching of chalcopyrite. This is mainly due to that
* Co-corresponding authors. Tel.: +86 731 8879212, +61 03 95458749.
E-mail address: [email protected] (Guanzhou Qiu); [email protected] (Miao Chen).
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using moderate thermophilies compared with mesophiles to bioleach chalcopyrite can
greatly improve the leaching reaction kinetics, avoids excessive chalcopyrite
passivation and finally improve the total copper extraction percentage (Cancho et al.,
2007; Wu et al., 2007; Zhou et al., 2009).
Bioleaching of chalcopyrite always involves the oxidation of elemental sulphur, iron
and copper depending on the leaching parameters (Nicol et al., 1984). The oxidation
of iron ion was simple and its valence was from Fe2+
to Fe3+
. The oxidation of copper
was mainly performed among Cu0, Cu
+ and Cu
2+, while the oxidation of sulphur was
very complex (from S2-
to S6+
). Due to these, there were several potential intermediate
species during dissolution of chalcopyrite, such as Cu2S, Cu1.92S, Cu1.6S, Cu1.4S and
CuS (Koch et al., 1971; Crundwell 1988).
In the electrochemistry researches, cyclic voltammetry was often used to detect the
intermediate species during dissolution of chalcopyrite (Li et al., 2006; Lopez -Juarez
et al., 2006). Nava and Gonzalez (2006) investigated the oxidation of chalcopyrite by
cyclic voltammetry and found that Cu1-rFe1-sS2-t, Cu1-xFe1-yS2-z, CuS and Fe2(SO4)3
(solid) were the oxidation products of chalcopyrite when the applied potential of
cyclic voltammetry was from 0.411 to 0.961V (vs Ag/AgCl). Mikhlin et al. (2004)
found that S0, Cu1-xFe1-yS2-z and CuS were the intermediate species during oxidation
of chalcopyrite when the applied potential was from 0.4 to 0.8V (vs Ag/AgCl). But
Yin et al. (1995) did not find the evidence of S0 on the chalcopyrite surface and they
proposed the formation of a copper sulphide CuS2 when the potential was from 0.4 to
0.5V (vs Ag/AgCl). Furthermore, Hiroyoshi et al. (2002) found that the addition of
copper ion would promote the dissolution of chalcopyrite, so they considered Cu2S
would formed due to the reaction of chalcopyrite with copper ion when the potential
was from 0.4 to 0.5V (vs Ag/AgCl). It can be seen that although there were many
researchers attempted to identify the process involved in the formation of intermediate
species by cyclic voltammetry, many inconsistencies existed compared with their
reports. These may be due to that the reactions of chalcopyrite would change mainly
according to the type of impurities or because of variations in stoichiometry or
depending on the leaching parameters (Shuey 1975; Prosser 1970).
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Although the Cu-S intermediate species could be analysed successfully by cyclic
voltammetry in this study, it was difficult to use normal XRD or EDX to detect these
species during bioleaching process, which had two possible reasons: 1) the amounts
of these species produced by bioleaching were small; 2) these species were very easy
to be oxidized during bioleaching. However, in the electrochemistry experiment,
Woods et al. (1987) found that the high concentration of copper ion would promote
the production of Cu-S intermediate species during chemical leaching. Therefore, in
the bioleaching experiment, when the high concentration of copper ions was added or
produced, the amounts of these intermediate species maybe also increase. This paper
investigated the potential Cu-S intermediate species during electrochemical
dissolution of chalcopyrite, and then these species were identified to be either the
oxidation production of chalcopyrite or the reduction production of copper ion and
sulphur. Finally, the chalcopyrite concentrate was bioleached by moderate
thermophiles and the effect of copper ion on the formation of Cu-S intermediate
species was analysed.
2. Materials and methods
2.1 Chalcopyrite sample
The chalcopyrite used in the electrochemistry experiments was obtained from Yushui
Copper Sulphide Mine in Meizhou, Guangdong, China. XRD analysis indicates that
the ore sample contains about 98% chalcopyrite and 2% silicate.
The chalcopyrite used in the bioleaching experiment was also obtained form Yushui
Copper Sulphide Mine. This ore sample was a chalcopyrite concentrate, and the XRD
analysis indicates that the sample mainly includes chalcopyrite (64%), pyrite (17%),
galena (15%), and gangue (4%). This chalcopyrite concentrate had been used for
culture moderate thermophiles for more than 2 years and thus the bioleaching
microorganisms were very adaptive to this concentrate (Zhou et al., 2009).
2.2 The Cu-S intermediate species during electrochemistry experiments
The chalcopyrite electrodes were made by the pure chalcopyrite. The pure
chalcopyrite was cut with a work surface of approximately 0.2 cm2 and, as far it was
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possible, with no visible imperfections. The specimens were placed on an epoxy resin
and were connected to a copper wire by silver paint on the back face. Preparation of
electrode surface after coarse grinding was completed on 1200-grit silicon carbide
paper. Furthermore, after each experiment, the electrode was taken out from the
electrolyte and then repeats to grind on 1200-grit silicon carbide paper to get a fresh
surface.
For the electrochemistry experiment, a three-electrode system was used. The cell
consisted of the chalcopyrite working electrode, a platinum counter electrode and an
Ag/AgCl reference electrode. The electrolyte used, modified 9K medium (Shown as
2.3), was prepared using analytical grade reagents. The electrochemical experiments
were carried out at 48 °C and pH 2.0, using a PARSTAT 2273 Potentiostat with
Power-Suite Software of the same company. Cycles were performed from 0 to 800
mV (vs Ag/AgCl), then to -800 mV (vs Ag/AgCl), and back to 0 mV (vs Ag/AgCl).
All tests were carried out at a scan rate of 30 mV/s (vs Ag/AgCl). In the paper, all
potential values are expressed vs. the Ag/AgCl electrode (3M KCl).
The mineral surface was characterised by SEM and EDX, which were performed on
an FEI Quanta 400 field emission, environmental scanning electron microscope
(ESEM) under high vacuum conditions. Secondary electron imaging was performed
using beam energies of 15 kV and probe currents of approximately 140 to 145 pA.
EDS was performed using a beam energy of 15 kV and a probe current of
approximately 800 pA.
2.3 Moderate thermophiles used in bioleaching experiments
Acid Mine Drainages (AMD) samples from several chalcopyrite mines in China were
collected. The samples were mixed and then inoculated into the culture medium for
enrichment of moderate thermophiles. This medium was modified 9K consisted of the
following compounds: (NH4)2SO4 3.0 g/L, Na2SO4 2.1 g/L, MgSO4·7H2O 0.5 g/L,
K2HPO4 0.05 g/L, KCl 0.1 g/L, Ca(NO3)2 0.01 g/L. And 10 g/L chalcopyrite
concentrate (with diameter of the particles less than 75 μm) was added as the energy
source. The moderate thermophiles were enriched at 48°C and initial pH of 2.0 in a
stirred tank reactor (shown as 2.4.).
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2.4 The Cu-S intermediate species during bioleaching of chalcopyrite concentrate
Bioleaching of chalcopyrite concentrate experiments were carried out in a 3 L glass
cylindrical reactor with a mechanic stirrer operating at 500 r/min. About 1950 mL
modified 9K medium was added into the reactor; 50 mL seed culture (no soluble
copper) was inoculated to get a cell density of 107 cells/mL. In addition, 80 g
chalcopyrite concentrate (with diameter of the particles less than 75 μm) was added
into the reactor to get a pulp density of 4%. After these, different concentration of
copper sulphate was added into the bioleaching solution to obtain the different
concentration of copper ion (0, 6, 12, 24, 36 g/L).
The reactor was placed in a thermostatic bath to keep the constant temperature at 48 ±
0.2°C. Sterile air was introduced into the base of the reactor at an approximate rate of
360 mL/min. The experiments were performed at initial pH 2.0. The acid
consumption was compensated by addition of 10 mol/L sulfuric acid to keep pH value
around 2. Distilled water was added to the reactor through a peristaltic pump in order
to compensate for evaporation losses. The levels of Cu2+
, Fe2+
, total iron in solution
were analysed at the end day of bioleaching experiment, while the cell density, pH
value and redox potential was analysed every day. The ore residue bioleached after 10
days was filtered to remove some of the water and then dried under vacuum (for 24
hours) for X-ray diffraction (XRD) analysis.
The components of the mineral sample and ore residue were analysed by XRD.
Copper and total iron concentrations in solution were determined by ICP-AES.
Ferrous iron concentration in solution was assayed by titration with potassium
dichromate. Ferric iron concentration is the concentration of total iron minus the
concentration of ferrous irons. The redox potential (or Eh) was measured using a
platinum electrode with an Ag/AgCl reference electrode. Free cells in solution were
observed and counted under an optical microscope.
3. Results and discussion
3.1 Cyclic Voltammetric study of chalcopyrite
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Cyclic voltammetry tests were performed to characterize the oxidation and reduction
reactions during dissolution of chalcopyrite. Fig.1 shows the results of cyclic
voltamperometry of chalcopyrite electrodes in the modified 9K electrolyte. There are
five anodic peaks (A1, A2, A3, A4 and A5) and four cathodic peaks (C1, C2, C3 and
C4). A4 and A5 are the very common anodic peaks during the study of chalcopyrite
electrochemical behaviour, which has been reported by many authors (Biegler and
Swift, 1979; Biegler and Horne, 1985; Gomez et al., 1996). There was a selective
dissolution of iron from the crystal lattice of chalcopyrite (peak A4) according to Eq.
(1) and Eq. (2). They reported that a blue layer was observed obviously on the
chalcopyrite surface after this reaction. This was associated with the formation of
covllite shown in Eq. (2). When at potential values more than 0.6 V (vs Ag/AgCl), the
blue layer of covllite could be destroyed according to Eq. (3).
CuFeS2 ↔ Cu1-xFe1-yS2-z + xCu2+
+ yFe2+
+ 2S + 2(x+y) e-
(1)
CuFeS2 ↔ 0.75CuS +1.25S0
+ 0.25Cu2+
+ Fe2+
+ 2.5e- (2)
CuS ↔ S0
+ Cu2+
+ 2e-
(3)
However, Hiroyoshi et al. (2001, 2002) considered that the dissolution of chalcopyrite
during potential 0.4—0.5 V (vs Ag/AgCl) was related to the production of Cu2S.
Because they found that after addition of 0.1 mol/L copper ion into the electrolyte, the
peak A4 would increase in a large scale and they proposed the reaction model as Eq.
(4):
CuFeS2 + 3Cu2+
+ 3Fe2+
↔ 2Cu2S + 4Fe3+
(4)
Furthermore, Yin et al. (1995) also did not agree with Eq(2), because they did not find
the evidence of S0 on the chalcopyrite surface and they proposed the formation of a
copper sulphide according to Eq(5). It can be seen from these that the oxidation
reaction of chalcopyrite at 0.4—0.5 V (vs Ag/AgCl) was different according to the
different authors’ reports. Therefore, it is necessary to investigate which of the Cu-S
intermediate species such as CuS, Cu2S and CuS2 was the oxidation product of
chalcopyrite in the experiment.
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CuFeS2 ↔ CuS2 + Fe2+
+ 2e-
(5)
At potential values more than 0.7 V (vs Ag/AgCl), it is reported as the oxidation of
ferrous iron to ferric iron and the oxidation of sulphur to sulphuric acid (Biegler and
Horne, 1985; Nava et al., 2002). But Lopez-Juarez et al. (2006) considered that the
oxidation of ferrous iron should be favoured (Eq. (6)), because a large quantity of S0
was still observed on the chalcopyrite surface with scanning electron microscope
(SEM) and energy dispersive x-ray analysis (EDX).
CuFeS2 ↔ 2S0
+ Cu2+
+ Fe3+
+ 5e- (6)
In the inverse scan, there was series reduction peaks appeared especially from -0.2 to
0.2 V (vs Ag/AgCl) of potential value. These peaks could be attributed to the
reduction of some species produced during the anodic scan like Cu2+
and Fe3+
(Eq. (7),
Eq. (8) and Eq. (9)), according to Holliday and Richmond (1990).
Fe3+
+ e- ↔ Fe
2+ (7)
Cu2+
+ S0 + 2e
- ↔ CuS (8)
Cu2+
+ 2e- ↔ Cu
0 (9)
When the potential value was lower than -0.3 V (vs Ag/AgCl), peak C3 and C4 were
observed. Arce and Gonzalez (2002) and Biegler and Horne (1985) attributed these
peaks to reduction of covellite and chalcopyrite, respectively (Eq. (10) and Eq. (11)).
Furthermore, Wood et al. (1987) considered that the reduction of covellite would
produce several kinds of Cu-S intermediate species such as Cu1.04S, Cu1.38S, Cu1.67S,
Cu1.83S, Cu1.93S and Cu1.96S.
2CuS + 2H+
+ 2e- ↔ Cu2S + H2S (10)
2CuFeS2 + 6H+
+ 2e- ↔ Cu2S + 2Fe
2+ + 3H2S
(11)
While Velasquez et al. (2001) recognized there was the reduction of chalcocite in
peak C4 according to Eq. (12). The reverse of this reaction accounts for the process
associated with anodic peak A1 (from -0.4 to -0.3 V, vs Ag/AgCl).
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Cu2S + H2O + 2e- ↔ 2Cu + HS
- + OH
- (12)
In the anodic scanning, peaks A1, A2 and A3 were reported not much during the
dissolution of chalcopyrite, but always existed in the electrochemitry study of
chalcocite and bornite (Velasquez et al., 2001; Arce and Gonzalez, 2002; Lu et al.,
2000). Furthermore, according to cathodic reaction shown as above, peaks A1 and A2
were considered as the oxidation of copper (Eq. (13)) and chalcocite (Eq. (14)).
2Cu + HS- + OH
- ↔ Cu2S + H2O + 2e
- (13)
Cu2S ↔ Cu1.92S + 0.08Cu2+
+ 0.16e- (14)
While the reaction about peak A3 was relatively complicated, Arce and Gonzalez
(2002) reported that peak A3 maybe associate with the oxidation of CuxS (1<x<2)
mainly included djurleite and geerite (Eq. (15) and (16)), which were the intermediate
species during dissolution of most copper sulphides.
Cu1.92S ↔ Cu1.60S + 0.32Cu2+
+ 0.64e-
(15)
Cu1.60S ↔ CuS + 0.60Cu2+
+ 1.20 e-
(16)
The difference of the electrochemical reactions associated to chalcopyrite dissolution
process could be associated to the different oxidation states of copper (i.e. Cu+, Cu
2+)
and sulphur (i.e. S2-
, S0) in the chalcopyrite structure. In the anodic scanning (from -
0.8 V to 0.8 V, vs Ag/AgCl), the states of copper and sulphur are from Cu0 to Cu
2+,
and S2-
to S0, respectively, while in the cathodic scanning (from 0.8 V to -0.8 V, vs
Ag/AgCl), the states of copper and sulphur are from Cu2+
to Cu0, and S
0 to S
2-,
respectively. The potential intermediate species during dissolution of chalcopyrite
mainly include Cu2S, Cu1-xS (1<x<2) and CuS.
3.2 The Cu-S intermediate species during electrochemistry experiments
The detailed oxidation process of chalcopyrite was not clear till now. But there were
some reports recognized that the oxidation of chalcopyrite would remove iron and
then became CuxS (1≤x≤2), which were the Cu-S intermediate species (Nava and
Gonzalez, 2006; Mikhlin et al., 2004; Yin et al., 1995; Hiroyoshi et al., 2002). There
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are many kinds of Cu-S intermediate species, such as CuS, Cu2S and Cu1.96S (Lee et
al., 2008). The investigation about their formation process and relations is very
important to understand the dissolution mechanism of chalcopyrite.
3.2.1 CuS
The Fig.1 showed that CuS could be produced by the oxidation of chalcopyrite when
the potential was from 0.4 to 0.5V (vs Ag/AgCl), but it was difficult to detect the
existence of CuS on the electrode surface by XRD or EDX, which was due to that the
production amount was very small and easy to be oxidized at higher potential than
0.5V (vs Ag/AgCl). For confirming the formation of CuS during the potential 0.4—
05V (vs Ag/AgCl), potentiostatic experiment was applied to the chalcopyrite
electrode in order to induce a higher amount of solid products formation on the
electrode surface.
The potentiostatic experiment (0.45V, vs Ag/AgCl) was applied to chalcopyrite
electrode surface for 60 s and then the surface was detected and analysed by SEM-
EDX. After the 60s anodic potentiostatic experiment, a blue layer on the electrode
surface could be observed (Fig.2). The EDX result showed that the amount of S and
Cu produced by the oxidation of chalcopyrite were large, but the amount of Fe was
very small. This indicated that the oxidation of chalcopyrite firstly removed Fe and
formed a blue layer which should be the complex substances of CuS and S0.
The copper concentration in the electrolyte after the potentiostatic experiment
performed for 60s on the electrode was analysed by ICP-OES, and showed a very low
value (data not shown). In this case when the applied potential was 0.45V (vs
Ag/AgCl), the reduction reaction of chalcopyrite or copper ion was not easy. As a
result, CuS on the electrode surface here should be the oxidation production of
chalcopyrite but not the reduction production, and this prove the correction of Eq(2).
3.2.2 Cu2S
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It can be seen from Fig.1 that the oxidation potential of chalcopyrite was much higher
than Cu2S, and this suggested that it is difficult to form Cu2S during the oxidation of
chalcopyrite. For further proving this suggestion, linear votalmmetry of chalcopyrite
electrode was carried out from the different start potential (-0.2V, -0.2V, -0.3V, -0.5V
and -0.75V, vs Ag/AgCl) to the end potential 0.65V (vs Ag/AgCl, the electrodes were
not taken out from the electrolyte after the 1st scan, but continue to be used for the
next scan). The experiment principle was that if Cu2S was the product of chalcopyrite
oxidation at potential 0.4—0.5V (vs Ag/AgCl) (Fig.1), the oxidation peak of Cu2S
would be detected at the next linear scan at potential -0.2—0V (vs Ag/AgCl).
Otherwise, Cu2S should be the reduction products of copper ion or CuS (at potential
lower than -0.3V, vs Ag/AgCl), or the oxidation production of Cu0 (at potential -0.4—
0.3V, vs Ag/AgCl).
It can be seen from Fig.3 that in the 1st
scan, the potential range was from -0.2V to
0.65V (vs Ag/AgCl) and the chalcopyrite was oxidized during this scan. After this,
the second scan was carried out and the potential range was same as the 1st one. In the
2nd
scan, the scan plot was rather similar with the 1st one and the oxidation peak of
Cu2S still did not appear during the potential -0.2—0 V (vs Ag/AgCl). This indicated
that Cu2S did not form by the chalcopyrite oxidation at the potential 0.4—0.5 V (vs
Ag/AgCl). When the start potential decreased to -0.3 V (vs Ag/AgCl, in the 3rd
scan),
a slightly oxidation peak was observed at potential -0.2—0 V (vs Ag/AgCl) and this
was due to that Cu2S began to form by the reduction of CuS (which formed as Eq(7)
from -0.2 to 0.2 V, vs Ag/AgCl). In the 4th
scan, the decrease of start potential to -0.5
V (vs Ag/AgCl) led the increase of reduction of CuS, and thus the oxidation peak of
Cu2S became more obvious. In the 5th
scan, when the start potential decreased to -0.75
V (vs Ag/AgCl), the oxidation peak of Cu2S increased due to another reduction
reaction (Eq. (10)). These concluded that Cu2S here was the reduction production of
CuS or chalcopyrite when the potential was lower than -0.3V (vs Ag/AgCl), but not
the oxidation product of chalcopyrite at potential 0.4—0.5V (vs Ag/AgCl).
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3.2.3 CuxS (1<x<2)
It is reported that CuxS (1<x<2) includes several intermediate species during
dissolution of chalcopyrite, such as Cu1.38S, Cu1.67S, Cu1.83S, Cu1.75S and Cu1.96S
(Nava and Gonzalez, 2006; Lee et al., 2008). Their oxidation peaks in cyclic
voltammetry are between the oxidation peak of Cu2S and CuFeS2, generally from
potential 0—0.4 V (vs Ag/AgCl). However, in this cyclic voltammetry experiment,
there was only one obvious oxidation peak of CuxS (1<x<2) in Fig.1 (peak A3). The
production of CuxS (1<x<2) was reported to have two potential ways: the oxidation of
Cu2S and the reduction of CuS. Therefore, according to Eq.(8) , the addition of copper
ion would promote the production of CuS and thus would benefit the formation of
CuxS (1<x<2) during the reduction reaction (Woods et al., 1987).
In the experiment, in order to investigate the formation of intermediate species CuxS
(1<x<2) during the dissolution of chalcopyrite electrode, copper ion was added into
the electrolyte to promote the formation of CuxS (1<x<2) and the linear voltammetry
of chalcopyrite electrode was carried out. It can be seen from Fig.4 that the addition
of copper ion greatly affected the anodic peak current and potential. As the increase of
addition of copper ion concentration, oxidation peak current increased as well and the
peak potential moved positively.
When the addition of copper ion was 1 g/L, three oxidation peaks was obtained. One
peak was at about potential 0.1V and considered as the oxidation of CuxS (B1)
(1<x<2) (Eq.(16)). One peak was at potential 0.4—0.5V (vs Ag/AgCl) and considered
as the oxidation of chalcopyrite (Eq.(2)). The other one peak was at potential 0.7V
(vs Ag/AgCl) and considered as the oxidation of CuS (Eq.(3)). Furthermore, a tight
blue layer could be observed as CuS when the linear voltammetry potential was lower
than 0.6 V (vs Ag/AgCl). The formation of CuS was due to the oxidation of
chalcopyrite and reduction of Cu2+
and S0 (Eq(8)). When the concentration of copper
addition increased to 3 g/L, the oxidation peak of chalcopyrite disappeared, which
maybe due to the CuS layer covered on the chalcopyrite electrode surface and block
the oxidation of chalcopyrite. But then one new oxidation peak was obtained at
potential -0.05V (vs Ag/AgCl). According to Fig.1 and Fig.3 this peak was related
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with the oxidation of Cu2S. When the concentration of addition copper increased to 6
g/L, another new oxidation peak at about potential 0.3V (vs Ag/AgCl) was observed
slightly, this should be the oxidation of another kind of CuxS (B5) (1<x<2). In this
case, four Cu-S intermediate species were obtained, and they were Cu2S (B4), CuxS-1
(B5), CuxS-2 (B1) and CuS (B3). When the concentration of addition copper
increased to 12 g/L, the reduction products increased in a large scale, covered on the
chalcopyrite electrode surface, and the anodic peak potential moved positively, thus
the oxidation peak of CuS disappeared below potential 1.0 V (vs Ag/AgCl).
3.3 The intermediate species during bioleaching of chalcopyrite
The results of electrochemistry experiment (section 3.2.3) showed that the high
concentration of copper ion would promote the reduction reaction and thus the
amount of reduction products increased, such as Cu2S and CuS. Therefore, during
bioleaching of chalcopyrite, when the concentration of copper was very high, the
intermediate species may be promoted and increase in a large scale. In the experiment,
different concentration of copper ion was added into the bioleaching solution and the
ore residue after bioleached for 10 days was analysed by XRD.
Table 1 showed the bioleaching parameters during bioleaching of chalcopyrite
concentrate after addition of different concentration of copper ion. When the addition
of copper ion was 0 g/L (A), copper extraction from chalcopyrite concentrate could
reach 4.32 g/L and the ferric iron concentration was 1.83 g/L. As the increase of
copper addition, the concentration of both ferric iron and ferrous iron decreased. In
addition, the redox potential value and cell density also decreased. Especially when
the addition of copper ion was 36 g/L (E), the ferric iron concentration decreased
remarkably to about 0.94 g/L, which accompanied with a very low redox potential
value (477 mV, vs Ag/AgCl). At high concentration of copper ion, the cell density of
moderate thermophiles for bioleaching of chalcopyrite concentrate was relatively low
and this would lead to the low copper and iron extraction.
The ore residues after bioleached for 10 days were analysed by XRD. It can be seen
from Fig.5 that the high concentration of copper ion in the bioleaching system greatly
affected the component of ore residue. The results showed that during bioleaching of
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chalcopyrite concentrate, the major components of ore residue were chalcopyrite,
pyrite, lead sulphate, jarosite and chalcanthite (the formation of chalcanthite was due
to that copper sulphate crystallized with water when the ore residue was drying under
vacuum). In the experiment A and B, when the addition of copper ion was only 0 and
6 g/L (Table 1), it was hard to find any Cu-S intermediate species by XRD analysis.
But when the addition of copper ion increased to 12 g/L (C), the XRD result showed
that Cu2S and CuS were produced in the ore residue. When the addition of copper ion
increased to 24 g/L (D), the other intermediate species like Cu34S32 and Cu1.96S could
be found. However, when the concentration of total copper ion increased to about 36
g/L (E), only Cu2S was detected, but its amount increased in a large scale (data not
shown). This may be due to that when the copper concentration was the highest (E),
the redox potential was only 477mV (vs Ag/AgCl), and then the formation of Cu2S
would be easier than any other intermediate species (Lee et al., 2008; Woods et al.,
1987).
As a result, it can be seen that during bioleaching of chalcopyrite concentrate the
different concentration of copper ion could affect the bioleaching process. When the
copper concentration was relatively low, the reduction reaction in the bioleaching
system was not obvious and Cu-S intermediate species were very difficult to be
detected by XRD. However, when the copper concentration increased, the reduction
reaction would be accelerated and the amount of reduction products increased. There
were several intermediate species formed, but CuS and Cu2S were the majority. When
the copper concentration was very high, such as in the experiment E, the Cu-S species
became simple and only Cu2S was the reduction product, but its amount increased in a
large scale than before.
However, in our previous studies and other author’s reports, it was hard to detect Cu-
S intermediate species in the ore residue by XRD during bioleaching of chalcopyrite.
There were two possible reasons: 1) in the previous studies, the ore residue sample
after bioleached was dried in the oven at 50-75°C, and in this case the Cu-S
intermediate species were very easy to be oxidized; 2) when the copper concentration
in the solution was low, the amount of Cu-S intermediate species was small and easy
to be dissolved by acid or bioleaching microorganisms, and thus it was hard to detect
them by XRD. These results indicate that during dissolution of chalcopyrite, the
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oxidation and reduction reactions were performed simultaneously, but at many cases,
such as when the copper concentration was low, the oxidation reaction was the
dominant reaction.
4. Conclusions
The analysis of the formation process of Cu-S intermediate species indicated that the
oxidation of chalcopyrite can only produce CuS, but not CuxS (1<x<2) and Cu2S, and
the later two species were mainly produced due to the reduction reaction of copper ion
and sulphur. During bioleaching of chalcopyrite, when the copper concentration was
high, the reduction reaction of copper ion and sulphur could be promoted and the Cu-
S intermediate species such as CuS and Cu2S formed largely. However, when the
copper concentration was relatively low (lower than 10 g/L); these intermediate
species amounts were very low and easy to be oxidized, and thus hard to be detected
by XRD.
Acknowledgements
This work was supported by the China National Basic Research Program (No.
2010CB630901), the National Natural Science Foundation of China (No. 31200382),
Postdoctoral Science Foundation of Central South University (No. 1332-
74141000076), and Australia CSIRO OCE Science Leader Grant.
References
Arce, E.M., Gonzalez, I., 2002. A comparative study of electrochemical behavior of
chalcopyrite, chalcocite and bornite in sulfuric acid solution. International Journal of
Mineral Processing 67(1-4), 17-28.
Biegler, T., Horne, M.D., 1985. The electrochemistry of surface oxidation of chalcopyrite.
Journal of the Electrochemical Society 132(6), 1363-1369.
Biegler, T., Swift, D.A., 1979. Anodic electrochemistry of chalcopyrite, Journal of Applied
Electrochemistry 9, 545–554.
ACC
EPTE
D M
ANU
SCR
IPT
ACCEPTED MANUSCRIPT
15
Cancho, L., Blázquez, M.L., Ballester, A., González, F., Muñoz, J.A., 2007. Bioleaching of
chalcopyrite concentrate with moderate thermophilic microorganisms in a continuous
reactor system. Hydrometallurgy 87(3-4), 100-111.
Crundwell, F.K., 1988. The influence of the electronic structure of solids on the anodic
dissolution and leaching of semiconducting sulphide minerals. Hydrometallurgy 21(2),
155-190.
Dutrizac, J.E, 1978. The kinetics of dissolution of chalcopyrite in ferric ion media.
Metallurgical and Materials Transactions B 9B, 431–439.
Gómez, C., Figueroab, M., Muñoza, J., Blázqueza, M.L., Ballestera A., 1996.
Electrochemistry of chalcopyrite. Hydrometallurgy 43 (1-3), 331-344.
Hiroyoshi, N., Miki, H., Hirajima, T., Tsunekawa, M., 2001. Enhancement of chalcopyrite
leaching by ferrous iron in acidic ferric sulphate solutions. Hydrometallurgy 60(3), 185-
197.
Hiroyoshi, N., Arai, M., Miki, H., Tsunekawa, M., Hirajima, T., 2002. A new reaction model
for the catalytic effect of silver ions on chalcopyrite leaching in sulfuric acid solutions.
Hydrometallurgy 63(3), 257-267.
Holliday, R.I., Richmond, W.R., 1990. An electrochemical study of the oxidation of
chalcopyrite in acidic solution. Journal of Electroanalytical Chemistry 288(1-2), 83-98.
Koch, D.F.A., in: Bockris, J.O.M., Conway, B.E., (Eds.), 1971. Modern Aspects of
Electrochemistry, vol. 10. Plenum Press, 211–237.
Lee, M. S., Nicol, M. J., Basson, P., 2008. Cathodic processes in the leaching and
electrochemistry of covellite in mixed sulfate–chloride media. Journal of Applied
Electrochemistry. 38:363–369.
Li, H.X., Qiu, G.Z., Hu, Y.H., Cang, D.Q., Wang, D.Z., 2006. Electrochemical
behavior of chalcopyrite in presence of Thiobacillus ferrooxidans. Transactions of
Nonferrous Metals Society of China 16(5), 1240-1245.
Lopez-Juarez, A., Gutierrez-Arenas, N., Rivera-Santillan, R.E., 2006. Electrochemical
behavior of massive chalcopyrite bioleached electrodes in presence of silver at 35°C.
Hydrometallurgy 83(1-4), 63-68
Lu, Z.Y., Jeffrey, M.I., Lawson, F., 2000. An electrochemical study of the effect of chloride
ions on the dissolution of chalcopyrite in acidic solutions. Hydrometallurgy 56(2), 145-
155.
Mikhlin, Y. L., Tomashevich, Y. V., Asanov, I. P., Okotrub, A.V., Varnek, V. A., Vyalikh,
D.V., 2004. Spectroscopic and electrochemical characterization of the surface layers of
chalcopyrite (CuFeS2) reacted in acidic solutions. Applied Surface Science 225(1-4), 395-
409.
ACC
EPTE
D M
ANU
SCR
IPT
ACCEPTED MANUSCRIPT
16
Nava, J.L., Oropeza, M.T., Gonzalez, I., 2002. Electrochemical characterisation of sulfur
species formed during anodic dissolution of galena concentrate in perchlorate medium at
pH 0. Electrochimica Acta 47(10), 1513-1525.
Nava, D., González, I., 2006. Electrochemical characterization of chemical species
formed during the electrochemical treatment of chalcopyrite in sulfuric acid
Electrochimica Acta 51(25), 5295-5303.
Nicol, M. J., in: Robinson, P.E., Srinivasan, E. S., Wood, R., (Eds), 1984. Processing of the
Cincinatti Ohio meeting of the electrochemical society. The Electrochemical Society.
Pennington, NJ, 1984, p152.
Prosser, A., in: Jones, M.J.(Ed.), proceeding of the ninth commonwealth minning and
metallurgical congress, 1969, vol.3, IMM, London, 1970, p59.
Rawlings, D.E., 2002. Heavy metal mining using microbes. Annual review of microbiology
56: 65-91.
Shuey, R.T., 1975. Semiconducting ore minerals. Developments in economic geology series,
Elsevier, Amsterdam, p242.
Velasquez, P., Leinen, D., Pascual, J., Ramos-Barrado, J.R., Cordova, R., Gomez, H.,
Schrebler, R., 2001. XPS, SEM, EDX and EIS study of an electrochemically modified
electrode surface of natural chalcocite (Cu2S). Journal of Electroanalytical Chemistry
510(1-2), 20-28.
Woods, R., Yoon, R.H., Young, C.A., 1987. Eh-pH diagrams for stable and metastable phases
in the copper-sulfur-water system International Journal of Mineral Processing. 20(1-
2),109-120.
Wu, C.B., Zeng, W.M., Zhou, H.B., Fu, B., Huang, J.F., Qiu, G.Z., Wang, D.Z., 2007.
Bioleaching of chalcopyrite by mixed culture of moderately thermophilic microorganisms.
Journal of Central South University Technology 14, 474-478.
Yin, Q., Kelsall, G.H., Vaughan, D.J., England, K.E.R., 1995. Atmospheric and
electrochemical oxidation of the surface of chalcopyrite (CuFeS2). Geochimica et
Cosmochimica Acta 59(6), 1091-1100.
Zeng, W.M., Qiu, G.Z., Zhou, H.B., Liu, X.D., Chen, M., Chao, W.L., Zhang, C.G., Peng
J.H., 2010. Characterization of extracellular polymeric substances extracted during
the bioleaching of chalcopyrite concentrate. Hydrometallurgy 100, 177-180.
Zeng W.M., Qiu G.Z., Chen M., Zhou H.B., Liu X.D., Chao W.L., Zhang Y.S., 2010.
Community structure and dynamics of the free and attached microorganisms during
moderately thermophilic bioleaching of chalcopyrite. Bioresource Technology 101, 7079-
7086.
ACC
EPTE
D M
ANU
SCR
IPT
ACCEPTED MANUSCRIPT
17
Zhou, H.B., Zeng, W.M., Yang, Z.F., Xie, Y.J., Qiu, G.Z., 2009. Bioleaching of chalcopyrite
concentrate by a moderately thermophilic culture in a stirred tank reactor. Bioresource
Technology 100, 515–520.
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Table 1 The bioleaching parameters during bioleaching of chalcopyrite concentrate
after addition of different concentration of copper ion in the stirred tank reactor after
10 days. A: without addition of copper ion, B: addition of 6 g/L copper ion, C:
addition of 12 g/L copper ion, D: addition of 24 g/L copper ion, E: addition of 36 g/L
copper ion.
Experiments Total copper
(g/L)
Ferric iron
(g/L)
Ferrous iron
(mg /L)
pH
value
Redox
potential
(mV)
Cell density
(108cells/mL)
A 4.32 1.83 151 1.66 584 7.9
B 10.28 1.82 144 1.67 582 7.8
C 16.04 1.79 148 1.67 579 7.2
D 27.73 1.72 143 1.7 562 5.6
E 37.58 0.94 84 1.84 477 0.4
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Fig.1. Cyclic voltammetry of chalcopyrite without bioleaching process in the modified 9K
medium at sweep rate = 30 mV/s. Temperature: 48°C, pH 2.0. Reference electrode: Ag/AgCl
electrode.
A1
A2
A3
A4
C1 C2
C3
C4
A5
-1.0 -0.8 -0.6 -0.4 -0.2 0.0 0.2 0.4 0.6 0.8 1.0
-3.5
-3.0
-2.5
-2.0
-1.5
-1.0
-0.5
0.0
0.5
1.0
1.5
2.0
2.5
3.0
3.5
I / m
A
E / V vs Ag/AgCl
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Fig.2. the formation of CuS and S0 on the electrode surface during dissolution of chalcopyrite
when the constant potential pulse was 0.45 V in the electrochemistry experiments. A: the
electrode surface observed by eye, B: SEM investigation of electrode surface, C: EDX
analysis of electrode surface.
C
B A
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Fig.3. The linear voltammetry of chalcopyrite from different start potential (-0.2V, -0.2V, -
0.3V, -0.5V and -0.75V) to the end potential 0.65V in the modified 9K medium at sweep rate
= 30 mV/s. Temperature: 48°C, pH 2.0. Reference electrode: Ag/AgCl electrode.
E/V vs Ag/AgCl
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Fig.4. the effect of different concentration of Cu2+
(1, 3, 6, 12 g/L) on the electrochemistry
behaviour of chalcopyrite electrode in the modified 9K medium at sweep rate = 30 mV/s.
Temperature: 48°C, pH 2.0. Reference electrode: Ag/AgCl electrode. A is the amplified
figure of linear voltammetry when the addition of Cu2+
was 1 g/L.
-0.2 0.0 0.2 0.4 0.6 0.8 1.0
0.0
0.5
1.0
1.5
2.0
-0.2 0.0 0.2 0.4 0.6 0.8
0.00
0.05
0.10
0.15
0.20
0.25
Cur
rent
/ A
E / V
1 g/L
Cu
rre
nt / A
E / V vs Ag/AgCl
1 g/L
3 g/L
6 g/L
12 g/L
B1 B2
B3
B1 B3
B4
B4
B5
B1
B3 B4
B1
B5 A
B1 B2
B3
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Fig.5. the XRD analysis of ore residue during bioleaching of chalcopyrite
concentration after addition of different concentration of Cu2+
in the stirred tank
reactor after 10 days. A: without addition of copper ion, B: addition of 6 g/L copper
ion, C: addition of 12 g/L copper ion, D: addition of 24 g/L copper ion, E: addition of
36 g/L copper ion.
A
C B
E D