The SAIMM Hydrometallurgy Conference 2009 24 – 26 February 2009 Misty Hills, Muldersdrift,...
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Transcript of The SAIMM Hydrometallurgy Conference 2009 24 – 26 February 2009 Misty Hills, Muldersdrift,...
![Page 1: The SAIMM Hydrometallurgy Conference 2009 24 – 26 February 2009 Misty Hills, Muldersdrift, Gauteng.](https://reader036.fdocuments.us/reader036/viewer/2022081504/56649f155503460f94c2ae28/html5/thumbnails/1.jpg)
The SAIMM Hydrometallurgy Conference 2009
24 – 26 February 2009
Misty Hills, Muldersdrift, Gauteng
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Leaching of the arsenopyrite/pyrite
flotation concentrates using metallic
iron in a hydrochloric acid medium.
Mahlangu T, Gudyanga, F.P., and Simbi, D.J.,
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Overview of presentation
BackgroundExperimental Results and discussionConclusionsAcknowledgements
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Background: ores
Au & Ag bearing arsenopyrite/pyrite concentrate
Au occurring in sub-microscopic form and/or in solid solution
Ores prevalent in the Central and Southern parts of Zimbabwe
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Background: Processing routesRoasting – custom roasting plant in
Kwekwe (now not operational)
Alternatives – bioleaching of concentrates (pilot plant operated for a while in the 1990s)
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Background: Alternatives
Exploration of reductive leaching process as a novelty
Release sulphur as H2S – oxidise to sulphate by strong oxidants such as H2O2
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Background: Alternatives
(2) )()1()1(2)1(2M
(1) )(22
2m
2
2
2 gSHm
pnSM
p
me
m
pnH
m
pnS
gSnHmMnenHSM
m
nppn
nm
)()1()1(2)1(2M
)(22
2m
2
2
2 gSHm
pnSM
p
me
m
pnH
m
pnS
gSnHmMnenHSM
m
nppn
nm
SHFeSCuHFeCuFeS 22
22 3362
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Background: Envisaged benefits
Break down the matrix to liberate the precious metals
Avoid the mineral surface passivation common in the oxidative leach systems
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Background: Pertinent problems
Neutralisation of the leach residues prior to cyanidation
Negative effects of residual sulphur, even at ppm levels
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Background: Reactions systems
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Background: Reaction systems
Thermodynamic feasibility of
Reductive reaction
Hydrogen evolution side reaction
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Background: Reaction systems
Kinetics
Hydrogen evolution side reaction kinetically faster than the reductive leach reactions
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Background: Focus areas
Effect of pH
Effect of iron/concentrate ratio
Effect of desulphurisation on gold cyanidation
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Experimental: Flotation concentrate
Mineralogical composition
FeS2 FeAsS PbS CuFeS2 ZnS Sb2S3 Other(%) (%) (%) (%) (%) (%) (%)
58.7 27.2 0.1 0.3 1.8 0.8 11.1
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Experimental: Flotation concentrate
Chemical composition
Fe As Pb Cu Zn Sb S Au Ag Other(%) (%) (%) (%) (%) (%) (%) (g/t) (g/t) (%)
36.7 12.5 0.1 0.1 1.2 0.6 28.7 64.7 43.1 20.2
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Iron shavings: screened washed and stored under deoxygenated conditions
AR grade reagents ofHCl; H2SO4; ferric sulphate;potassium dichromate;High purity nitrogenSodium cyanideSodium hydroxide
Experimental: Reagents
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Experimental procedure
Reductive leaching
500ml solutionTemperature – 105oC45 – 60mins N2 pre-spargingpH adjusted with HClTotal leaching time – 300min
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Results: Effect of pH
02468
10121416
0.05 0.15 0.25 0.35 0.45 0.55 0.65
pH
%S
leac
hed
from
F
eAsS
/FeS
2
15min 30min 60min 120min 180min 240min 300min Direct acid leaching
Iron to concentrate ratio = 0
Inverse relationship with pH
No pyrite acid leach
molkJG
SHAsFeHFeAsSo
o
/45.62
2 22
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Results: Effect of pH
0
2
4
6
8
10
12
14
16
0.04 0.24 0.44 0.64
pH
15min
30min
60min
120min
180min
240min
300min
(a)
0
5
10
15
20
25
0.04 0.24 0.44 0.64
pH
15min
30min
60min
120min
180min
240min
300min
05
1015202530354045
0.04 0.24 0.44 0.64
pH
15min
30min
60min
120min
180min
240min
300min
0
10
20
30
40
50
60
70
0.04 0.24 0.44 0.64
pH
15min
30min
60min
120min
180min
240min
300min
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Results: Effect of pH & iron-to-concentrate ratio
0
10
20
30
40
50
60
70
0.1 0.15 0.25 0.34 0.44 0.54 0.62
pH
%S
leac
hd
fro
m F
eAsS
/FeS
2
0.16
0.32
0.64
0.96
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FeS2 + Fe + 4H+ = 2Fe2+ + 2H2S
Go = -58.14 kJ/mol
FeAsS + 2H+ = Fe2+ + Aso + H2S
Go = -62.45 kJ/mol
FeAsS + Fe + 2H+ = Feo + Aso + Fe2+ + H2S
Go = -62.43 kJ/mol
Results: Effect of pH & iron-to-concentrate ratio
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Results: Galvanic interactions
H2S
Fe2+ or FeCln2-n
H+
FeS2/FeAsS
Product layer
Fe
Fe = Fe2+ + 2e- orFe + nCl- = FeCln
2-n + 2e-
e-
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Results: Galvanic interactions
222 HFeHFe
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0.1 0.15 0.25 0.34 0.44 0.54 0.620.16
0.960
10
20
30
40
50
60
70
%S
lea
chd
fro
m F
eAsS
/FeS
2
pH
60-70
50-60
40-50
30-40
20-30
10-20
0-10
Results: Effect of pH & iron-to-concentrate ratio
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Results: Effect of pH & iron-to-concentrate ratio
0
10
20
30
40
50
60
70
0 0.5 1 1.5
Iron/concentrate ratio
%S
leac
hed
from
FeA
sS/F
eS2
15min
30min
60min
120min
180min
240min
300min
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Effect of desulphurisation on Au & Ag cyanidation
Size-by-size analysis
- Wet screening/sieving-Au & Ag size – by – size analysis
0.23%NaCNpH 11Time 48hrsAeration
Cyanidation
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Effect desulphurisation on Gold and silver recovery
0
10
20
30
40
50
60
70
80
90
100
-212+150µm -150+106µm -106+75µm -75+53µm -53µm
% M
etal
dis
trib
uti
on
Ag
Au
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Effect desulphurisation on Gold dissolution
0
2
4
6
8
10
12
14
16
0 10 20 30 40 50 60 70
%S leached from arsenopyrite/pyrite
%A
u e
xtra
ctio
n
.
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Effect desulphurisation on silver dissolution
0
2
4
6
8
10
12
14
16
18
0 10 20 30 40 50 60 70
%S leached from arseonpyrite/pyrite
%A
g ex
trac
tion
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ConclusionsReductive leach of the
arsenopyrite/pyrite concentrate thermodynamically feasible
FeAsS – both chemical and reductive leach reactions operational
FeS2 – postulated to leach through a reductive leach reaction
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ConclusionsProcess strongly influenced by both pH
and iron-to-concentrate ratio
Strong interaction between pH and iron-to-concentrate ratio
Galvanic interactions promote the hydrogen evolution reaction in preference to the reductive leach reactions
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ConclusionsRelatively low desulphurisation
levels
Low levels of gold and silver dissolution
Process is not effective as a pre-treatment process for refractory gold concentrates
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AcknowledgementsDepartment of Metallurgical
engineering – University of Zimbabwe
Rio Tinto Zimbabwe
Department of Materials Science and Metallurgical Engineering – University of Pretoria
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Thank you
?