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R. Paunova et al. Int. Journal of Engineering Research and Applications www.ijera.com
ISSN: 2248-9622, Vol. 5, Issue 12, (Part - 3) December 2015, pp.92-100
www.ijera.com 92 | P a g e
Phase Transformations and Thermodynamics in the System
Fe2О3– V2О5 – MnО – SiО2 of Non-Isothermal Heating
R. Paunova, D. Grigorova, R. Alexandrova
Department of Ferrous Metallurgy and Metal Foundry, University of Chemical Technology and Metallurgy
Bulgaria
ABSTRACT
Thermodynamic characteristics in the system Fe2O3 – MnO – V2O5 –SiO2 have been investigated. Two mixtures
have been prepared. The first mixture was synthetic, prepared from pure oxides in proportion according to the
chemical composition of the waste catalyst and manganese concentrate. The second one contained the waste
vanadium catalyst and manganese concentrate. The synthetic mixture has been used as a standard in order to
establish the influence of impurities in the concentrate, and the waste catalyst on the thermodynamics of the
studied system.
Experiments carried out in the temperature up to 1473 K for the system containing waste vanadium catalyst and
manganese concentrate occur to formation of new phases formation as FeV2O4 and Iron Vanadium Oxide type
and Jacobsite types MnFe2O4 and (Mn6Fe4)(Mn4Fe1.6)O4. EMF method with difference reference electrode
(Ni/NiO, Mo/MoO2 and air) relationship of delta GoT = f(T) in the temperature range 1073 – 1173 К of mixtures
was obtained. The experimental data for the system show that the reference electrodes air and Ni/NiO are more
suitable than Mo/MoO2.
The obtained results will be used as an investigations base to the production of complex iron vanadium
manganese alloy using the waste materials.
Keywords – thermodynamics, DTA, EMF method, vanadium catalyst, manganese concentrate.
I. INTRODUCTION
From a metallurgical point of view, the study of
binary and ternary systems has great practical
significance even for ferroalloy production to obtain
alloys. Complex alloys are becoming more and more
widely used in metallurgy for deoxidation, alloying,
modifying and desulfurization; they also improve the
mechanical, physical and chemical properties of
steel and iron. It is more effective to obtain elements
as a complex ferroalloy than as separate elements.
In the present studies, the waste vanadium
catalyst was used. Annually, between 500 and 1000
tons vanadium catalyst are released from sulphur
acid production which contains a significant quantity
of deficit vanadium. The toxicity of the vanadium
causes certain environmental problems which is an
additional consideration to look for ways to utilize
this valuable waste product.
The complex systems are used in various fields
of Chemistry and Metallurgy. Ternary systems of the
type MeO-V2O5-Fe2O3 are used as catalysts because
vanadates, which are formed, as a result, catalyze the
oxidation processes of many compounds [1]. The
similar systems is also used in the electrode
materials preparation, and glasses with relatively
high electrical conductivity and high thermal
stability or for correction of the phase diagram. [1, 2,
3, 4, 5, 6, 7, 8].
Other studies have focused on the structure of
complex compounds produced by the solid-phase
method - Co4Fe3.33 (VO4) 6 [9], Mn3Fe4 (VO4) 6 [9,
11] and Zn3Fe4V6O24 [10]. The equilibrium in the
system V2O5-Fe2O3-Mn2O3 (MnO) was examined by
some authors [12]. They found out the formation of
the solid solution of the type Fe2Mn2V4O15 based on
manganese pyrovanadat. DTA and XRD analyses
were used in the investigation of all these systems.
In the binary system MnxFe3-xO4, containing
manganese oxides, the heat capacity for different
values of “x”was determined as well as the entropy
changes [13]. The phase equilibrium of the Mn-Fe-O
system (Fe / Mn = 2) and the partial pressure of
oxygen of 10-1
Pa to 105
Pa were examined in the
temperature range from 1223 to 1393 K, by
measuring the electrical conductivity and the mass
of the sample [14]. The enthalpy and Gibbs free
energy of (MnxFe1-x)3O4 at 298 K were defined
calorimetrically[15].
Some other authors analyzed the
thermodynamics of the processes in the ternary
RESEARCH ARTICLE OPEN ACCESS
R. Paunova et al. Int. Journal of Engineering Research and Applications www.ijera.com
ISSN: 2248-9622, Vol. 5, Issue 12, (Part - 3) December 2015, pp.92-100
www.ijera.com 93 | P a g e
system Fe2O3-V2O5-MnO using data for the binary
systems respectively or some known thermodynamic
parameters.
To determine the oxidation potential of the
system Fe + FeV2O4-V2O3, K.T. Jacob and C.B.
Alcock [16] used the EMF method. The same
method was used to determine the thermodynamic
data for Mn3O4, Mn2O3 and MnO2 [17, 18]. A.N.
Grundy et al. [19] studied the thermodynamics and
the phase diagram of system Mn-O, using
CALPHAD method. A. Petric and K.T. Jacob
determined the activity of Fe3O4 in the solid solution
Fe3O4-FeV2O4 [20]. In this paper [21] the authors
analyzed in detail the reactions occurring in the
system FeO-V2O5 and their Gibbs energy
respectively.
The standard Gibbs energy of spinel phase
MnV2O4 formation in the temperature range 1200-
1600o
C was calculated using the equation of
mixtures in the liquid iron or liquid copper and the
known thermodynamic parameters [22, 23].
The purpose of these investigations is to
describe the phase changes that occur in the non-
isothermal heating synthetic ternary system (Fe2O3-
MnO-V2O5), and ternary system containing waste
vanadium catalyst, manganese concentrate, and
Fe2O3. The thermodynamic characteristics of this
system will be used as a basis for the production of
complex alloy with the participation of waste
material.
II. EXPERIMENTAL AND DISCUSSION
2.1. Materials and Apparatus
The chemical composition (mass %) of
manganese concentrate is shown in Table 1.
Table 1 Chemical composition of manganese
concentrate, %.
MnO FeS2 Fe2O3 P2O5 SiO2 MgO CaO Al2O3
44,56 2,25 1,79 0,31 12,4 2,00 3,90 2,10
The chemical composition (mass %) of waste
vanadium catalyst is shown in Table 2.
Table 2 Chemical composition of waste vanadium
catalyst, %.
V2O5 Fe2O3 SiO2 K2O Na2O Al2O3 SO3
4,12 3,4 57,12 6,71 3,93 0,82 23,88
Experiments were carried out using manganese
concentrate, waste vanadium catalyst and chemically
pure oxides Fe2O3, MnO (MnO2), V2O5, SiO2.
The synthetic Mix 1 is composed of pure
oxides. The quantitative ratio between oxides is
calculated so as to be correlated with Mix 2
containing manganese concentrate and the waste
vanadium catalyst. In this mixture are given only
oxides, which could influence the process of the
complex alloy obtaining.
Mix 1 – pure oxides - V2O5 - MnO - Fe2O3 – SiO2.
Mix 2 – waste vanadium catalyst, manganese
concentrate, and Fe2O3.
The composition of the mixtures is as follows:
2,5% V2O5; 22,5 % MnO; 35 % SiO2 and 40 %
Fe2O3.
The mixtures were investigated by DTA method
within the temperature range 293 K – 1473 K using
thermogravimetric apparatus STA PT1600.
The thermodynamics of mixtures were also
studied by EMF method using galvanic cells with a
solid electrolyte ZrO2 (Y2O3) and reference
electrodes Ni/NiO, air, and Mo/MoO2
The equilibrium of oxides in the system Fe2O3 -
MnO - V2O5- SiO2 was studied with the following
galvanic cells:
Pt system ZrO2(Y2O3)air Pt
2OP 2
"OP
Pt system ZrO2(Y2O3)Ni/NiO Pt
2OP 2
"OP
Pt system ZrO2(Y2O3)Мо/МоО3Pt
2OP 2
"OP
PO2= 0,2095 atm; lg PO2= - 0,6788 for the air
electrode.
The GT (NiO) values reported by some other
authors [24 - 26] were used in this paper.
2Ni + O2 = 2NiO (1)
Gо
(NiO) = -233651 + 84.893 T, J / mol
44,4
12225
lg 2



T
PO (2)
The GT (MoO2) values reported by some
other authors [27, 28] were also used in this paper.
2Mo + 2O2 = 2MoO2 (3)
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ISSN: 2248-9622, Vol. 5, Issue 12, (Part - 3) December 2015, pp.92-100
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Gо
( МоО2 ) = -570563 + 173.Т
051,9
29852
lg 2



T
PO (4)
2.2. DTA Results
The derivatogram of Mix 1 (pure oxides Fe2O3-
MnO2-V2O5- SiO2) is presented in Fig.1. The DTA
curve shows two low-temperature endothermic
effects. The first one (Т ~ 107о
С) corresponds to the
evaporation of physical moisture and the second one
(Т ~348о
С) – to partial dissociation of MnO2 to
Mn2O3. In the temperature range from Т  582o
C to
Т  667o
C solid solution between Fe2O3 and Mn2O3
from a peritectic type was formed. The peritectic
solution decomposes at about 930o
C. A solid
solution between Mn2O3 and Mn3O4 is formed which
can be confirmed by the phase diagram (Fe2O3 -
Mn2O3) [30]. The X-ray analysis (Fig.2) shows that
in the end product the following phases were found:
cubic Mn2O3, rhombic Hematite Fe2O3, tetragonal
Hausmannite (Mn3O4) as well, tetragonal α-
Cristoballite (SiO2).
Derivatogram of Mix 2 (waste vanadium
catalyst, Mn-concentrate, and Fe2O3) is presented in
Fig.3. The DTA curve shows one intensive
endothermic effect and three less intensive
endothermic effects. One of them at about Т 715o
C
corresponds to FeV2O4 or FeV2O6 formation. In this
sample, the formation of these ferrovanadates is
possible at low temperature and even at low
vanadium oxide concentration in the system Fе-V-O
these compositions could be formed [29]. In waste
vanadium catalyst (as opposed to pure V2O5 in mix
1), vanadium oxides are in the form of VxOy (V2O3,
VO, V2O4, V6O13) and formation of these vanadates
is possible by reason of its repeated thermal
transformations. X-ray analysis confirms the fact
(Fig.4), that except for rhombic Hematite (Fe2O3),
tetragonal Cristaloballite (SiO2), cubic Bixbyite
(Mn2O3), tetragonal Hausmannite (Mn3O4),
Coulsonite Fe2VO4 (Fe2O3.VO) is also present. In
the temperature range from Т  575o
C to Т  680o
C
solid solution is formed between Fe2O3 and Mn2O3
from a peritectic type that decomposes at about
930o
C to solid solution between Mn2O3 and Mn3O4,
which can be confirmed by the phase diagram
(Fe2O3 - Mn2O3)[30].
The melting phase in Mix 2 was registered upon
heating up to 1200o
C. The X-ray analysis (Fig.5.) of
the obtained product from Mix 2 treated at this
temperature, showed mainly presence of Jacobsite
(Mn6Fe4)(Mn4Fe1.6)O4, as well as vanadium oxide
(V3O4), Coulsonite Fe2VO4 (Fe2O3.VO), Hematite
and α -Quartz.
Fig.1. Derivatogram of Mix 1 (pure oxides Fe2O3 - MnO2-V2O5 – SiO2)
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ISSN: 2248-9622, Vol. 5, Issue 12, (Part - 3) December 2015, pp.92-100
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Hematite, syn
01-080-0382 (C) - Hausmannite - Mn3O4 - Y: 8.65 % - d x by: 1. - WL: 1.5406 - Tetragonal - a 5.76500 - b 5.76500 - c 9.44200 - alpha 90.000 - beta 90.000 - gamma 90.000 - Body-centered - I41/amd (141) - 4 - 31
01-082-1403 (C) - Cristobalite beta, syn - SiO2 - Y: 50.50 % - d x by: 1. - WL: 1.5406 - Tetragonal - a 4.97800 - b 4.97800 - c 6.93210 - alpha 90.000 - beta 90.000 - gamma 90.000 - Primitive - P41212 (92) - 4 - 171
01-071-0636 (C) - Manganese Oxide - Mn2O3 - Y: 74.58 % - d x by: 1. - WL: 1.5406 - Cubic - a 9.41460 - b 9.41460 - c 9.41460 - alpha 90.000 - beta 90.000 - gamma 90.000 - Body-centered - Ia-3 (206) - 16 - 834.
01-086-2368 (C) - Hematite, syn - Fe2O3 - Y: 61.65 % - d x by: 1. - WL: 1.5406 - Rhombo.H.axes - a 5.03550 - b 5.03550 - c 13.74710 - alpha 90.000 - beta 90.000 - gamma 120.000 - Primitive - R-3c (167) - 6 - 30
Operations: Background 1.000,1.000 | Import
File: 5.raw - Type: 2Th/Th locked - Start: 10.000 ° - End: 80.000 ° - Step: 0.040 ° - Step time: 1. s - Temp.: 25 °C (Room) - Time Started: 8 s - 2-Theta: 10.000 ° - Theta: 5.000 ° - Chi: 0.00 ° - Phi: 0.00 ° - X: 0.0 mm -
Lin(Counts)
0
100
200
300
400
500
600
700
800
2-Theta - Scale
10 20 30 40 50 60 70 80
Fig.2. X- ray analysis of obtained product of Mix 1 (heated up to Т= 1198K).
Fig.3. Derivatogram of Mix 2 (Fe2O3, waste vanadium catalyst and manganese concentrate).
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Hematite, syn
01-080-0382 (C) - Hausmannite - Mn3O4 - Y: 6.09 % - d x by: 1. - WL: 1.5406 - Tetragonal - a 5.76500 - b 5.76500 - c 9.44200 - alpha 90.000 - beta 90.000 - gamma 90.000 - Body-centered - I41/amd (141) - 4 - 31
01-075-1519 (C) - Coulsonite, syn - Fe2VO4 - Y: 24.88 % - d x by: 1. - WL: 1.5406 - Cubic - a 8.42100 - b 8.42100 - c 8.42100 - alpha 90.000 - beta 90.000 - gamma 90.000 - Face-centered - Fd-3m (227) - 8 - 597.1
00-041-1442 (*) - Bixbyite-C, syn - Mn2O3 - Y: 16.05 % - d x by: 1. - WL: 1.5406 - Cubic - a 9.40910 - b 9.40910 - c 9.40910 - alpha 90.000 - beta 90.000 - gamma 90.000 - Body-centered - Ia-3 (206) - 16 - 832.998
01-077-1316 (A) - Cristobalite low, syn - SiO2 - Y: 43.48 % - d x by: 1. - WL: 1.5406 - Tetragonal - a 4.97090 - b 4.97090 - c 6.92780 - alpha 90.000 - beta 90.000 - gamma 90.000 - Primitive - P41212 (92) - 4 - 171.
01-086-2368 (C) - Hematite, syn - Fe2O3 - Y: 80.94 % - d x by: 1. - WL: 1.5406 - Rhombo.H.axes - a 5.03550 - b 5.03550 - c 13.74710 - alpha 90.000 - beta 90.000 - gamma 120.000 - Primitive - R-3c (167) - 6 - 30
Operations: Background 1.000,1.000 | Import
File: 6.raw - Type: 2Th/Th locked - Start: 10.000 ° - End: 80.000 ° - Step: 0.040 ° - Step time: 1. s - Temp.: 25 °C (Room) - Time Started: 9 s - 2-Theta: 10.000 ° - Theta: 5.000 ° - Chi: 0.00 ° - Phi: 0.00 ° - X: 0.0 mm -
Lin(Counts)
0
100
200
300
400
500
600
700
800
900
2-Theta - Scale
10 20 30 40 50 60 70 80
Fig.4. X- ray analysis of the obtained product of Mix 2 (heated up to Т= 1183К).Jacobsite syn, precipitated
01-085-1054 (C) - Quartz alpha - SiO2 - Y: 17.01 % - d x by: 1. - WL: 1.5406 - Hexagonal - a 4.90390 - b 4.90390 - c 5.39430 - alpha 90.000 - beta 90.000 - gamma 120.000 - Primitive - P3221 (154) - 3 - 112.344 - I
01-075-1519 (C) - Coulsonite, syn - Fe2VO4 - Y: 22.77 % - d x by: 1. - WL: 1.5406 - Cubic - a 8.42100 - b 8.42100 - c 8.42100 - alpha 90.000 - beta 90.000 - gamma 90.000 - Face-centered - Fd-3m (227) - 8 - 597.1
00-034-0615 (I) - Vanadium Oxide - V3O4 - Y: 29.18 % - d x by: 1. - WL: 1.5406 - Cubic - a 8.45700 - b 8.45700 - c 8.45700 - alpha 90.000 - beta 90.000 - gamma 90.000 - Face-centered - F (0) - 8 - 604.852 - F16=
01-085-0599 (C) - Hematite - Fe2O3 - Y: 18.21 % - d x by: 1. - WL: 1.5406 - Rhombo.R.axes - a 5.42000 - b 5.42000 - c 5.42000 - alpha 55.120 - beta 55.120 - gamma 55.120 - Primitive - R-3c (167) - 2 - 99.8086 -
01-088-1965 (C) - Jacobsite syn, precipitated - (Mn.6Fe.4)(Mn.4Fe1.6)O4 - Y: 49.72 % - d x by: 1. - WL: 1.5406 - Cubic - a 8.49700 - b 8.49700 - c 8.49700 - alpha 90.000 - beta 90.000 - gamma 90.000 - Face-cent
Operations: Background 1.000,1.000 | Import
File: 6-17112009.raw - Type: 2Th/Th locked - Start: 10.000 ° - End: 80.020 ° - Step: 0.060 ° - Step time: 1. s - Temp.: 25 °C (Room) - Time Started: 9 s - 2-Theta: 10.000 ° - Theta: 5.000 ° - Chi: 0.00 ° - Phi: 0.00 ° -
Lin(Counts)
0
10
20
30
40
50
60
70
80
90
100
110
120
130
140
150
160
170
180
190
2-Theta - Scale
10 20 30 40 50 60 70 80
Fig.5. X- ray analysis of obtained product of Mix 2 (heated up to Т= 1498К).
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2.3. EMF results
Partial pressure of the oxygen in the mixtures
was calculated by the following equations:
For air reference electrode
6788.0
20193.
lg 2

T
E
PO (5)
For reference electrode Ni/NiO
44.4
1222520193.
lg 2

TT
E
PO (6)
For reference electrode Мо/МоО2
051.9
2985220193.
lg 2

TT
E
PO (7)
The obtained results of the EMF experimental
data is shown in Table 3. The values are an average
result of six measurements.
In the studied system Fe2O3-MnO-V2O5-SiO2, a
number of reactions could take place. Equations G
= f (T) were deduced for the main reactions, using
thermodynamic data for Ho
, So
and Cp obtained by
some authors [23, 24]. The calculated results for
these reactions and the reported ones by some other
authors were compared with our results obtained
experimentally. The dependences of G = f (T) for
the investigated mixtures in air, Ni/NiO and
Mo/MoO2 as reference electrode are shown in Fig. 6,
7 and 8.
The proposed reactions (shown in Table 4), were
accorded with the results of X-ray analysis (Figure
2.4, 5) of the obtained products of both tested
mixtures.
Table 3. EMF experimental data of both mixtures
Mix 1
air Ni/NiO Mo/MoO3
T, K E, V 2
lg OP  T, K E, V 2
lg OP  T, K E, V 2
lg OP 
1093 0.588 - 25.64 1113 0.376 - 22.22 1093 0.463 - 37.92
1123 0.546 - 23.24 1123 0.373 - 21.86 1123 0.444 - 35.88
1133 0,497 - 21.03 1133 0.370 - 21.50 1133 0.437 - 35.19
1143 0,488 - 20.49 1143 0.363 - 20.99 1143 0.436 - 34.77
1153 0,482 - 20.08 1153 0.362 - 20.73 1153 0.435 - 34.35
1163 0,478 - 19.75 1163 0.360 - 20.43 1163 0.436 - 34.01
1173 0,472 - 19.35
Mix 2
air Ni/NiO Mo/MoO3
T, K E, V 2
lg OP  T, K E, V 2
lg OP  T, K E, V 2
lg OP 
1083 0.564 - 24.84 1123 0.406 - 23.22 1093 0.494 - 39.23
1093 0.548 - 23.94 1133 0.390 - 22.32 1103 0.424 - 35.85
1103 0,526 - 22.81 1143 0.359 - 20.83 1123 0.390 - 33.65
1113 0,520 - 22.36 1153 0.328 - 19.36 1133 0.359 - 32.00
1123 0,518 - 22.08 1163 0.320 - 18.84 1143 0.356 - 31.52
1133 0,498 - 21.07 1173 0.314 - 18.40 1163 0.354 - 30.74
1143 0,470 - 19.76
1153 0.462 - 19.27
The deduced dependences G = f (T) based on experimental data are as follows:
Mix 1
- for air reference electrode ΔG exp.= -864 166+580,74.T , J.mol-1
(R2
= 0,8922),
- for Ni/NiO reference electrode ΔG exp.= -393 685+169,11.T , J.mol-1
(R2
= 0,9722)
- for Mo/MoO2 reference electrode ΔG exp.= -594 159+230,08.T , J.mol-1
(R2
= 0,9215).
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Mix 2
- for air reference electrode ΔG exp.= -808 621+540,62.T , J.mol-1 (R2 = 0,9633)
- for Ni/NiO reference electrode ΔG exp.= -1.106
+809,18.T , J.mol-1
(R2
= 0,9473)
- for Mo/MoO2 reference electrode ΔG exp.= -2.107
+35776.T -15,513. Т2
, J.mol-1
(R2
= 0,9706)
where R is a correlation coefficient
Table 4 Gibbs Energy Equations of the expected reactions.
Mix 1
2Fe3O4 + ½ O2 = 3Fe2O3 G1 = -586770 + 340.2.T, J.mol-1
[34]
6MnO + O2 = 2 Mn3O4
ΔG 2 = -563241 + 1761.758.T-
220.490.T.lnT + 0.101819.T2 [18]
G3 = -222470 + 111,1.T ,J.mol-1
[19]
ΔG 4=-445606+221,70.T J.mol-1
[17]
6MnO+O2=2Mn3O4
ΔG 5= -443067+0,7.106
.T-2
+144,4.T-
(22,1.10-3
).T2
+15.67.lnT , J.mol-1 [33]
6MnO+O2=2Mn3O4 ΔG 6= -541,31+0,3593.T , J.mol-1
in this work
Mix 2
2 Fe+O2+2V2O3=2FeV2O4 ΔG 7 = -577500+124,7 . T ,J.mol-1
in this work
Fe2O3+MnO=Fe2MnO4 ΔG 8= -17669 -6,8286.T ,J.mol-1
in this work
4Fe3O4+O2=6Fe2O3 ΔG 9= -417348+147,73.T , J.mol-1
in this work
V2O3+FeO+O2=FeV2O6 ΔG 10= -449912+35,441.T , J.mol-1
in this work
2FeO+V2O4=Fe2O3+V2O3 ΔG 11= -77323+48,84.T , J.mol-1
[21]
FeO+V2O3=FeV3O4 ΔG 12= -24700-2,25.T , J.mol-1
[21]
Fig.6. Dependence of G = f (T) for Mix 1 (air as a
reference electrode)
Fig.7. Dependence of G = f (T) for Mix 1 (Ni/NiO
as a reference electrode)
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Fig.8. Dependence of G = f (T) for Mix 1
(Mo/MoO2 as a reference electrode)
1080 1090 1100 1110 1120 1130 1140 1150 1160
-450000
-400000
-350000
-300000
-250000
-200000
-150000
-100000
-30000
-25000
-20000
-15000
-10000
-5000
0
delta G10
delta G7
delta G12
delta G11
delta G3
delta G9
delta G8
delta G exp.
deltaG,J/mol
T, K
Fig.9. Dependence of G = f (T) for Mix 2 (air
as a reference electrode)
1120 1130 1140 1150 1160 1170 1180
-450000
-400000
-350000
-300000
-250000
-200000
-150000
-100000
-30000
-25000
-20000
-15000
-10000
-5000
0
delta G 11
delta G 3
delta G 9
delta G 8
delta G 12
delta G 10
delta G 7
delta G exp.
deltaG,J/mol
T, K
Fig.10. Dependence of G = f (T) for Mix 2 (Ni/NiO
as a reference electrode)
1090 1100 1110 1120 1130 1140 1150 1160 1170
-450000
-400000
-350000
-300000
-250000
-200000
-150000
-100000
-30000
-25000
-20000
-15000
-10000
-5000
0
delta G 11
delta G 8
delta G 12
delta G 3
delta G 9
delta G 10
delta G 7
delta G exp.
deltaG,J/mol
T, K
Fig.11. Dependence of G = f (T) for Mixture 2
(Mo/MoO2 as a reference electrode)
The comparison of the experimental data of the
three types of reference electrodes with the
theoretically calculated values for Hematite showed
that the obtained results with reference electrodes air
and Ni/NiO were very close to the theoretical values
(particularly for Mixture 1), while those of
Mo/MoO3 essentially differed. That is why when
thermodynamics of the processes including iron
oxides is studied; these two reference electrodes are
more suitable than molybdenum.
III. CONCLUSION
1. It was found out that the phase
transformations up to 1473 K and forming of new
phases in the mixtures, for example FeV2O4
(coulsonite) (at 1173K) and Iron Vanadium Oxide
type (Fe6.5V11..5O35) (at 1473K) and Jacobsite types
MnFe2O4 (at 1173K) and (Mn6Fe4)(Mn4Fe1.6)O4 (at
1473K ) could happen only if in the initial
materials contained waste vanadium catalyst and
manganese concentrate. The X-ray analysis
confirmed the presence mainly of hematite phase,
cubic and tetragonal Mn2O3, hausmanit (Mn3O4).
2. Based on the experimental results obtained
after the heating of mixtures containing oxides of
iron, manganese and vanadium the relationship of
Go
T = f(T) in the temperature range 1073 – 1173 К
was obtained, using EMF method with the three
different reference electrodes (Ni/NiO, Mo/MoO3
and air). Gibbs energy for Mix 1 and Mix 2 were
very close to the theoretically calculated values for
Fe2O3 using reference electrodes Ni/NiO and air
while that of Mo/MoO2 essentially differed. The X-
ray analysis confirmed the presence of hematite
phase.
3. It was proved that waste vanadium catalyst
and manganese concentrate were more appropriate
precursors for the production of complex iron
vanadium manganese alloy than the pure oxides -
V2O5 and MnO2.
REFERENCES
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Fe2O3, Journal of Thermal Analysis and Calorimetry,
88(1), 2007, 201-205.
[2] A. Blonska-Tabero and B. Monika, Comparative studies
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Phase equilibria of the MnFeO system (Fe/Mn = 2),
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and Mn3O4, Contrib. Mineral Petrol 114, 1993, 315-320.
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Mn-O, J. Phase Equilib., 24, 2003, 21-39.
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Fe3O4-FeV2O4 and Fe3O4-FeCr2O4 Spinel Solid Solution,
Journal of the American Ceramic Society, 1982( online
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Temperature, Journal of Iron and Steel Research,
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Phase Transformations and Thermodynamics in the System Fe2О3– V2О5 – MnО – SiО2 of Non-Isothermal Heating

  • 1. R. Paunova et al. Int. Journal of Engineering Research and Applications www.ijera.com ISSN: 2248-9622, Vol. 5, Issue 12, (Part - 3) December 2015, pp.92-100 www.ijera.com 92 | P a g e Phase Transformations and Thermodynamics in the System Fe2О3– V2О5 – MnО – SiО2 of Non-Isothermal Heating R. Paunova, D. Grigorova, R. Alexandrova Department of Ferrous Metallurgy and Metal Foundry, University of Chemical Technology and Metallurgy Bulgaria ABSTRACT Thermodynamic characteristics in the system Fe2O3 – MnO – V2O5 –SiO2 have been investigated. Two mixtures have been prepared. The first mixture was synthetic, prepared from pure oxides in proportion according to the chemical composition of the waste catalyst and manganese concentrate. The second one contained the waste vanadium catalyst and manganese concentrate. The synthetic mixture has been used as a standard in order to establish the influence of impurities in the concentrate, and the waste catalyst on the thermodynamics of the studied system. Experiments carried out in the temperature up to 1473 K for the system containing waste vanadium catalyst and manganese concentrate occur to formation of new phases formation as FeV2O4 and Iron Vanadium Oxide type and Jacobsite types MnFe2O4 and (Mn6Fe4)(Mn4Fe1.6)O4. EMF method with difference reference electrode (Ni/NiO, Mo/MoO2 and air) relationship of delta GoT = f(T) in the temperature range 1073 – 1173 К of mixtures was obtained. The experimental data for the system show that the reference electrodes air and Ni/NiO are more suitable than Mo/MoO2. The obtained results will be used as an investigations base to the production of complex iron vanadium manganese alloy using the waste materials. Keywords – thermodynamics, DTA, EMF method, vanadium catalyst, manganese concentrate. I. INTRODUCTION From a metallurgical point of view, the study of binary and ternary systems has great practical significance even for ferroalloy production to obtain alloys. Complex alloys are becoming more and more widely used in metallurgy for deoxidation, alloying, modifying and desulfurization; they also improve the mechanical, physical and chemical properties of steel and iron. It is more effective to obtain elements as a complex ferroalloy than as separate elements. In the present studies, the waste vanadium catalyst was used. Annually, between 500 and 1000 tons vanadium catalyst are released from sulphur acid production which contains a significant quantity of deficit vanadium. The toxicity of the vanadium causes certain environmental problems which is an additional consideration to look for ways to utilize this valuable waste product. The complex systems are used in various fields of Chemistry and Metallurgy. Ternary systems of the type MeO-V2O5-Fe2O3 are used as catalysts because vanadates, which are formed, as a result, catalyze the oxidation processes of many compounds [1]. The similar systems is also used in the electrode materials preparation, and glasses with relatively high electrical conductivity and high thermal stability or for correction of the phase diagram. [1, 2, 3, 4, 5, 6, 7, 8]. Other studies have focused on the structure of complex compounds produced by the solid-phase method - Co4Fe3.33 (VO4) 6 [9], Mn3Fe4 (VO4) 6 [9, 11] and Zn3Fe4V6O24 [10]. The equilibrium in the system V2O5-Fe2O3-Mn2O3 (MnO) was examined by some authors [12]. They found out the formation of the solid solution of the type Fe2Mn2V4O15 based on manganese pyrovanadat. DTA and XRD analyses were used in the investigation of all these systems. In the binary system MnxFe3-xO4, containing manganese oxides, the heat capacity for different values of “x”was determined as well as the entropy changes [13]. The phase equilibrium of the Mn-Fe-O system (Fe / Mn = 2) and the partial pressure of oxygen of 10-1 Pa to 105 Pa were examined in the temperature range from 1223 to 1393 K, by measuring the electrical conductivity and the mass of the sample [14]. The enthalpy and Gibbs free energy of (MnxFe1-x)3O4 at 298 K were defined calorimetrically[15]. Some other authors analyzed the thermodynamics of the processes in the ternary RESEARCH ARTICLE OPEN ACCESS
  • 2. R. Paunova et al. Int. Journal of Engineering Research and Applications www.ijera.com ISSN: 2248-9622, Vol. 5, Issue 12, (Part - 3) December 2015, pp.92-100 www.ijera.com 93 | P a g e system Fe2O3-V2O5-MnO using data for the binary systems respectively or some known thermodynamic parameters. To determine the oxidation potential of the system Fe + FeV2O4-V2O3, K.T. Jacob and C.B. Alcock [16] used the EMF method. The same method was used to determine the thermodynamic data for Mn3O4, Mn2O3 and MnO2 [17, 18]. A.N. Grundy et al. [19] studied the thermodynamics and the phase diagram of system Mn-O, using CALPHAD method. A. Petric and K.T. Jacob determined the activity of Fe3O4 in the solid solution Fe3O4-FeV2O4 [20]. In this paper [21] the authors analyzed in detail the reactions occurring in the system FeO-V2O5 and their Gibbs energy respectively. The standard Gibbs energy of spinel phase MnV2O4 formation in the temperature range 1200- 1600o C was calculated using the equation of mixtures in the liquid iron or liquid copper and the known thermodynamic parameters [22, 23]. The purpose of these investigations is to describe the phase changes that occur in the non- isothermal heating synthetic ternary system (Fe2O3- MnO-V2O5), and ternary system containing waste vanadium catalyst, manganese concentrate, and Fe2O3. The thermodynamic characteristics of this system will be used as a basis for the production of complex alloy with the participation of waste material. II. EXPERIMENTAL AND DISCUSSION 2.1. Materials and Apparatus The chemical composition (mass %) of manganese concentrate is shown in Table 1. Table 1 Chemical composition of manganese concentrate, %. MnO FeS2 Fe2O3 P2O5 SiO2 MgO CaO Al2O3 44,56 2,25 1,79 0,31 12,4 2,00 3,90 2,10 The chemical composition (mass %) of waste vanadium catalyst is shown in Table 2. Table 2 Chemical composition of waste vanadium catalyst, %. V2O5 Fe2O3 SiO2 K2O Na2O Al2O3 SO3 4,12 3,4 57,12 6,71 3,93 0,82 23,88 Experiments were carried out using manganese concentrate, waste vanadium catalyst and chemically pure oxides Fe2O3, MnO (MnO2), V2O5, SiO2. The synthetic Mix 1 is composed of pure oxides. The quantitative ratio between oxides is calculated so as to be correlated with Mix 2 containing manganese concentrate and the waste vanadium catalyst. In this mixture are given only oxides, which could influence the process of the complex alloy obtaining. Mix 1 – pure oxides - V2O5 - MnO - Fe2O3 – SiO2. Mix 2 – waste vanadium catalyst, manganese concentrate, and Fe2O3. The composition of the mixtures is as follows: 2,5% V2O5; 22,5 % MnO; 35 % SiO2 and 40 % Fe2O3. The mixtures were investigated by DTA method within the temperature range 293 K – 1473 K using thermogravimetric apparatus STA PT1600. The thermodynamics of mixtures were also studied by EMF method using galvanic cells with a solid electrolyte ZrO2 (Y2O3) and reference electrodes Ni/NiO, air, and Mo/MoO2 The equilibrium of oxides in the system Fe2O3 - MnO - V2O5- SiO2 was studied with the following galvanic cells: Pt system ZrO2(Y2O3)air Pt 2OP 2 "OP Pt system ZrO2(Y2O3)Ni/NiO Pt 2OP 2 "OP Pt system ZrO2(Y2O3)Мо/МоО3Pt 2OP 2 "OP PO2= 0,2095 atm; lg PO2= - 0,6788 for the air electrode. The GT (NiO) values reported by some other authors [24 - 26] were used in this paper. 2Ni + O2 = 2NiO (1) Gо (NiO) = -233651 + 84.893 T, J / mol 44,4 12225 lg 2    T PO (2) The GT (MoO2) values reported by some other authors [27, 28] were also used in this paper. 2Mo + 2O2 = 2MoO2 (3)
  • 3. R. Paunova et al. Int. Journal of Engineering Research and Applications www.ijera.com ISSN: 2248-9622, Vol. 5, Issue 12, (Part - 3) December 2015, pp.92-100 www.ijera.com 94 | P a g e Gо ( МоО2 ) = -570563 + 173.Т 051,9 29852 lg 2    T PO (4) 2.2. DTA Results The derivatogram of Mix 1 (pure oxides Fe2O3- MnO2-V2O5- SiO2) is presented in Fig.1. The DTA curve shows two low-temperature endothermic effects. The first one (Т ~ 107о С) corresponds to the evaporation of physical moisture and the second one (Т ~348о С) – to partial dissociation of MnO2 to Mn2O3. In the temperature range from Т  582o C to Т  667o C solid solution between Fe2O3 and Mn2O3 from a peritectic type was formed. The peritectic solution decomposes at about 930o C. A solid solution between Mn2O3 and Mn3O4 is formed which can be confirmed by the phase diagram (Fe2O3 - Mn2O3) [30]. The X-ray analysis (Fig.2) shows that in the end product the following phases were found: cubic Mn2O3, rhombic Hematite Fe2O3, tetragonal Hausmannite (Mn3O4) as well, tetragonal α- Cristoballite (SiO2). Derivatogram of Mix 2 (waste vanadium catalyst, Mn-concentrate, and Fe2O3) is presented in Fig.3. The DTA curve shows one intensive endothermic effect and three less intensive endothermic effects. One of them at about Т 715o C corresponds to FeV2O4 or FeV2O6 formation. In this sample, the formation of these ferrovanadates is possible at low temperature and even at low vanadium oxide concentration in the system Fе-V-O these compositions could be formed [29]. In waste vanadium catalyst (as opposed to pure V2O5 in mix 1), vanadium oxides are in the form of VxOy (V2O3, VO, V2O4, V6O13) and formation of these vanadates is possible by reason of its repeated thermal transformations. X-ray analysis confirms the fact (Fig.4), that except for rhombic Hematite (Fe2O3), tetragonal Cristaloballite (SiO2), cubic Bixbyite (Mn2O3), tetragonal Hausmannite (Mn3O4), Coulsonite Fe2VO4 (Fe2O3.VO) is also present. In the temperature range from Т  575o C to Т  680o C solid solution is formed between Fe2O3 and Mn2O3 from a peritectic type that decomposes at about 930o C to solid solution between Mn2O3 and Mn3O4, which can be confirmed by the phase diagram (Fe2O3 - Mn2O3)[30]. The melting phase in Mix 2 was registered upon heating up to 1200o C. The X-ray analysis (Fig.5.) of the obtained product from Mix 2 treated at this temperature, showed mainly presence of Jacobsite (Mn6Fe4)(Mn4Fe1.6)O4, as well as vanadium oxide (V3O4), Coulsonite Fe2VO4 (Fe2O3.VO), Hematite and α -Quartz. Fig.1. Derivatogram of Mix 1 (pure oxides Fe2O3 - MnO2-V2O5 – SiO2)
  • 4. R. Paunova et al. Int. Journal of Engineering Research and Applications www.ijera.com ISSN: 2248-9622, Vol. 5, Issue 12, (Part - 3) December 2015, pp.92-100 www.ijera.com 95 | P a g e Hematite, syn 01-080-0382 (C) - Hausmannite - Mn3O4 - Y: 8.65 % - d x by: 1. - WL: 1.5406 - Tetragonal - a 5.76500 - b 5.76500 - c 9.44200 - alpha 90.000 - beta 90.000 - gamma 90.000 - Body-centered - I41/amd (141) - 4 - 31 01-082-1403 (C) - Cristobalite beta, syn - SiO2 - Y: 50.50 % - d x by: 1. - WL: 1.5406 - Tetragonal - a 4.97800 - b 4.97800 - c 6.93210 - alpha 90.000 - beta 90.000 - gamma 90.000 - Primitive - P41212 (92) - 4 - 171 01-071-0636 (C) - Manganese Oxide - Mn2O3 - Y: 74.58 % - d x by: 1. - WL: 1.5406 - Cubic - a 9.41460 - b 9.41460 - c 9.41460 - alpha 90.000 - beta 90.000 - gamma 90.000 - Body-centered - Ia-3 (206) - 16 - 834. 01-086-2368 (C) - Hematite, syn - Fe2O3 - Y: 61.65 % - d x by: 1. - WL: 1.5406 - Rhombo.H.axes - a 5.03550 - b 5.03550 - c 13.74710 - alpha 90.000 - beta 90.000 - gamma 120.000 - Primitive - R-3c (167) - 6 - 30 Operations: Background 1.000,1.000 | Import File: 5.raw - Type: 2Th/Th locked - Start: 10.000 ° - End: 80.000 ° - Step: 0.040 ° - Step time: 1. s - Temp.: 25 °C (Room) - Time Started: 8 s - 2-Theta: 10.000 ° - Theta: 5.000 ° - Chi: 0.00 ° - Phi: 0.00 ° - X: 0.0 mm - Lin(Counts) 0 100 200 300 400 500 600 700 800 2-Theta - Scale 10 20 30 40 50 60 70 80 Fig.2. X- ray analysis of obtained product of Mix 1 (heated up to Т= 1198K). Fig.3. Derivatogram of Mix 2 (Fe2O3, waste vanadium catalyst and manganese concentrate).
  • 5. R. Paunova et al. Int. Journal of Engineering Research and Applications www.ijera.com ISSN: 2248-9622, Vol. 5, Issue 12, (Part - 3) December 2015, pp.92-100 www.ijera.com 96 | P a g e Hematite, syn 01-080-0382 (C) - Hausmannite - Mn3O4 - Y: 6.09 % - d x by: 1. - WL: 1.5406 - Tetragonal - a 5.76500 - b 5.76500 - c 9.44200 - alpha 90.000 - beta 90.000 - gamma 90.000 - Body-centered - I41/amd (141) - 4 - 31 01-075-1519 (C) - Coulsonite, syn - Fe2VO4 - Y: 24.88 % - d x by: 1. - WL: 1.5406 - Cubic - a 8.42100 - b 8.42100 - c 8.42100 - alpha 90.000 - beta 90.000 - gamma 90.000 - Face-centered - Fd-3m (227) - 8 - 597.1 00-041-1442 (*) - Bixbyite-C, syn - Mn2O3 - Y: 16.05 % - d x by: 1. - WL: 1.5406 - Cubic - a 9.40910 - b 9.40910 - c 9.40910 - alpha 90.000 - beta 90.000 - gamma 90.000 - Body-centered - Ia-3 (206) - 16 - 832.998 01-077-1316 (A) - Cristobalite low, syn - SiO2 - Y: 43.48 % - d x by: 1. - WL: 1.5406 - Tetragonal - a 4.97090 - b 4.97090 - c 6.92780 - alpha 90.000 - beta 90.000 - gamma 90.000 - Primitive - P41212 (92) - 4 - 171. 01-086-2368 (C) - Hematite, syn - Fe2O3 - Y: 80.94 % - d x by: 1. - WL: 1.5406 - Rhombo.H.axes - a 5.03550 - b 5.03550 - c 13.74710 - alpha 90.000 - beta 90.000 - gamma 120.000 - Primitive - R-3c (167) - 6 - 30 Operations: Background 1.000,1.000 | Import File: 6.raw - Type: 2Th/Th locked - Start: 10.000 ° - End: 80.000 ° - Step: 0.040 ° - Step time: 1. s - Temp.: 25 °C (Room) - Time Started: 9 s - 2-Theta: 10.000 ° - Theta: 5.000 ° - Chi: 0.00 ° - Phi: 0.00 ° - X: 0.0 mm - Lin(Counts) 0 100 200 300 400 500 600 700 800 900 2-Theta - Scale 10 20 30 40 50 60 70 80 Fig.4. X- ray analysis of the obtained product of Mix 2 (heated up to Т= 1183К).Jacobsite syn, precipitated 01-085-1054 (C) - Quartz alpha - SiO2 - Y: 17.01 % - d x by: 1. - WL: 1.5406 - Hexagonal - a 4.90390 - b 4.90390 - c 5.39430 - alpha 90.000 - beta 90.000 - gamma 120.000 - Primitive - P3221 (154) - 3 - 112.344 - I 01-075-1519 (C) - Coulsonite, syn - Fe2VO4 - Y: 22.77 % - d x by: 1. - WL: 1.5406 - Cubic - a 8.42100 - b 8.42100 - c 8.42100 - alpha 90.000 - beta 90.000 - gamma 90.000 - Face-centered - Fd-3m (227) - 8 - 597.1 00-034-0615 (I) - Vanadium Oxide - V3O4 - Y: 29.18 % - d x by: 1. - WL: 1.5406 - Cubic - a 8.45700 - b 8.45700 - c 8.45700 - alpha 90.000 - beta 90.000 - gamma 90.000 - Face-centered - F (0) - 8 - 604.852 - F16= 01-085-0599 (C) - Hematite - Fe2O3 - Y: 18.21 % - d x by: 1. - WL: 1.5406 - Rhombo.R.axes - a 5.42000 - b 5.42000 - c 5.42000 - alpha 55.120 - beta 55.120 - gamma 55.120 - Primitive - R-3c (167) - 2 - 99.8086 - 01-088-1965 (C) - Jacobsite syn, precipitated - (Mn.6Fe.4)(Mn.4Fe1.6)O4 - Y: 49.72 % - d x by: 1. - WL: 1.5406 - Cubic - a 8.49700 - b 8.49700 - c 8.49700 - alpha 90.000 - beta 90.000 - gamma 90.000 - Face-cent Operations: Background 1.000,1.000 | Import File: 6-17112009.raw - Type: 2Th/Th locked - Start: 10.000 ° - End: 80.020 ° - Step: 0.060 ° - Step time: 1. s - Temp.: 25 °C (Room) - Time Started: 9 s - 2-Theta: 10.000 ° - Theta: 5.000 ° - Chi: 0.00 ° - Phi: 0.00 ° - Lin(Counts) 0 10 20 30 40 50 60 70 80 90 100 110 120 130 140 150 160 170 180 190 2-Theta - Scale 10 20 30 40 50 60 70 80 Fig.5. X- ray analysis of obtained product of Mix 2 (heated up to Т= 1498К).
  • 6. R. Paunova et al. Int. Journal of Engineering Research and Applications www.ijera.com ISSN: 2248-9622, Vol. 5, Issue 12, (Part - 3) December 2015, pp.92-100 www.ijera.com 97 | P a g e 2.3. EMF results Partial pressure of the oxygen in the mixtures was calculated by the following equations: For air reference electrode 6788.0 20193. lg 2  T E PO (5) For reference electrode Ni/NiO 44.4 1222520193. lg 2  TT E PO (6) For reference electrode Мо/МоО2 051.9 2985220193. lg 2  TT E PO (7) The obtained results of the EMF experimental data is shown in Table 3. The values are an average result of six measurements. In the studied system Fe2O3-MnO-V2O5-SiO2, a number of reactions could take place. Equations G = f (T) were deduced for the main reactions, using thermodynamic data for Ho , So and Cp obtained by some authors [23, 24]. The calculated results for these reactions and the reported ones by some other authors were compared with our results obtained experimentally. The dependences of G = f (T) for the investigated mixtures in air, Ni/NiO and Mo/MoO2 as reference electrode are shown in Fig. 6, 7 and 8. The proposed reactions (shown in Table 4), were accorded with the results of X-ray analysis (Figure 2.4, 5) of the obtained products of both tested mixtures. Table 3. EMF experimental data of both mixtures Mix 1 air Ni/NiO Mo/MoO3 T, K E, V 2 lg OP  T, K E, V 2 lg OP  T, K E, V 2 lg OP  1093 0.588 - 25.64 1113 0.376 - 22.22 1093 0.463 - 37.92 1123 0.546 - 23.24 1123 0.373 - 21.86 1123 0.444 - 35.88 1133 0,497 - 21.03 1133 0.370 - 21.50 1133 0.437 - 35.19 1143 0,488 - 20.49 1143 0.363 - 20.99 1143 0.436 - 34.77 1153 0,482 - 20.08 1153 0.362 - 20.73 1153 0.435 - 34.35 1163 0,478 - 19.75 1163 0.360 - 20.43 1163 0.436 - 34.01 1173 0,472 - 19.35 Mix 2 air Ni/NiO Mo/MoO3 T, K E, V 2 lg OP  T, K E, V 2 lg OP  T, K E, V 2 lg OP  1083 0.564 - 24.84 1123 0.406 - 23.22 1093 0.494 - 39.23 1093 0.548 - 23.94 1133 0.390 - 22.32 1103 0.424 - 35.85 1103 0,526 - 22.81 1143 0.359 - 20.83 1123 0.390 - 33.65 1113 0,520 - 22.36 1153 0.328 - 19.36 1133 0.359 - 32.00 1123 0,518 - 22.08 1163 0.320 - 18.84 1143 0.356 - 31.52 1133 0,498 - 21.07 1173 0.314 - 18.40 1163 0.354 - 30.74 1143 0,470 - 19.76 1153 0.462 - 19.27 The deduced dependences G = f (T) based on experimental data are as follows: Mix 1 - for air reference electrode ΔG exp.= -864 166+580,74.T , J.mol-1 (R2 = 0,8922), - for Ni/NiO reference electrode ΔG exp.= -393 685+169,11.T , J.mol-1 (R2 = 0,9722) - for Mo/MoO2 reference electrode ΔG exp.= -594 159+230,08.T , J.mol-1 (R2 = 0,9215).
  • 7. R. Paunova et al. Int. Journal of Engineering Research and Applications www.ijera.com ISSN: 2248-9622, Vol. 5, Issue 12, (Part - 3) December 2015, pp.92-100 www.ijera.com 98 | P a g e Mix 2 - for air reference electrode ΔG exp.= -808 621+540,62.T , J.mol-1 (R2 = 0,9633) - for Ni/NiO reference electrode ΔG exp.= -1.106 +809,18.T , J.mol-1 (R2 = 0,9473) - for Mo/MoO2 reference electrode ΔG exp.= -2.107 +35776.T -15,513. Т2 , J.mol-1 (R2 = 0,9706) where R is a correlation coefficient Table 4 Gibbs Energy Equations of the expected reactions. Mix 1 2Fe3O4 + ½ O2 = 3Fe2O3 G1 = -586770 + 340.2.T, J.mol-1 [34] 6MnO + O2 = 2 Mn3O4 ΔG 2 = -563241 + 1761.758.T- 220.490.T.lnT + 0.101819.T2 [18] G3 = -222470 + 111,1.T ,J.mol-1 [19] ΔG 4=-445606+221,70.T J.mol-1 [17] 6MnO+O2=2Mn3O4 ΔG 5= -443067+0,7.106 .T-2 +144,4.T- (22,1.10-3 ).T2 +15.67.lnT , J.mol-1 [33] 6MnO+O2=2Mn3O4 ΔG 6= -541,31+0,3593.T , J.mol-1 in this work Mix 2 2 Fe+O2+2V2O3=2FeV2O4 ΔG 7 = -577500+124,7 . T ,J.mol-1 in this work Fe2O3+MnO=Fe2MnO4 ΔG 8= -17669 -6,8286.T ,J.mol-1 in this work 4Fe3O4+O2=6Fe2O3 ΔG 9= -417348+147,73.T , J.mol-1 in this work V2O3+FeO+O2=FeV2O6 ΔG 10= -449912+35,441.T , J.mol-1 in this work 2FeO+V2O4=Fe2O3+V2O3 ΔG 11= -77323+48,84.T , J.mol-1 [21] FeO+V2O3=FeV3O4 ΔG 12= -24700-2,25.T , J.mol-1 [21] Fig.6. Dependence of G = f (T) for Mix 1 (air as a reference electrode) Fig.7. Dependence of G = f (T) for Mix 1 (Ni/NiO as a reference electrode)
  • 8. R. Paunova et al. Int. Journal of Engineering Research and Applications www.ijera.com ISSN: 2248-9622, Vol. 5, Issue 12, (Part - 3) December 2015, pp.92-100 www.ijera.com 99 | P a g e Fig.8. Dependence of G = f (T) for Mix 1 (Mo/MoO2 as a reference electrode) 1080 1090 1100 1110 1120 1130 1140 1150 1160 -450000 -400000 -350000 -300000 -250000 -200000 -150000 -100000 -30000 -25000 -20000 -15000 -10000 -5000 0 delta G10 delta G7 delta G12 delta G11 delta G3 delta G9 delta G8 delta G exp. deltaG,J/mol T, K Fig.9. Dependence of G = f (T) for Mix 2 (air as a reference electrode) 1120 1130 1140 1150 1160 1170 1180 -450000 -400000 -350000 -300000 -250000 -200000 -150000 -100000 -30000 -25000 -20000 -15000 -10000 -5000 0 delta G 11 delta G 3 delta G 9 delta G 8 delta G 12 delta G 10 delta G 7 delta G exp. deltaG,J/mol T, K Fig.10. Dependence of G = f (T) for Mix 2 (Ni/NiO as a reference electrode) 1090 1100 1110 1120 1130 1140 1150 1160 1170 -450000 -400000 -350000 -300000 -250000 -200000 -150000 -100000 -30000 -25000 -20000 -15000 -10000 -5000 0 delta G 11 delta G 8 delta G 12 delta G 3 delta G 9 delta G 10 delta G 7 delta G exp. deltaG,J/mol T, K Fig.11. Dependence of G = f (T) for Mixture 2 (Mo/MoO2 as a reference electrode) The comparison of the experimental data of the three types of reference electrodes with the theoretically calculated values for Hematite showed that the obtained results with reference electrodes air and Ni/NiO were very close to the theoretical values (particularly for Mixture 1), while those of Mo/MoO3 essentially differed. That is why when thermodynamics of the processes including iron oxides is studied; these two reference electrodes are more suitable than molybdenum. III. CONCLUSION 1. It was found out that the phase transformations up to 1473 K and forming of new phases in the mixtures, for example FeV2O4 (coulsonite) (at 1173K) and Iron Vanadium Oxide type (Fe6.5V11..5O35) (at 1473K) and Jacobsite types MnFe2O4 (at 1173K) and (Mn6Fe4)(Mn4Fe1.6)O4 (at 1473K ) could happen only if in the initial materials contained waste vanadium catalyst and manganese concentrate. The X-ray analysis confirmed the presence mainly of hematite phase, cubic and tetragonal Mn2O3, hausmanit (Mn3O4). 2. Based on the experimental results obtained after the heating of mixtures containing oxides of iron, manganese and vanadium the relationship of Go T = f(T) in the temperature range 1073 – 1173 К was obtained, using EMF method with the three different reference electrodes (Ni/NiO, Mo/MoO3 and air). Gibbs energy for Mix 1 and Mix 2 were very close to the theoretically calculated values for Fe2O3 using reference electrodes Ni/NiO and air while that of Mo/MoO2 essentially differed. The X- ray analysis confirmed the presence of hematite phase. 3. It was proved that waste vanadium catalyst and manganese concentrate were more appropriate precursors for the production of complex iron vanadium manganese alloy than the pure oxides - V2O5 and MnO2. REFERENCES [1] A. Blonska-Tabero, Phase relations in the CoO-V2O5- Fe2O3, Journal of Thermal Analysis and Calorimetry, 88(1), 2007, 201-205. [2] A. Blonska-Tabero and B. Monika, Comparative studies in subsolidus areas of ternary oxide systems PbO-V2O5- In2O3 and PbO-V2O5-Fe2O3, Journal of Thermal Analysis and Calorimetry, 113(1), 2013, 137-145. [3] M. Kurzawa, A. Blonska-Tabero and I. Rychlowska- Himmel, Phase relations in subsolidus area of ZnO- V2O5-Fe2O3, Journal of Thermal Analysis and Calorimetry, 74(2) 2003.
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