wettability and agglomeration characteristics of non
TRANSCRIPT
I
Wettability and Agglomeration Characteristics of
Non-Metallic Inclusions
Changji Xuan
Doctoral Thesis
Division of Processes
Department of Materials Science and Engineering
School of Industrial Engineering and Management
KTH Royal Institute of Technology
SE-100 44 Stockholm
Sweden
Akademisk avhandling som med tillstånd av Kungliga Tekniska Högskolan i Stockholm,
framlägge för offentlig granskning för avläggande av Teknologie Doktorsexamen.
Onsdagen den 30 Mars 2016, kl. 10.00 i Kollegiesalen, Brinellvägen 8,
Kungliga Tekniska Högskolan, Stockholm
ISBN 978-91-7595-867-5
II
Changji Xuan Wettability and Agglomeration Characteristics of Non-Metallic
Inclusions
Division of Processes
Department of Materials Science and Engineering
School of Industrial Engineering and Management
KTH Royal Institute of Technology
SE-100 44 Stockholm
Sweden
ISBN 978-91-7595-867-5
Copyright © Changji Xuan (玄昌吉), 2016
Tryck: Universitetsservice US AB
III
To my beloved parents and Baihui
送给我亲爱的爸爸妈妈和百慧
IV
Abstract
In this thesis, both the wettability and the agglomeration characteristics of non-metallic
inclusions in liquid iron/steel were studied by using both experimental results and
thermodynamic considerations. The mechanisms of the wettability of different types of
inclusions were discussed. Also, the agglomeration behaviors of the inclusions were analyzed.
Firstly, the wettability of different types of inclusions (including Al2O3, MgO, Ti2O3, TiO2
and TiN) in contact with the liquid iron/steel was studied. For the TiN case, there is no
reaction formation at the interface between TiN and pure iron/steel. In the case of pure Fe, the
oxygen increase is the main factor for a contact angle decrease. As for the steel case, a sharp
decrease of the contact angle is due to the effects of both an increased oxygen content in the
liquid steel and a formation of a Ti(N,C,O) phase at the interface. For the Al2O3 and MgO
cases, the formation of a FeAl2O4 and a MgO-FeO reaction layer at the interface, respectively,
lead to a contact angle decrease. In the case of the Ti2O3/pure Fe case, the reaction at the
interface cannot be identified. For the Ti2O3/steel case, the formation of an Al2TiO5 reaction
layer is the main reason for a steep decrease of the contact angle. In the TiO2 case, the melting
region appears at the temperature below the melting point of pure iron. This is due to the
strong formation of a solid solution TiOx-FeO. The main source of the oxygen for the solid
solution formation is due to a TiO2 substrate decomposition and a low partial pressure of
oxygen in the chamber.
Regarding to the non-metallic particle additions (TiO2 and TiN) into the molten steel, the
steel composition should be controlled to have a small Al content (< 0.005mass%) and a high
Ti content (> 0.035mass%), so as to get a high number of Ti-rich oxide inclusions with a
small size. This conclusion is supported from the view point of the van der Waals force,
liquid-capillary force and wettability.
Regarding the Ti/Al complex deoxidation in the melt, the “mainly occupied clustered
inclusions” with spherical shape is due to a TiOx-FeO liquid inclusion precipitation after an
addition of Ti as a pre-deoxidizer. The much lower cluster number in the Ti/Al case than that
in the Al case is mainly due to a coagulation of single TiOx-FeO liquid inclusions. Also, the
cluster formation in a complex Ti/Al deoxidation is started after an Al addition rather than
after a Ti addition.
Regarding the Al2O3 cluster formation in deoxidation, the cavity bridge force is larger than
the van der Waals force. However, the difference between them is smaller than 7 times. In the
V
reoxidation process, the influence of the cavity bridge force due to the wettability decreased,
and became similar to that of the liquid-capillary force.
Key words: wettability; non-metallic inclusion; agglomeration mechanism; attraction force;
complex deoxidation; particle addition.
VI
Acknowledgement
I am extremely grateful to my supervisor Professor Pär G. Jönsson for his endless support
and kind guidance on my Ph. D study. I appreciate all the research opportunities you created
for me. Your warm care really encourages me a lot.
I would like to say many thanks to my supervisor Professor Keiji Nakajima for his strict
and patient guidance on my research. Your critical altitude helps me develop a strong heart to
face the life. I will never forget the cherished moment when we were struggling on writing
articles all days and nights. I hope I can inherit your spirit about the research: Keep on
opening the scientific eye.
Thanks to my supervisor Docent Andrey V. Karasev. Thank you for bringing me to the
metallurgical research world. Your kind teaching and training are very helpful for inspiring
my self interest in this field.
Thanks to Professor Hiroyuki Shibata and Dr. Sohei Sukenaga at Tohoku University
(IMRAM) for the big support on my sessile drop measurements in Sendai, Japan. Thanks to
Professor Zhe Zhao (KTH) for teaching and helping me perform the Spark Plasma Sintering
experiments. Also thanks to all the team members in NAMOS project for the technical
support and effective discussions. Dr. Wangzhong Mu and Dr. Yanyan Bi are acknowledged
for the discussion on inclusions and thermodynamic calculations. Thanks to my dear friend
Arkadiy Davydenko for big encouragement and help in my daily life in Sweden.
Thanks to all my colleagues in TPM division and MSE department. It is enjoyable to meet
you in Sweden. Thank you for sharing nice memory with you all.
European Commission Research Fund for Coal and Steel (RFCS) and Jernkontoret are
acknowledged for the financial support.
Finally, I hope to say many thanks to my parents and my wife Baihui Sheng. Without your
endless love and accompany I will never perform the successful work.
Changji Xuan, Stockholm, December 2015.
VII
Supplements
Supplement I: Wettability of TiN by Liquid Iron and Steel
Changji Xuan, Hiroyuki Shibata, Zhe Zhao, Pär G. Jönsson, Keiji Nakajima, ISIJ
International, 55 (2015), No. 8, 1642.
Supplement II: Wettability of Al2O3, MgO and Ti2O3 by Liquid Iron and Steel
Changji Xuan, Hiroyuki Shibata, Sohei Sukenaga, Pär G. Jönsson, Keiji Nakajima, ISIJ
International, 55 (2015), No. 9, 1882.
Supplement III: Effect of the Ti, Al Contents on the Inclusion Characteristics in Steels with
TiO2 and TiN Particle Additions
Changji Xuan, Wangzhong Mu, Zuriñe I. Olano, Pär G. Jönsson, Keiji Nakajima, Steel
Research International, 86 (2015), DOI: 10.1002/sirn.201500267.
Supplement IV: Wetting Behavior of Single Crystal TiO2 by Liquid Iron
Changji Xuan, Andrey V. Karasev, Hiroyuki Shibata, Pär G. Jönsson, ISIJ International, 56
(2016), No. 5, accepted.
Supplement V: Evaluation of Agglomeration Mechanisms of Non-metallic Inclusions and
Cluster Characteristics Produced by Ti/Al Complex Deoxidation in Fe-10 mass%Ni Alloy
Changji Xuan, Andrey V. Karasev, Pär G. Jönsson, submitted to ISIJ International, 2016.
Supplement VI: Attraction Force Estimations of Al2O3 Agglomerations in the Melt
Changji Xuan, Andrey V. Karasev, Pär G. Jönsson, to be submitted to Steel Research
International, 2016.
Contribution statement
Supplement I: Literature survey, experimental work and major part of writing.
Supplement II: Literature survey, experimental work and major part of writing.
Supplement III: Literature survey, major part of experimental work and major part of writing.
Supplement IV: Literature survey, experimental work and major part of writing.
Supplement V: Literature survey, major part of experimental work and major part of writing.
Supplement VI: Literature survey, theoretical calculation and major part of writing.
VIII
Parts of the work presented at the following conferences
Effect of the Ti, Al Contents on the Inclusion Characteristics in Steels with TiO2 and TiN
Particle Additions
Changji Xuan, Wangzhong Mu, Zuriñe I. Olano, Pär G. Jönsson, Keiji Nakajima
The 9th International Conference on Clean Steel, Sep. 2015, Budapest, Hungary.
Assesment of Cluster Characteristics in Fe-10%Ni Alloy Deoxidized with M (M= Al, Zr and
Mg) and Ti/M
Andrey V. Karasev, Changji Xuan, Ryo Inoue, Pär G. Jönsson,
The 8th International Conference on Clean Steel, May 2012, Budapest, Hungary.
IX
Contents
Chapter 1 Introduction ......................................................................................................................... 1
1.1 Background ................................................................................................................................... 1
1.2 Objectives and overview of the work ............................................................................................ 3
Chapter 2 Methodology ........................................................................................................................ 5
2.1 Sample preparation ........................................................................................................................ 5
2.1.1 Ceramic substrates making by Spark Plasma Sintering (SPS) ............................................... 5
2.1.2 Preparation of steel samples ................................................................................................... 7
2.2 Contact angle measurement by using sessile drop method ......................................................... 10
2.3 Electrolytic extraction method .................................................................................................... 13
2.4 Theoretical works ........................................................................................................................ 13
2.4.1 Equilibrium calculation of inclusions precipitation .............................................................. 13
2.4.2 Hamaker constant estimation of liquid iron ......................................................................... 13
Chapter 3 Results and Discussion ...................................................................................................... 16
3.1 Wettability of Al2O3, MgO, Ti2O3, TiO2 and TiN ....................................................................... 16
3.1.1 Contact angle analysis .......................................................................................................... 16
3.1.2 Estimation of oxygen partial pressure using H2-O2-H2O system.......................................... 22
3.1.3 Wettability mechanism ......................................................................................................... 23
3.2 TiO2 and TiN particle additions into steel ................................................................................... 36
3.2.1 Typical inclusions characteristic .......................................................................................... 36
3.2.2 Particle size distribution ....................................................................................................... 38
3.2.3 Thermodynamic equilibrium calculations ............................................................................ 40
3.2.4 The effect of attraction forces on particle agglomeration in steel samples .......................... 41
3.3 Agglomeration behavior of inclusions after a complex Ti/Al deoxidation ................................. 45
3.3.1 Typical single inclusion/cluster morphologies ..................................................................... 45
3.3.2 Typical cluster composition in Ti/Al deoxidation ................................................................ 46
3.3.3 Number of clusters ............................................................................................................... 47
3.3.4 Thermodynamic consideration for TiOx-FeO formation in Ti pre-deoxidation ................... 48
3.3.5 Collision rate estimation in Al and Ti/Al deoxidation ......................................................... 51
3.4 Attraction force estimations between Al2O3 inclusions in the melt............................................. 55
3.4.1 van der Waals force of Al2O3 in the melt ............................................................................. 55
3.4.2 Cavity bridge force due to the un-wetting behavior ............................................................. 56
3.4.3 Comparison of different attraction forces for Al2O3 cluster formation ................................. 58
Chapter 4 Conclusions ........................................................................................................................ 60
X
Chapter 5 Future work ....................................................................................................................... 62
References ............................................................................................................................................ 63
1
Chapter 1 Introduction
1.1 Background
It is well known that a control of the non-metallic inclusions in the liquid steel is extremely
important for the steelmaking industry. On one hand, the cluster formation in steel is
considered to be detrimental for both the casting process (clogging) and the mechanical
properties of the final product. For complex deoxidation processes, several studies have been
presented before [1-5]. The particle size, number and particle composition based on different
element addition type, order and amount have systematically been analyzed. Moreover, the
thermodynamic calculations of the prediction of the stable inclusion precipitation have also
been widely studied [6-10].
On the other hand, by using the specific type of inclusions with small sizes, the nucleation
of the intragranular ferrite (IGF) can be favorable according to the oxide metallurgy concept
[11]. Several researches [13-15] have been performed this research by adding effective
particles into the molten steel. Even though the promotion of the effective nucleation has been
proved, a detailed analysis is still needed regarding to the inclusion characteristics after an
addition. It is due to that the controlling of the dispersion potency and the characteristics (e.g.
size, number and composition) of the inclusions can strongly determine the yield ratio of the
addition.
In both the above situations, the study of the inclusions agglomeration behavior in the melt
is the key point. According to the different influencing factors, the agglomeration of the
inclusions can generally be summarized as described below.
Collision-coalescence
The collision-coalescence of the inclusions in the melt can be promoted by Brawnian
collisions (random movements of inclusions in the melt), Stoke collisions (flotation of
inclusions due to the density difference between inclusion and melt) and turbulent collisions
(movement of inclusions along with the melt flow) [16-21]. When the two inclusions have a
small distance to each other (nan-size level), the collision behavior can also be promoted by
the van der Waals force [22-24]. The latter force can affect the agglomeration coefficient of
the inclusions in liquid steel [22]. However, the Hamaker constant of liquid iron needs to be
known so as to obtain van der Waals force. Mizoguchi et al. [22], Sasai et al. [23] and
Taniguchi et al. [25] used the solid iron Hamaker constant (= 21.2x10-20
J [26]) as an
approximation for a liquid iron medium. But it is unclear whether the Hamaker constant of
2
solid iron can represent that of liquid iron or not. Furthermore, Lin et al. [27] reported the
Hamaker constant of liquid iron caltulation by using Fowkes module [28]. However, in their
estimation only the adhesion work of Al2O3 in liquid iron and AAl2O3 were selected for the
calculation. Also, due to the scattered Hamaker constant values for different oxide inclusions
(e.g.: AAl2O3=15.5 [29], AMgO=10.6 [29]), the deviation of this estimation method is relatively
high. It means that a detailed study on the estimation of the Hamaker constant of liquid iron is
still needed.
Wettability
After the collisions of inclusions occurs, the wettability of the inclusions in contact with
the melt can affect the agglomeration degree. For a strong wetting case (a contact angle < 90
degrees), the agglomeration is not favorable even though the collision might take place.
However, for un-wetting case (a contact angle > 90 degrees), the agglomeration is favorable
due to the wettability attraction force. For an un-wetting case (contact angle > 90 degrees), the
agglomeration behavior is promoted by the cavity bridge force [23-24]. As one of the most
important factors for an agglomeration, the wettability results of oxide inclusions such as
Al2O3 and ZrO2 have already been represented by many researchers [30-37]. However few
experiments were performed for other inclusion types. Even though Shibata et al. [36] and
Ogino et al. [35] reported results for MgO, the mechanism of its wetting behavior has not
been clearly discussed. As for the other typical particles such as Ti2O3, TiO2 and TiN, very
few wettability experiments have been performed before. Meanwhile the explanations about
the wetting mechanism of these different materials have not been systematically discussed. It
seems that an establishment of a clear picture about the wetting behaviors and the
mechanisms of the wettability for different type of inclusions are quite necessary.
Solid phase sintering
When collision happens, the solid phase sintering behavior of the inclusions at the
contacting region can enhance the agglomeration process. The solid phase sintering can be
described by the apparent self-diffusion coefficient, Dv. Previously Coble et al. [38] and
Kingery et al. [39] have systematically represented the self-diffusion coefficient of Al2O3
inclusions. The Al2O3 medium of the system is a protection atmosphere. Moreover, Ooi et al.
[40] measured the Dv values for Al2O3 clusters in liquid iron. Also, Sasai et al. [23] estimated
the FeAl2O4 solid bridge sintering effect in a re-oxidation process for an Al2O3 cluster
formation case.
3
To sum up, it is clear that a systematical study on how these above mentioned factors
influence agglomeration is quite significant. Specifically, a quantitative study of the
agglomeration behavior and mechanism of the inclusions in liquid steel is desired.
1.2 Objectives and overview of the work
In this thesis, firstly the continuous wetting behaviors of different types of substrates were
measured. Based on both experimental results and thermodynamic considerations, the
mechanisms of the wettability of different type inclusions were discussed. Secondly,
according to the investigations of the inclusions characteristics (e.g. size, number,
composition and morphology), the agglomeration behaviors of the inclusions were analyzed.
The mechanisms of the agglomeration phenomenon were explained based on both
experimental studies and theoretical studies. The outline of the supplements in this thesis is
summarized as shown in Fig. 1-1.
Fig. 1-1 The outline of each supplement in the present thesis.
According to Fig. 1-1, it can be seen that the content of this thesis is divided into four parts
so as to study the agglomeration behavior of different types of inclusions in the liquid metal.
4
Part 1 Wettability
The first part corresponds to Supplement I [41], Supplement II [32] and Supplement IV[42].
The wettability of such different inclusions as Al2O3, MgO, Ti2O3, TiO2 and TiN were studied
experimentally. The wetting mechanisms were discussed based on both experimental results
and thermodynamic considerations.
Part 2 Particle addition into molten steel
The second part of this thesis corresponds to Supplement III [43]. The characteristics of the
inclusions (size, number and composition) after TiN and TiO2 particle addition into the steel
were analyzed. Regarding to the particle size distribution results in different steel samples, the
agglomeration degree of inclusions was discussed based on the van der Waals force, liquid-
capillary force and wettability.
Part 3 Deoxidation
The third part of this thesis, which corresponds to Supplement V [44], shows an analysis of
the agglomeration behaviors of the inclusions in Fe-10 mass%Ni alloy by a complex Ti/Al
deoxidation method. An explanation of the agglomeration mechanism in a complex Ti/Al
deoxidation was pointed out.
Part 4 Deoxidation
The fourth part is related to Supplement VI [45]. The main study is focused on the
theoretical estimation of attraction forces (van der Waals force, cavity bridge force) for Al2O3
agglomeration in the melt. The effect of different attraction forces on the Al2O3 agglomeration
was compared.
5
Chapter 2 Methodology
2.1 Sample preparation
2.1.1 Ceramic substrates making by Spark Plasma Sintering (SPS)
The SPS (Spark Plasma Sintering) apparatus (SPS-2050, Sumitomo Coal Mining Co. Ltd.,
Japan) used in the present work is shown in Fig. 2-1. It includes a uniaxial pressure device in
which the water-cooled punches also work as electrodes. Moreover, it includes a water-cooled
reaction chamber which can be evacuated, a pulsed DC generator, as well as a system
controlling the pressure, temperature and punch position.
The prepared powders (TiN and Ti2O3) with prescribed sizes had weights ranging between
2 and 3g. Firstly, the powder was filled into a graphite die (outside diameter, 30.2mm; inside
diameter, 15mm; height, 30.2mm). Afterwards, the graphite die was sintered in the SPS
equipment under a ~5Pa vacuum pressure. Here, the graphite die inner region was separated
by using as graphite paper with a thickness of 150µm.
The uniaxial pressure program for the sintering procedure is represented as is shown in Fig.
2-2. A prescribed uniaxial pressure was applied during the sintering procedure. Afterwards, at
the end of sintering procedure the pressure was released. The temperature program in the
sintering process is reported in Fig. 2-2 as well. Prescribed holding temperatures of 1573-
1873K and holding times of 5min were applied. The temperature of the die was monitored
and regulated by an optical pyrometer. The heating rate during the sintering is about
100K/min. When the sintering is finished, the pulse current was shut off and the pellet was
cooled with liquid N2. The relative densities of the substrates were measured by using the
Archimedes immersion method and using a 99.9% methanol solution. The surface roughness
was measured with a surface roughness apparatus (Talysurf Ultra precision measurement
system FTS PGI 800).
6
Fig. 2-1. Basic configuration of a SPS apparatus.
Type: SPS-2050 Max. Pressure: 210MPa Max. Temperature: 2473K Max. Current: 5000A
7
Fig. 2-2. Illustration of the SPS sintering conditions (a Uniaxial pressure program and a
temperature program).
2.1.2 Preparation of steel samples
2.1.2.1 Ingot making with TiN and TiO2 particle addition
Four types of 35kg ingots were prepared and they were denoted “Eref”, “ETiO2”, “ETiN”,
and “EwTiO2”. The raw materials were melted in a crucible and poured into a metal mold
using an induction furnace. For the “Eref” sample (without an addition of powder), the
holding and pouring temperatures were controlled to be 1843 K. For the “ETiO2” and “ETiN”
samples with TiO2 and TiN particle additions, respectively, the holding and pouring
temperatures were set as 1873 K. The sample preparation procedure is shown in Fig. 2-3 (a).
Overall, 20 pellets (100g+8mass% TiO2/TiN powder) were added into the crucible. In
addition, 2 more pellets were placed inside the mold. The pellet-packets addition was divided
into three times and the interval time for each addition was 4min. At a time of 7min after a
final pellet-packets addition, Al and FeS were added into the melt as well. Then, the melt was
poured into the mold.
As for the “EwTiO2” sample where TiO2 particles were added, the holding and pouring
temperatures were controlled to have a value of 1923 K, as is shown in Fig. 2-3 (b). It can be
seen that the wires (876g) with a 20mass% TiO2 powder were placed inside the crucible. The
wire-packets additions were divided into four times and the addition interval time was 4min.
Fu
rna
ce
co
ntr
ol te
mp
era
ture
[K
]
Pre
ssu
re f
or
pre
ssio
ng
po
wd
er
[MP
a]
0 1.5 2 4.5
Time [min]
3min
Liquid N2
cooling
Holding time:
Prescribed holding
100K/min
temperature
873K
Prescribed Pressure 89.2 MPa
1573-1873K
5min
8
Also, Al and FeS were added into the liquid steel at 7min after the final wire-packet addition
had been made. Finally, the ingot was forged and normalized in order to obtain a homogenous
composition. The chemical compositions of these four samples are shown in Table 2-1.
(a) Information on the Pellet-packets addition and the placement of the pellet-packets inside
the mold.
(b) Wire-packets addition
Fig. 2-3. Schematic diagram of the melting process including the different particle addition
times.
1st 2nd 3rd
Pellet-packets
(total: 20 pellets)Various
alloys
4min 4min 7min
Electriciron
Pellet-packets(total: 2 pellets)inside mold
15min
1873-1883K
Al, FeS
Pouring
1st 2nd 3rd
Wire-packetsVarious
alloys
Electriciron
1923K
Al, FeS
Pouring
4th
4min 4min 4min 7min
19min
9
Table 2-1. Chemical composition of samples from the four trials
Sample [mass%] [ppm]
C Mn Si P S Cr Ni Mo V Cu Al Ti O N
Eref 0.28 1.43 0.69 0.014 0.044 0.15 0.12 0.041 0.097 0.15 0.008 0.011 27 133
ETiO2 0.28 1.24 0.67 0.015 0.035 0.15 0.16 0.045 0.096 0.14 0.005 0.025 75 133
EwTiO2 0.32 1.32 0.72 0.016 0.046 0.11 0.13 0.038 0.093 0.16 0.008 0.026 61 146
ETiN 0.29 1.34 0.68 0.007 0.042 0.11 0.13 0.038 0.086 0.15 0.007 0.034 28 229
2.1.2.2 Deoxidation of Fe-10mass%Ni alloys by Ti, Al and Ti/Al
The deoxidation experiments were carried out by a charging Fe-10mass%Ni alloys (~160g)
into a high-frequency induction furnace under an Ar protection. A praphite susceptor (wall
thickness is equal to 10mm) was installed between the crucible and induction coil so as to
avoid an induction stirring of the melt. After a holding time of 20min at a temperature of
1873K, the composition of the melt became homogeneous. Also, high purity Al2O3 crucibles
were used in the present work. The sampling procedures for Ti, Al and Ti/Al deoxidations are
schematically shown in Fig. 2-4. In case of 0.03 mass%Ti deoxidation in Fig. 2-4 (a), the
melt was deoxidized with Ti. Thereafter, the melt was mechanically stirred for 10s by using
an Al2O3 rod. After that, the melt was sampled with a quartz tube (QT) after holding times of
1 and 5min. Then, in order to preserve the inclusion characteristics a water quenching was
performed for the quartz tube. As for 0.06 mass%Al deoxidation in Fig. 2-4 (b), the
procedures were almost same as that in the Ti deoxidation experiments. After a holding time
of 10 min, the melt was cooled down from 1873 to 1473 K followed by water quenching. The
ingot sample (IC) was cut off from a central vertical slice. For the complex Ti/Al deoxidation
in Fig. 2-4 (c), the melt was firstly pre-deoxidized with a 0.03%Ti addition followed by 10s of
stirring. After a holding time of 1min at a temperature 1873K, 0.06%Al was added and then
the melt was stirred for 10s. The samples were taken at holding times of 1, 5 and 10min. A
small piece of sample was also cut off from the ingot sample (IC). The basic conditions of the
different deoxidations are listed in Table 2-2.
(a)
10
Fig. 2-4. Schematic illustration of (a) Ti, (b) Al and (c) Ti/Al deoxidation experiments.
Table 2-2. Main conditions in the Ti, Al and Ti/Al deoxidation experiment
Exp. No.
Deoxidation
First
addition
[mass%]
Second
addition
[mass%]
Sampling
Holding
Time
[min]
1 Ti 0.03%Ti - QT-1 1
QT-5 5
2
Al
0.06%Al
-
QT-1 1
QT-5 5
IC-15 15
3
Ti/Al
0.03%Ti
0.06%Al
QT-1 1
QT-5 5
QT-10 10
IC-15 15
2.2 Contact angle measurement by using sessile drop method
The basic conditions of the substrates and the chemical compositions of the pure iron and
steel materials are shown in Tables 2-3 and 2-4. The metal sample was placed on the
substrate, which in turn as placed on a platinum plate, as shown in Fig. 2-5. The temperature
was measured by using a thermocouple welded on the platinum plate back. Afterwards, the
sample was heated up at a heating rate of 100K/min and using an Ar protection atmosphere.
The sample was maintained at around 1815K for a prescribed time and then it was cooled
(b)
(c)
11
using a cooling rate of 20K/min. The oxygen partial pressure of the inlet gas was maintained
at a value between 10-20
and 10-23
atm. A gas purification of the gas was done before it entered
the inlet. During an experiments, the contact angle was measured after the metal sample was
melted. Also, the temperature and oxygen partial pressures were continuously recorded by
using a digital data logger. After a temperature of 1623K was achieved, the digital image was
continuously captured each few seconds during the entire experiment.
Table 2-3. Chemical composition of the pure Fe and carbon steel samples.
Pure Iron /steel Composition
Pure Fe [mass ppm]
O N H S P Mn C Al
67 7 5 2 - - 8 -
Cr Cu Si Mo Cl Ni V Ti
- 14 5 - 40 - - -
Carbon steel [mass %]
O N H S P Mn C Al
0.0015 0.0126 - 0.042 0.012 1.43 0.28 0.013
Cr Cu Si Mo Cl Ni V Ti
0.18 - 0.65 0.037 - 0.13 0.084 0.022
Table 2-4. Basic conditions of the substrates used for the contact angle measurements
Substrate
type
Making method Size: dia. x height
[mm]
Surface roughness, Ra [nm]
Al2O3 SC 10 x 1 ~5
MgO (100) SC 10 x 1 ~5
Ti2O3 SPS 15 x 2 ~3µm
TiO2 (100) SC 10 x 1 ~5
TiN SPS 15 x 2 <200
*SC: Single crystal, SPS: Spark plasma sintering.
12
Fig. 2-5. Schematic diagram of the contact angle measurement apparatus.
13
2.3 Electrolytic extraction method
The sample was dissolved by using the potentiostatic electrolytic extraction (EE) method.
A 10%AA electrolyte (10v/v% acetylacetone-1w/v% tetramethylammonium chloride-
methanol) was selected for the extraction. Also, the extraction conditions were set as follows:
a 3-4v voltage, ~60mA current and a 500-1000 coulomb. The dissolved weight varied from
0.12 to 0.2g. After the extraction, a polycarbonate (PC) membrane film filter (open pore size:
0.05µm and 0.4µm) was used to collect the undissolved inclusions during a filtration.
Thereafter, the characteristics of the inclusions were investigated by using a scanning electron
microscope (SEM). The number of inclusions per volume, Nv, was determined as follows.
The metal volume, Vmetal, which corresponds to the region measured on a film filter is given
by Eq. (2-1) [5].
f
obs
Fe
metalA
AW
V (2-1)
where ∆W is the dissolved sample weight, ρFe is the metal density (0.0078gmm-3
), Af is the
area of a film filter (1411.242mm2: 42.4mm in diameter) and Aobs is the observation area. The
Nv value is expressed by using the total observed number of the inclusions, n, as shown in Eq.
(2-2) [5].
metal
VV
nN (2-2)
where Vmetal is the volume of the dissolved sample. The morphology (such as circularity) and
size of the inclusions were measured by using the image software WinROOF®.
2.4 Theoretical works
2.4.1 Equilibrium calculation of inclusions precipitation
Koseki et al. [46] and Ichikawa et al. [47] have verified the equilibrium by using Thermo-
Calc to predict the inclusions characteristics for a wide composition range. In the present
study, the Thermo-Calc.3.0.1 version and the TCFE7 database for the calculations.
2.4.2 Hamaker constant estimation of liquid iron
Based on Fowkes module [28], the interfacial tension between a solid and a liquid phase
can be described in Eq. (2-3), and Young’s equation is shown in Eq. (2-4):
𝛾𝑙𝑠 = 𝛾𝑙 + 𝛾𝑠 − 2√𝛾𝑙𝑑𝛾𝑠
𝑑 (2-3)
14
𝛾𝑙𝑠 = 𝛾𝑠 − 𝛾𝑙 ∙ 𝑐𝑜𝑠𝜃 (2-4)
where γls is the interfacial tension between the solid and liquid, γs and γl are the surface tension
of the solid and liquid, respectively. The parameters γsd and γl
d are the London dispersion
force contribution to the surface tension for the solid and liquid, respectively. Also, Ɵ is the
contact angle. By combining Eq. (2-3) and (2-4), γsd can be described as shown in Eq. (2-5).
𝛾𝑠𝑑 = 𝛾𝑙
2(1 + 𝑐𝑜𝑠𝜃)2/4𝛾𝑙𝑑 (2-5)
For solid particles in H2O (T=293 K) and for the liquid iron system (T=1873 K), Eq. (2-5) can
be expressed as shown in Eq. (2-6) and (2-7), respectively.
𝛾𝑠𝑑 = 𝛾H2O
2(1 + 𝑐𝑜𝑠𝜃𝐻2𝑂/𝑠)2/4𝛾H2O
𝑑 (2-6)
𝛾𝑠𝑑 = 𝛾Fe(l)
2(1 + 𝑐𝑜𝑠𝜃𝐹𝑒(𝑙)/𝑠)2/4𝛾Fe(l)
𝑑 (2-7)
where γH2O is the surface tension of H2O at room temperature (=0.0728 N/m [48]), and γFe(l) is
the surface tension of liquid iron (T=1873 K). The latter can be obtained by using a function
suggested by Takiuchi et al. [49] in Eq. (2-8):
𝛾Fe(l) = 1.90 − 0.327ln(1 + 96𝑎𝑂) [N/m] (2-8)
The London dispersion force contribution to the surface tension for H2O, γH2Od is equal to
0.0218 N/m [48]. The Hamaker constant of substance “1” in vacuum can be described by Eq.
(2-9) [28].
𝐴11 = 6𝜋2𝑑12𝛾1
𝑑 (2-9)
where, d1 is the interfacial separation of the atomic centers at contact. The value of d is equal
to 4.3x10-10
m [50] for H2O (T=293 K), 4.0x10-10
m [50] for inorganic materials (T=293 K),
and 2.58x10-10
m [51] for liquid iron (T=1873 K), respectively. Due to the high melting point
of the ceramic particles (e.g. Al2O3), the A11 value at room temperature can be equal to that at
high temperatures [27]. Then, the value of γsd (T=293 K) is equal to that of γs
d (T=1873 K)
according to Eq. (2-5). Thus, Eq. (2-6) and (2-7) can be combined as is shown in Eq. (2-10).
𝛾Fe(l)𝑑 =
𝛾𝐻2𝑂𝑑
𝛾𝐻2𝑂2 ∙
(1+𝑐𝑜𝑠𝜃𝐹𝑒(𝑙)/𝑠)2
(1+𝑐𝑜𝑠𝜃𝐻2𝑂/𝑠)2 𝛾Fe(l)
2 = 4.1133(1+𝑐𝑜𝑠𝜃𝐹𝑒(𝑙)/𝑠)
2
(1+𝑐𝑜𝑠𝜃𝐻2𝑂/𝑠)2 𝛾Fe(l)
2 (2-10)
It can be seen that in order to calculate γFe(l)d an approximate value of the term (1+cosƟFe(l)/s)
2
/ (1+ cosƟH2O/s) 2
is needed. Table 2-5 shows the contact angle results of different
oxide/nitride ceramic materials in contact with H2O (T=293 K) and liquid iron (T=1813-1873
K). According to the results in Table 2-5, the average value of the term (1+cosƟFe(l)/s)2 / (1+
15
cosƟH2O/s)2 is equal to 0.051±0.008. After combining Eq. (2-9) and (2-10), the Hamaker
constant of liquid iron, A11 at a 1873 K temperature can be written as shown in Eq. (2-11).
𝐴11 = (82.7 ± 12.7) ∙ 𝛾Fe(l)2 (2-11)
For Al-killed steels with an oxygen content of 60ppm, the liquid iron surface tension can be
determined to be 1.751 N/m [27] by using Eq. (2-8). Consequently, the Hamaker constant of
liquid iron can be determined to have a value of 25.3x10-19
J by using Eq. (2-11).
Table 2-5. Contact angle values of various oxide/nitride substrates in contact with H2O/liquid
iron.
Material
ƟFe(l)/s [degree] ƟH2O/s in room temperature [degree] (1+ cosƟ Fe(l)/s)2/
(1+cosƟH2O/s) 2 Aver T [K] Aver
MgO
130 30)
126.5
- 35 54)
32.5
0.048 128 37)
1823
30 55)
123 33)
1873
125 37)
1873
Al2O3 132 35)
132 1873 65.8 56)
51.4 0.042
132 34)
1873 37 57)
Ti2O3 127.9 32)
123.5 1823 18 58)
18 0.053
119 30)
1813-1873
ZrO2
119 37)
127
1823 56.8 59)
56
0.065 122 37)
1823 50 60)
140 52)
1873 50 61)
67 62)
TiN
132 53)
128.9
1823 30.7 63)
45.9
0.048 125 53)
1823
132.8 41)
1813-1873 61 64)
125.7 41)
1813-1873
ZrN 140 53)
140 1823 88.5 63)
88.5 0.052
16
Chapter 3 Results and Discussion
3.1 Wettability of Al2O3, MgO, Ti2O3, TiO2 and TiN in contact with iron/steel
3.1.1 Contact angle analysis
(1) Al2O3
Fig. 3-1 shows the contact angle of Al2O3 in contact with pure iron as a function of the
time. It was found that the contact angle decreases slightly from 105.1 to 103.6 degrees during
the first 90s after a full melting has been obtained. After the initial melting, the temperature
was stable up to 720s, with a corresponding contact angle value of 103 degrees. Thereafter, a
quenching was performed at 860s. The contact angle results in the present work were found to
closely fit the results of Shibata et al. [36]. Specifically, the difference is smaller than 2%.
Fig. 3-1. Contact angle of Al2O3/pure Fe as a function of time after full melting.
(2) MgO
In the MgO/pure Fe case, the contact angle first decreased from 99.2 to 90.0 degrees
during the first ~120s of the experiment, as is shown in Fig. 3-2. Thereafter, the value was
kept constant up to a time of 600s. During these experiments, the melt was quenched after
900s. The present result is consistent with the reporting data of Shibata et al. [36]. Specifically,
the difference is smaller than 4%.
0
50
100
150
0 200 400 600 800 1000
Data 1
Shibatat [1]-11-20Shibata [1]-1012Shibata [1]-0001oginiol[3]Al2O3-Angle
Con
tact a
ngle
[d
eg
ree
]
Time [s]
MarkAtmosphere(P inlet)
Liquid metalmelting
point [ C]
MeasuringTemp. [ C]
Ceramicmaterial
Experiments
H-1600Sinteredmaterial
Ogino et al.(1973) [3]
(0001)
-1600(1012)
(1120)
1536.51540Singlecrystal
This work trial412
Shibata et al.(2009) [2]
Singlecrystal
Ar (10-19
)
2
Ar (10-21
)
oo 2O
Quenchedt=860s
Present worktrial412
Exp.
Ogino [33]
Sub-
Sintered
SCShibata [36]
Trial 412
1873
Temp.
1873
1815 1809.5
point [K]Melting
H2
Atmo-
Ar
Mark
Ar
[K]strate
SC
sphere
17
In addition, it can be seen that the contact angle values (t=0s) of Ogino et al. [33]
obtained for a sintered substrate (132 degrees for Al2O3 and 121 degrees for MgO) are larger
than those found in the present work (105.1 degrees for Al2O3 and 99.2 degrees for MgO).
This difference is probably due to the different surface roughness of the substrates and the
different oxygen partial pressures in the chamber in the two experimental setups.
Fig. 3-2. Contact angle values of MgO/pure Fe as a function of time after a full melting has
been reached.
(3) Ti2O3
Fig. 3-3 shows the contact angle values for a Ti2O3/pure Fe system. It was found that the
values decreased from around 128 to 121.0 degrees during the experiment. Overall, the
contact angle value in the present work is similar to that of Humenik et al. [30], who reported
a value of 119 degrees (t=0s). In the steel case (Fig. 3-4), the contact angle value decreased
sharply from 143.8 to 95.4 degrees during the first 173s of the experiments after a full melting
had been reached. Afterwards, the contact angle had a constant value of 90 degrees up to a
time of 703s.
0
50
100
150
0 200 400 600 800 1000
Data 4 22:16:33 2014-01-10MgO-413Hument [6]Ogino [3]shibata [2]Shibata [1]
Time [s]
Con
tact a
ngle
[d
eg
ree
]
MarkAtmosphere(P inlet)
Liquid metalmelting
point [ C]
MeasuringTemp. [ C]
Ceramicmaterial
Experiments
--1550Sinteredmaterial
Humenik et al.(1953) [1]
H-1600Sinteredmaterial
Ogino et al.(1973) [3]
-1600Singlecrystal
Shibata et al.(100) (2003) [4]
-1600Singlecrystal
Shibata et al.(100) (2009) [2]
1540.81540Singlecrystal
Present work(100) trial413
Shibata [1](2009) Single
crystal
Ar (10-18
)
2
Ar (10-19
)
oo 2O
Ar (1.4 10-18
)
Quenchedt=900s
Exp.Sub- Temp. Melting
point [K]Atmo-
Mark
Humenik[30]
Ogino [33]
Shibata[65]
Shibata[36]
Trial 413
Sintered
Sintered
SC
1823
1873
1873
1873
1816 1813.8
Ar
H2
Ar
Ar
[K]strate sphere
SC
SC
18
Fig. 3-3. Contact angle values of Ti2O3/pure Fe as a function of time after a full melting has
been reached.
Fig. 3-4. Contact angle values of Ti2O3/steel a function of time after a full melting has been
reached.
0
50
100
150
0 200 400 600 800 1000
Data 30
Ti2O3-Fe-418Ti2O3-Fe-502Humen [6]
Time [s]
Con
tact a
ngle
[d
eg
ree
]
MarkAtmosphere(P inlet)
Liquid metalmelting
point [ C]
MeasuringTemp. [ C]
Ceramicmaterial
Experiments
Vacuum-1550Sinteredmaterial
Humenik et al.(1953) [1]
Ar (7.3 10-21
)1541.81540Trial418
Ar (6.6 10-21
)1537.21540Trial502
oo 2O
Sinteredmaterial
Presentwork
Quenched
1823K Vacuum
t=906s
t=860sQuenched
Exp.Sub- Temp. Melting
point [K]Atmo-
Mark
Trial 418
Trial 502
Humenik[30] Sintered 1823
18161815
1816.8
1810.2
Vacuum
Ar
(Trial 418)
(Trial 502)
Ar
[K]strate
Sintered
sphere
0
50
100
150
0 200 400 600 800 1000
Data 33
Ti2O3-steel-1
Con
tact a
ngle
[d
eg
ree
]
Time [s]
MarkAtmosphere(P inlet)
Liquid metalmelting
point [ C]
MeasuringTemp. [ C]
Ceramicmaterial
Experiments
Ar (3.3 10-21
)1482.51540Sinteredmaterial
Present work Trial512
oo 2O
Quenchedt=943s
Exp. Sub-[K]
Meltingpoint [K]
Atmo-Mark
Trial 512 Sintered 1815 1765 Ar
Temp.strate sphere
19
(4) TiO2
Table 3-1 shows the dynamic change of the wetting process for the pure iron cylinder in
contact with a single crystal TiO2 substrate. It was found that a small melting region started to
appear at a temperature of 1739 K. Therefore, this moment was selected as the initial time (t=
0 s) for the observation. When the temperature reached a value of 1813 K (t= 45 s), the iron
specimen was fully melted and had obtained a strong wetting when being in contact with the
substrate surface. During the following 30 seconds at a temperature of 1813 K, the droplet
was continuously spread on the substrate surface, as illustrated in Table 3-1.
Table 3-1. Dynamic observations of the wetting behavior of a pure Fe droplet on TiO2
substrate
T= 1739 K; t= 0s
T= 1769 K; t= 20s
T= 1791 K; t= 35s
T= 1813 K; t= 45s
T= 1813 K; t= 65s
T= 1813 K; t= 75s
The measured temperatures and contact angles are shown as a function of the holding time
in Fig. 3-5. The wetting contact angle decreased from 45 to 37 degrees during 45 s. When the
full melting stage was achieved at 1813 K, the value continuously decreased from 37 to 30.5
degrees within 30 s at the given temperature. The strong wetting behavior for the TiO2
substrate observed in the present work is consistent with that of Humenik et al. [30] and
Amondarain et al. [31]. Specifically, Amondarain et al. [31] reported that the value of the
contact angle between TiO2 and liquid iron can significantly decrease with an increasing
holding time at a constant temperature.
20
Fig. 3-5. Contact angle values of TiO2/pure Fe a function of time.
(5) TiN
In case of TiN/pure Fe (Fig. 3-6), different holding times (t=150s and 900s) were selected
in the present work. The contact angle has a constant value of ~130degrees during the first
150s. After that, the contact angle gradually decreases and reaches a value of 87.9 degrees at a
holding time of 900s. The contact angle results in the present work is quite close to these of
Chuchmarev et al. [53] using a NH3 atmosphere, who measured a value of 132 degrees. The
contact angle values reported by Amadeh et al. [66] (125120degrees for 1000s at 1823K;
11085degrees for 1000s at 1843K) partially corresponded to the present results.
For the TiN/steel case, the contact angle decreased sharply from a value of ~110 to 76
degrees during the first 50s, as seen in Fig. 3-7. Afterwards, the contact angle value decreases
gradually with time. Finally, the contact angle reaches a value of 50 degrees at a holding time
of 981s. These results were a little bit smaller than the value reported by Chuchmarev et al.
[53], who measured a value of 122 degrees. In addition the contact angle values reported by
Amadeh et al. [66] at a 1843 K temperature can fit the final stage of the present results.
0
10
20
30
40
50
60
70
80
90
1700
1750
1800
1850
0 10 20 30 40 50 60 70 80
TiO2-Fe-414
Temperature
Time [s]
Te
mp
era
ture
, T
[K
]
Con
tact
an
gle
, [d
egre
e] Contact angle
Quenched
Full melting
Temperature
21
Fig. 3-6. Contact angle values of TiN/pure Fe as a function of time after a full melting has
been reached.
Fig. 3-7. Contact angle values of TiN/steel as a function of time after a full melting has been
reached.
0
50
100
150
0 200 400 600 800 1000
Data 3
TiN-504FeTiN 507FeChuvu [5]
Time [s]
Con
tact a
ngle
[d
eg
ree
]
Quenched 1843K
1823K
Quenched
MarkAtmosphere(P inlet)
Liquid metalmelting
point [ C]
MeasuringTemp. [ C]
Ceramicmaterial
Experiments
NH-1500-1550Sinteredmaterial
Chuchmarev [5](1967)
Ar-1550, 1570Sinteredmaterial
Amadeh et al.(2001) [6]
Ar (5.4 10-21
)15401540Trial504
Ar (2.6 10-21
)15391540Trial507
Ar (10-18
)
3
Ar (10-19
)
oo 2O
Ar (1.4 10-18
)
Sinteredmaterial
t=900st=150s
Chuch- [53]
Atmo-Mark
Meltingpoint [K]
Sub-
Amadeh [66]
NH3
Ar
Ar
Ar1812
1813
1773-1823
Temp.
1823,1843
1815
1814
Trial 504
Trial 507
Exp. spherestrate [K]
Sintered
Sintered
Sintered
marev
MarkAtmosphere(P inlet)
Liquid metalmelting
point [ C]
MeasuringTemp. [ C]
Ceramicmaterial
Experiments
NH-1500-1550Sinteredmaterial
Chuchmarev [5](1967)
Ar-1550, 1570Sinteredmaterial
Amadeh et al. [6](2001)
Ar (5.6 10-21
)1467.61540Trial511
Ar (9.3 10-21
)1423.81540Trial513
0
50
100
150
0 200 400 600 800 1000
Data 6
TiN-511steelTiN-513steelChu [5]
Time [s]
Con
tact a
ngle
[d
eg
ree
] 3
oo 2O
Sinteredmaterial
1843K
Quenched
1823K
Quenchedt=298s
t=981s
marev
Exp. Sub- MarkAtmo-Melting
point [K]
NH3
Ar
Ar
Ar1697
1741
1773-1823
[K]Temp.
1823,1843
1816
1815
Trial 511
Trial 513
Sintered
Sintered
Sintered
sphereChuch- [53]
strate
Amadeh [66]
22
3.1.2 Estimation of the oxygen partial pressure using H2-O2-H2O system
Although the argon gas purity is as extremely high as 99.9996% it still contains small
amounts of impurities such as H2O and O2. The oxygen partial pressure in the chamber can be
estimated by using the H2-O2-H2O equilibrium system. The chemical reaction of the H2O
formation is shown below [67].
O(g)2H)g(O)g(2H 222
109.88T-493070G o (J/mol) (3-1)
22
2
22
2
2
2
2
2
KOH
OH
OH
OH
PP
P
aa
a
(3-2)
where T is the temperature. The working temperature of the inlet oxygen sensor is 923K. The
ratio of PH2O and PH2 at 923K can be assumed to be constant, and to be independent of the
temperature. Thus, the PO2 value at desired temperature can be obtained by using Eq. (3-3).
2
9232
2
2
1
KH
OH
T
OP
P
KP
(3-3)
where KT is the equilibrium constant at the desired temperature, PH2O is the partial pressure of
H2O (g), and PH2 is the partial pressure of H2 (g). The calculated results for all samples are
listed in Table 3-2. The obtained PO2 value can be the highest PO2 value that can be achieved
in the chamber at ~1815K. Based on this estimation, it is possible to discuss the
thermodynamic considerations for the possible chemical reactions which take place at the
interface.
Table 3-2. PO2 values at temperatures between 1813-1815 K, calculated based on the
(PH2O/PH2) ratio at 923K.
Sample
PO2 at 923K
(inlet) [atm]
PO2 at T=1813-1815K calculated from
(PH2O/PH2) at 923K [atm]
1) Al2O3/Fe 6.85x10-23
3.54 x10-9
2) MgO/Fe 7.52 x10-22
3.89 x10-8
3)Ti2O3/Fe 3.13-5.75 x10-21
1.62-2.97 x10-7
Ti2O3/Steel 3.98 x10-21
2.06 x10-7
4) TiO2/Fe 9.02x10-22
1.12x10-8
23
3.1.3 Wettability mechanisms
(1) Al2O3
Fig. 3-8 shows the spot analysis of an interfacial cross section between pure Fe and an
Al2O3 substrate. The reaction layer is identified as a FeAl2O4 phase and the thickness is about
4µm.
Fig. 3-8. Cross sectional analysis for a Al2O3/pure Fe sample.
In case of the Al2O3/pure Fe system, the following chemical reactions may occur at the
interface:
FeO(l))g(1/2OFe(l) 2
44.82T+-233023G o[J/mol] [68-69] (3-4)
)s(OFeAl)g(1/2O(s)OAlFe(l) 42232
82.044T+-328348G o [J/mol] [70] (3-5)
(s)OAl)g(3/2O)l(2Al 322
324.15T+-1682300G o[J/mol][69-71] (3-6)
24
Fig. 3-9 shows the equilibrium PO2 values for the different chemical reactions. The “gray
region” represents the highest PO2 range in the chamber, which was estimated in section 3.1.2.
Based on thermodynamics, it can be seen that for the Al2O3/pure Fe, a FeO and FeAl2O4
formation might take place. Furthermore, that the Al2O3 substrate is thermodynamically stable.
The results of Shibata et al. [36] fit this prediction due to that FeO particles inside of the iron
and a FeAl2O4 reaction layer are identified at the interface. Although no FeO particles were
observed in the present work, a FeAl2O4 reaction layer at the interface was identified, as is
shown in Fig. 3-8. The formation of the FeAl2O4 reaction layer at the interface leads to a
decrease of the contact angle value during the first 90s of the experiments. Afterwards, the
contact angle value is almost stable. This means that the reaction layer formation reached an
equilibrium state.
Fig. 3-9. Equlibrium PO2 values for different chemical reactions as a function of the
temperature.
10-23
10-21
10-19
10-17
10-15
10-13
10-11
10-9
10-7
10-5
1800 1850 1900 1950 2000 2050
Al2O3MgOTi2O3-418Ti2O3-502Ti2O3-512
PO
2 [
atm
]
T [K]
Fe(l)+1/2O2(g)=FeO(l)
Fe(l)+1/2O2(g)+Al2O3(s)=FeAl2O4(s)
2Al(l)+3/2O2(g)=Al2O3(s)2Ti(l)+3/2O2(g)=Ti2O3(s)
Ti2O3(s)+4Al+7/2O2(g)=2Al2TiO5(s)
25
(2) MgO
In the case of the MgO/pure Fe system, a reaction layer of a MgO-FeO solid solution was
identified. The thickness of the reaction layer was about 20µm, as is shown in Fig. 3-10.
Fig. 3-10. Cross sectional analysis for a MgO/pure Fe sample.
Previously Dan et al. [68] has reported that FeO(l) can be formed at the interface of MgO
in contact with liquid iron. Once FeO is formed, it will immediately be dissolved into the
MgO surface. Then, it will form a FeO-MgO solid solution. According to this point, the molar
fraction of FeO (in MgO) can be thermodynamically estimated. This was done by using a [O]
content value of 635ppm, which was measured with an oxygen/nitrogen/hydrogen combustion
analyzer.
FeO(l)OFe(l) (in magnesiowüstite)
47.69T-115855G o[J/mol] [68] (3-7)
OlFe
lFeOo
aa
aRTKRT
)(
)(lnlnG (3-8)
26
6.969exp )5.736-/13934.09(
)(
)(
T
OlFe
lFeO
aa
aK (T=1815K) (3-9)
where aFeO(l), aFe(l) and aO are the activities for FeO(l), Fe(l) and [O], respectively. The value
of aFe(l) can be assumed to be unity and aO is expressed by the following Eq. (3-10):
OOO xfa (3-10)
where ƒO is the activity coefficient of oxygen in Fe and xO is the mass percentage of oxygen
in liquid Fe (ƒO has been reported to be unity [72]). In this case, the activity of FeO can be
obtained by Eq. (3-11):
OO xa 6.969 (3-11)
When xO is 635ppm, aFe(l) can be determined to have a value of 0.443 (in MgO). Also, the
molar fraction of FeO, NFeO, in the MgO-FeO solid-solution can be estimated to be 0.211.
This can be done by using the relation between aFeO and the molar fraction of FeO in a MgO-
FeO solid-solution [73], as is shown in Fig. 3-11. This thermodynamic estimation show
similar results as the experimental observation results, which is shown in Fig. 3-10. The
decrease of the contact angle during the first 120s after a full melting is possible due to a
MgO-FeO solid-solution is formed at the interface. After that, the reaction layer formation has
reached an equilibrium state and the contact angle value is kept stable.
Fig. 3-11. Activity of wüstite as a function of NFeO in the system “FeO”-MgO.
0
0,2
0,4
0,6
0,8
1
0 0,2 0,4 0,6 0,8 1
Data 206 13:48:20 2014-12-02
11001300D
aF
eO
NFeO
0.9
0.7
0.3
0.5
0.1
0.1 0.3 0.5 0.7 0.9
1373K
1573K
0.211
0.443
MgO FeO
Activity curve for a solutionobeying Raoult's law
Estimationresult
27
(3) Ti2O3
In the case of the Ti2O3/pure Fe system, it can be seen that Ti2O3 does not react with pure
Fe at the interface. Instead, the following reaction takes place.
(s)OTi)g(3/2O)l(2Ti 322
267.2T+-1520750G o [J/mol] [74] (3-12)
According to the thermodynamic result in Fig. 3-12, the Ti2O3 substrate is stable for the
Ti2O3/pure Fe case at a temperature 1815K. The slight decrease of the contact angle with time
might be because of the increased oxygen content in the melt.
Fig. 3-12. Cross sectional analysis for a Ti2O3/pure Fe sample.
For the Ti2O3/steel case (in Fig. 3-13), it was found that a Al2TiO5 reaction layer with a
thickness of ~5µm was identified. The measured contents of Al, Ti and O cannot strictly fit
the Al2TiO5 stoichiometric content. This might be due to a mixing of Al2TiO5 with the Ti2O3
substrate surface.
28
Fig. 3-13. Cross sectional analysis of a Ti2O3/Steel sample.
Due to the high Al (= 0.013 mass%) content in steel, Al2TiO5 particles may form according
to the following reaction.
)s(TiOAl2(g)7/2OAl4)s(OTi 52232
533.11T+-2868076G o [J/mol] [69, 75-77] (3-13)
According to the equilibrium PO2 value estimated in Fig. 3-9, it can be seen that a
precipitation of Al2TiO5 is thermodynamically possible. This consideration is consistent with
the cross sectional observation. According Fig. 3-4, the reaction layer formation of Al2TiO5 at
the interface almost arrived at the equilibrium state during the first 173s after a full melting of
the steel. Afterwards, the contact angle has almost kept a constant value of 90 degrees.
(4) TiO2
In the case of the TiO2/pure Fe system, the cross sectional analysis is shown in Fig. 3-14
and Fig. 3-15. It can be seen that the reaction layer (melting region) is made up of a complex
Fe-Ti-O oxide phase. Base on the ratio of Fe/Ti, the reaction layer roughly included a mixture
of FeO·2TiO2 and FeO·TiO2. The vertical cross sectional analysis at the central part of the
interface between the pure Fe and TiO2 substrate was also investigated by using SEM-EDS, as
29
is shown in Fig. 3-16. The thickness of the Fe-Ti-O reaction layer is about 7 µm. Also the
composition of the complex reaction layer near the pure Fe side is close to the compound
FeO·TiOx. Furthermore, the reaction layer near the TiO2 substrate is close to FeO·2TiOx. In
addition, the ratio of the Ti/O (in at%) on the TiO2 substrate side is shown in Fig. 3-17. On
the surface of the substrate, the composition is close to pure TiO2. However, according to the
ratio of Ti/O, the composition of the substrate inside varied mostly between TiO2 and Ti2O3. It
means that a TiO2 decomposition has occurred at the given experimental condition.
Fig. 3-14. Cross section image of a solid pure Fe droplet on a TiO2 substrate.
Fig. 3-15. Element mapping of the melting region between a pure Fe droplet and a TiO2
substrate.
30
(a)
(b)
Fig. 3-16. Cross sectional analysis of the reaction layer of the interface at the central part of a
Fe/TiOx sample.
Fig. 3-17. Ti/O ratio in a TiO2 substrate and in a TiOx-FeO reaction layer.
-20
-15
-10
-5
0
5
10
15
0 20 40 60 80 100
Data 1 21:17:05 2014-10-18
Ti-disFe-disO-dis
Ver
tica
l d
ista
nce
[μ
m]
Content [atom%]
Ti
Fe
Ti=4.17 [mass%]
O
Fe
TiOx
-30
-20
-10
0
10
at%Ti / at%O
Dis
tan
ce
fro
m s
ub
stra
te s
urf
ace
[µm
]
Substrate surface
TiO
2
Ti 4
O7
Ti 3
O5
Ti 2
O3
0.2 0.4 0.6 0.8 1.0
TiO
Fe droplet
TiO2 substrate
TiO -FeOx
31
In order to explain the wetting behavior of the TiO2/pure Fe system, the formation
mechanism of the melting region needs to be considered from a thermodynamic point of view.
The standard Gibbs free energies of the different chemical reactions are summarized in Table
3-3. Regarding to these reactions, the relationship between the equilibrium partial pressure of
oxygen and temperature is shown in Fig. 3-18. The gray zone corresponds to the temperature
range during the wetting experiment at which the melting region was visually observed.
According to the analysis result in Fig. 3-17, a decomposition of the TiO2 substrate has taken
place. The critical equilibrium value of PO2 for the TiO2 decomposition at 1739 K is about
4x10-12
atm. The actual PO2 near the sample for the experiment of TiO2/pure Fe case might be
close to this value. In this case, it can be seen that at temperatures higher than ~1700 K, the
reactions of (1), (2), (7) and (8) might not take place thermodynamically. However, due to the
decomposition of the TiO2 substrate (reactions (9)-(11)), the produced O2 might support
reactions (1), (2), (7) and (8) and then form a Fe-Ti-O reaction layer.
Table 3-3. Standard Gibbs free energy changes for different reactions
No. Chemical reaction ΔGo
[J/mole]
T [K] Ref.
1 Fe(s) + 1/2 O2(g) = ”FeO”(s) -264002 + 64.591∙T 298-1650 [79]
2 Fe(l) + 1/2 O2(g) = FeO(l) -256061 + 53.681∙T 1644-2273 [76]
3 Ti(s) + O2(g) = TiO2(s) -940982 + 177.569∙T 298-1943 [76]
4 3Ti(s) + 5/2 O2(g) = Ti3O5(s) -2435080 + 420.492∙T 298-1943 [76]
5 2Ti(s) + 3/2 O2(g) = Ti2O3(s) -150256 + 258.069∙T 298-1943 [76]
6 7 Ti3O5(s) = 5 Ti4O7(s) + Ti(s) 127680 + 59.9∙T 1750-1950 [71]
7 Fe(s) + 1/2 O2(g) + TiO2(s) = FeTiO3(s) -271600 + 63.35∙T 1173-1373 [80]
8 Fe(s) + 1/2 O2(g) + FeTiO3(s) = Fe2TiO4(s) -282400 + 62.93∙T 1173-1373 [80]
9 4 TiO2(s) =Ti4O7(s) + 1/2 O2(g) 380352 – 109.607∙T 1750-1950 *
10 3 TiO2(s) =Ti3O5(s) + 1/2 O2(g) 387866 – 112.215∙T 298-1943 *
11 2 TiO2(s) =Ti2O3(s) + 1/2 O2(g) 379908 – 97.069∙T 298-1943 *
*: Reactions (9)-(11) representing a TiOx decomposition were obtained by using a
combination of the respective chemical reactions (3)-(6).
32
Fig. 3-18. Relation between the equilibrium PO2 value and the temperature for different
reactions.
(5) TiN
The solubility of TiN is thermodynamically estimated based on the following equations:
NiTsTiN )( (3-14)
KRTG lno (3-15)
NTi aaK (3-16)
where ΔGo is the standard Gibbs free energy of a TiN formation, R is the gas constant, K is
the equilibrium constant for reaction (3-14). Furthermore, aTi and aN are the activities of Ti
and N in the iron/steel melt, respectively. The solubility line of TiN for pure Fe and steel (Si =
0.65 mass%) content is shown in Fig.3-19. In addition, the O, N and Ti contents in the
iron/steel sample after the experiment are also plotted in Fig. 3-19. For the TiN/pure Fe case,
it was found that TiN will be dissolved into the liquid iron during the first 150s holding time.
After that, the TiN substrate will not be dissolved anymore. As for the TiN/steel case, the TiN
substrate will always be kept stable and a dissolution will not take place.
33
Fig. 3-19. Solubility diagram for TiN in contact with pure Fe and steel.
Fig. 3-20 shows the cross sectional analysis of the interface between pure Fe and a TiN
substrate. It can be seen that iron is partially saturated into the open pores near the interface
and some peelings can be identified. It was also found that the TiN substrate has been slightly
dissolved into the iron. However, there no chemical reaction could be found at the interface.
At the initial stage (t=150s), the TiN substrate was slightly dissolved into the liquid iron
until the melt composition approached the solubility product line (t=150s), as is shown in Fig.
3-19. This dissolution process corresponds to a remarkable increase of the Ti and N contents
from 0.0001 to 0.057mass% and 0.0008 to 0.0103mass%, respectively, as is shown in Fig. 3-
21. Therefore, the substrate surface became rough and it contained protuberances and peeled-
off particles, as is shown in Fig. 3-20. According to the Thermo-Calc calculation, a slight
precipitation of Ti(N0.988,O0.012)=0.036mass% and Ti2O3=0.778mass% is formed at the
interface (t=150s). According to Fig. 3-21, it can also be seen that the oxygen content in iron
is stable at a value of around 0.0066mass% during the first 150s. At this stage, the contact
angle is almost stable.
When the composition of the melt exceeds the solubility product line (t=900s), TiN is
thermodynamically stable in liquid iron. At the interface, a small amount of Ti(N,O) phase
(=0.068mass%) combined with a TiOx phase (=1.017mass%) is slightly precipitated. Since
the precipitation amount is quite small, the effect of this value on the contact angle value is
0,0001
0,001
0,01
0,1
1
10
0,0001 0,001 0,01 0,1 1 10
Ti-con-Fe
Ti-con-steelFe-error barSteel-error bar
[Ti] c
onte
nt [m
ass%
]
[N] content [mass%]
T=1815K
t=981s
t=298s
t=0s
t=0s
t=80s
t=150s
t=900s
Pure Fe
Steel
[81-82]
eSiTi=+2.1 [81]
Si=0.65 [mass%]
eSiTi=+1.43 [82]
Si=0.0008 [mass%]
??????
??
??????
??
Pure Fe
Steel
SEM-EDS
34
negligible. In addition, the O content was found to increase from 0.0066mass% (t=150s) to
0.0129mass% (t=900s). Consequently, it is possible that the slight decrease of the contact
angle in the TiN/pure Fe case is due to the oxygen increase in the iron.
Fig. 3-20. Cross sectional analysis for a TiN/pure Fe sample.
Fig. 3-21. Relation between the contents of O, N, Ti in the metal and the holding time.
0,0001
0,001
0,01
0,1
1
10
0 200 400 600 800 1000
Data 300
O-FeN-FeTi-FeO-steelN-steelTi-steel
Con
ten
t [m
ass%
]
time [s]
Pure Fe Steel
ON
Ti
35
In case of the TiN/steel system, the dissolution of a TiN substrate in steel case will not
happen according to the former discussion. Thus, the substrate surface is relatively smooth as
is shown in Fig.3-22. According to the Thermo-Calc calculations, a reaction layer at the
interface can precipitate in form of Ti(N0.456,C0.537,O0.006)=0.154mass%, Ti2O3=0.477mass%
and TiO=0.740mass% at 298s and Ti(N0.849,C0.143,O0.008)=0.351mass% and Ti2O3=3.005mass%
at 981s, respectively. These predictions fit with a gradual increase of the Ti (from 0.205 to
0.725mass%) and N (from 0.0153 to 0.0707mass%) contents, as is shown in Fig. 3-21. It has
been known that liquid iron has a strong wetting behavior in contact with TiC [83]. Thus, the
slight precipitation of Ti(N,C,O) at the interface can be a reason of the sharp decrease of the
contact angle. In addition, the oxygen increase from 0.0015 to 0.0106mass% in the steel
(t=981) can also lead to a decreased contact angle value.
Fig. 3-22. Cross sectional analysis results for a TiN/Steel sample.
36
3.2 TiO2 and TiN particle additions into steel
The analysis in this section will only concentrate on the “Oxide+MnS+TiN” group
inclusions, which has the potential to form intragranular ferrite (IGF). Some inclusions in the
“MnS+TiN” group were also detected in the present work, but they will not be discussed here.
3.2.1 Typical inclusions characteristics
The phases of the typical particles found in the samples were obtained through a phase
identifications by using SEM-EDS mappings and spot analyses, as is shown in Table 3-4.
TiO2 particle addition
1) Al = 0.008 mass% constant, Ti = 0.011 0.026 mass% increase:
When the Al content has a stable value of 0.008 mass% and the Ti content is increased
from 0.011 (Eref) to 0.026 mass% (EwTiO2), the particle has a Ti-poor/free oxide phase (an
Al2O3 phase and a MnAl2O4 phase). In addition, a MnS phase and/or a TiN phase are
precipitated around the oxide phase.
2) Ti ≈ 0.025 mass% constant, Al = 0.008 0.005 mass% decrease:
When the Ti content has a stable value of ~0.025 mass% and the Al content has decreased
from 0.008 (EwTiO2) to 0.005 mass% (ETiO2), the oxide phase in the particle changes from a
Ti-poor/free oxide phase (a MnAl2O4 phase and a “Liquid#1/#2” phase) to a Ti-rich oxide
phase (an Al2TiO5 phase and a Mn(Al,Ti)2O4 phase). Here, the “Liquids#1” and “Liquid#2”
phases represent an oxy-sulfide phase with a high S content and an oxide phase with a high Si
content, respectively. In addition, a MnS phase and/or a TiN phase are precipitated around
these oxide phases.
TiN particle addition
In the ETiN trial (Al = 0.007mass%, Ti = 0.034mass%), the typical phase includes a Ti-
poor/free oxide phase (Al2O3 phase, “Liquid#1” phase) covered with TiN and (Ti, Al)N
phases.
37
Table 3-4. SEM-EDS mappings and spot analyses of typical particles
Sample SEM micrograph EDS mapping and spot analysis
ETiO2
(Al = 0.005 mas%,
Ti = 0.025 mass%)
Equivalent circle diameter: 1.279µm,
Circularity: 0.370
Magnification: x15000
Equivalent circle diameter: 1.645µm,
Circularity: 0.765
(x15000 magnification)
Magnification: x15000
EwTiO2
(Al = 0.008 mas%,
Ti = 0.026 mass%)
Equivalent circle diameter: 1.791µm,
Circularity: 0.533
Magnification: x15000
Eref
(Al = 0.008 mas%,
Ti = 0.011 mass%)
Equivalent circle diameter: 1.727µm,
Circularity: 0.750 Magnification: x15000
ETiN
(Al = 0.007 mas%,
Ti = 0.034 mass%)
Equivalent circle diameter: 0.974µm,
Circularity: 0.625
Magnification: x20000
38
3.2.2 Particle size distribution
(1) TiO2 particle addition
1) Al = 0.008 mass% constant, Ti = 0.011 0.026 mass% increase:
When the Al content is stable at a value of 0.008 mass% and the Ti content increases from
0.011(Eref) to 0.026 mass% (EwTiO2), the total number of inclusions increases from
4.02x105
to 1.14x106 mm
-3 according to Fig. 3-23. Furthermore, the peak sizes decrease from
0.605 to 0.303 µm. Thus, it is clear that the TiO2 particle addition can strongly affect the
particle size distribution.
2) Ti ≈ 0.025 mass% constant, Al = 0.008 0.005 mass% decrease:
When the Ti content is stable at a value of ~0.025 mass% and the Al content decreases
from 0.008 (EwTiO2) to 0.005 mass% (ETiO2), the total particle numbers increase from
1.14x106 to 4.35x10
6 mm
-3 according to Fig. 3-23. Thus, it was found that the decrease in the
Al content affects the particle size distribution.
(2) TiN particle addition
In case of the ETiN trial (Al = 0.007mass%, Ti = 0.034mass%), the total particle number
Nv value is 7.81x105
mm-3
, as is shown in Fig. 3-23. This value is larger than the values in the
Eref trial, but smaller than those in the ETiO2 trial. The peak particle size value is 0.428 µm,
which is smaller than that found in the Eref trial but larger than that found in the ETiO2 trial.
In summary, according to the result of Grong et al. [84], the total number of particles Nv,
required for a high grain refining potential should be larger than 5.0x106 mm
-3. From the
former comparison, it can be seen that with the lowest Al content (=0.005 mass%), the total
number of particles, Nv, in the ETiO2 trial (4.35x106
mm-3
) is close to this suggested critical
value.
39
Fig. 3-23. A comparison of the particle size distributions in the ETiO2, EwTiO2, Eref and
ETiN samples.
1000
104
105
106
107
0,1 1 10 100
ETiO2EwTiO2ErefETiN
Particle size, d, [μm]Part
icle
num
ber
pe
r unit v
olu
me,
Nv,
[mm
-3]
ETiO2
ETiN
Eref
EwTiO2
103
ETiO2
EwTiO2
Eref
ETiN
4.35x106
1.14x106
4.02x105
7.81x105
Nv [mm-3
]
40
3.2.3 Thermodynamic equilibrium calculations
The equilibrium calculations of the inclusion precipitation were done by using Thermo-
Calc 3.0.1 and using the TCFE7 database. The chemical compositions used in the calculations
are listed in Table 3-5. The calculations for case 2 to case 5 correspond to the trials Eref,
EwTiO2, ETiO2 and ETiN trials, respectively. Also, the predicted precipitation phase at 1523
K is assumed to be the final inclusion phase. This is due to that the phase types are fixed and
will not change to a large extent with a decreasing temperature.
Table 3-5. Chemical composition of steels used in the equilibrium calculations using Thermo-
Calc.[mass.%]
No. Sample C Mn Si S Mo V Al Ti O N
(1) 0.20 0.90 0.49 0.050 0.039 0.082 0.008 0.005 0.0020 0.0123
(2) Eref 0.28 1.43 0.69 0.044 0.041 0.097 0.008 0.011 0.0027 0.0133
(3) EwTiO2 0.32 1.32 0.72 0.046 0.038 0.093 0.008 0.026 0.0061 0.0146
(4) ETiO2 0.28 1.24 0.67 0.035 0.045 0.096 0.005 0.025 0.0075 0.0133
(5) ETiN 0.29 1.34 0.68 0.042 0.038 0.086 0.007 0.034 0.0028 0.0229
(6)
0.28 1.24 0.67 0.010 0.045 0.096 0.003 0.035 0.0075 0.0133
(7) 0.28 1.24 0.67 0.035 0.045 0.096 0.001 0.035 0.0075 0.0133
(8) 0.28 1.24 0.67 0.035 0.045 0.096 0.001 0.050 0.0075 0.0133
The inclusion stability diagram of the Fe-Al-Ti-O system has previously been reported by
Matsuura et al. [9] and it is shown in Fig. 3-24. The present Thermo-Calc calculations were
also inserted into the diagram. Generally, it was found that the stability phase diagram can fit
the Thermo-Calc calculation result. In addition, the thermodynamic calculations can support
the experimental observation results reported in section 3.2.1.
41
Fig. 3-24. Calculated equilibrium oxide phase diagram for a Fe-Al-Ti-O melt at a 1873 K
temperaure.
3.2.4 The effect of attraction forces on particle agglomeration in steel samples
3.2.4.1 Van der Waals force
The van der Waals force Fv between the two spherical inclusions (material1) with the same
radius r in the molten steel (material 2) can be expressed as is shown in Eq. (3-17) [28].
)12zr/AF 2
121v ( (3-17)
22211121 A-AA
(3-18)
where, A121 is the Hamaker constant between the two spherical inclusions in the molten steel
(J), which can be calculated from Eq. (3-18). The parameter z is the distance between the
spherical inclusions (m). The parameters A11 and A22 are the Hamaker constants for the
inclusion and iron in vacuum (J). The Hamaker constants for Al2O3, TiO2, TiN and Fe (liquid)
are equal to 1.55x10-19
J [50], 2.26x10-19
J [50], 1.823x10-19
J [85] and 10.5x10-19
J [27]. Thus,
the following values of A121 can be obtained: 3.98x10-19
J for Al2O3, 3.02x10-19
J for TiO2 and
3.59x10-19
J for TiN. The z value can be assumed to be 10nm [22]. The van der Waals force
was calculated as a function of the inclusion radius, as is shown in Fig. 3-25. It was found that
the van der Waals force for the different inclusion types increased in the following order: i)
0,01
0,1
1
0,0001 0,001 0,01 0,1
Data 12 16:06:02 2014-01-17
TI
[mass.%
Ti]
[mass.% Al]
<Ti2O3>
<Al2O3>
<Ti3O5>
<Al2TiO5>(1)
(2)
(3)
(5)
(6)(4)
(6)(7)
(8)
Al2O3+TiN+MnSAl(-Ti) oxide
+Liquid#1+TiN+MnS
Ti(-Al) oxide+TiN+MnS
Ti(-Al) oxide+Liquid#1
+TiN+MnS
Ti-Al oxide+Liquid#1
+TiN+MnS
1873K
42
TiO2, ii) TiN and iii) Al2O3. In addition, the relation between the contact angle and the
Hamaker constant, A121 are also shown in Fig. 3-26.
3.2.4.2 Liquid-capillary Force
In case of Al2O3, its strong agglomeration behavior has already been reported by
Mizoguchi et al. [22]. They calculated the liquid-capillary force FL due to the FeO liquid
bridge, as is shown in Fig. 3-25.
In the present work, the wettability measurements for the TiO2 case show that a TiOx-FeO
solid solution was formed. For the liquid steel with a high oxygen content and a TiO2 particle
addition, the liquid TiOx-FeO might also provide a liquid-capillary force that promotes on
agglomeration of inclusions. However, this phenomenon was not detected in the steel sample
in the present work since the oxygen content in reference sample only was 27ppm. Also, the
wettability of the TiN/steel system shows that the strong wetting behavior is due to an
increased oxygen content and a small precipitation of Ti(N,C,O) at the interface. However, a
liquid phase precipitation was not identified.
3.2.4.3 Wettability
The contact angle values of TiO2, TiN and Al2O3 are summarized in Fig. 3-26. Even
though many researchers have presented contact angle values for Al2O3, the reported results
are quite scattered due to the formation of a FeAl2O4 reaction layer. In this work, a value of
132 degrees, reported by Ogino et al. [35] by using an extremely low PO2 value (=1.0x10-
17atm) in the chamber, was selected. It can be seen that for the un-wetting cases (TiN, Al2O3),
the contact angle values of TiN are smaller than that of Al2O3. It means that the agglomeration
of Al2O3 after collision is more favorable than that of TiN. As for the TiO2 case, the results of
Humenik et al. [30] are summarized in Fig. 3-26. According to the results in the present work,
the actual measured value for the TiO2/pure Fe system is the contact angle of the TiOx-
FeO/TiO2 system. Due to the reaction layer formation, which covered the pure Fe droplet, the
exact contact angle value for the TiO2/pure Fe system cannot be obtained. In the present work,
the obtained oxide inclusions after TiO2 particle addition into the steel are generally identified
as AlxTiyO inclusions. According to the contact angle measurements for the Ti2O3/steel
system, the final contact angle value is 90 degrees. This wetting contact angle value is
actually that of AlxTiyO/steel, due to the AlxTiyO reaction layer formation. In this case, the
agglomeration is not favorable even though collisions might happen. This is due to the strong
wettability of the AlxTiyO phase.
43
In summary, based on the Van der Waals force, liquid-capillary force and wettability, the
agglomeration degrees of the different inclusions is increased in the following order: TiO2
(AlxTiyO) < TiN < Al2O3.
3.2.4.4 Agglomeration behavior
According to the SEM-EDS observations, the typical phases of the inclusions in the ETiO2
sample contain Ti-rich and Ti-poor oxide phases. The phases in the ETiN sample include
(Ti,Al)N and a Ti-poor oxide phase. As for the EwTiO2 and Eref samples, only Ti-poor oxide
phases were identified. Furthermore, according to the particle size distribution, the total
particle number and peak size varies in the following order: 1) Total particle number: ETiO2 >
EwTiO2 > ETiN > Eref, and 2) Peak size: ETiO2 = EwTiO2 < ETiN < Eref. These
experimental results correspond to the theoretical studies mentioned above in section 3.2.4.1
to section 3.2.4.3.
Fig. 3-25. Attraction forces between Al2O3, TiN and TiO2 particles present in molten steel.
10-15
10-13
10-11
10-9
10-7
10-5
0,001
0,1
0,1 1 10
Fv-TiO2Fv-Al2O3Fv-TiNFL-0.1FL-0.5
Particle radius, r [μm]
TiO2
TiN
Al2O3
r1=0.1μm
r1=0.5μm
Liquid-capillary for Al2O3 [22]
van der Waals
Attra
ctive fo
rce,
F [N
] 10-3
10-1
44
Fig. 3-26. Relationship between the Hamaker constant (A121) at room temperature and the
contact angle of liquid Fe in contact with substrates made of TiO2, TiN and Al2O3.
0
50
100
150
3 3,5 4 4,5
Angle-TiO2Angle-TiNAngle-Al2O3Cu-TiNCu-Al2O3
Hamaker constant [x10-20
J]
Con
tact
an
gle
[d
eg
ree]
[39]
[33]
Oginol
[30]
[30]
[30]
[41][53]
[66]
Amadeh
Rutile
NaCl
Corrundum
[41][66]
TiO2
TiN
Al2O3
45
3.3 Agglomeration behavior of inclusions after a complex Ti/Al deoxidation
3.3.1 Typical single inclusion/cluster morphologies
Table 3-6 reports the typical inclusion/cluster morphologies found in the Ti, Ti/Al and Al
deoxidation trials. In case of Ti, a cluster formation cannot be identified. Instead, single
inclusions of TiOx-FeO with a spherical shape and with sizes smaller than ~6 µm were
detected. As for the Ti/Al and Al cases, a cluster formation was found. Fig. 3-27
quantitatively shows the circularity of the single inclusions/clusters for the Ti, Ti/Al and Al
deoxidations. It was found that the circularity of the single inclusions/clusters decreased in the
following order: i) Ti (0.858), ii) Ti/Al (0.578) and iii) Al (0.193). It means that the clusters
found after a Ti/Al deoxidation are much more compact than those found after an Al
deoxidation.
Table 3-6. Typical single inclusion/cluster morphologies found in the Ti, Ti/Al and Al
deoxiation experiments.
Ti Ti/Al Al
Fig. 3-27. Circularity of single inclusion/clusters after a deoxidation with Ti, Ti/Al and Al.
0
0,2
0,4
0,6
0,8
1
aver
Deoxidation method
Circula
rity
of sin
gle
inclu
sio
n / c
luste
r
Ti Ti / Al Al
Single
Inclusion
Cluster
Cluster
Spherical
Regular
46
Fig. 3-28 shows the frequency of clustered inclusions after a deoxidation with Ti, Ti/Al
and Al. Based on the morphology type, the clustered inclusions were divided into a spherical
and a regular type, as shown in Table 3-6. Because clusters cannot be found in the Ti case,
the single inclusions were used in the comparison. It can be seen that the frequency of the
spherical inclusions decreased in the following order: i) Ti (100%), ii) Ti/Al (69.5%) and iii)
Al (34%). As for the regular type frequency, it increased from 30.5% in the Ti/Al case to 66%
in the Al case.
Fig. 3-28. Frequency of different types of clustered inclusions found in steel samples after a
deoxidation with Ti, Ti/Al and Al.
3.3.2 Typical cluster composition in Ti/Al deoxidation
Table 4-7 shows the elemental mapping analysis of the clusters obtained after a complex
Ti/Al deoxidation after a holding time of 1min. Based on the 2D cross section investigation, it
is concluded that the TiOx-FeO inclusions formed in the Ti pre-deoxidation have been
completely reduced into Al2O3 inclusions within 1min after an Al addition was made.
0
20
40
60
80
100
0 0,5 1 1,5 2 2,5 3
B
Fre
qu
en
cy o
f clu
ste
red
in
clu
sio
ns [
%]
Deoxidation method
Regular
Spherical
AlTi / AlTi
47
Table 3-7. Elemental mapping of typical clusters found after a complex Ti/Al deoxidation
Observation
method
Typical image
(x8000 magnification)
Ti Al
2D
investigation
by using
cross section
Fe O
3.3.3 Number of clusters
Fig. 3-29 shows a comparison of the total number of clusters per unit volume, NV-C, after a
deoxidation with Ti/Al and Al. It shows that as the holding time is increased from 1 to 15min,
the total number of the clusters (550150 mm-3
) in the Ti/Al case is much smaller than that
(5700260 mm-3
) in the Al case. According to the above analysis, it is obvious that the
agglomeration behavior for a complex Ti/Al deoxidation is much weaker than that of an Al
deoxidation. As was described above, the initial TiOx-FeO inclusions in the Ti/Al deoxidation
had been completely reduced into pure Al2O3 phase within 1min after Al addition. Therefore,
the smaller number of clusters in the Ti/Al deoxidation in comparison to the Al deoxidation
cannot be explained by the density differences of the formed clusters. Also, the difference of
the cluster number in these two experiments was evaluated according to the collision rate of
inclusions and clusters in the melt.
48
Fig. 3-29. Total number of clusters found in the steel samples after an Al and a Ti/Al
deoxidation.
3.3.4 Thermodynamic consideration for a TiOx-FeO formation during a Ti pre-deoxidation
The experimental results of the equilibrium relation between [Ti] and [O] in liquid iron
saturated with different Ti-oxide types are summarized in Fig. 3-30. In case of the critical [Ti]
content between Ti3O5 and Ti2O3, Suzuki et al. [86] and Pak et al. [87] reported the same
value of 0.25 mass%, which corresponds to the recommended JSPS data [77]. Also, Cha et al.
[74] obtained a little larger value of 0.36 mass%. For the critical [Ti] content between TiOx-
FeO and Ti3O5, Suzuki et al. [86] reported a value of 0.013 mass%, which corresponds to the
recommended JSPS data [77]. The chemical reactions for Ti2O3/Ti3O5 is expressed in Eq. (3-
19). Moreover, the thermodynamic data are summarized in Table 3-8.
Table 3-8. Standard Gibbs free energy changes of different chemical reactions
Chemical reaction △G0
(J/mole) Temper. [K] Ref.
O)g(1/2O2 (in liquid iron) 3.39T-117110- - 77
(s)OTi)g(5/2O)s(3Ti 532 420.492T2435080- 298-1943
76 (s)OTi)g(3/2O)s(2Ti 322 258.069T1502056- 298-1943
100
1000
104
0 5 10 15
Ti/AlAl
Holding time [min]
Nv-c
[m
m-3
]
Al
Ti/Al
103
102
49
O)s(O3Ti)s(O2Ti 3253
70.167T-246882G o [J/mol] [76-77]…………………… ……….(3-19)
O
OTi
OOTio aRTa
aaRTKRT lnlnlnG
2
3
53
32
.......................(3-20)
]%[ Omassfa OO .........................................................(3-21)
]%[]%[]%[log TimasseOmasseimassef Ti
O
O
O
i
i
OO .....................(3-22)
where 𝑎𝑇𝑖3𝑂5, 𝑎𝑇𝑖2𝑂3 and 𝑎𝑂 are the activities of Ti3O5 (s), Ti2O3 (s) and [O] (in liquid iron),
respectively. Furthermore, 𝑓𝑂 is the activity coefficient for [O], 𝑒𝑜𝑜 (= 0.0344-701/Ti [9]) and
𝑒𝑜𝑇𝑖 (= 0.76-1750/T [77]) are the interaction parameters.
The boundary line for Ti3O5 /Ti2O3 was obtained as is shown in Fig. 3-30. It can be seen
that the boundary line of Ti3O5 /Ti2O3 can almost fit the critical point of [Ti] with a value of
0.25 mass%. The boundary line of TiOx-FeO/Ti3O5 can be estimated based on the critical [Ti]
content between TiOx-FeO and Ti3O5 (= 0.013mass% [77, 86]). In the Fe-Ti-O system, the
shape of the boundary line between different Ti-oxide phases is determined by the values of
𝑒𝑜𝑜and 𝑒𝑜
𝑇𝑖 values, which are constant at 1873 K. Thus, the boundary line of TiOx-FeO/Ti3O5
can be estimated as the “dot-line” shown in Fig. 3-30.
The compositions of the sample obtained after a Ti deoxidation (t=1, 5min) in the present
work have been inserted into Fig. 3-30. At a holding time of 1min, the composition is located
in the TiOx-FeO stable region. When the holding time increased to 5min, the composition
started to approach the equilibrium line.
50
Fig. 3-30. Equilibrium relation between the dissolved O and Ti contents at a 1873 K
temperature.
0,0001
0,001
0,01
0,1
1
0,0001 0,001 0,01 0,1 1
O-sol-ChaO-sol-SuzukiO-parktotal O-0.2TiTiO2-Ti3O5Ti3O5-Ti2O3FeO0.025
O c
onte
nt [m
ass%
]
Ti content [mass%]
Cha [74]
Suzuki [86]
Park [87]
Ti2O3
0.025%Ti0.2%Ti
0.013% 0.25%
TiOx-FeO
Ti3O5
T=1873K
Present work
0.03%Ti
1min5min
51
3.3.5 Collision rate estimation in Al and Ti/Al deoxidation
According to Fig. 3-31, the particle size distribution of the inclusions in the cluster is
needed to estimate the collision rate for an Al2O3 cluster formation. Here, we assume that the
Al2O3 cluster formation is mainly due to the collisions of particle-particle in the clusters (P-P),
particle (in the cluster)-cluster (P-C) and cluster-cluster (C-C). It is well known that the
collision-coalescence among the inclusions in the melt happens due to the combined effects of
Brownian collisions 𝛽𝑖𝑗𝐵, Stoke collisions 𝛽𝑖𝑗
𝑆 and turbulent collisions 𝛽𝑖𝑗𝑇 . Therefore, the total
collision volume 𝛽𝑖𝑗𝑇𝐶 can be expressed as follows [88-93]:
𝛽𝑖𝑗𝑇𝐶 = 𝛽𝑖𝑗
𝐵 + 𝛽𝑖𝑗𝑆 + 𝛽𝑖𝑗
𝑇 (3-23)
with
𝛽𝑖𝑗𝐵 =
2𝑘𝑇(𝑟𝑖+𝑟𝑗)2
3𝜇𝑟𝑖𝑟𝑗 (3-24)
𝛽𝑖𝑗𝑠 =
2𝑔𝜋(𝜌𝑓−𝜌𝑜𝑥)
9𝜇(𝑟𝑖 + 𝑟𝑗)
3|𝑟𝑖 − 𝑟𝑗| (3-25)
𝛽𝑖𝑗𝑇 = 1.3𝛼𝑡√𝜋𝜌𝑓𝜀/𝜇(𝑟𝑖 + 𝑟𝑗)
3 (3-26)
where k is the Boltzman constant (= 1.3807x10-23
J/K), T is the temperature (= 1873 K), µ
is the dynamic viscosity of steel (0.006 kg/m.s [94]), g is the gravitational acceleration (= 9.81
m/s2), ρf and ρox are the density of steel (= 7100 kg/m
3) and Al2O3 inclusions (= 3950 kg/m
3)
respectively. The parameter αt is the agglomeration coefficient, ε is the turbulent energy
dissipation rate (= 0.01 m2/s
3 [94]), ri and rj are the radii of the two colliding inclusions. The
agglomeration coefficient, αt, is needed to estimate the turbulent collision 𝛽𝑖𝑗𝑇 . According to
the inclusion radii ri, the agglomeration coefficient can be calculated as follows [95-96]:
/)/(
727.0
242.0
121
2/13
A
r fi
t (3-27)
where A121 is the Hamaker constant for Al2O3 in liquid iron (= 14.3 x10-19
[J] [45]). The
values of ri corresponds to 0.5 times the value of the peak sizes in each size distribution line in
Fig. 3-31. The collision rate of the inclusions in the melt can be expressed as follows[97]:
𝑑𝑛𝑖𝑗
𝑑𝑡= 𝛽𝑖𝑗
𝑇𝐶𝑛𝑖𝑛𝑗 (3-28)
where t is time [s], ni and nj are the number of the collision inclusions with the radii sizes ri
and rj, respectively.. Furthermore, the selected values of ri corresponds to the 0.5 time values
of the peak sizes represented in Fig. 3-31. Moreover, the value of rj corresponds to each size
52
step in the size distribution curve. The selected values for ni and nj correspond to the Nv-pc
value for the cluster sizes ri and rj in the size distribution. By using Eq. (3-23)-(3-28), the total
collision rate (=∑𝑑𝑛𝑖𝑗
𝑑𝑡) of the clustered inclusions-clustered inclusions, CR(P-P), was obtained
as is shown in Fig. 3-32. The total collision rates between particle-clustered, CR(P-C) and
cluster-cluster, CR(C-C) interactions were calculated in the similar manner, as is shown in Fig.
3-32. It can be seen that the formation and growth rates of clusters in the Al deoxidation
experiments are significantly larger in comparison to those in the Ti/Al deoxidation
experiments. This is due to the larger values of the total collision rates. The values of CR(P-P),
CR(P-C) and CR(C-C) in the Ti/Al case at a 1 min of holding time are about 1400, 170 and 70
times smaller than those in the Al case. However, the difference between these total collisions
rates in both experiments decrease with an increased holding time. As a result, the CR(Al) /
CR(Ti/Al) ratio at a 15 min of holding time decreases by up to about 180, 65 and 7 times,
respectively.
It is interesting to point out that the Brownian collisions have no practically effect on
formation and growth of clusters because the values of 𝛽𝑖𝑗𝐵 for inclusions and clusters in both
experiments varied mostly between 0.01 and 3.0% of the total collision volume. The turbulent
collision (𝛽𝑖𝑗𝑇 ~51-93%) and Stokes` collision (𝛽𝑖𝑗
𝑆 ~6-48%) are the main reasons for a
formation and growth of clusters in the Al and Ti/Al experiments. Moreover, it was found that
the 𝛽𝑖𝑗𝑆 values for the particle-cluster and cluster-cluster collisions are significantly larger in
the Al experiment than those in the Ti/Al experiment. It may be explained by the larger size
of clusters and, as a result, by the larger the Stokes` collisions in the Al experiment.
53
(a)
(b)
Fig. 3-31. Clustered inclusion size distribution after (a) an Al, and (b) a Ti/Al deoxidation.
1
10
100
1000
104
105
0,1 1 10
1min5min10min15min
Particle size, dv-pc [μm]
Nv-p
c [
mm
3]
1min
5min
15min
Al deoxidation
103
102
1
10
100
1000
104
105
0,1 1 10
1min5min10min15min
Particle size, dv-pc [μm]
Nv-p
c [m
m3]
1min
5min
10min
15min
Ti/Al complexdeoxidation
103
102
54
Fig. 3-32. Relation between the total cluster collision rate and the holding time after an Al and
a Ti/Al deoxidation.
10-11
10-10
10-9
10-8
10-7
10-6
10-5
0 5 10 15
Al-P-PTi/Al-P-PAl-C-CTi/Al-C-CAl-P-CTi/Al-P-C
Holding time [min]
To
tal co
llisio
n r
ate
, C
R
Al
Ti/Al
P-PP-CC-C
55
3.4 Attraction force estimations between Al2O3 inclusions in the melt
3.4.1 van der Waals force of Al2O3 in the melt
The van der Waals force Fv between the two solid particles with the same radius r (as the
simplified assumption) in the liquid iron is expressed as shown in Eq. (3-29) [22].
𝐹𝑣 = 𝐴121 ∙ 𝑟/(12𝑧2) (3-29)
where A121 is the Hamaker constant between the solid particles in the liquid (J), z is the
distance between solid particles including their surface roughness, given on an atomic scale
(m). The Hamaker constant A121 between the solid particles in the liquid can be expressed as
shown in Eq. (3-30) [28]:
𝐴121 = (√𝐴11 −√𝐴22)2 (3-30)
where, A11 and A22 are the Hamaker constants in vacuum for the solid and liquid, respectively
(J). For an Al-killed steel (O= 60 ppm), the Hamaker constant of liquid iron is equal to 25.3
x10-19
J. The Hamaker constant of the Al2O3, A11 is equal to 15.5x10-20
J [50]. By using Eq.
(3-30), the Hamaker constant A121 of Al2O3 in the liquid iron at temperature 1873 K can be
calculated as 14.3x10-19
J. Thus, the van der Waals force was obtained by substituting the
values of A121 into Eq. (3-29), as is shown in Fig. 3-33. Three different distances (with the
value as 0.4nm [98], 1nm and 10nm) between oxide particles were estimated. It can be seen
that the van der Waal force is increased with an increased particle radius and a decreased
distance between the particles. When the radius of the particle is equal to 1µm and the
distance between particles is equal to 0.4 nm (closest distance for estimation the maximum
van der Waals force) [98], the van der Waal force has a value of 0.74x10-6
N.
56
Fig. 3-33. Relationship between the van der Waals force and the particle radius for Al2O3
inclusions.
3.4.2 Cavity bridge force due to the un-wetting behavior
Fig. 3-34. A schematic illustration of the un-wetting particle attraction.
For such un-wetting inclusions as Al2O3, a void region is formed between the particles, as
is shown in Fig. 3-34. The parameters R and r are the radius of the void region and the radius
of the inclusion, respectively. The cavity bridge force Fc [N] can be described as the sum of
the pressure difference, ΔPFe (=3.86x103Pa [23]) between the void region and the liquid iron
and the surface tension, γFe of the liquid iron. It is described by the Fisher equation [99] as
follows:
F𝑐 = 𝜋𝑅2∆𝑃𝐹𝑒 + 2𝜋𝑅𝛾𝐹𝑒 (3-31)
10-11
10-10
10-9
10-8
10-7
10-6
10-5
10-4
0,1 1 10
Fv-CeO2-1
Fv-TiO2-1
Fv-Al2O3-1
Fv-Ti2O3-1
CeO2-10
TiO2-10
Al2O3-10
Ti2O3-10
0,4-CeO2
0,4-Al2O3
0,4-Ti2O3
0,4-TiO2
Particle radius, r [μm]
Att
raction f
orc
e [
N]
r1=0.5μm
van der Waals
Van der Waals force
Al2O3
z=1nm
z=10nm
z=0.4nm
57
The surface tension, γFe of the liquid iron at a temperature of 1873K is equal to 1.75 N/m
[49]. The value of R can be obtained by using the equation below, which was derived by Sasai
et. al. [23]:
R = [−3𝛾𝐹𝑒 + (9𝛾𝐹𝑒2 − 8𝛾𝐹𝑒 ∙ ∆𝑃𝐹𝑒 ∙ 𝑟 ∙ 𝑐𝑜𝑠𝜃]
0.5/2∆𝑃𝐹𝑒 (3-32)
where Ɵ is the contact angle.
3.4.2.1 Al deoxidation
In an Al deoxidation, Al2O3 inclusions will be formed. The contact angle of Al2O3 in
contact with the liquid iron is equal to 132 degrees [33-34]. By using Eq. (13) and (14), the
cavity bridge force is calculated as is shown in Fig. 3-35. It can be seen that as the particle
radii is increased from 0.1 to 10µm, the cavity bridge force is increased from 4.90x10-7
to
4.90x10-5
N.
3.4.2.2 Reoxidation
When reoxidation occurs, the oxygen content in the melt rises locally or temporarily to the
oxygen concentration in equilibrium with FeAl2O4. In this case, the contact angle of
FeAl2O4/pure Fe needs to be considered. A contact angle value of 103 degrees was suggested,
based on the results in the present work. By using Eq. (3-31) and (3-32), the cavity bridge
force in the reoxidation case is calculated as is shown in Fig. 3-35. It can be seen that as the
particle radii increased from 0.1 to 10µm, the cavity bridge force increased from 1.65x10-7
to
1.65x10-5
N.
58
Fig. 3-35. Relationship between the cavity bridge force and particle radius.
3.4.3 Comparison of different attraction forces for Al2O3 cluster formation
Table 3-9 shows the different attraction forces for an Al2O3 cluster formation (r=1µm). In
case of an Al deoxidation, the difference is smaller than seven times. This despite that the
cavity bridge force is larger than that of the van der Waals force. Also, the estimation of van
der Waals force in the present work (= 0.74x10-6
N) is much larger than that presented by
Mizoguchi et al. [22] (≈ 10-10
N) and Sasai et al. [23] (≈ 10-9
N). This difference is because
that different Hamaker constants of the liquid iron were used. In their work, the solid iron
Hamaker constant with a value of 21.2x10-20
J was selected for the calculation. In the present
work, the Hamaker constant value of liquid iron corresponding to 25.3x10-19
J was used. The
latter was derived as explained in section 2.4.
When the reoxidation process was promoted, the cavity bridge force decreased from
4.91x10-6
N to 1.18x10-6
N. In the reoxidation case, Sasai et al. [23] and Mizoguchi et al. [22]
recognized the strong effect of the FeO liquid-capillary force (2.92x10-6
N and 1x10-6
N).
However, according the analysis in the present work, it still has a similar level as that of the
FeO liquid-capillary force. However, the cavity bridge force decreased in reoxidation case. It
means that both of them have important roles in the Al2O3 agglomeration.
10-8
10-7
10-6
10-5
0,0001
0,1 1 10
FvFs-Al2O3Fs-FeAl2O4
Att
raction f
orc
e [
N]
Cavity bridge forceAl2O3
FeAl2O4 van der Waals force
Al2O3
Particle radius, r [μm]
10-4
59
Table 3-9. Comparison of different attraction forces in case of Al2O3 particles with a radius of
1µm.
Attraction force Mizoguchi et
al.22)
Sasai et al. 23-24)
Present work
Van der Waals force [N] ~10-10 22)
~10-9
23)
0.74x10-6
Cavity bridge force
[N]
Deoxidation
(Al2O3)
- 3.50x10-6 24)
4.91x10-6
Reoxidation
(FeAl2O4)
- Negligible 23)
1.18x10-6
FeO liquid-capillary force [N] 1x10-6
22)
2.92x10-6
23)
-
60
Chapter 4 Conclusions
Wettability (Supplement I, II and IV)
(1) TiN has a good resistance towards corrosion of liquid iron and steel. In the case of pure
Fe, the oxygen increase in the liquid iron is the main reason for a contact angle decrease
during an experiment. In the steel case, a sharp decrease of the contact angle with time was
found. It is due to both an increased oxygen content in the liquid steel and due to a slight
formation of a Ti(N,C,O) phase at the interface.
(2) For Al2O3 and MgO in contact with liquid iron, a formation of a FeAl2O4 and a MgO-
FeO reaction layer at the interface, respectively, lead to a contact angle decrease with time. In
the Ti2O3/pure Fe case, an interfacial reaction cannot occur. As for the Ti2O3/steel case, the
steep decrease of the contact angle is due to the formation of an Al2TiO5 reaction layer.
(3) For TiO2 in contact with liquid iron, the melting region appears at the temperature
below the melting point of the pure iron. This is due to the strong formation of a TiOx-FeO
solid solution. This formation is due to the direct reactions among the pure iron, TiO2 (s) and
the oxygen gas. The main source of the oxygen for the reactions is from the decomposition of
the TiO2 substrate and the low oxygen partial pressure in the chamber.
Particle addition into molten steel (Supplement III)
For the TiO2 and TiN particles addition, the steel composition should be controlled to have
a small Al content (<0.005mass%) and a high Ti content (> 0.035mass%) so as to obtain a
high number of fine particles with a Ti-rich oxide phase. This consideration can be supported
from the Van der Waals force, liquid-capillary force and wettability. The agglomeration
degree of the studied inclusions were found to be as follows: TiO2 (AlxTiyO) < TiN < Al2O3.
Complex deoxidation (Supplement V)
(1) The average circularity of clusters is about 3 times larger in Ti/Al deoxidation than
those in Al deoxidation. It means that the clusters in the Ti/Al case are more compacted than
that in the Al case. The number of clusters, NV-C in all samples of the Ti/Al case is much
smaller (around 11-2 times) than those in the Al case. However due to the cluster formation
and the flotation, the difference between them decreased significantly with an increased
holding time.
61
(2) The evaluated total collision rates between particle-particle in clusters, particle-cluster
and cluster-cluster in the Ti/Al case at 1min of the holding time are about 1400, 170 and 70
times smaller than those in the Al case. However, the difference sharply decreased to ~180,
65 and 7 times at a 15 min holding time. The turbulent and Stokes’ collision are the main
factors that result in a formation and growth of clusters in the Al and Ti/Al deoxidation
experiments. Their specific collision volumes of (𝛽𝑖𝑗𝑇 and 𝛽𝑖𝑗
𝑆 ) correrspond to ~51-93% and
~6-48% from the total collision volume, respectively.
Theoretical consideration (Supplement VI)
By using Fowkes module, the variation of the Hamaker constant of the liquid iron, A11,
with the surface tension of liquid iron was determined to be as follows:
𝐴11 = (82.7 ± 12.7) ∙ 𝛾Fe(l)2
For the agglomeration behavior of Al2O3, the cavity bridge force is larger than van der
Waals force in the deoxidation case. Specifically, the difference between them is smaller than
7 times. In the case of reoxidation, the influence of the cavity bridge force in liquid iron
decreased and became similar to that of the liquid-capillary force.
62
Chapter 5 Future work
Rare earth elements such as Ce are commonly used as alloying elements/deoxidizers in the
steel making industry. However, due to the cluster formation of CeOx, it might cause clogging
problems during the continuous casting process. Thus, a further study regarding the
agglomeration of CeOx in the liquid steel is important.
Today, wettability measurements of CeOx in contact with iron or steel are extremely rare.
For CeO2, only Amondarain et al. [31] reported a strong wetting behavior in an approximate
manner. However, the wetting mechanism of CeO2/steel has not been discussed yet. Also, a
systematical experiment with a low PO2 value in the chamber is quite necessary so as to
obtain more accurate results. As for Ce2O3 case, no available wettability data exist. However,
Ce2O3 has been recognized to have a strong agglomeration behavior. Thus, the wettability
measurement of Ce2O3 has a significant meaning. In the open market, neither CeO2 nor Ce2O3
substrates with high relative densities are available. However, CeO2 substrate can be prepared
by using cold press sintering of a CeO2 powder. For Ce2O3, firstly the Ce2O3 powder needs to
be prepared by using a reduction treatment of CeO2. Afterwards, the substrate can be prepared
by using cold press sintering as well. During Ce2O3 sintering, a protective atmosphere is
needed so as to avoid an oxidation reaction.
63
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[3] A.V. Karasev and H. Suito: ISIJ Inter., 48 (2008), 1507.
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