Applied Thermodynamics: Grain Boundary Segregation

Chemical composition of interfaces—free surfaces and grain boundaries—is generally described by the Langmuir–McLean segregation isotherm controlled by Gibbs energy of segregation. Various components of the Gibbs energy of segregation, the standard and the excess ones as well as other thermodynamic state functions—enthalpy, entropy and volume—of interfacial segregation are derived and their physical meaning is elucidated. The importance of the thermodynamic state functions of grain boundary segregation, their dependence on volume solid solubility, mutual solute–solute interaction and pressure effect in ferrous alloys is demonstrated.


Introduction
The fundamental laws of thermodynamics are applied in many fields of materials science.Their application is particularly important in the field of interfacial segregation, i.e. the accumulation of solute or impurity atoms at an interface.The segregation results in changing bonds at the interface and-in the case of grain boundaries (i.e.interfaces between two differently oriented crystals in a solid)-often in their weakening which results in reduction of material cohesion and consequently, in intergranular brittle fracture leading to irreversible degradation of the material [1].Although numerous papers published in the last decades provide us with a database of chemical composition of interfaces under specific conditions (for reviews see e.g.[2,3]), it is more desirable to disclose general trends that are capable of predicting materials' behavior under different thermal and structural conditions using appropriate thermodynamic variables [4,5].Unfortunately, some thermodynamic data published in literature are of unclear physical meaning and their incorrect interpretation can result in misunderstanding of the fundamentals of interfacial segregation.To avoid this problem, we characterize individual components of the Gibbs energy of grain boundary segregation and consequently, their enthalpy, entropy and volume counterparts, and show the differences among them.Additionally, a reliable application of the basic thermodynamic state functions-the standard enthalpy and entropy of interfacial segregation-as well as of the excess volume is shown.

LangmuirMcLean Segregation Isotherm
Of the two different approaches describing interfacial segregation in a general way, i.e. the Gibbs segregation isotherm and the Langmuir-McLean segregation isotherm, the latter is more convenient (and thus applied as well) as it operates with characteristic changes of the Gibbs energy, G (e.g.[1,4,5]).In this approach the segregation of a solute I at an interface Φ in a binary M-I system can be understood as an exchange of the components M and I between Φ and the volume V [6]: The molar Gibbs energy of "reaction" (1), G r , being the difference of the chemical potentials,   j (let us note that index j denotes any component in the system throughout the whole paper, i.e. j = I,M here, and  = ,V), of the right-hand and left-hand terms, is equal to zero in equilibrium [6]: In Equation (2), , where 0 , ) (   M j is the standard chemical potential of pure component j at temperature T and structure of M (for j = M, we use simple notation "M" instead of the notation M(M)), and  j a is the activity of j at .As this definition is applicable to both the crystal volume V and the interface , we obtain: with the standard molar Gibbs energy of segregation: The activities in Equation ( 3) can be replaced by concentrations, , where  j  are the activity coefficients, and  j X are the atomic fractions of components j for  = ,V.Consequently: in a binary M-I system, accepting for both, the volume and the interface.In a multicomponent systems with limited amount of segregation sites, i.e. fraction of interface saturation X ,sat [2], we may write Equation (5) as: In Equations ( 5) and (5a), G I is the Gibbs energy of segregation consisting of two terms, G I 0 and where is the partial molar excess Gibbs energy of segregation [1]: Equation (5a) with condition (6) represents the general form of the segregation isotherm.It was derived without any non-thermodynamic assumption and, therefore, can be used to describe interfacial segregation independently of the system nature.However, a serious terminological misunderstanding exists as G I in Equations ( 5) and (5a) is frequently incorrectly called "excess Gibbs energy of segregation", G xs (e.g.[7]) or G ex (e.g.[8]).This ambiguous terminology thus evokes confusion.However, the meaning of excess in the sense of the Lewis theory of non-ideal solutions [9] is the only correct because it represents the deviations between real and ideal behavior (see Equation ( 6)).In fact, the adjective "interfacial excess" is an unnecessary over-determination because the term interfacial itself already denotes the extra contribution of interfaces with respect to the bulk, and therefore it should not be used in this context [5].

Thermodynamic State Functions in Interfacial Segregation and Their Physical Meaning
It is evident from the considerations above that there exist three types of thermodynamic state functions of interfacial segregation.In the case of the Gibbs energy, one speaks about the Gibbs energy of segregation, the standard (ideal) Gibbs energy of segregation and the excess Gibbs energy of segregation, the latter characterizing the difference between the Gibbs energy of segregation and the ideal Gibbs energy of segregation.In the following, we will explain the physical meaning of all relevant thermodynamic quantities including the segregation volume which is rarely treated in such a detail.
According to the basic thermodynamic definition: G I 0 is composed of the standard molar enthalpy, H I 0 , and entropy, S I 0 , of segregation, both of which are defined in the same way as G I 0 in Equation (4), i.e.: where 0 ,  j h and 0 , V j h , and 0 ,  j s and 0 , V j s are the respective molar enthalpy and entropy parts of the chemical potentials of solute j at  and V. Let us mention that S I 0 involves all entropy contributions except the configuration entropy [1,5].As the segregation data are frequently correlated according to the Guttmann model of interfacial segregation in multicomponent systems [10], in which only the summary term (which contains all interaction terms) appears:   (10) where H I and S I are the molar enthalpy and molar entropy of segregation of I at interface .
Application of the fundamental thermodynamic relationship to the grain boundary segregation provides us with [11]: where  is the grain boundary energy and A is the grain boundary molar area.According to Equation (11) the molar segregation volume, V I , is defined as: V I is constructed in the same way as other segregation quantities: Equation ( 13) is very close to Equation (1) in Reference [12] for  = GB supposing the relaxations terms  and V r [12] are inherently implemented in the four terms of Equation (13).In the following we will discuss the segregation volume for grain boundaries.
Similarly to G I (Equation ( 6)), V I also consists of two parts, the standard molar segregation volume, V I 0 , and the partial molar excess segregation volume, As V I is not involved in any model, we will treat this quantity separately later.Let us note that in some cases the values of the thermodynamic variables are improperly interpreted, resulting in a lack of physical meaning.For example, this is the case when a single value of G I is determined on basis of the measurements of X I  at different temperatures (e.g., with Equation ( 5)) but averaged over the whole temperature range so that it represents an effective value.Similarly, an averaging may be done for systems with different bulk compositions or over numerous interfaces of different crystallography in polycrystals.For details see e.g.References [1,5].

Thermodynamic State Functions of Interfacial Segregation: G I , H I , S I and V I
Among the state functions of this mode, the Gibbs energy of interfacial segregation, G I , is the most important one as it completely determines interfacial concentration, X I  , at temperature T for bulk atomic fraction, X I V (cf.Equation (5a)).Its importance consists in reflecting the real behavior of the system as indicated by Equation (10).Principally, G I changes not only with changing temperature but also with changing concentrations X I V and X I  due to solute interaction (Figure 1).The corresponding values of H I and S I may also depend on temperature and concentration [1,5].This means that these values can hardly provide us with any general information, e.g. about the anisotropy of grain boundary segregation, because any orientation dependence of H I and S I varies in a complex way with temperature and composition [1,5].Besides G I , H I and S I , the segregation volume, V I , may be considered as another variable of equal importance.However, it seems that it has not been included in the description of interfacial segregation till now.
It follows from Equations (5a) and (12), that in case of a binary system M-I [13]: Integration of Equation ( 15) results in an expression showing that the segregation volume plays an important role in grain boundary segregation under pressure: where P 0 is the normal pressure.This relationship is principally similar to Equation (4) given by Zhang and Ren [14].

Standard Molar Thermodynamic Functions of Interfacial Segregation:
The standard molar thermodynamic state functions possess a special importance in interfacial segregation as they have a very clear physical meaning.According to the definition (Equation ( 4)), as a combination of standard chemical potentials, is principally independent of concentration (see Figure 1a).5)-( 7)).Certainly this represents a limitation although many systems behave nearly ideally (e.g.phosphorus in dilute Fe-P alloys [15,16]).Moreover, in an infinitesimally diluted solid solution the amount of interfacial solute enrichment is very low.Therefore it is highly probable that the solute atoms segregate at a those sites of the boundary which possess the lowest Gibbs segregation energy.Therefore, ΔG I 0 characterizes the interfacial segregation of element I at a specific site of interface Φ in the ideal system.ΔH I 0 and ΔS I 0 are defined in analogy to ΔG I 0 with corresponding physical meaning.According to Equations ( 3) and ( 8), the standard molar state functions control the relation between the activities at an interface and in the volume in the whole concentration range of a binary M-I system.Similarly to ΔG I 0 and according to Equations (9a) and (9b), ΔH I ° and ΔS I ° are concentration independent.Analogously to ΔG I 0 , ΔH I 0 and ΔS I 0 , we may define the standard molar specific heat of segregation, 0 , , as a combination of molar specific heats of pure substances, 0 , The value 0 ) ( 0   are insensitive to the presence of structural defects such as dislocations as well as grain boundaries [17], i.e. although an increase of P c was reported in case of nanocrystaline materials [18].However, the different enhancements of P c of nanocrystalline palladium and copper were ascribed to lower densities of these substances in the nanometer-sized crystalline state [18] representing transition between crystalline and glassy states.In case of a large bicrystal with specified grain boundary we may well accept the relation It means that ΔH I 0 and ΔS I 0 are independent of temperature and ΔG I 0 is thus a linear function of temperature.As the standard state is defined as pure component j at temperature T and structure of M, . It means that all non-zero contributions to V I originate from the real behavior of the system (V I = E I V  ).The fact that ΔV I 0 = 0 has a serious consequence for other standard state functions: According to Equation ( 12) and (S I 0 /P) T = (V I 0 /T) P , both ΔG I 0 and ΔS I 0 , and consequently ΔH I 0 are independent of pressure.The independence of temperature and pressure is a principal property of ΔH I 0 and ΔS I 0 which thus change exclusively with the structure (i.e.energy) of the interface (or an interface site) and with the nature of the system.Therefore, ΔH I 0 and ΔS I 0 can be used for general purposes, for example, to characterize the anisotropy of interfacial segregation which is directly related to the grain boundary classification [1,5] despite their application is limited to ideal (infinitesimally diluted) systems.

Excess Thermodynamic Functions of Interfacial Segregation:
According to Equation ( 6), the excess molar Gibbs energy of segregation, , represents the difference between real and ideal behavior with respect to interfacial segregation and is exactly defined by the a combination of the activity coefficients (Equation ( 7)).It is thus evident that E I G  depends on composition and non-linearly on temperature (cf.schematic Figure 1b).However, the values of the activity coefficients are unknown and hardly measurable, particularly for interfaces.Therefore, is usually approximated by various models, e.g. by the regular solid solution (Fowler) model for a binary system: where α IM is the coefficient of binary I-I interaction in M, or by various models for segregation in multicomponent systems, e.g. by the Guttmann model: with the ternary interaction coefficients, IJ  , characterizing the I-J interaction in M, where J represent other solutes in the system [10].
As only the summarizing term  2. Here, the equilibrium composition is calculated for both the grain boundary of the binary M-I system in the temperature range 473-1673 K according to Equations ( 5) and ( 19) assuming a bulk concentration of X I V = 0.001 (i.e.0.1 at.%), interstitial segregation of I at the grain boundary and the values of H I GB,0 = 30 kJ/mol and S I GB,0 =  J/(mol•K) (as for P, Sb and Sn in -Fe).Figure 2 clearly shows the strong influence of the solute-solute interaction in the binary M-I alloy on the value of X I

GB
. In case of attractive interaction,  IM  0, the grain boundary concentration of the segregant obviously is increased.Even in case of relatively low values of  IM , e.g. IM = +10 kJ/mol, the grain boundary enrichment of I is by tens of at.% higher than without interaction ( IM = 0).Repulsive interaction decreases the solute enrichment to a similar extent.This behavior is well understood because repulsive interaction does not allow putting another atom of the same kind in close surrounding of the atom segregated at the interface while attractive interaction exhibits an opposite effect [19].The effect of ternary interactions ( IJ  , Figure 2b) is much less pronounced as that of the binary interactions [20].Combination of Equations ( 12), ( 15) and ( 19) for a binary alloy with the above condition provides us with:

Relationship between ΔH I 0 and ΔS I 0 of Grain Boundary Segregation and Volume Solid Solubility
The chemical potential of the solute I at the bulk solid solubility limit, is related to the activity at the bulk solid solubility limit, a I V,* .We can express the Gibbs energy of segregation in an M-I system at the limit of solid solubility, G I * , as: It follows from the basic thermodynamic relationships that: Compilation of numerous literature data [21] shows that the activity of solute I at the solubility limit of numerous elements can be expressed by: as is apparent in Figure 3.In Equation (25), v is the exponent which is characteristic for the host element.For many binary systems, the product T lnX I V,* was found to be independent of temperature (Figure 4) [1,22].It means that S I V,* = S I V,0 if conditions ( 24) and ( 25) are fulfilled, and: i.e. [1,5]: is the molar enthalpy of segregation of a solute with complete volume solid solubility in solvent M, and the symbol  characterizes a specific grain boundary [1,5].As the product T lnX I V,* = const, the above mentioned condition of temperature independence of H I 0 is preserved.Equation ( 27) represents an extension and a refinement of the expression X I  /X I V = K/X I V,* , (K = 1.8-10.8)given by Hondros and Seah which relates the grain boundary enrichment ratio to the solid solubility limit [2], and the qualitative idea of Watanabe to extend this simple dependence to account for anisotropy of grain boundary segregation [23] and to construct the so called grain boundary segregation diagram.This idea was later experimentally proved [24].The grain boundary segregation diagram for solute segregation in -iron at [100] symmetrical grain boundaries is shown in Figure 5 [1,5].Analysis of the measured data on segregation of phosphorus, silicon and carbon at individual grain boundaries in -iron show that the value of the exponent v = 0.77 [1,4,5] which is in good agreement with the value v = 0.6 obtained on basis of Equation ( 25) from data of Reference [21] (Figure 3).The value of varies from 8 to +8 kJ/mol according to the grain boundary character (the lower value corresponds to highly segregated general grain boundaries while the latter one corresponds to the special grain boundaries characterized by low segregation levels: for a detailed explanation of this characterization see e.g.[1]).
The above mentioned measurements of grain boundary segregation in iron [1,4,5] provided us with the values of both H I 0 and S I 0 .As an example, the dependence of H I 0 and S I 0 on the misorienation angle for [100] symmetrical grain boundaries is shown in Figure 6.It is obvious that the orientation dependences of H I 0 and S I 0 are qualitatively equivalent for all segregating elements.

Compensation Effect in Grain Boundary Segregation
In principle, we can express the change of the standard molar segregation Gibbs energy of interfacial segregation, G I 0 , at constant temperature and pressure with a single intensive variable  as [25]: . , , Analogously, we can express H I 0 and S I 0 as: , and We may define a temperature T CE as: at which: It means that the change of H I 0 with changing  is compensated by corresponding changes of S I 0 caused by a change of .Then T CE is the compensation temperature and the phenomenon is called compensation effect [1,5,26].If we suppose that  is a variable describing the structure of the grain boundary, we can read Equation ( 31) as providing us with the constant value of the standard Gibbs energy of a solute at any grain boundary, i.e., all grain boundaries fulfilling the above conditions exhibit the same level of grain boundary segregation.If  represents the nature of the solute, all grain boundaries will exhibit the same value of the grain boundary enrichment ratio, X I  /X I V .The former case is documented for example on the basis of experimental data for phosphorus segregation at individual grain boundaries of -iron in Figure 7. Let us note that condition (31) does not identify a phase transformation characterized by minimum of the Gibbs energy: phase transformation is a subcategory of the compensation effect.At T CE no transformation of the boundaries occurs but they coexist besides each other, despite the temperature changes in the vicinity of T CE [25,27].
The plot of the relation between H I 0 and S I 0 for solute segregation in -iron is shown in Figure 8.
We can distinguish two branches of this dependence: they differ in the type of segregation site: the upper one corresponds to interstitial segregation (S 0,CE = 56 J/(mol•K)) while the lower one to substitutional segregation (S 0,CE = 5 J/(mol•K)) [1,4,5].Individual full symbols of the same type correspond to the segregation of a solute at individual grain boundaries in -iron, empty symbols are data found in literature (for the sources of the data, see [1,5]).Let us note that various solutes segregating at the same type of the site also fit with a single dependence (i.e. with either upper or lower branch in Figure 8).The slope of both dependences corresponds to T CE = 930 K which suggests that the compensation temperature is characteristic for the matrix [1,5,28].Splitting of the compensation effect into two branches confirms the fact that the compensation effect is only fulfilled if a single mechanism of the phenomenon is active.Therefore, it can be applied to otherwise independent standard quantities H I 0 and S I 0 albeit not to H I and S I which additionally change with temperature and composition.Let us only briefly mention that Equations ( 27) and ( 32) with the above mentioned values of and S 0,CE can be used to predict the values of H I 0 and S I 0 of any element at any grain boundary in -iron [1,4,5].It is likely that such prediction may be done for other metallic solvents.We can also express the dependence of S I 0 on the volume solid solubility.Combination of Equations ( 27) and (32) provides us with: where the notation site refers to the type of segregation, i.e., either interstitial or substitutional.Using the mentioned data, dependence (33) is shown in Figure 9.It is clearly seen that the majority of the experimental data corresponding to both individual grain boundaries (solid symbols) and to grain boundaries in polycrystals found in the literature (empty symbols) fit fairly well to the theoretical lines of individual branches (the upper line of each branch corresponds to special boundaries while the lower one to general boundaries).
The compensation effect was observed not only in case of grain boundary and surface segregation but also for other interfacial properties, such as grain boundary migration and diffusion [5,26,27], and is present in many phenomena of physics, chemistry and biology [25].

Segregation Volume and Pressure Dependence of Grain Boundary Segregation
During time-dependent experimental studies of non-equilibrium segregation under constant stress, in the beginning a steep change of the grain boundary concentration is observed, followed by the return from an extreme value to a value almost corresponding to that measured without pressure or strain; see e.g. Figure 10 according to Reference [29]).
According to Equation ( 14) (where we use for simplicity X ,sat = X GB,sat = 1, which is often applied in correlation of data on grain boundary segregation [1]), E I V  can be obtained from experimental data [29] on pressure/stress dependence of grain boundary segregation of solutes.According to our method [30] the peak-to-peak heights in original Auger spectra were transformed into concentrations supposing simplification of the alloy to a binary Fe-P system.This procedure provides us with the values of X P GB = 0.303 representing the state under normal pressure and X P GB = 0.308 for the state in the stressed sample after equilibration (Figure 10).According to Equation ( 14) we obtain [13].Similar value E S V   5.5 × 10 6 m 3 /mol for sulphur was determined from the data of Misra [31] who studied grain boundary segregation of sulphur in a low-alloy steel (doped by 0.01 wt.% S) under plastic stress conditions at 883 K by 343 MPa.However, no changes of X P GB were observed after prolonged annealing of a phosphorus-doped 2.25Cr1Mo steel at 793 K under various loads [32] suggesting = 0 and thus, ideal behavior of this system.)/T CE .Solid symbols refer to segregation at individual grain boundaries [4,5], empty symbols are literature data corresponding to measurements on polycrystals [1].The dashed lines were calculated according to Equation (33).

The value of
can also be estimated in other ways.First,  GB Fe V 7.1 × 10 6 m 3 /mol if pure Fe is considered instead of the 2.6NiCrMoV steel [33].As the average boundary density is of about 50% of the bulk density [33], 42 × 10 5 m 3 /mol.Based on the density of FeS (4.82 g/cm 3 [34]), 1.76 × 10 5 m 3 /mol if GB is regarded as a Fe-48 at.%S since the atomic fraction of S in 2.6NiCrMoV is 48 at.% after stress-aging for 20 h [35].Then = 3.0× 10 6 m 3 /mol were calculated using the density functional theory technique for segregation of S, P and Se, respectively, at {012} grain boundary in Ni [36].GB in the order of several percent.This also explains why the equilibrium segregation under pressure only slightly differs from that under normal pressure [29] (see Figure 10).Let us now consider the effect of E I V  on X I GB in more detail.Supposing the values H I 0 =  30 kJ/mol and S I 0 = 25 J/(mol•K) (these values may represent e.g.phosphorus segregation in bcc iron [1]) and X I V = 0.0001, the grain boundary concentration of the solute under normal pressure at temperature of 800 K is X I GB (P = 0) = 0.1554 (i.e.15.54 at.%).The pressure dependence of the calculated X I GB is plotted in Figure 11 for the values of ranging from 8 × 10 6 m 3 /mol to 0. It is obvious from Figure 11 that X I GB starts to change when the pressure is higher than 10 MPa: under these higher pressures the increase of X I GB becomes quite steep.We may conclude that although the effect of elastic deformation on grain boundary segregation is small the grain boundary segregation significantly changes with increasing pressure.At high hydrostatic pressures (P  10 GPa) this effect is rather large: In this case, the equilibrium grain boundary concentration should reach the values up to 100 at.% (cf. Figure 11) [13].However, during such treatment many other processes occur in the material, e.g.dynamic recrystallization, which will influence the final segregation level; in the present modeling these effects were not taken into account.
Similarly to the basic thermodynamic state variables of segregation (H I 0 and S I 0 ; cf. Figure 6) we may expect that = 2  10 6 m 3 /mol describe segregation of I at general and special grain boundary, respectively, the pressure dependence of X I GB for both types of the grain boundaries at 800 K is shown in Figure 12 for X I V = 0.0001.As expected, the segregation level is lower at the special grain boundary compared to the general one.The concentration change at the special grain boundary requires higher pressure.
However, its increase may seem to be surprisingly steeper than in case of the general grain boundary.
In both cases a complete saturation of the grain boundary is reached under ultimate pressures.
The first term at the right-hand side (in front of the brackets) is positive as well as the first (left) one in the brackets (supposing that less than half of the saturation limit is segregated) as X I GB increases with increasing both pressure and X I V .The sign of (i.e.slope of the concentration dependence of the segregation volume) will depend on the value of the term . Intuitively, we may expect the decrease of E I V  (i.e. increase of its absolute value) with increasing X I V (and thus with increasing X I GB ).For this case, should be positive and prevail over the first term in the brackets on the right hand side of Equation (34).In analogy to Equation ( 34), the dependence of We may expect that (negative) value of  (21) we may demonstrate the effect of pressure on the Fowler interaction coefficient,  IM (cf.Equation ( 19)), as: Supposing X GB,sat = 1 and X I GB >> X I V , we obtain: The concentration dependences of the value of d IM /dP for various values of  IM and E I V  are shown in Figures 13 and 14.It is obvious that the value of the fraction on the right-hand side of Equations ( 36) and (37) is of the order of units in case of high grain boundary concentrations.It means that the value of d IM /dP is of the same order as E I V  , i.e. at the level of 10 6 m 3 /mol.This suggests that a change of  IM by 1 kJ/mol results in an apparent change of GB I X when pressure or stress reaches values of the order of hundreds of MPa.The change of  IM with pressure is more pronounced for low grain boundary concentrations, however, the interaction in case of the dilute alloys can be neglected (cf.Equation ( 19)).It means that, usually, the pressure change of the interaction coefficient can be neglected.

Conclusions
Application of basic thermodynamics to a field of material science with important practical consequences-interfacial segregation-is presented in detail.Based on the Langmuir-McLean segregation isotherm, individual modes of thermodynamic intensive variables-which are used to describe this phenomenon-are discussed from the point of view of their physical meaning together with their potential for application.To the best of our knowledge, the segregation volume is fully defined and discussed for the first time here.It is shown that the standard molar segregation volume is zero at any temperature according to the definition of the standard states while the partial molar excess segregation volume reaches non-zero values in real systems.It is concluded that the grain boundary segregation is not affected by pressure in ideal systems whereas the real systems exhibit apparent pressure dependence.The dependences of the standard molar enthalpy of segregation on the bulk solid solubility and the enthalpy-entropy compensation effect are displayed to enable formulation of a relationship between the standard molar entropy of grain boundary segregation and the volume bulk solid solubility.In addition, a fundamental relationship is derived between the segregation excess volume and pressure changes of the grain boundary concentration of the segregant, and various important consequences of the segregation volume are established.

Figure 1 .
Figure 1.Schematic representation of the dependence of the types of G I  (G I , G I ° andE I G ) appearing in Equation (6) on (a) bulk concentration, and (b) temperature, both in a binary system[1].

Figure 3 .
Figure 3. Dependence of the activity at the volume solid solubility limit, a I V,* , and corresponding atomic fraction, X I V,* , for numerous solutes in -iron correlated according to Equation (25) [1,21].

Figure 4 .
Figure 4. Temperature dependence of the product T lnX I V,* for various solutes in -iron [1,22].

Figure 5 .
Figure 5. Grain boundary segregation diagram for [100] symmetrical grain boundaries in -iron [1,4,5].Notice that the lines characterizing the dependence of H I 0 on T lnX I V,* are parallel for individual grain boundaries.The value of the slope in Equation (27) is v = 0.77.

Figure 9 .
Figure 9. Dependence of standard entropy of grain boundary segregation in -iron on the volume solid solubility term, (T lnX I V,* 4 × 10 9 m 3 /mol, and E S V  = 1.0 × 10 5 m 3 /mol.On the other hand, the values of E S V  = 8.1 × 10 6 m 3 /mol, E P V  = 3.0× 10 6 m 3 /mol and E Se V 

Figure 10 .
Figure 10.Time dependence of grain boundary segregation of phosphorus in a 0.05 wt% P-doped low alloy steel at 773 K under tensile (▲) or compressive (•) stress of 30 MPa (according to Reference [29]).

Figure 11 .
Figure 11.Pressure dependence of X I GB in a model M-I(0.01 at.%) alloy at 800 K for various values of E I V  as indicated at the curves (in 10 6 m 3 /mol) [13].

Figure 12 .
Figure 12.Pressure dependence of X I GB at special and general grain boundaries in a model M-I(0.01 at.%) alloy at 800 K.The values H I ° = 30 kJ/mol, S I ° = 25 J/(mol•K) and E I V  = 5  10 6 m 3 /mol were used for general grain boundary, and H I ° = 10 kJ/mol, S I ° = 40 J/(mol•K) and E I V = 2  10 6 m 3 /mol for special grain boundary[13].
(e.g.close to the melting point).To bring this expectation in accordance with Equation(35), the term in the complex brackets should be positive.As P decreases with increasing temperature), the term in the edge brackets on the right-hand side of Equation (35) is negative.Therefore, side of Equation (35) must be negative and of higher absolute value than the other term in the complex brackets.Then  

Figure 13 .
Figure 13.Concentration dependence of d IM /dP for various values of  IM (in units of RT) in a binary M-I alloy for the value of

Figure 14 .
Figure 14.Concentration dependence of d IM /dP for various values of