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Thermodynamics of Perovskite: Solid, Liquid, and Gas Phases

Written By

Sergey Shornikov

Submitted: 26 December 2019 Reviewed: 22 January 2020 Published: 27 October 2020

DOI: 10.5772/intechopen.91309

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The present work is devoted to the review of experimental data on thermodynamic properties of perovskite in the condensed state, as well as the gas phase components over perovskite and its melts at high temperatures.


  • perovskite
  • thermodynamics

1. Introduction

Calcium titanate (CaTiO3) or perovskite was found by Rose [1] in the Ural Mountains in 1839 and named after the Russian Statesman Count Lev Perovski. Perovskite is a relatively rare mineral, which is a promising material for use as matrices for safe long-term storage of actinides and their rare earth analogs that are present in radioactive waste [2]. It is of particular interest for petrology and cosmochemical research as a mineral which is a part of refractory Ca-Al inclusions often found in carbonaceous chondrites, which are the earliest objects of the solar system with unusual isotopic characteristics [3, 4, 5].

In addition to perovskite, two more calcium titanates, Ca3Ti2O7 [6] and Ca4Ti3O10 [7], melting incongruently, were found in the CaO-TiO2 system. The other calcium titanates, Ca4TiO6 [8], Ca3TiO5 [9], Ca8Ti3O14 [8, 10], Ca2TiO4 [9], Ca5Ti4O13 [11], Ca2Ti3O8 [6], CaTi2O5 [12, 13], CaTi3O7 [14], Ca2Ti5O12 [15], and CaTi4O9 [16], are mentioned in the literature. They also seem to be unstable, which does not exclude their possible existence [17]. Compiled in this paper on the basis of data [7, 18], as well as the results of recent studies by Gong et al. [19], the phase diagram of the CaO-TiO2 system in the high-temperature region is shown in Figure 1.

Figure 1.

The phase diagram of the CaO-TiO2 system [7, 18, 19]: (1) CaO + liquid; (2) CaO + Ca3Ti2O7; (3) Ca3Ti2O7 + liquid; (4) Ca4Ti3O10 + liquid; (5) Ca3Ti2O7 + Ca4Ti3O10; (6) Ca4Ti3O10 + CaTiO3; (7, 8) CaTiO3 + liquid; (9) CaTiO3 + TiO2; (10) TiO2 + liquid; (11) liquid.


2. The thermodynamic properties of perovskite solid phase

Thermochemical data on perovskite [20, 21, 22, 23, 24] are based on calorimetric measurements of entropy of perovskite formation ΔS298(CaTiO3), obtained by Shomate [25], and high-temperature heat capacity of perovskite Cp(CaTiO3) in the temperature ranges of 15–398 K [26], 293–773 K [27], 376–1184 K [28], 383–1794 K [29], and 413–1825 K [30]. The differences between the data do not exceed 5 J/(mol K) up to a temperature of 1200 K, but they are quite contradictory at higher temperatures (Figure 2).

Figure 2.

Heat capacity of perovskite: (1–5) determined via high-temperature calorimetry [26, 27, 28, 29, 30], respectively, and (6) taken from [22].

Naylor and Cook [29] determined the enthalpy of perovskite phase transition: 2.30 ± 0.07 kJ/mol at 1530 ± 1 K. The overlapping phase transitions in perovskite observed by Guyot et al. [30] (Figure 2) were explained as consequences of a structural change, i.e., a transition from orthorhombic (Pbnm) to orthorhombic (Cmcm) structure at 1384 ± 10 K and the overlapping of transitions from orthorhombic to tetragonal (I4/mcm) and tetragonal to cubic phase (Pm3¯m) at 1520 ± 10 K with heat effects of 1.0 ± 0.5 and 5.5 ± 0.5 kJ/mol, respectively. The considerable anomaly of perovskite heat capacity above 1520 K could be caused by strong disordering of the cubic phase up to the temperature of perovskite melting. However, based on diffraction data about perovskite structure obtained in the temperature range of 296–1720 K, Yashima and Ali [31] concluded that the Cmcm phase does not exist and claimed that the first transition is the (Pbnm) → (I4/mcm) at 1512 ± 13 K, followed by the (I4/mcm) → (Pm3¯m) transition at 1635 ± 2 K.

Panfilov and Fedos’ev [32] determined the enthalpy of the reaction with a calorimetric bomb by burning stoichiometric mixtures of rutile TiO2 and calcium carbonate CaCO3 (here and below, the square brackets denote the condensed phase; the parentheses denote the gas phase):


They then calculated the enthalpy of perovskite formation ΔH298(CaTiO3): −41.84 ± 1.88 kJ/mol (Table 1). Although the obtained value was determined with poor accuracy, due to the difficulty of determining the amounts of substances in the reaction products (1), it corresponded satisfactorily to the more accurate results of Kelley et al. [33], who determined this value according to the reaction:

Experimental approachT, KΔHT, kJ/molΔST, J/(mol K)Refs.
HF/HCl solution calorimetry2981.05 ± 0.21[25]
HF/HCl solution calorimetry298−40.48 ± 0.421.86 ± 0.71[33]
Bomb calorimetry298−41.84 ± 1.88[32]
Adiabatic calorimetry298−40.48 ± 1.652.40 ± 0.35[26]
Adiabatic calorimetry298−47.11 ± 1.412.72 ± 0.23[28]
Na6Mo4O15 solution calorimetry298−42.98 ± 1.96[34]
EMF888–972−37.05 ± 3.284.62 ± 3.54[35]
EMF900–1250−40.07 ± 0.053.15 ± 0.05[36]
Pb2B2O5 solution calorimetry973−38.73 ± 1.34[37]
Na6Mo4O15 solution calorimetry975−42.25 ± 1.05[38]
Na6Mo4O15 solution calorimetry975−41.88 ± 1.36[39]
Na6Mo4O15 solution calorimetry976−42.86 ± 1.71[40]
Pb2B2O5 solution calorimetry1046−42.38 ± 1.82[37]
(Li,Na)BO2 solution calorimetry1068 ± 2−40.45 ± 1.15[41]
Pb2B2O5 solution calorimetry1073−40.43 ± 1.874.37 ± 1.23[42]
Pb2B2O5 solution calorimetry1074−43.78 ± 1.73[43]
Pb2B2O5 solution calorimetry1078−42.83 ± 3.12[44]
EMF1180–1290−26.88 ± 8.0511.07 ± 6.44[45]
Raman spectroscopy13002.82 ± 1.29[46]
Thermochemical calculations1600–1800−37.19 ± 0.145.85 ± 0.09[22]
Thermochemical calculations1600–2100−38.23 ± 0.045.00 ± 0.02[23]
Thermochemical calculations1600–2100−37.47 ± 0.035.60 ± 0.02[24]
DTA1740 ± 20−37.55 ± 3.76[47]
Knudsen mass spectrometry1791–2241−39.98 ± 0.543.15 ± 0.28[48]
Knudsen mass spectrometry2241–23987.73 ± 1.7624.39 ± 0.76[48]

Table 1.

Enthalpy and entropy of perovskite formation from simple oxides (calculated per 1 mol of compound).


by solution calorimetry in a mixture of hydrofluoric and hydrochloric acids. The reactions of dissolution were more complete than combustion reaction (1).

Navrotsky et al. [19, 26, 34, 37, 38, 39, 40, 41, 42, 43] performed a number of studies by various calorimetric methods, using adiabatic calorimetry [26] and solution calorimetry in the (Li, Na)BO2 [41], Pb2B2O5 [37, 42, 43], and Na6Mo4O15 [19, 34, 38, 39, 40] salts in the temperature range 973–1074 K. They determined the value of ΔHT(CaTiO3), which lies in the range of −44 to −39 kJ/mol; the accuracy of measurements was 2 kJ/mol (Table 1). The differences could be due to the properties of the solvents that were used. Perovskite and its oxides are poorly soluble in oxide solvent Pb2B2O5; Na6Mo4O15 liquid alloy is quite volatile and cannot be used at temperatures above 1000 K; (Li,Na)BO2 solution is hygroscopic, which creates difficulties in synthesizing [49]. The ΔH1078(CaTiO3) value determined by Koito et al. [44] by similar method (solution calorimetry in Pb2B2O5 salt) is less accurate but close to the results obtained by Navrotsky et al. [19, 34, 37, 38, 39, 40, 41, 42, 43].

The data obtained by Sato et al. [28] using adiabatic calorimetry deviate negligibly (by as much as 7 kJ/mol) in the enthalpy values of (HTH298) in the temperature range above 1000 K. Approximately the same systematic deviation is observed in determination of enthalpy of perovskite formation from oxides (per 1 mole of the compound) due to its use in calculations of the rough semiempirical approximation proposed in [50]. At the same time, the entropy of perovskite formation determined by Sato et al. [28] is in satisfactory agreement with the results obtained by Kelley and Mah [20], Woodfield et al. [26], and Prasanna and Navrotsky [42] and calculated by Gillet et al. [46] based on information obtained on Raman spectra (Table 1).

Golubenko and Rezukhina [45] studied the heterogeneous reaction using a solid electrolyte galvanic cell (EMF method) in the temperature range of 1180–1290 K:


A mixture of FeO and Fe (or NbO and Nb) was used as the reference electrode, and a mixture of La2O3-ThO2 crystals was used as the solid electrolyte. The Gibbs energy of perovskite ΔGT(CaTiO3) was calculated based on a compilation of fairly approximate literature data and their own estimates of the thermodynamic properties of the [Ti2O] compound. This produced a considerable error in determining this value (Figure 3). Rezukhina et al. [35] later made more precise measurements of ΔGT(CaTiO3) in the temperature range of 888–972 K, inside a galvanic cell with CaF2 as the electrolyte (Figure 3). However, the non-systematic errors in determining ΔHT(CaTiO3) and ΔST(CaTiO3) values were considerable (Table 1).

Figure 3.

The Gibbs energy of the formation of perovskite, determined via (1, 2) calorimetry [28, 42], respectively; (3–6) EMF [35, 36, 45, 51], respectively; (7–9) Knudsen effusion mass spectrometric method in [48, 52, 53], respectively; (10, 11) calculated from thermochemical data in [24, 26], respectively.

Taylor and Schmalzried [51] (at 873 K) and Jacob and Abraham [36] (at 900–1250 K) also determined the perovskite Gibbs energy via EMF using the same solid electrolyte. The obtained ΔGT(CaTiO3) values were close to the results of Rezukhina et al. [35].

Klimm et al. [47] used differential thermal analysis (DTA) to determine the enthalpy of reaction (2) at 1740 ± 20 K. The obtained value is consistent with the results of thermochemical calculations, although it has a significant error.

Suito et al. [54, 55] has studied the equilibrium at 1873 K:


in CaO-TiOx (or CaO-TiOx-Al2O3) slags with liquid nickel, relative to oxygen and nitrogen, depending on the content of Ti (or Al) in the metal. Crucibles made of CaO or Al2O3 were used. The activity (ai) of titanium oxide was estimated indirectly, depending on the content of Al, Ti, and O in the slag, and using data on the Gibbs energies of oxide formation (Figure 4).

Figure 4.

Activities of CaO (1–3) and TiO2 (4–8) in perovskite, determined (1–3, 6–8) via Knudsen effusion mass spectrometry [48, 52, 53] and (4, 5) in studying the heterogeneous equilibria of multicomponent melts [54, 55], respectively.

Banon et al. [52] (at 2150 K) and Shornikov et al. [48, 53, 56] (at 1791–2398 K) determined the values of CaO and TiO2 activities (Figure 4) and ΔGT(CaTiO3) via Knudsen effusion mass spectrometric method. The resulting values correlated with one another within the experimental error (up to 2.5 kJ/mol); however, the ΔGT(CaTiO3) was obtained at a temperature ∼1000 K higher than in the earlier results (Figure 3).

As it is seen in Figure 4, the values of oxide activities in perovskite determined via Knudsen effusion mass spectrometric method agree with one another in the investigated temperature range. As the temperature grows, there is a slight trend toward the higher activities of calcium and titanium oxides in the crystalline perovskite phase. This trend is less noticeable in the area of the liquid phase. The activities of titanium oxide calculated based on studying of equilibria in slags [54, 55] are fairly approximate but not inconsistent with the results in [48, 52, 53].

The values of Gibbs energy of perovskite formation determined at 800–1200 K via EMF [35, 36, 51] and solution calorimetry [42] correlate satisfactorily with the obtained via Knudsen effusion mass spectrometric method [48, 52, 53, 56]. Figure 3 shows a good agreement between these data and the results from thermochemical calculations performed by Woodfield et al. [26]. The difference between our findings and the thermochemical data calculated by Bale et al. [24] is large in the perovskite melting area, but is still less than 3 kJ/mol.

The ΔHT(CaTiO3) and ΔST(CaTiO3) values determined in [48] correlate with the results from studies performed via solution calorimetry [37, 41, 42, 44] and EMF [35, 36] at lower temperatures and by Raman spectroscopy [46] and DTA [47] at similar temperatures (Table 1).


3. Melting of perovskite

The data characterizing the melting of simple oxides [23, 24, 57, 58, 59, 60] are quite rough (Table 2). According to different thermochemical data, perovskite’s melting temperature lies in the range of 2188 to 2243 K.

CompoundT, KΔHmelt, kJ/molΔSmelt, J/(mol K)References
3200 ± 5079.5024.84[58]
3210 ± 1055.2017.20[60]
2220 ± 2056.65 ± 11.3325.52 ± 5.10[47]
2241 ± 1047.61 ± 1.8421.24 ± 0.81[48]
2130 ± 2066.94 ± 16.7031.43 ± 7.84[23, 58]
2185 ± 1068.00 ± 8.0031.12 ± 3.66[57]

Table 2.

Temperatures, enthalpies, and entropies of the melting of compounds in the CaO-TiO2 system (calculated for 1 mol of compound).

Klimm et al. [47] estimated the perovskite melting enthalpy as 56.65 ± 11.33 kJ/mol at 2220 ± 20 K (Table 2) which is close to earlier thermochemical estimates [24, 59].

Shornikov [48] based on his own data (Table 1) has obtained more accurate values, characterizing the perovskite melting (Table 2). They coincide satisfactorily with the experimental data obtained by Klimm et al. [47] and the thermochemical estimates made by Bale et al. [24]. The enthalpy of perovskite melting estimated using Walden’s empirical rule [62] is also close to the result obtained by Shornikov [48]: ΔHmelt = 8.8 [J/(g-at K)] Tmelt = 49.39 kJ/mol.


4. The thermodynamic properties of perovskite melts

Thermodynamic information about the CaO-TiO2 melts is quite scarce and limited by the results of only a few experimental studies. Consider the available experimental data, obtained by the Knudsen effusion mass spectrometry.

Banon et al. [52] investigated the evaporation of 24 compositions of the CaTiO3-Ti2O3-TiO2 system from molybdenum containers at 1900–2200 K. The synthesized compositions contained up to 90.2 mol% Ti2O3 and up to 42 mol% TiO2 as well as CaTiO3 compound. Based on the partial vapor pressures (Ca), (TiO), and (TiO2) over melts at 2150 K, the authors calculated the Ti, TiO, Ti2O3, TiO2, and CaTiO3 activities, as well as mixing energies in the melts. In the case of the CaTiO3-TiO2 melts, the TiO2 and CaTiO3 activities were calculated by extrapolation from the data relating to the CaTiO3-Ti2O3-TiO2 system and thus had, according to the authors themselves, low accuracy, which apparently was caused by inconsistency with different versions of the CaO-TiO2 phase diagram [7, 9, 11, 18]. Nevertheless Banon et al. [52], interpreting the obtained high values of TiO2 activities in the region close to titanium dioxide (Figure 5), assumed the presence of immiscibility of the CaO-TiO2 melts in this region.

Figure 5.

The activities of CaO (1, 2), TiO2 (3, 4), and CaTiO3 (5, 6) in the CaO-TiO2 melts, determined at 2057 K (1) in [63], at 2150 K (3, 5) in [52], and at 2250 K (2, 4, 6) in [64].

Stolyarova et al. [63] investigated the properties of the gas phase over 14 compositions of the CaO-TiO2-SiO2 system and also determined the values of oxide activity and melt mixing energy by high-temperature mass spectrometry during the evaporation of melts from tungsten effusion containers at 1800–2200 K. The synthesized compositions contained up to 70 mol% CaO, up to 69 mol% SiO2, and up to 40 mol% TiO2. As it is shown in Figure 5, one of the two studied compositions of the CaO-TiO2 system at 2057 K was in the “CaO + liquid” region, and thus its value should be close to 1. The second composition was in the region of “Ca4Ti3O10 + liquid,” according to the information presented in [7, 18], or in the region of “Ca3Ti2O7 + liquid,” as follows from the data presented by Tulgar [11]. However, the calculated values are quite close (Figure 5), which contradicts the CaO-TiO2 phase diagram (Figure 1). A possible reason for the discrepancies seems to be a significant error in the measurements of CaO activities in the melt, which may be, in our opinion, more than 50%.

Shornikov [64] investigated the evaporation from molybdenum containers of more than 200 compositions of the CaO-TiO2 system containing from 34 to 98 mol% TiO2 at 2241–2441 K. The studied compositions were the CaO-TiO2-SiO2 residual melts containing up to 1 mol% SiO2 that was lost during high-temperature evaporation. The determined composition of the gas phase over the CaO-TiO2 melts allowed to conclude that evaporation reactions are typical for individual oxides predominate.

The oxide activities in the CaO-TiO2 melts were calculated according to Lewis equations [65]:


where pi and pi are the partial pressures of vapor species over individual oxide and melt, respectively. However, it is preferable to calculate the values of oxide activities using the Belton-Fruehan approach [66] via the following equation:


in which the ratio of the oxide activities in the melt could be easily converted to the ratio of the partial pressures, proportional to the ion currents (Ii):


and thus to evade the needs in additional thermochemical data, used in Eq. (5).

The consistency of the values of TiO2 activities calculated by relation (7) was verified using the Gibbs-Duhem equation [67]:


Values of chemical potentials (Δμi), partial enthalpy (ΔHi), and entropy (ΔSi) of oxides in the CaO-TiO2 melts were calculated by known equations [67]:


which are related to the corresponding integral thermodynamic mixing functions:


and are represented in Figure 6.

Figure 6.

The thermodynamic properties of the CaO-TiO2 melts at 2278 K [64] (the chemical potentials of oxides and the mixing energy (a), the partial enthalpies of oxides and the enthalpy of formation (b), and the partial entropies of oxides and the entropy of formation (c)); symbols: (1) CaO, (2) TiO2, (3) integral thermodynamic characteristics (mixing energy, enthalpy, and entropy of formation of the melts, respectively; the vertical dashed line marks the boundary of the “CaO + liquid” region and the melt) and the comparison of mixing energies (d) in the CaO-TiO2 (4), CaO-SiO2 (5), and CaO-Al2O3 (6) melts determined by the Knudsen effusion mass spectrometric method in [64, 68, 69], respectively (the dashed lines correspond to heterogeneous areas).

The results presented by Banon et al. [52] correlate with the data found in [64]. Some difference in values, as mentioned above, is probably due to the procedures for extrapolating information obtained by Banon et al. [52] for compositions of the CaTiO3-Ti2O3-TiO2 triple system, which could reduce their accuracy. The observed behavior of TiO2 activity in melts in the concentration region close to rutile may indicate some immiscibility of the melt, which follows from the observed inflection of the concentration dependence (Figure 5, line 3). However, in our opinion, the behavior of TiO2 and CaTiO3 activities (Figure 5, lines 4 and 6) are close to the ideal. The maximum value corresponds to the area of compositions close to perovskite (Figure 5, lines 5 and 6). Differences with values obtained by Stolyarova et al. [63] (Figure 5, points 1), are caused, apparently, by the low accuracy of the latter.

The partial and integral thermodynamic regularities presented in Figure 6 characterizing the CaO-TiO2 melts are symbate. The enthalpy and entropy of melt formation are positive. The extreme values of the integral thermodynamic properties of the melts are in the concentration ranges close to perovskite, which confirms its stability in the melt. Some displacement of the extremum of integral thermodynamic functions can be caused by the presence of oxide compounds with a large amount of CaO in comparison with perovskite CaTiO3 in the melt. A comparison of mixing energies in the CaO-TiO2 melts at 2300 K with those for the CaO-SiO2 [68] and CaO-Al2O3 [69] melts (Figure 6d) indicates a stronger chemical interaction in the CaO-TiO2 melts than the CaO-Al2O3 melts, but smaller than in the CaO-SiO2 melts. It manifests in more positive values of the mixing energy of the melts.


5. The gas phase over perovskite

The evaporation processes and the thermodynamic properties of simple oxides CaO and TiO2 were considered in detail in reference books [23, 24, 57, 70, 71].

The gas phase over calcium oxide consists of the molecular components (O), (O2), (O3), (O4), (Ca), (Ca2), and (CaO) possibly formed by the following reactions:


The gas phase over titanium oxide contains similar vapor molecular forms (O), (O2), (O3), (O4), (Ti), (Ti2), (Ti3), (TiO), and (TiO2) formed by similar reactions:


Balducci et al. [72] detected (Ti2O3) and (Ti2O4) molecules in the gas phase over cobalt titanate CoTiO3 at 2210–2393 K by the Knudsen effusion mass spectrometric method, which can be involved in the following equilibria:


Note that the predominant components of the gas phase over these oxides are (Ca), (CaO), (TiO), (TiO2), (O), and (O2); the content of other vapor species does not exceed 1% of the total concentration at 1700–2200 K.

The properties of the gas phase over perovskite were studied in less detail. The experimental conditions and results of high-temperature studies of perovskite evaporation we will consider below.

Zakharov and Protas [73] studied ion emission from the perovskite surface under the action of laser radiation and identified the ion of a complex molecule (CaTiO3) in addition to the ions of simple oxides (O+, Ca+, CaO+, Ti+, TiO+) in the mass spectra of the vapor. They explained the presence of this ion by the similarity of high-temperature evaporation of alkaline-earth oxide titanates, which is confirmed by the composition of the observed condensates (BaTiO3, SrTiO3, and CaTiO3) formed under similar conditions [74, 75]. The intensity ratio of ion currents in the mass spectra of vapor over perovskite obtained at laser pulse duration of 800–1000 μs at a wavelength of 6943 Å and energy of 3–5 J was as follows: IO:ICa:ICaO:ITi:ITiO:ICaTiO3 = 0.41:100:0.17:4.32:0.54:0.05. Note that the TiO2+ ion was not observed in the mass spectrum of vapor over both perovskite CaTiO3 and rutile TiO2. This is explained by the peculiarity of the mass spectrometric experiment using a laser, in which the easily ionizable molecular species dominate the mass spectra of vapor and the not readily ionizable molecules are discriminated. This selectivity of detected ions in the mass spectra of vapor significantly limits the accuracy and applicability of this method [76]. According to the data of [57], the estimated temperature of heating of perovskite under the action of laser radiation based on the possible equilibrium in the gas phase.


is 4890 ± 70 K, which is approximate, but does not contradict the conditions of similar laser-impact mass spectrometry experiments in the range 4000–6000 K.

Banon et al. [52] studied the evaporation of the CaTiO3-Ti2O3-TiO2 melts from molybdenum Knudsen effusion cells at 1900–2200 K by differential mass spectrometry. The mass spectra were recorded at a low ionizing voltage of 13 eV in order to avoid possible fragmentation of the TiO2+ molecular ion into Ti+ and TiO+ fragmentation ions, which were also molecular ions.

Atomic calcium was the dominant component of the gas phase over the composites. The complex gaseous oxide (CaTiO3) was not detected. The partial pressures of the (Ca), (TiO), (TiO2), and (O) vapor over perovskite at 2150 K were calculated using the thermochemical data of [57] and are shown in Figure 7 as a function of the inverse temperature (for easily understanding, the temperature scale was scaled appropriately).

Figure 7.

The partial pressure of Ca (a), TiO (b), TiO2 (c), and O (d) over perovskite (1–3) and oxides of calcium (4, 5, 9) and titanium (6–8, 10) vs. the inverse temperature, determined via Knudsen mass spectrometry: (1) in [77], (2) in [52], (4) in [78], (5) in [79], (6) in [80], (7) in [81], and (8) in [71]; using the vacuum furnace (according to Langmuir), (3) in [4]; and calculated, (9) and (10), according to the thermochemical data [57]; the vertical dashed lines (11) and (12) indicate melting points of titanium oxide and perovskite, respectively.

Gaseous perovskite was also not detected in the mass spectrometric studies of high-temperature evaporation of various compositions of the CaO-TiO2-SiO2 system from molybdenum and tungsten Knudsen effusion cells at 1700–2500 K [53, 63, 82, 83] presumably because the sensitivity of the equipment used in [63, 83] was insufficient for determining the CaTiO3+ ion or because this was not the purpose of the study [53, 82].

Lopatin and Semenov [84] studied the evaporation of a mixture of calcium carbonate and titanium dioxide from tungsten cells by the Knudsen effusion mass spectrometry method in the temperature range 2100–2500 K. The following ions were detected in the mass spectra of vapor over the mixture: Ca+, CaO+, Ti+, TiO+, TiO2+, and CaTiO3+. The energies of ion appearance in the mass spectra allowed the authors to determine the molecular origin of the Ca+, CaO+, TiO+, TiO2+, and CaTiO3+ ions. The TiO+ ion also contained a fragment component of the TiO2+ ion, and the Ti+ ion was completely fragmentary. The energy of appearance of the CaTiO3+ molecular ion was determined to be 9 ± 1 eV (the energy of appearance of the gold ion was used as a standard). The partial pressures of vapor species (pi) were calculated by comparison with the accepted partial vapor pressures of gold taken as standard pressures (ps) by the equation:


where Ii (Is) is the intensity of the ion current of the ith component of vapor (standard substance) recorded at a temperature Ti (Ts). The calculation should also include the ratios of the effective ionization cross sections of the ith molecular form and the standard substance (σis), isotope distributions (ηis), and individual ion efficiencies (γis), which depend on various parameters of ion current recording devices. The pressures pCaO, pTiO2, and pCaTiO3 calculated by (31) were used to determine the temperature dependence of the equilibrium constant in the gas phase:


and subsequently calculate the enthalpies of formation (ΔfH298) and atomization (ΔatH298) of the CaTiO3 molecule (Table 3).

ReactionT, KΔrH298, kJ/molΔrHT, kJ/molΔrST, J/(mol K)Refs.
(CaTiO3) = (CaO) + (TiO2)2287–2466545 ± 8284 ± 4428 ± 19[84]
2000298 ± 30[85]
1956–2182287 ± 1218 ± 6[77]
[Ca] + [Ti] + 3/2(O2) = (CaTiO3)2287–2466−826 ± 26[84]
1956–2182−760 ± 10−242 ± 5[77]
(CaTiO3) = (Ca) + (Ti) + 3(O)2287–24662225 ± 26[84]
20001983 ± 81[85]
1956–21821993 ± 15396 ± 7[77]
[CaTiO3] = (CaTiO3)20001030 ± 22[85]
1956–21821027 ± 10297 ± 5[77]

Table 3.

Enthalpies and entropies of the reactions involving the CaTiO3 molecule.

Zhang et al. [4] studied the isotope fractionation of calcium and titanium during the evaporation of a perovskite melt suspended on an iridium wire in a vacuum furnace at a temperature of 2278 K (according to Langmuir method). The change in the composition of the residual perovskite melt during evaporation suggested that the component that evaporated predominantly from the melt was its calcium component. The total vapor pressure over perovskite could be evaluated from the data obtained (Figure 7).

Shornikov [64, 77] investigated the evaporation of perovskite at 1791–2182 K and its melts at 2241–2441 K from molybdenum Knudsen effusion cells by high-temperature mass spectrometric method.

The TiO2+, Ca+, TiO+, and O+ ions prevailed in the mass spectra of vapor over perovskite and its melts at the ionizing electron energy of 20 eV, as well as other ions characteristic of the mass spectra over individual oxides [57, 58, 71]. A small amount of CaTiO3+ ion was observed, which was fragmented into CaTi+, CaTiO+, and CaTiO2+ ions (ICaTi:ICaTiO:ICaTiO2:ICaTiO3 = 6:10:13:100). The ratio of the ion current intensities in the mass spectra of vapor over perovskite at 2182 K was the following: ICa:ICaO:ITi:ITiO:ITiO2:ICaTiO3:IO:IO2 = 80:0.04:0.1:75:100:0.02:40:0.3. It corresponded to that observed by Samoilova and Kazenas [78] in the same temperature range at evaporation of CaO from alundum cell and by Semenov [86] at evaporation of TiO2 from a tungsten cell.

The ratio of the ion current intensities in the mass spectra of vapor over perovskite melt containing 57.81 ± 0.15 mol% TiO2 at 2278 K was the following: ICa:ICaO:ITi:ITiO:ITiO2:ICaTiO3:IO:IO2 = 25:0.02:0.1:56:100:0.13:0.44:0.012, which is different from that for the case of perovskite [77].

The presence of MoOi+ (i = 0–3) ions in the mass spectra of vapor over perovskite was due to the evaporation of molybdenum cell at high temperature:


as well as the interaction of perovskite with the cell material (ITiO2:IMo:IMoO:IMoO2: IMoO3 = 100:0.8:2.6:7.3:0.6) that was detected according to the following equilibria:


Note that Berkowitz et al. [81] found that during evaporation of titanium oxide from a molybdenum liner inserted into a tantalum crucible at 1881 K, pMoO2 was initially 10–102 times higher than pTiO2 . The pMoO2 value gradually decreased and became comparable with the pTiO2 value, which is significantly different from the other results [52, 53, 56, 64, 77, 82]. The high pMoO2 observed in [81] probably was due to poor quality of the molybdenum liner material (or its alloy). Possibly it was made using powder technology from MoO3 reduced to metal molybdenum at ∼1300 K. It could lead to such an excess of partial pressure of (MoO3) and its decrease as it evaporates from the surface layers of the liner material.

The appearance energies of ions in the mass spectra of vapor over perovskite were determined by the Warren method [87] and corresponded to the accepted values of the ionization energies of atoms and molecules [88]. The appearance energy of CaTiO3+ ion in the mass spectra of vapor over perovskite was equal to 8.5 ± 0.6 eV (the appearance energy of silver ion was used as a standard) and corresponded to obtained by Lopatin and Semenov [84].

The established molecular composition of the gas phase over perovskite allowed us to draw a conclusion on the predominant evaporation of perovskite according to the reactions (17), (18), (20), (23), (24), and (25), typical for evaporation of simple oxides [57, 71, 78, 86]. The presence of a small amount of (CaTiO3) molecules in the gas phase over perovskite is probably due to the reaction:


The partial pressure values of vapor species in the gas phase over perovskite were determined by the Hertz-Knudsen equation, written in the following form [89]:


where qi is the amount of ith substance component evaporated from the effusion cell, Mi is the molecular weight, t is time of evaporation, T is temperature, Cor is the Clausing coefficient characterized the effusion hole, and sor is the hole area.

The Kα constant value was calculated taking into account the evaporation coefficient (αi) of substance component associated with the molecule changing during its transition to the gas phase from the surface with an Sv area, using the Komlev equation [90]:


where Cc is the Clausing coefficient characterized effusion cell.

The Clausing coefficient is associated with the collision of vapor species inside the effusion orifice channel of effusion cell and their reverse reflection from the channel walls. Its value does not exceed 1 and depends on the ratio of the diameter of the effusion hole to its thickness.

Taking into account predominance of typical for CaO and TiO2 vapor species in the gas phase over perovskite and small amounts of CaTiO3, the αi values were used from [91].

The partial pressures of vapor species over perovskite at 1791–2182 K and its melts at 2278 K calculated using the relationships (38) and (39) with an error not exceeding 8% are shown in Figure 8.

Figure 8.

The partial pressure values of vapor species over perovskite (a) [77] and over the CaO-TiO2 melts at 2278 K (b) [64]: (1) Ca, (2) CaO, (3) Ti, (4) TiO, (5) TiO2, (6) O, (7) O2, and (8) CaTiO3.

The partial pressure of atomic oxygen determined using the relationships (38) and (39) agrees satisfactorily with those calculated using the thermochemical data [57] on Kr(T) equilibrium constants of possible reactions (18), (20), (24), (25), and (36) in the gas phase over perovskite in the following relations:


It should be noted that the pO values calculated according to the independent reactions in the gas phase over perovskite (40)(45) were the same. It confirmed the assumption about the molecular origin of the identified ions in the mass spectrum of vapor over perovskite.

As it follows from Figure 8a, the defined partial pressures of vapor species over perovskite can be represented as linear logarithmic dependence vs. the inverse temperature:


Note that the relationship (45) is the same as the expression for the reaction constant [57]:


which allows to determine the enthalpy (ΔrHT) and entropy (ΔrST) of a reaction.

The partial pressures of the predominant vapor species of the gas phase over perovskite (Ca, TiO, TiO2 and O) are compared in Figure 7 with the results on evaporation of simple oxides (CaO and TiO2) under similar redox conditions caused by the interaction of oxygen with molybdenum [79, 81], tungsten [71], and tantalum [80] effusion cells or in chemically neutral conditions (in the absence of this interaction) for alundum cell [78].

We used the TiO and TiO2 activities as well as the Gibbs energy of perovskite obtained by Banon et al. [52] and thermochemical data [52] on equilibriums (17), (18), (23), and (24) to estimate the partial pressure of vapor species over the perovskite at 2150 K. Therefore, the obtained values characterized by the evaporation of perovskite were not under reducing conditions (from molybdenum cell), but, in contrary, under chemically neutral conditions (in the absence of interaction of perovskite with the cell material).

Figure 7 also shows the partial pressures of vapor species over calcium and titanium oxides calculated using thermochemical data [57]. By comparison of the experimental data obtained in [71, 77, 78, 79, 80, 81] and the calculated results, we can see the effect of reducing properties of cell materials on gas phase composition: tantalum [80], molybdenum [79, 81], tungsten [71], and alundum [78]. As we noted earlier [85], the greatest effect of cell materials on the vapor composition are observed with the oxygen-“deficient” species such as atomic calcium (Figure 7a), titanium monoxide (Figure 7b), and atomic oxygen itself (Figure 7d). There are no differences in the partial pressure of gaseous titanium dioxide (Figure 7c) determined in evaporation experiments using molybdenum [81] and tungsten [71] cells.

The total vapor pressure over the perovskite melt at 2278 K obtained by Zhang et al. [4] is consistent with the extrapolated values of partial pressures of the predominant vapor species of the gas phase—atomic calcium and titanium dioxide (Figure 7a and c) found in [77].

Similar slopes of lg pCa and lg pO vs. the inverse temperature for calcium oxide and perovskite in Figure 7a and d (lines 1, 5 and 9, respectively) indicate a predominant effect of calcium component on evaporation of calcium from perovskite. This also can explain the difference in the slope of lg pTiO in Figure 7b in the case of perovskite (line 1) and rutile (line 10) according to the equilibriums (18) and (24).

The enthalpy and entropy of reactions involving CaTiO3 gaseous complex oxide calculated by the relationship (46) are given in Table 3. They are in a good agreement with those found by Lopatin and Semenov [84] and our earlier estimates [85].

The concentration dependences of partial pressures of vapor species over perovskite melts show a sharp decrease in pCa and pCaO (Figure 8b, lines 1 and 2) with increasing of TiO2 content in the melt. The vapor species containing titanium—(Ti), (TiO), and (TiO2)—are increased with increasing TiO2 concentration up to 65–70 mol% TiO2, and further they are almost constant in the region of 75–100 mol% TiO2 (Figure 8b, lines 3–5), which may indicate the immiscibility of the melt observed by Banon et al. [52]. The partial pressures of (O) and (O2) slightly vary throughout the concentration range under consideration, showing a minimum in the perovskite concentration (Figure 8b, lines 6 and 7). The (CaTiO3) partial pressures have maximum values in the melt region with a high calcium content compared to the perovskite concentration (Figure 8b, line 8), as it was noted earlier.


6. Conclusions

The thermodynamic properties of perovskite determined by different calorimetric approaches and EMF method agree with the results obtained via Knudsen effusion mass spectrometry at high temperatures. The resulting values of oxide activities in perovskite, as well as the Gibbs energy, the entropy and enthalpy of the formation of perovskite from simple oxides, and the melting enthalpy of perovskite are consistent with each other. The enthalpy of perovskite formation is constant throughout the temperature range, and the entropy of perovskite formation tends to increase slightly.

The oxide activities in perovskite melts were determined by mass spectrometric Knudsen effusion method. The thermodynamic properties of melts (chemical potentials of oxides and mixing energies, as well as partial and integral enthalpies and entropies of melt’s formation) were calculated based on the experimental data. The obtained experimental information testifies to the symbate behavior of thermodynamic functions characterizing the melts. The extreme values of the integral thermodynamic properties of melts are in the concentration region close to perovskite, which confirms its stability in the melt. The displacement of the extremum of the integral thermodynamic functions in the CaO-TiO2 melts can be caused by the presence in the melt of oxide compounds with a large amount of CaO compared to perovskite. A comparison of mixing energies in the CaO-TiO2 melts with those for the CaO-SiO2 and CaO-Al2O3 melts indicates a stronger chemical interaction in the CaO-TiO2 melts than the similar CaO-Al2O3 melts, but smaller than in the CaO-SiO2 melts.

The evaporation of perovskite and its melts from a molybdenum cell at high temperature was studied by the Knudsen effusion mass spectrometric method. The molecular components typical of simple oxides and the (CaTiO3) gaseous complex oxide were identified in the gas phase over perovskite. The partial vapor pressures of the molecular components of the gas phase over perovskite were determined. A comparison of these values with the available experimental data and with the values corresponding to simple oxides showed that the character of perovskite evaporation is mainly affected by the calcium component of perovskite. The observed concentration dependences of the partial pressures of vapor species over the perovskite melts correspond to those characterizing the condensed phase.



This study was financially supported by the Presidium of the Russian Academy of Sciences (Program No. 7 “Experimental and Theoretical Studies of Solar System and Star Planetary System Objects. Transition Processes in Astrophysics”) and by the Russian Foundation for Basic Research (Grant No. 19-05-00801A “Thermodynamics of Formation Processes of Substance of Refractory Inclusions in Chondrites”).



I am grateful to Oleg Yakovlev (Vernadsky Institute of Geochemistry and Analytical Chemistry of the Russian Academу of Sciences) for his constant interest in this study and useful discussions and to Mikhail Nazarov (Vernadsky Institute of Geochemistry and Analytical Chemistry of the Russian Academу of Sciences) for his support during this work. I express my special gratitude to Marina Ivanova (Vernadsky Institute of Geochemistry and Analytical Chemistry of the Russian Academу of Sciences; National Museum of Natural History of Smithsonian Institution) for her help in working on the manuscript.


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Written By

Sergey Shornikov

Submitted: 26 December 2019 Reviewed: 22 January 2020 Published: 27 October 2020