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Kazuhiro Nagata - One of the best experts on this subject based on the ideXlab platform.
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Gibbs Energy Change of Carbothermal Nitridation Reaction of Al2O3 to Form AlN and Reassessment of Thermochemical Properties of AlN
Journal of the American Ceramic Society, 2004Co-Authors: Wataru Nakao, Hiroyuki Fukuyama, Kazuhiro NagataAbstract:The experimental method for the high-temperature reaction equilibria in the AlN-Al2O3 system has been established. The equilibrium N2-CO gas compositions coexisting with AlN- Al2O3-graphite have been successfully measured by quadrupole mass spectrometry and gas chromatography. From the obtained results, the standard Gibbs energy change of the forming reaction of AlN by carbothermal nitridation is determined at temperatures ranging from 1723 to 1899 K: From the obtained result, the standard Gibbs energy of formation of AlN and the third-law enthalpy of formation of AlN at 298.15 K are derived as The disagreement between the present results and values in the NIST–JANAF Thermodynamic Table is discussed.
Wataru Nakao - One of the best experts on this subject based on the ideXlab platform.
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Gibbs Energy Change of Carbothermal Nitridation Reaction of Al2O3 to Form AlN and Reassessment of Thermochemical Properties of AlN
Journal of the American Ceramic Society, 2004Co-Authors: Wataru Nakao, Hiroyuki Fukuyama, Kazuhiro NagataAbstract:The experimental method for the high-temperature reaction equilibria in the AlN-Al2O3 system has been established. The equilibrium N2-CO gas compositions coexisting with AlN- Al2O3-graphite have been successfully measured by quadrupole mass spectrometry and gas chromatography. From the obtained results, the standard Gibbs energy change of the forming reaction of AlN by carbothermal nitridation is determined at temperatures ranging from 1723 to 1899 K: From the obtained result, the standard Gibbs energy of formation of AlN and the third-law enthalpy of formation of AlN at 298.15 K are derived as The disagreement between the present results and values in the NIST–JANAF Thermodynamic Table is discussed.
Hiroyuki Fukuyama - One of the best experts on this subject based on the ideXlab platform.
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Gibbs Energy Change of Carbothermal Nitridation Reaction of Al2O3 to Form AlN and Reassessment of Thermochemical Properties of AlN
Journal of the American Ceramic Society, 2004Co-Authors: Wataru Nakao, Hiroyuki Fukuyama, Kazuhiro NagataAbstract:The experimental method for the high-temperature reaction equilibria in the AlN-Al2O3 system has been established. The equilibrium N2-CO gas compositions coexisting with AlN- Al2O3-graphite have been successfully measured by quadrupole mass spectrometry and gas chromatography. From the obtained results, the standard Gibbs energy change of the forming reaction of AlN by carbothermal nitridation is determined at temperatures ranging from 1723 to 1899 K: From the obtained result, the standard Gibbs energy of formation of AlN and the third-law enthalpy of formation of AlN at 298.15 K are derived as The disagreement between the present results and values in the NIST–JANAF Thermodynamic Table is discussed.
S.k. Rakshit - One of the best experts on this subject based on the ideXlab platform.
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Thermodynamic studies on Rb 2 CeO 3
Journal of Thermal Analysis and Calorimetry, 2017Co-Authors: P. Samui, P. Ginishkumar, N. Sebastian, N. K. Shukla, S.k. RakshitAbstract:Rb2CeO3 compound was prepared by conventional solid-state reaction route. The Gibbs energy formation of the compound was determined by measuring the partial pressure of CO2 over the equilibrium phase mixture {Rb2CO3(s) + CeO2(s) + Rb2CeO3(s)} using Knudsen effusion quadrupole mass spectrometry. Gibbs energy formation of the compound, $$\Delta_{\text{f}} G_{\text{m}}^{o}$$ , as a function of temperature is obtained as: $$\Delta_{\text{f}} G_{\text{m}}^{\rm o} \left( {{\text{Rb}}_{2} {\text{CeO}}_{3} ,{\text{s}},T} \right)({\text{kJ}}\;{\text{mol}}^{ - 1} ) \, \left( { \pm 7} \right)\; = \; - 1601 + 0.41 \times \left( {T/K} \right)(991 \le T/K \le 1124)$$ The molar heat capacity of the compound, $$C^{\text o}_{\text{p,m}}$$ , was measured from 390 to 1100 K using a differential scanning calorimeter and is given as: $$C^{\rm o}_{\text{p,m}} \left( {{\text{Rb}}_{2} {\text{CeO}}_{3} ,{\text{s}},T} \right) \, ({\text{J}}\;{\text{mol}}^{ - 1} \;{\text{K}}^{ - 1} ) = 210.8 + 0.0061 \times \left( {T/K} \right){-}6348435/\left( {T/K} \right)^{2}$$ Based on these experimental data, Thermodynamic Table of the compound was also generated from 298.15 to 1000 K. Standard molar enthalpy of formation $$\Delta_{\text{f}} H_{\text{m}}^{\rm o}$$ (298.15 K) and standard molar entropy $$S_{\text{m}}^{\text o}$$ (298.15 K) of Rb2CeO3 are −1643 kJ mol−1 and 61.5 J K−1 mol−1, respectively.
P. Samui - One of the best experts on this subject based on the ideXlab platform.
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Thermodynamic studies on Rb 2 CeO 3
Journal of Thermal Analysis and Calorimetry, 2017Co-Authors: P. Samui, P. Ginishkumar, N. Sebastian, N. K. Shukla, S.k. RakshitAbstract:Rb2CeO3 compound was prepared by conventional solid-state reaction route. The Gibbs energy formation of the compound was determined by measuring the partial pressure of CO2 over the equilibrium phase mixture {Rb2CO3(s) + CeO2(s) + Rb2CeO3(s)} using Knudsen effusion quadrupole mass spectrometry. Gibbs energy formation of the compound, $$\Delta_{\text{f}} G_{\text{m}}^{o}$$ , as a function of temperature is obtained as: $$\Delta_{\text{f}} G_{\text{m}}^{\rm o} \left( {{\text{Rb}}_{2} {\text{CeO}}_{3} ,{\text{s}},T} \right)({\text{kJ}}\;{\text{mol}}^{ - 1} ) \, \left( { \pm 7} \right)\; = \; - 1601 + 0.41 \times \left( {T/K} \right)(991 \le T/K \le 1124)$$ The molar heat capacity of the compound, $$C^{\text o}_{\text{p,m}}$$ , was measured from 390 to 1100 K using a differential scanning calorimeter and is given as: $$C^{\rm o}_{\text{p,m}} \left( {{\text{Rb}}_{2} {\text{CeO}}_{3} ,{\text{s}},T} \right) \, ({\text{J}}\;{\text{mol}}^{ - 1} \;{\text{K}}^{ - 1} ) = 210.8 + 0.0061 \times \left( {T/K} \right){-}6348435/\left( {T/K} \right)^{2}$$ Based on these experimental data, Thermodynamic Table of the compound was also generated from 298.15 to 1000 K. Standard molar enthalpy of formation $$\Delta_{\text{f}} H_{\text{m}}^{\rm o}$$ (298.15 K) and standard molar entropy $$S_{\text{m}}^{\text o}$$ (298.15 K) of Rb2CeO3 are −1643 kJ mol−1 and 61.5 J K−1 mol−1, respectively.