The heat capacity and derived thermophysical properties of In2O3 from 0 to 1000 K

The heat capacity from 5 to 350K of In2O3 has been measured by adiabatic calorimetry. For the thermophysical properties at room temperature Cop(298.15 K) = (99.08 +/- 0.09) J mol -1 K -1 and So(298.15 K) = (101.80 +/- 0.06) J mol-1 K-1 have been derived. Enthalpy increments relative to 298.15 K have been measured by drop calorimetry from 502 to 959.2 K: [Ho(T)-Ho(298.15 K)}/J mol-1=109.1383(T/K)+13.73786 x 10-3(T/K)2 +16.22947 x 105(T/K)-1-39,204.2.The thermodynamic functions, including the formation properties [Delta]fHo and [Delta]fGo(T), have been derived for temperatures up to 1000K.Peer Reviewedhttp://deepblue.lib.umich.edu/bitstream/2027.42/30191/1/0000576.pd

The heat capacity and derived thermophysical properties of some alkaline earth silicates and zirconates from 5 to 1000 K--I. Crystalline SrSiO3 and Sr2SiO4

The heat capacities of SrSO3 and Sr2SiO4 were measured from 5 to 350 K. by adiabatic calorimetry, and the derived thermophysical properties, H[deg], S[deg], and {G[deg] - H[deg] (0)}/T were calculated. For the standard molar entropies at 298.15 K the values (95.65 +/- 0.21) J mol-1 K-1 and (155.44 +/- 0.25) J mol-1 K-1, respectively were found, Enthalpy increments relative to 298.15 K were measured by drop calorimetry for SrSiO3 from 503.0 to 886.4 K and for Sr2SiO4 from 503.0 to 886.2 K.The thermodynamic functions including the formation properties [Delta]HT[deg](t) and [delta]DG[deg](T), were derived for temperatures up to 1000 K.Peer Reviewedhttp://deepblue.lib.umich.edu/bitstream/2027.42/30026/1/0000394.pd

Low-temperature heat capacity and thermodynamic functions of IrO2

The heat capacity from 5 to 350 K of IrO2 has been measured by quasi-adiabatic equilibrium calorimetry. The values for the thermodynamic properties at 298.15 K have been calculated as Cp, m(T)/R = 6.687, [Delta]0TSmo/R = 6.133, [Delta]0THmo/(R [middle dot] K) = 1039.5, and [Phi]mo(T, 0)/R = 2.647. The low-temperature heat capacity shows typical metallic behavior with an electronic coefficient [gamma]/R = 0.00067 K-1. The entropy at 298.15 K is shown to be consistent with the volumetric dependence of this quantity.Peer Reviewedhttp://deepblue.lib.umich.edu/bitstream/2027.42/27003/1/0000570.pd

The thermodynamic properties of cesium metaborate CsBO2 from 5 to 1000 K

The low-temperature heat capacities of cesium metaborate were measured by adiabatic calorimetry from 9 to 346 K. High-temperature enthalpy increments of CsBO2 were measured by drop calorimetry from 414 to 671 K. In addition, the melting data were measured by DSC. The thermodynamic functions CpXXX(T), SXXX(T), {HXXX(T)-HXXX(298.15 K)}, [Delta]fHXXX(T) and [Delta]fGXXX(T) were calculated up to the melting point.Peer Reviewedhttp://deepblue.lib.umich.edu/bitstream/2027.42/27264/1/0000274.pd

Recent thermochemical research on reactor materials and fission products

By adiabatic calorimetric measurements from 5 to 350 K and enthalpy increment determinations above the ambient temperature the thermophysical properties of such uranium compounds as UF3, UC13, UBr3, URu3, URh3, UPd3 and fission product combinations such as RuO2, RuSe2, and CsBO2 have been obtained. In addition, the enthalpies of formation of these substances have been determined by EMF and enthalpy of solution measurements. By combining these measurements the formation properties have been derived as a basis for modeling, critical evaluation and prediction. Some examples of these applications are given.Peer Reviewedhttp://deepblue.lib.umich.edu/bitstream/2027.42/27772/1/0000166.pd

The thermochemical and thermophysical properties of Cs2RuO4 and Cs2MnO4 at temperatures from 5 K to 1000 K

Low-temperature heat capacities from 5 K to 350 K by adiabatic calorimetry and high-temperature enthalpy increments above T = 450 K to 800 K by drop calorimetry of Cs2RuO4 and Cs2MnO4 have been measured. The two compounds exhibit solid-to-solid phase transitions at T = 906.8 K and T = 1051.9 K, respectively, and melt at T = 1211.8 K and T = 1175.5 K, respectively. The enthalpies of transition and the melting temperatures have been determined by d.s.c. measurements. From the results, smoothed thermochemical and thermophysical functions have been tabulated at selected temperatures up to 1000 K. For the standard molar entropies of Cs2RuO4 and Cs2MnO4 at T = 298.15 K the values Som/R = 31.64 and 28.77, respectively, have been found.Peer Reviewedhttp://deepblue.lib.umich.edu/bitstream/2027.42/29933/1/0000290.pd

CsOH: Low-temperature heat capacity and high-temperature enthalpy increment

Heat capacities of CsOH(s) have been measured by adiabatic calorimetry from 5 to 350 K, and a reversible [lambda]-type transition has been observed at 233.96 K. C0p(298.15 K) = (69.96+/-0.10) J mol-1K-1, and S0(298.15 K) = (104.22+/-0.08) J mol-1K-1. High-temperature enthalpy increments of solid as well as liquid CsOH have been measured from 440 to 683 K by drop calorimetry. In combination with DSC-measurements the orthorhombic/cubic transition and the melting point were located at (498.2+/-0.5) K and (615.5+/-0.5) K, respectively.Peer Reviewedhttp://deepblue.lib.umich.edu/bitstream/2027.42/28885/1/0000721.pd

Chemical-looping combustion - a thermodynamic study

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