2 edition of Low-temperature heat capacities and enthalpy of formation of aluminum sulfide (Al2S3) found in the catalog.
Low-temperature heat capacities and enthalpy of formation of aluminum sulfide (Al2S3)
H. C. Ko
Bibliography: p. 9.
|Statement||by H. C. Ko, J. M. Stuve, and R. R. Brown : Albany Metallurgy Research Center.|
|Series||Report of investigations - Bureau of Mines ; 8203, Report of investigations (United States. Bureau of Mines) -- 8203.|
|Contributions||Stuve, J. M., Brown, Robert R., United States. Bureau of Mines.|
|The Physical Object|
|Pagination||, 9 p. ;|
The CRC Handbook of Chemistry and Physics (HBCP) contains over tables in over documents which may be divided into several pages, all categorised into 17 major subject areas. The result is a change to the potential energy of the system. The heat absorbed or released from a system under constant pressure is known as enthalpy. Mathematically, we can think of the enthalpy of reaction as the difference between the potential energy from the product bonds and the potential energy of the reactant bonds.
The thermochemical data available include enthalpies of formation, enthalpies of phase transitions, and heat capacities. Thermochemical properties of many reactions that support enthalpy of formation values are provided. Automated tools are used Cited by: Calphad assessment of Zr-C system by Guillemet relied on phase equilibria data from Sara and Rudy, selected values for enthalpies of formation and high temperature heat contents for ZrC ZrC , and low-temperature heat capacity and entropy for ZrC Cited by: 3.
The latent heat of the A3 transformation and the ferromagnetic transition of pure iron is summarised by Houdremont () as shown in figure latent heat of the A3 transformation ranges from 12 kJ kg ÿ1to 28 kJ kg. The latent heat from austenite to pearlite of standard plain carbon steels is also inaccurately known (Krielaart et al ). Pubs Warehouse Home > Browse > Article > Journal Article > American Mineralogist. Browse the USGS Publication Warehouse Publications in the Series American Mineralogist. Discrete Zr and REE mineralization of the Baerzhe rare-metal deposit, China, , American Mineralogist () -
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Low-temperature heat capacities and enthalpy of formation of aluminum sulfide (Al2S3). Washington: Dept. of the Interior, Bureau of Mines, (OCoLC) Calorimetric determinations of low-temperature heat capacities and the standard enthalpy of formation were made by the Bureau of Mines for aluminum sulfide, al2s3.
The standard entropy (s deg), enthalpy of formation (hf deg), and calculated Gibbs energy of formation (gf deg) at K are +/- Cal/deg-mole, +/- Kcal/mole. Enthalpy of formation and low-temperature heat capacities of basic aluminum sulfite (A1?O?SO?H?0) [Ko, H.
C.] on *FREE* shipping on qualifying : $ Low-temperature heat capacities and enthalpy of formation of copper difluoride (CuF) (Report of investigations - Bureau of Mines) [Beyer, R. P] on *FREE* shipping on qualifying offers. Low-temperature heat capacities and enthalpy of formation of copper difluoride (CuF) (Report of investigations - Bureau of Mines)Author: R.
P Beyer. Low-temperature heat capacities of the title compound were measured by a precision automated adiabatic calorimeter over the temperature range from 80 to K, and heat capacities and thermodynamic data were also obtained.
In addition, the standard molar enthalpy of formation of the title complex was determined by an isoperibol solution Cited by: 1. Low-temperature heat capacities of the solid coordination compound Zn(His)SO 4 H 2 O(s) were precisely measured by a precision automated adiabatic calorimeter over the temperature range between T=78 and K.
The initial dehydration temperature of the coordination compound was determined to be, T d = K, by analysis of the heat-capacity curve.
The experimental values of molar heat Cited by: 2. Research done at the Bureau of Mines has produced calorimetric data for the low temperature heat capacity from 12 to k and the high temperature relative enthalpy from to k for aluminum sulfide (al2s3).
The heat capacity measurments yielded s deg = +- Cal k-1 mol-1 for the standard entropy at K (1 cal = J). ∆fH° Standard molar enthalpy (heat) of formation at K in kJ/mol ∆ f G° Standard molar Gibbs energy of formation at K in kJ/mol S° Standard molar entropy at K in J/mol KFile Size: KB.
Low-temperature heat capacities of the solid coordination compound Cr(C6H4NO2)3(s) have been measured by a precision automated adiabatic calorimeter over the temperature range T = 78 K to T = K. The experimental values of the molar heat capacities in the temperature region were fitted to a polynomial equation of heat capacities (Cp,m) with the reduced temperatures (X), [X = f(T)], by a Cited by: 3.
Abstract. Molar heat capacities (C p,m) of aspirin were precisely measured with a small sample precision automated adiabatic calorimeter over the temperature range from 78 to phase transition was observed in this temperature region.
The polynomial function of C p,m vs. T was established in the light of the low-temperature heat capacity measurements and least square fitting Cited by: fields, low-temperature heat capacity and constant-volume combustion energy of the compound have been measured by a precision automated adiabatic calorimeter in the temperature range 78 - K and a oxygen-bomb combustion calorimeter at K, respectively.
The thermodynamic functions and standard molar enthalpy of formation of theCited by: 1. The low-temperature heat capacity of covellite has been reported in previous investigations.“4-‘7) In the most recent, released during the course of this study, Ferrante et u1.(17) presented heat capacities from 5 to K, and enthalpies from to K by drop calorimetry.
The standard enthalpy of formation was determined to be − kJ mol−1 with isoperibol reaction calorimeter at K. Low-temperature heat capacity and standard enthalpy of formation of neodymium glycine perchlorate complex [Nd Cited by: 2.
The low-temperature experimental heat capacities of crystalline IND from to K were measured by PPMS and fit to a theoretical model in the low temperature range (T. The low-temperature heat capacity of Na2Lu (MoO4)(PO4) was measured by adiabatic calorimetry in the range of – K.
The experimental data were used to calculate the thermodynamic. Low-Temperature Heat Capacities and Enthalpy of Formation of Aluminum Sulfide (Al2S3) (report of investigations #; Washington: Dept.
of the Interior, Bureau of Mines, ), by H. Ko, J. Stuve, and R. Brown (page images at HathiTrust). Brown, R. (Robert R.): Low-Temperature Heat Capacities and Enthalpy of Formation of Aluminum Sulfide (Al2S3) (report of investigations #; Washington: Dept.
of the Interior, Bureau of Mines, ), also by H. Ko and J. Stuve (page images at HathiTrust). Sodium hydroxide, also known as lye and caustic soda, is an inorganic compound with the formula NaOH.
It is a white solid ionic compound consisting of sodium cations Na + and hydroxide anions OH −. Sodium hydroxide is a highly caustic base and alkali that decomposes proteins at ordinary ambient temperatures and may cause severe chemical is highly soluble in water, and readily E number: E (acidity regulators, ).
Carbon dioxide, CO 2, is a colourless and odorless gas. It is relatively nontoxic and noncombustible, but it is heavier than air and may asphyxiate by the displacement of air.
When CO 2 is solved in water, the mild carbonic acid, is CO 2 in solid form is called dry ice. Carbon dioxide phase diagram. ri / low-temperature heat capacities and enthalpy of formation of aluminum sulfide (al2s3), pb, $ 10 ri / fluorine recovery from phosphate rock concentrates, pb, $ 10 ri / studies of incipient combustion and its detection, pb, $ 28 ri / casting titanium and.
where Cp is the molar heat capacity; a, b, and c, are constants; and T is the temperature in degrees Kelvin. Table 3 shows the speciﬁc heat capacity of solids as a function of temperature, the speciﬁc heat capacity of liquids at the melt-ing point (T m), and the enthalpy of fusion for most common elements found in cast metals.
Changes in.Standard enthalpy of formation of smithite, AgAsSr, from the elements The standard enthalpy of formation of smithite was obtained by determining the heat efects associated with consecutive drops of the same sample (i.e., sample + silica container) from room temperature into the calorim-eter.
In the first drop, /o reaction occurs between theAuthor: O. J. Kr.Osborne and others provides the best reference heat capacities for copper.
Between T = 30 and K, our observed heat capacities differ from the reference values by less than % (generally less than %), except at about T = 60 K where one value differs by .