Low-Temperature Heat Capacities and Entropies at 298.15 Degrees K. of Some Sodium
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Low-Temperature Heat Capacities and Entropies at 298.15 Degrees K. of Some Sodium and Calcium-Aluminum Silicates. by United States. Bureau of Mines.

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Published by s.n in S.l .
Written in English

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Edition Notes


SeriesReport of investigations (United States. Bureau of Mines) -- 5855
ContributionsKing, E., Weller, W.
ID Numbers
Open LibraryOL21743472M

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Abstract. This publication contains tables of recommended values for the standard enthalpies (heats) of formation, Gibbs (free) energies of formation, entropies, enthalpy contents and heat capacities at K, and enthalpies of formation at O K for compounds of uranium, protactinium, thorium, actinium, lithium, sodium, potassium, rubidium, cesium, and francium. ∆fH° Standard molar enthalpy (heat) of formation at K in kJ/mol ∆fG° Standard molar Gibbs energy of formation at K in kJ/mol S° Standard molar entropy at K in J/mol K Cp Molar heat capacity at constant pressure at K in J/mol K The standard state pressure is File Size: KB.   The heat capacity of azurite exhibits anomalous behavior at low temperatures. At K the molar heat capacities C 0 p and the third law entropies S 0 are ± and ± J mol −1 K −1 for azurite and ± and ± J mol −1 K −1 for by: King EG, Kelley KK () Low-temperature heat capacities of copper ferrites (with a summary of entropies at ° K of spinel minerals). US Bur Mines Rep Invest Koehler MF, Barany R, Kelley KK () Heats and free energies of formation of ferrites and aluminates of calcium, magnesium, sodium, and lithium.

Engel P) The standard entropy of Pb(s) at K is J K–1 mol– that the heat capacity of Pb(s) is given by n C P, m Pb, s J mol 1 K 1 T K 10 5 T2 K2 K The melting point is °C and the heat of fusion under these conditions is   At very low temperatures, heat capacity, C, is directly proportional to T3 for most substances. Find an expression for the absolute molar entropy, S, at a low temperature T, in terms of C.   The smoothed molar heat capacities and thermodynamic functions of the sample were calculated based on the fitted polynomial of the heat capacity as a function of the reduced temperature (X) according to the following thermodynamic equations: H (T) − H ( K) = ∫ K T C p, m d T S (T) − S ( K) = ∫ K T C p, m T.   ΔS = kJ / K = 5 kJ⋅K-1 The thing is, this is the correct answer, but I have no idea why you should know to use K as the temperature. It's not given in the question, and I would have thought that the above equation for ΔS could only be used in cases where the temperature remains constant, not like in this example where it.

Suppose we have moles of supercooled water turning into ice at C and bar. Calculate the values of ∆Ssys, ∆Ssurr, and ∆Suniv for this process. The molar heat capacities at constant pressure of ice and liquid water are constant, and have the values of J/(mol K) and J/(mol K), respectively. heat capacities of gibbsite, al(oh)//3, between 13 and k and magnesite, mgco//3, between 13 and k and their standard entropies at 5k, and the heat capacities of calorimetry conference. Standard enthalpies of formation at K of all three zeolites were determined by solution calorimetry. Thermodynamic functions have been calculated for natrolite to K and for scolecite to K. The heat capacity and standard entropy at K have been estimated for mesolite.   Molar entropies at T = K were calculated from low temperature heat capacity measurements. Furthermore, the results of calorimetric measurements of the enthalpies of drop-solution in a sodium oxide-molybdenum oxide melt for several stoichiometric mixed oxides in the above mentioned system are reported from which the values of enthalpy of.