The heat capacities of certain liquids

1957 ◽  
Vol 239 (1217) ◽  
pp. 230-246 ◽  
Keyword(s):  
Heat Capacity ◽  
Carbon Tetrachloride ◽  
Carbon Disulphide ◽  
Heat Capacities ◽  
Constant Volume ◽  
Pressure Data ◽  
Different Temperatures ◽  
Structural Contribution ◽  
Liquid Heat ◽  
Total Heat Capacity

The heat capacities and adiabatic compressibilities of carbon tetrachloride, chloroform, methylene dibromide and m ethyl iodide have been measured between about — 30 and 30° C. The heat capacities at constant volume have been derived, and it is emphasized th a t these quantities apply to particular volumes existing at different temperatures. An isotherm for liquids, based on high-pressure data, has been used to obtain an expression for the effect of change of volume on the heat capacity at constant volume. This relation has been applied to mercury, carbon disulphide, carbon tetrachloride, chloroform and water. Satisfactory agreement has been obtained with the results found in other ways by Bridgman (1911, 1912) on mercury and water and by Gibson & Loeffler (1941) on carbon tetrachloride and water. From the results found in this work on the resolution of the various energy contributions to the liquid heat capacities of polyatomic molecules other than water, it is concluded that the concept of molecular rotation about a preferred axis can explain most of the facts established. There remains, however, a structural contribution to the total heat capacity which is approximately R cal mole -1 deg. -1 .

The heat capacities of acetone, methyl iodide and mixtures thereof in the liquid state

1962 ◽  
Vol 267 (1330) ◽  
pp. 384-394 ◽  
Keyword(s):  
Heat Capacity ◽  
Methyl Iodide ◽  
Atmospheric Pressure ◽  
Excess Heat Capacity ◽  
Liquid Mixtures ◽  
Heat Capacities ◽  
Constant Volume ◽  
Isothermal Compression ◽  
Compound Formation ◽  
Total Heat Capacity

The heat capacities of liquid mixtures of acetone and methyl iodide of various compositions have been determined at atmospheric pressure in the temperature range — 20 to 35 °C. The corresponding compressibilities have also been measured, and the heat capacities at constant volume determined as functions of the temperature and volume. The heat capacities increase on isothermal compression, and with rising temperature at constant volume. Resolution of the total heat capacity into its many components shows that the configurational contribution to the heat capacity at the melting point is R cal mole -1 deg -1 for methyl iodide and about 2 R cal mole -1 deg -1 for acetone. The excess heat capacity at constant volume over that estimated on an additivity basis is small, and rises with a rise in temperature to about 3 % of the total value a t 35 °C. A comparison of the present data with those relating to the acetone + chloroform system indicates that compound formation is less likely in the acetone + methyl iodide system .

scholarly journals Saturated-liquid heat capacity: New polynomial models and review of the literature experimental data

2003 ◽  
Vol 68 (6) ◽  
pp. 479-495 ◽  
Author(s):  
Jovan Jovanovic ◽  
Dusan Grozdanic
Keyword(s):  
Experimental Data ◽  
Heat Capacity ◽  
Heat Capacities ◽  
Review Of The Literature ◽  
Saturated Liquid ◽  
Correlation Models ◽  
Polynomial Models ◽  
Liquid Heat

In this paper a review of selected literature experimental data for saturated-liquid heat capacities was presented. Two-, three- and four-parameter polynomial correlation models are tested on those data. Obtained results lead to the conclusion that correlation quality depends on the number of parameters, and slightly on the type of models. The best two three- and four-parameter models were proposed.

Saturated and compressed liquid heat capacity at constant volume for 1-hexyl-3-methylimidazolium bis[(trifluoromethyl)sulfonyl]imide)

2014 ◽  
Vol 52 (5) ◽  
pp. 657-679 ◽  
Author(s):  
N.G. Polikhronidi ◽  
R.G. Batyrova ◽  
I.M. Abdulagatov ◽  
J.W. Magee ◽  
J.T. Wu
Keyword(s):  
Heat Capacity ◽  
Constant Volume ◽  
Compressed Liquid ◽  
Liquid Heat

Heat capacities and enthalpies of fusion and transformation for solvates of some salts with dimethyl sulfoxide and dimethylformamide

1988 ◽  
Vol 53 (12) ◽  
pp. 3072-3079
Author(s):  
Mojmír Skokánek ◽  
Ivo Sláma
Keyword(s):  
Heat Capacity ◽  
Phase Transformation ◽  
Phase Transformations ◽  
Dimethyl Sulfoxide ◽  
Liquidus Temperature ◽  
Molar Heat Capacity ◽  
Solid Phase ◽  
Zinc Nitrate ◽  
Heat Capacities ◽  
Liquid Phases

Molar heat capacities and molar enthalpies of fusion of the solvates Zn(NO3)2 . 2·24 DMSO, Zn(NO3)2 . 8·11 DMSO, Zn(NO3)2 . 6 DMSO, NaNO3 . 2·85 DMSO, and AgNO3 . DMF, where DMSO is dimethyl sulfoxide and DMF is dimethylformamide, have been determined over the temperature range 240 to 400 K. Endothermic peaks found for the zinc nitrate solvates below the liquidus temperature have been ascribed to solid phase transformations. The molar enthalpies of the solid phase transformations are close to 5 kJ mol-1 for all zinc nitrate solvates investigated. The dependence of the molar heat capacity on the temperature outside the phase transformation region can be described by a linear equation for both the solid and liquid phases.

Liquid heat capacity of the solvent system (piperazine+n-methyldiethanolamine+water)

2010 ◽  
Vol 42 (1) ◽  
pp. 54-59 ◽  
Author(s):  
Yu-Ru Chen ◽  
Alvin R. Caparanga ◽  
Allan N. Soriano ◽  
Meng-Hui Li
Keyword(s):  
Heat Capacity ◽  
Solvent System ◽  
Liquid Heat

Effects of pressure and temperature on the structure of liquid acetone

1967 ◽  
Vol 45 (2) ◽  
pp. 123-130 ◽  
Author(s):  
W. A. Adams ◽  
K. J. Laidler
Keyword(s):  
Heat Capacity ◽  
Internal Pressure ◽  
Structural Changes ◽  
Constant Volume ◽  
Tait Equation ◽  
Liquid Acetone ◽  
Structure Of Liquid

The compressibility of acetone has been redetermined at temperatures of 25 to 55 °C, and at pressures from atmospheric to 1 kbar. The results have been fitted to the Tait equation, and values of (∂P/∂T)V and of the internal pressure have been calculated. The heat capacity at constant volume has also been deduced as a function of pressure and temperature. The variations in these and other derived quantities have been shown to lead to conclusions about structural changes in the liquid.

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