Particle composition and heat capacity of high-temperature SF6present at constant volume: Discussion on formula expressing relationship between constant-pressure and constant-volume heat capacities

2015 ◽  
Vol 10 (6) ◽  
pp. 683-688
Author(s):  
Yasunobu Yokomizu ◽  
Takanori Kobayashi ◽  
Toshiro Matsumura
Keyword(s):  
Heat Capacity ◽  
High Temperature ◽  
Constant Pressure ◽  
Heat Capacities ◽  
Constant Volume ◽  
Particle Composition ◽  
Volume Heat

scholarly journals The constant-volume heat capacities of gaseous perfluorocyclobutane and propylene

AIChE Journal ◽  
1960 ◽  
Vol 6 (1) ◽  
pp. 43-49 ◽  
Author(s):  
Noel De Nevers ◽  
Joseph J. Martin
Keyword(s):  
Heat Capacities ◽  
Constant Volume ◽  
Volume Heat

Verification of the calculation of the constant-volume heat capacity difference of substances in the liquid and gas phases from the temperature dependence of heat of vaporization

1983 ◽  
Vol 48 (8) ◽  
pp. 2141-2146
Author(s):  
Věra Uchytilová ◽  
Václav Svoboda
Keyword(s):  
Heat Capacity ◽  
Temperature Dependence ◽  
Constant Volume ◽  
Heat Of Vaporization ◽  
Gas Phases ◽  
Volume Heat ◽  
Pure Substances ◽  
The Difference ◽  
Heats Of Vaporization ◽  
The Ideal

The possibilities were verified of the proposed method for calculating the difference between constant-volume heat capacities of liquids and gases in the ideal state from known data on the volumetric behaviour and temperature dependence of heats of vaporization of pure substances.

FALSIFICATIONS OF POISSON ADIABATE, HUGONIO ADIABATE, LAPLACE SOUND SPEEDS. MODERNIZATION OF FOUNDATIONS OF THERMODYNAMICS

2020 ◽  
Vol 5 (333) ◽  
pp. 58-67
Author(s):  
K.B. Jakupov ◽  
Keyword(s):  
Shock Wave ◽  
Heat Capacity ◽  
Specific Heat ◽  
Specific Heat Capacity ◽  
Speed Of Sound ◽  
Constant Pressure ◽  
Energy Balance Equation ◽  
Ideal Gas ◽  
Constant Volume ◽  
Capacity Coefficient

The inequality of the universal gas constant of the difference in the heat capacity of a gas at constant pressure with the heat capacity of a gas at a constant volume is proved. The falsifications of using the heat capacity of a gas at constant pressure, false enthalpy, Poisson adiabat, Laplace sound speed, Hugoniot adiabat, based on the use of the false equality of the universal gas constant difference in the heat capacity of a gas at constant pressure with the heat capacity of a gas at a constant volume, have been established. The dependence of pressure on temperature in an adiabatic gas with heat capacity at constant volume has been established. On the basis of the heat capacity of a gas at a constant volume, new formulas are derived: the adiabats of an ideal gas, the speed of sound, and the adiabats on a shock wave. The variability of pressure in the field of gravity is proved and it is indicated that the use of the specific coefficient of ideal gas at constant pressure in gas-dynamic formulas is pointless. It is shown that the false “basic formula of thermodynamics” implies the falseness of the equation with the specific heat capacity at constant pressure. New formulas are given for the adiabat of an ideal gas, adiabat on a shock wave, and the speed of sound, which, in principle, do not contain the coefficient of the specific heat capacity of a gas at constant pressure. It is shown that the well-known equation of heat conductivity with the gas heat capacity coefficient at constant pressure contradicts the basic energy balance equation with the gas heat capacity coefficient at constant volume.

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 .

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