Heat capacity of gaseous

Calculate the molar heat capacity (see Problem 14.78) of each element in Table 14.4. What can you generalize about the molar heat capacities of gaseous elements and those of metallic elements ... 

The normal boiling point of liquid ammonia is 240 K the enthalpy of vaporization at that temperature is 23.4 kj mol . The heat capacity of gaseous ammonia at constant pressure is 38 J moC ... 

Estimate the heat capacity of gaseous isobutane at 1000 K and 200 mm Hg by using the Kothari-Doraiswamy relation... 

Taking the mean molar heat capacities of gaseous hydrogen, iodine and hydrogen iodide as 6.95, 8.02 and 7.14 cal. deg. , respectively, calculate the heat of formation of hydrogen iodide from the gaseous elements at 225 C. The heat of sublimation of solid iodine is 58.5 cal. g. at 25 C. 

For the heat capacities of gaseous paraffins and olefins, with more than three carbon atoms, Edmister (see ref. 9) suggested the empirical formula... 

The heat capacity of gaseous argon at constant pressure is 20.8 JK"1 mol 1. Estimate the entropy change when one mole of argon is heated from 300 K to 1200 K at 1 atm pressure. 

Figure 13.3 Specific heat capacity of gaseous HF as a function of temperature. (Data from Franck and Meyer [12].)...

In Figure 13.3, the unusual curvature of the specific heat capacity of gaseous HF as a function of temperature is shown with the pressure as a parameter. For P = 0, it is an almost constant function with Cp = dp 1.46J/(g/K). For finite pressures, there is a strong influence of the association reactions, and a peak is formed. For the curve on the left-hand side, the top of the peak is approx. 40 times larger than dp. With increasing pressure, the peak becomes less steep, and it is transferred to higher temperatures. The simple association model can reproduce this complicated shape quite well however, the agreement is not exact. 

When the product is gaseous (e.g. carbon forming carbon dioxide), the effect is due to the displacement of the matter of heat from the interstices between the oxygen particles by particles of carbon this is proved by the facts that the oxygen gas contracts by a tenth when carbon burns in it (in fact it does not contract at all), and that the heat capacity of gaseous fixed air (carbon dioxide) is less than that of an equal volume of oxygen gas (it is actually considerably greater). 

The heat (q) is the product of the amount (number of moles, n) of water, the molar heat capacity of gaseous water, Qj,ter( ) the temperature change during this step,... 

FIG. 17. Constant-pressure heat capacity of gaseous Freon-22 at elevated pressures. Experimental data 1, Ernst et al. [3.36, 3.40] 2, Gruzdev and Shumskaya [2.9]. Tabular data 3, [0.51] 4, Altunin and Gadetsky [3.1]. 

A review by Morsy [3.54] presents the experimental data by Huang about constant-volume heat capacity of gaseous Freon-22 in the temperature interval 323-473 K at pressures up to 3.4 MPa. Most probably, the investigation was carried out on the experimental apparatus built by Nevers and Martin and was used by them to determine of Freon-C318 and propylene at T = 330-420 K and p 160 kg/m. This work also indicates that the maximum error in could... 

Constant-pressure heat capacity of gaseous Freon-23 was measured in two studies (see Table 41). But numerical results are given only in a paper by V. A. Gruzdev and A. I. Shumskaya [2.9]. These researchers point out the good agreement of experimental values of Cp in the interval T = 300-360 K with the calculated values in Ref. [4.5]. The data by Barho [0.37] covering the heat capacity in the ideal gas state turned out to be high. The discrepancy exceeds the sum of experimental and calculation errors. In the present work, the initial values of thermodynamic functions in the ideal gas state are taken from the data in Ref. [1.39]. 

Coefficients to the linear frX,Us = C + SUp Second set of Coefficients Us = Cl + SI Up for Volumes less than MINV or VSW Heat Capacity of Condensed Component (cal/g/deg) Heat Capacity of Gaseous Component (cal/g/deg) Total Internal Energy (Mbar-cc/g)... 

There is no doubt that the very fundamental quantity for the description of the thermodynamic behavior of pure substances is the heat capacity at constant pressure, Cp. The molar heat capacity of gaseous substances increases steadily with molecular size, as more and more vibrational degrees of freedom become available to store energy. The heat capacities of liquids and solids are much larger than gas phase ones, as... 

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