The Thermodynamic Properties of 1,1-Dichloroethane: Heat Capacities from 14 to 294°K., Heats of Fusion and Vaporization, Vapor Pressure and Entropy of the Ideal Gas. The Barrier to Internal Rotation1

1956 ◽  
Vol 78 (6) ◽  
pp. 1077-1080 ◽  
Author(s):  
James C. M. Li ◽  
Kenneth S. Pitzer
Keyword(s):  
Thermodynamic Properties ◽  
Vapor Pressure ◽  
Ideal Gas ◽  
Heat Capacities ◽  
The Ideal

Thermodynamic properties of three adamantanols in the ideal gas state

2003 ◽  
Vol 405 (1) ◽  
pp. 85-91 ◽  
Author(s):  
M.B Charapennikau ◽  
A.V Blokhin ◽  
G.J Kabo ◽  
V.M Sevruk ◽  
A.P Krasulin
Keyword(s):  
Thermodynamic Properties ◽  
Ideal Gas ◽  
The Ideal

Ideal gas processes – and two ideal gas case studies too

2018 ◽  
Author(s):  
Dennis Sherwood ◽  
Paul Dalby
Keyword(s):  
Case Studies ◽  
Constant Pressure ◽  
Ideal Gas ◽  
Heat Capacities ◽  
Carnot Cycle ◽  
State Function ◽  
Ideal Gases ◽  
First Case ◽  
The Ideal

This chapter brings together, and builds on, the results from previous chapters to provide a succinct, and comprehensive, summary of all key relationships relating to ideal gases, including the heat and work associated with isothermal, adiabatic, isochoric and isobaric changes, and the properties of an ideal gas’s heat capacities at constant volume and constant pressure. The chapter also has two ‘case studies’ which use the ideal gas equations in broader, and more real, contexts, so showing how the equations can be used to tackle, successfully, more extensive systems. The first ‘case study’ is the Carnot cycle, and so covers all the fundamentals required for the proof of the existence of entropy as a state function; the second ‘case study’ is the ‘thermodynamic pendulum’ – a system in which a piston in an enclosed cylinder oscillates to and fro like a pendulum under gravity, in both the absence, and presence, of friction.

Stereoisomerism and thermodynamic properties of propyl ethers in the ideal gas state

2019 ◽  
Vol 133 ◽  
pp. 292-299
Author(s):  
I.V. Garist ◽  
V.N. Emel'yanenko ◽  
K.U. Kavaliova ◽  
G.N. Roganov
Keyword(s):  
Thermodynamic Properties ◽  
Ideal Gas ◽  
The Ideal

Introduction to statistical thermodynamics of condensed matter

2005 ◽  
Author(s):  
Boris S. Bokstein ◽  
Mikhail I. Mendelev ◽  
David J. Srolovitz
Keyword(s):  
Thermodynamic Properties ◽  
Intermolecular Interactions ◽  
Disordered Systems ◽  
Condensed Matter ◽  
Thermodynamic Description ◽  
Statistical Thermodynamics ◽  
Ideal Gas ◽  
The Other ◽  
Particle Correlation ◽  
The Ideal

In this Chapter we apply statistical thermodynamics to condensed matter. We start with a description of the structure of liquids and the relation between this structure and its thermodynamic properties. Taking the low density limit, we derive a general equation of state appropriate for both liquids and gases. Next, we turn to a statistical thermodynamic description of solids. Finally, we consider the statistical theory of solutions. Recall that interactions between molecules in an ideal gas can be ignored for the purpose of determining thermodynamic properties. Therefore, we can assume that the spatial position of a molecule is independent of the positions of all of the other molecules in the gas. In real gases under high pressure and, even more so, in condensed matter, the intermolecular interactions play an important role and the positions of molecules are not independent. In other words, intermolecular interactions lead to the formation of correlations in the location of the molecules or, equivalently, to the development of structure. The energy of the system and the other thermodynamic properties depend on this structure. Therefore, we now turn to a discussion of structure. There are two distinct approaches to this problem. The first approach is designed for crystalline materials and is based upon a description of crystal symmetry. The description of this method is outside the scope of this text. The second is based upon the introduction of probability functions for atom locations and is applicable to disordered systems such as dense gases, liquids, and amorphous solids. Consider, as we are apt to do, the ideal gas. In this case, the probability of finding s molecules at points r1, r2, . . . , rs is simply In contrast with the ideal gas, the positions of molecules in high density gases or condensed matter are not independent of each other. Therefore, we write where Fs(r1, . . . , rs) is called the s-particle correlation function. Note three obvious properties of such functions. First, the system does not change when we exchange two molecules. This implies that the correlation functions should be symmetric with respect to their arguments.

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