Intensive property: defined

The electron affinity of an atom or ion is the counterpart of the ionisation potential. It is an intensive property, defined as the energy released when the atom in its ground state accepts an electron, i.e. the difference in energy between the ground state of E and that of E- with the sign convention that exothermic electron affinities are positive. Electron affinities, like ionisation potentials, are expressed in eV. 

According to EU purity criteria, color intensity is defined as the absorbance of a 0.1% (w/v) solution of caramel color solids in water in a 1 cm cell at 610 nm. The color intensity must be 0.01 to 0.12 for class I (E 150a), 0.05 to 0.13 for class II (E 150b), 0.08 to 0.36 for class III (E 150c), and 0.10 to 0.60 for class IV (E 150d). Ammonia caramels show the highest tinctorial power and are most commonly used as food colorants. Class I has the weakest coloring properties and is mostly used as flavor. 

The chemical potentials sought are intensive properties of the system, in the usual thermodynamic language [26]. Furthermore, AUa is a quantity of molecular order of magnitude. Specifically, the AUa defined by (9.13) should be system-size independent for typical configurations of thermodynamically large systems. Because of... 

We can express the use of all the different units in evolution in the language of thermodynamics. While the genome is defined by a DNA sequence so that each base has a singular intensive property as in a computer code of symbols, by way of contrast, the protein content of a cell is an extensive property being concentration dependent and therefore varies under circumstances such as temperature and pressure although... 

A phase is defined as a state of matter that is uniform throughout in terms of its chemical composition and physical state in other words, a phase may be considered a pure substance or a mixture of pure substances wherein intensive properties do not vary with position. Accordingly, a gaseous mixture is a single phase, and a mixture of completely miscible liquids yields a single hquid phase in contrast, a mixture of several solids remains as a system with multiple solid phases. A phase rule therefore states that, if a limited number of macroscopic properties is known, it is possible to predict additional properties. 

Properties such as internal energy, volume and entropy are called extensive because their values for a given phase are proportional to the mass or volume of the phase. The value of an extensive property of an entire system is the sum of the values of each of the constituent phases. The molar value of an extensive property is that for a properly defined gram-molecular weight or mole of material. The specific value of an extensive property is that per unit weight (eg, one gram of material). A property is called intensive if its value for a given phase is independent of the mass of the phase. Temp and pressure are examples of such intensive properties... 

The state of a system is defined by its properties. Extensive properties are proportional to the size of the system. Examples include volume, mass, internal energy, Gibbs energy, enthalpy, and entropy. Intensive properties, on the other hand, are independent of the size of the system. Examples include density (mass/volume), concentration (mass/volume), specific volume (volume/mass), temperature, and pressure. 

This shows that the natural variables of G for a one-phase nonreaction system are T, P, and n . The number of natural variables is not changed by a Legendre transform because conjugate variables are interchanged as natural variables. In contrast with the natural variables for U, the natural variables for G are two intensive properties and Ns extensive properties. These are generally much more convenient natural variables than S, V, and k j. Thus thermodynamic potentials can be defined to have the desired set of natural variables. 

Pressure, volume, temperature, and number of moles are thermodynamic properties or thermodynamic variables of a system—in this case, a gas sample. Their values are measured by experimenters using thermometers, pressure gauges, and other instruments located outside the system. The properties are of two types those that increase proportionally with the size of the system, such as n and K called extensive properties, and those defined for each small region in the system, such as P and T, called intensive properties. Terms that are added together or are on opposite sides of an equal sign must contain the same number of... 

The Gibbs phase rule allows /, the number of degrees of freedom of a system, to be determined. / is the number of intensive variables that can and must be specified to define the intensive state of a system at equilibrium. By intensive state is meant the properties of all phases in the system, but not the amounts of these phases. Phase equilibria are determined by chemical potentials, and chemical potentials are intensive properties, which are independent of the amount of the phase that is present. The overall concentration of a system consisting of several phases, however, is not a degree of freedom, because it depends on the amounts of the phases, as well as their concentration. In addition to the intensive variables, we are, in general, allowed to specify one extensive variable for each phase in the system, corresponding to the amount of that phase present. 

We have defined solutions as homogeneous phases, with uniform concentrations throughout. Clearly, the surface of a solution provides a different environment than its bulk, and we should expect intensive properties (concentrations as well as intensive thermodynamic properties) to vary in this region. The mechanical and thermal variables, P and T, however, can be taken as uniform throughout the solution. It should be emphasized that the surface region of the solution is very thin, just a few molecular diameters thick. Bulk properties of the solution will, thus, only be affected by the surface if the solution is composed of very small droplets. 

The dead state is defined by specifying the mass (material species), chemical composition, and two thermostatic properties. In this work, T and P are chosen as these two properties. Thus, the dead state for a specific system is fixed when the intensive properties (Tq,Pq,xa Q.Xg q...) are specified where A, B,. .. 

The pressure P and temperature T define the values at each point of the system and are therefore called intensive properties, some of which can be expressed as derivatives of extensive properties, such as the temperature... 

In nonequilibrium systems, the intensive properties of temperature, pressure, and chemical potential are not uniform. However, they all are defined locally in an elemental volume with a sufficient number of molecules for the principles of thermodynamics to be applicable. For example, in a region A , we can define the densities of thermodynamic properties such as energy and entropy at local temperature. The energy density, the entropy density, and the amount of matter are expressed by uk(T, Nk), s T, Nk), and Nk, respectively. The total energy U, the total entropy S, and the total number of moles N of the system are determined by the following volume integrals ... 

Density, an intensive property, is defined as mass per unit volume. It can be calculated by dividing the mass of a sample by its volume. If a density is given, it may be used as a factor to solve for mass or volume. Density, may be used to help identify a substance. Samples of lower density float in fluids of higher density. (Section 2.5)... 

An intensive property may be defined as a property that is unchanged when the size of the system is increased by adding to it any number of systems that are identical to the original system. An extensive property is one that increases in proportion to the size (for example, volume) of the system in such a process. Thus an intensive property may be formed from any extensive property through division by any other extensive property. 

Wyman (5,6,7) introduced the binding potential, which he represented by the Russian L for linkage. This is a molar thermodynamic property that is defined by a Legendre transform that introduces the chemical potential of the ligand as an independent intensive property. The binding potential is given by... 

The upper limit of the vapor pressure line is the point A. This is known as the critical point and the temperature and pressure represented by this point are the critical temperature To and the critical pressure Pc, respectively. At this point the intensive properties of the liquid phase and the vapor phase become identical and they are no longer distinguishable. For a single-component system the critical temperature may also be defined as the temperature above which a vapor cannot be liquefied, regardless of the applied pressure. Similarly, the critical pressme of a single-component system may be... 

Define or explain the following terms energy, system, closed system, nonflow system, open system, flow system, surroundings, property, extensive property, intensive property, state, heat, work, kinetic energy, potential energy, internal energy, enthalpy, initial state, final state, point (state) function, state variable, cyclical process, and path function. 

Define the following terms, and illustrate each with a specific example (a) matter (b) energy (c) mass (d) exothermic process (e) intensive property. 

Let L sys t) be an extensive property of the system at time t, ip r,t) is the corresponding intensive property. If Vsys t) denotes a system material volume at time t, CV a control volume, and CS the control volume surface, the extensive system property can be defined by ... 

On the other hand, many important properties of materials are intensive properties. The values of intensive properties are essentially independent of the amount of material present, provided of course that this amount is not zero. An intensive property can usually be expressed in terms of the quotient of a pair of extensive properties. For example, the density equals the molecular weight per repeat unit divided by the molar volume. The solubility parameter equals the square root of the cohesive energy density (defined as the cohesive energy divided by the molar volume). As shown in Chapter 1, the glass transition temperature (an intensive property) can often be estimated in terms of the molar glass transition function divided by the molecular weight of a repeat unit of the polymer. 

The twelve structural parameters defined above are all extensive variables. In order to convert them into intensive variables for use in the correlation for Tg, which is an intensive property, they will all be scaled by the number N of vertices in the hydrogen-suppressed graph of the repeat unit, as described by Equation 2.8 in Section 2.C. In other words, xj/N, x2/N,. .., x12/N, will be used as linear regression variables in the correlation for Tg. 

The thermal conductivity is an intensive property (Section 2.C). In other words, its value is independent of the size of the system being considered. Consequently, the intensive ( -type) connectivity indices, which are defined by Equation 2.8 as the corresponding extensive (X type) connectivity indices divided by the number N of vertices in the hydrogen-suppressed graph (i.e., =%/N), were used in the correlation for X(298K). 

Furthermore, in calculations performed manually instead of using software implementing our method, the calculation of the properties of many homopolymers with large repeat units can be simplified by treating them formally as alternating copolymers of smaller repeat units of polymers whose properties have already been calculated. Simple additivity is then assumed to hold for the extensive properties of the alternating copolymer, such as its connectivity indices, cohesive energy, and molar volume. All extensive properties can thus be calculated. Intensive properties, such as the solubility parameter, are defined in terms of extensive properties. Their prediction therefore does not require any detailed calculations either. 

The value of G(A) is equal to the work of thinning the film in a reversible, isobaric, and isothermal process from infinity to a finite thickness A, with TT(A) = —(dG/ dh)T pL ij vgi vs- Derjaguin et al. (1987) point out that the choice of 11(A) as the basic thermodynamic property is not a mere change of notation, but 11(A) has advantages in cases where Gibbs thermodynamic theory is not well defined, such as, when interfacial zones overlap to the extent that the film does not retain the intensive properties of the bulk phase. The use of the disjoining pressure is advantageous from an experimental point of view because of the relative ease to account for different contributions (e.g., electrostatic effects). 

All measurable properties of matter fall into one of two additional categories extensive properties and intensive properties. The measured value of an extensive property depends on how much matter is being considered. Mass, which is the quantity of matter in a given sample of a substance, is an extensive property. More matter means more mass. Values of the same extensive property can be added together. For example, two copper pennies will have a combined mass that is the sum of the masses of each penny, and the length of two tennis courts is the sum of the lengths of each tennis court. Volume, defined as length cubed, is another extensive property. The value of an extensive quantity depends on the amount of matter. 

The measured value of an intensive property does not depend on how much matter is being considered. Density, defined as the mass of an object divided by its volume, is an intensive property. So is temperature. Suppose that we have two beakers of water at the same temperature. If we combine them to make a single quantity of water in a larger beaker, the temperature of the larger quantity of water will be the same as it was in two separate beakers. Unlike mass, length, and volume, temperature and other intensive properties are not additive. 

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