GIBBS, JOSIAH WILLARD(Gibbs, Josiah Willard) (1839–1903), American physicist and mathematician. Born February 11, 1839 in New Haven (Connecticut). He graduated from Yale University, where his success in Greek, Latin and mathematics was awarded prizes and awards. In 1863 he received the degree of Doctor of Philosophy. He became a university teacher, teaching Latin for the first two years and only then mathematics. In 1866–1869 he continued his education at the Universities of Paris, Berlin and Heidelberg. After returning to New Haven, he headed the department of mathematical physics at Yale University and held it until the end of his life.
Gibbs presented his first work in the field of thermodynamics to the Connecticut Academy of Sciences in 1872. It was called Graphical methods in the thermodynamics of liquids (Graphical Methods in the Thermodynamics of Fluids) and was devoted to the method of entropy diagrams. The method made it possible to graphically represent all the thermodynamic properties of a substance and played a major role in technical thermodynamics. Gibbs developed his ideas into next job – Geometric representation methods thermodynamic properties substances using surfaces (Methods of Geometrical Representation of the Thermodynamic Properties of Substances by Means of Surfaces, 1873), introducing three-dimensional phase diagrams and obtaining the relationship between internal energy system, entropy and volume.
In 1874–1878 Gibbs published a treatise On the equilibrium of heterogeneous substances (On the Equilibrium of Heterogeneous Substances), whose ideas formed the basis of chemical thermodynamics. In it Gibbs outlined general theory thermodynamic equilibrium and the method of thermodynamic potentials, formulated the phase rule (now bearing his name), built a general theory of surface and electrochemical phenomena, derived a fundamental equation that establishes a connection between the internal energy of a thermodynamic system and thermodynamic potentials and allows one to determine the direction chemical reactions and equilibrium conditions for heterogeneous systems.
Gibbs's work on thermodynamics was almost unknown in Europe until 1892. One of the first to appreciate the importance of his graphical methods was J. Maxwell, who built several models of thermodynamic surfaces for water.
In the 1880s, Gibbs became interested in the work of W. Hamilton on quaternions and the algebraic work of G. Grassmann. Developing their ideas, I created a vector analysis in his modern form. In 1902 work Basic principles of statistical mechanics (Elementary Principles in Statistical Mechanics) Gibbs completed the creation of classical statistical physics. His name is associated with such concepts as “Gibbs paradox”, “canonical, microcanonical and grand canonical Gibbs distributions”, “Gibbs adsorption equation”, “Gibbs-Duhem equation”, etc.
Gibbs was elected a member of the American Academy of Arts and Sciences in Boston, a member of the Royal Society of London, and was awarded the Copley Medal and Rumford Medal. Gibbs died in New Haven on April 28, 1903.
GIBBS, Josiah Willard
American physicist and mathematician Josiah Willard Gibbs born in New Haven, Connecticut. He graduated from Yale University, where his achievements in Greek, Latin and mathematics were recognized with prizes and awards. In 1863, Gibbs received his Ph.D. and became a university professor; For the first two years he taught Latin and only then mathematics. In 1866–1869 Gibbs continued his education at the Sorbonne and Collège de France in Paris, and at the Universities of Berlin and Heidelberg. After returning to New Haven, he headed the department of mathematical physics at Yale University and held it until the end of his life.
Gibbs presented his first work in the field of thermodynamics to the Connecticut Academy of Sciences in 1872. It was called “Graphical Methods in the Thermodynamics of Liquids” and was devoted to the method of entropy diagrams. The method made it possible to graphically represent all the thermodynamic properties of a substance and played a major role in technical thermodynamics. Gibbs developed his ideas in his next work, “Methods for the geometric representation of the thermodynamic properties of substances by means of surfaces” (1873), introducing three-dimensional phase diagrams and obtaining the relationship between the internal energy of a system, entropy and volume.
In 1874–1878 Gibbs published a treatise “On the Equilibrium of Heterogeneous Substances,” the ideas of which formed the basis of chemical thermodynamics. In it, Gibbs outlined the general theory of thermodynamic equilibrium and the method of thermodynamic potentials, formulated the phase rule (now bearing his name), constructed a general theory of surface and electrochemical phenomena, generalized the principle of entropy, applying the second law of thermodynamics to a wide range of processes, and derived the fundamental equation establishing the connection between the internal energy of a thermodynamic system and thermodynamic potentials. The equations he obtained made it possible to determine the direction of chemical reactions and equilibrium conditions for mixtures of any complexity, as well as for heterogeneous systems.
Gibbs's work on thermodynamics was almost unknown in Europe until 1892. One of the first to appreciate the value of his graphical methods was James Clerk Maxwell, who constructed several models of thermodynamic surfaces for water.
In the 1880s, Gibbs became interested in the work of W. Hamilton on quaternions and the algebraic work of G. Grassmann. Developing their ideas, he created vector analysis in its modern form. In 1902, with the work “Basic Principles of Statistical Mechanics,” Gibbs completed the creation of classical statistical physics. His name is associated with such concepts as the “Gibbs paradox”, “canonical, microcanonical and grand canonical Gibbs distributions”, “Gibbs adsorption equation”, “Gibbs-Duhem equation”, etc. Gibbs’s works showed remarkably precise logic and thoroughness in finishing results. Not a single error has yet been discovered in his works; all his ideas have been preserved in modern science.
In 1880, Gibbs was elected to the American Academy of Arts and Sciences in Boston. Was also a member
Born on February 11, 1839 in New Haven (Connecticut) in the family of a famous philologist and professor of theology. He graduated from Yale University, where his success in Greek, Latin and mathematics were awarded prizes and awards. In 1863 he received the degree of Doctor of Philosophy. He became a university teacher, teaching Latin for the first two years and only then mathematics. In 1866–1869 he continued his education at the Universities of Paris, Berlin and Heidelberg, where he met the leading mathematicians of the time. Two years after returning to New Haven, he headed the department of mathematical physics at Yale University and held it until the end of his life.
Gibbs presented his first work in the field of thermodynamics to the Connecticut Academy of Sciences in 1872. It was called Graphical Methods in the Thermodynamics of Fluids and was devoted to the method of entropy diagrams developed by Gibbs. The method made it possible to graphically represent all the thermodynamic properties of a substance and played a major role in technical thermodynamics. Gibbs developed his ideas in the following work - Methods of Geometrical Representation of the Thermodynamic Properties of Substances by Means of Surfaces, 1873), introducing three-dimensional phase diagrams and obtaining the relationship between the internal energy of the system, entropy and volume.
In 1874–1878, Gibbs published a fundamental treatise on the equilibrium of heterogeneous substances (On the Equilibrium of Heterogeneous Substances), which became the basis of chemical thermodynamics. In it, he outlined the general theory of thermodynamic equilibrium and the method of thermodynamic potentials, formulated the phase rule (now bearing his name), constructed a general theory of surface and electrochemical phenomena, derived a fundamental equation that established the connection between the internal energy of a thermodynamic system and thermodynamic potentials and made it possible to determine the direction of chemical reactions and equilibrium conditions for heterogeneous systems. The theory of heterogeneous equilibrium - the most abstract of all Gibbs' theories - subsequently found wide practical application.
Gibbs's work on thermodynamics was little known in Europe until 1892. One of the first to appreciate the significance of his graphical methods was J. Maxwell, who built several models of thermodynamic surfaces for water.
In the 1880s, Gibbs became interested in the work of W. Hamilton on quaternions and the algebraic work of G. Grassmann. Developing their ideas, he created vector analysis in its modern form. In 1902, with the work Elementary Principles in Statistical Mechanics, Gibbs completed the creation of classical statistical physics. The statistical research methods he developed allow us to obtain thermodynamic functions, characterizing the state of systems. Gibbs gave a general theory of the magnitude of fluctuations of these functions from equilibrium values and a description of irreversibility physical processes. His name is associated with such concepts as “Gibbs paradox”, “canonical, microcanonical and large canonical Gibbs distributions”, “Gibbs adsorption equation”, “Gibbs-Duhem equation”, etc.
Gibbs was elected a member of the American Academy of Arts and Sciences in Boston, a member of the Royal Society of London, and was awarded the Copley Medal and Rumford Medal. Gibbs died at Yale on April 28, 1903.
Gibbs I
(Gibbs)
James (December 23, 1682, Footdismere, near Aberdeen, - August 5, 1754, London), English architect. He studied in Holland and Italy (in 1700-09 with C. Fontana (See Fontana)), collaborated with C. Ren. Representative of classicism. G.'s buildings are distinguished by their impressive simplicity and integrity of composition, elegance of detail (the churches of St. Mary-le-Strand, 1714-1717, and St. Martin-in-the-Fields, 1722-1726, in London; the Radcliffe Library in Oxford, 1737 -49).
Lit.: Summerson J., Architecture in Britain. 1530-1830, Harmondsworth, 1958. Josiah Willard (11.2.1839, New Haven, - 28.4.1903, ibid.), American theoretical physicist, one of the founders of thermodynamics and statistical mechanics. Graduated from Yale University (1858). In 1863 he received a Doctor of Philosophy degree from Yale University, and from 1871 he became a professor there. G. systematized thermodynamics and statistical mechanics, completing their theoretical construction. Already in his first articles, G. developed graphical methods for studying thermodynamic systems, introduced three-dimensional diagrams, and obtained relationships between the volume, energy, and entropy of matter. In 1874-78, in the treatise “On the Equilibrium of Heterogeneous Substances”, he developed the theory of thermodynamic potentials (See Thermodynamic potentials), proved the phase rule ( general condition equilibrium of heterogeneous systems), created thermodynamics surface phenomena and electrochemical processes; G. generalized the principle of entropy, applying the second law of thermodynamics to a wide range of processes, and derived fundamental equations that make it possible to determine the direction of reactions and equilibrium conditions for mixtures of any complexity. The theory of heterogeneous equilibrium, one of the most abstract theoretical contributions of G. to science, has found wide practical application. In 1902, “Basic principles of statistical mechanics, set forth with special application to the rational basis of thermodynamics” were published, which was the completion of classical statistical physics, the fundamental principles of which were laid in the works of J. TO. Maxwell and L. Boltzmann. Statistical method research developed by G. allows one to obtain thermodynamic functions characterizing the state of matter. G. gave a general theory of fluctuations of the values of these functions from equilibrium values determined by formal thermodynamics, and an adequate description of the irreversibility of physical phenomena. G. is also one of the creators of vector calculus in its modern form (“Elements of vector analysis”, 1881-1884). G.'s works showed a remarkably precise logic and thoroughness in finishing the results. Not a single error has yet been discovered in G.'s works; all his ideas have been preserved in modern science. Works: The collected works, v. 1-2, N. Y. - L., 1928; The scientific papers, v. 1-2, N.Y., 1906; in Russian lane - Basic principles of statistical mechanics, M. - L., 1946; Thermodynamic works, M., 1950. Lit.: Semenchenko V.K., D.V. Gibbs and his main works on thermodynamics and statistical mechanics (To the 50th anniversary of his death), “Advances in Chemistry”, 1953, vol. 22, century. 10; Frankfurt W. I., Frank A. M., Josiah Willard Gibbs, M., 1964. O. V. Kuznetsova.
Big Soviet encyclopedia. - M.: Soviet Encyclopedia. 1969-1978 .
See what "Gibbs" is in other dictionaries:
- (English Gibbs, sometimes Gibbes) English surname. Gibbs, Josiah Willard American physicist, mathematician and chemist, one of the founders of the theories of phenomenological and statistical thermodynamics, vector analysis, statistical ... ... Wikipedia
- (Gibbs) Josiah Willard (1839 1903), American physicist. One of the creators of statistical mechanics. Developed the general theory of thermodynamic equilibrium (including limited systems), the theory of thermodynamic potentials, derived the main... ... Modern encyclopedia
- (Gibbs) Joshua Willard (1839 1903), American theoretical scientist in the field of physics and chemistry. Professor at Yale University. Dedicated his life to developing the fundamentals physical chemistry. The application of THERMODYNAMICS in relation to physical processes has led... ... Scientific and technical encyclopedic dictionary
Gibbs- Gibbs, a: Gibbs distribution... Russian spelling dictionary
Gibbs D.W.- GIBBS Josiah Willard (18391903), Amer. theoretical physicist, one of the creators of thermodynamics and statistics. mechanics. Developed the theory of thermodynamics. potentials, discovered the general equilibrium condition for heterogeneous systems phase rule, derived the equation... ... Biographical Dictionary
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Books
- Woodworking Practical course, Gibbs N.. Wood is a magnificent material. Many craftsmen have special feelings for it not because of its beauty and strength, but rather because of the desire to tame this malleable and at the same time...
] Translation from English edited by V.K. Semenchenko.
(Moscow - Leningrad: Gostekhizdat, 1950. - Classics of natural science)
Scan: AAW, processing, Djv format: mor, 2010
- CONTENT:
Editor's Foreword (5).
Josiah Willard Gibbs, his life path and basic scientific works. V.K. Semenchenko (11).
Works by J.W. Gibbs (list) (24).
J.W. Gibbs
THERMODYNAMIC WORK
I. GRAPHICAL METHODS IN THE THERMODYNAMICS OF LIQUIDS
Values and ratios that will be presented in diagrams (29).
Main idea and general properties diagrams (31).
Entropy-temperature diagrams compared with diagrams commonly used (39).
Happening ideal gas (42).
The case of condensing vapors (45).
Diagrams in which isometric, isopiestic, isothermal, isodynamic and isentropic lines of an ideal gas are simultaneously straight lines (48).
Volume-entropy diagram (53).
Location of isometric, isopiestic, isothermal and isentropic lines around point (63).
II. METHOD OF GEOMETRICAL REPRESENTATION OF THERMODYNAMIC PROPERTIES OF SUBSTANCES USING SURFACES
Depiction of volume, entropy, energy, pressure and temperature (69).
The nature of that part of the surface that represents states that are not homogeneous (70).
Surface properties related to the stability of thermodynamic equilibrium (75).
Main features of the thermodynamic surface for substances in solid, liquid and vapor states (81).
Problems related to the dissipated energy surface (89).
III. ON THE EQUILIBRIUM OF HETEROGENEOUS SUBSTANCES
A preliminary note on the role of energy and entropy in the theory of thermodynamic systems (95).
CRITERIA FOR EQUILIBRIUM AND STABILITY
Suggested criteria (96).
Meaning of the term possible changes (98).
Passive resistances (98).
Legitimacy of criteria (99).
CONDITIONS FOR EQUILIBRIUM OF CONTACTING HETEROGENEOUS MASSES NOT SUBJECT TO. THE INFLUENCE OF GRAVITY, ELECTRIC FIELD, CHANGES IN THE SHAPE OF SOLID MASSES OR SURFACE TENSION
Statement of the problem (103).
Conditions of equilibrium between the initially existing homogeneous parts of a given mass (104).
Meaning of the term homogeneous (104).
Selection of substances considered as components. Actual and possible components (105).
Derivation of particular equilibrium conditions when all parts of the system have the same components (106).
Determination of potentials for the constituent parts of various homogeneous masses (107).
The case where some substances are only possible components in part of the system (107).
A type of particular equilibrium conditions when there are convertibility relations between substances that are considered as components of different masses (109).
Conditions relating to the possible formation of masses other than those originally present (112).
Very small masses cannot be treated in the same way as large masses (118).
The sense in which formula (52) can be considered as expressing the found conditions (119).
Condition (53) is always sufficient for equilibrium, but not always necessary (120).
A mass for which this condition is not satisfied is at least practically unstable (123).
(This condition is discussed later in the chapter “Stability”, see page 148)
Effect of solidification of any part of a given mass (124).
Influence of additional equations of imposed conditions (127).
Influence of the diaphragm (balance of osmotic forces) (128).
FUNDAMENTAL EQUATIONS
Definition and properties of fundamental equations (131).
About the quantities φ, y, e (135).
Expression of the equilibrium criterion through quantity (136).
Expressions of the equilibrium criterion in known cases using quantity (138).
POTENTIALS
The value of the potential for a substance of a given mass is independent of other substances that may be chosen to represent the composition of that mass (139).
The definition of potential that makes this property obvious (140).
We can distinguish in the same homogeneous mass the potentials for an indefinite number of substances, each of which has a very specific meaning. For potentials different substances of the same homogeneous mass, the equation is really the same as for units of these substances (140).
The potential values depend on arbitrary constants, which are determined by the determination of the energy and entropy of each elementary substance (143).
ABOUT THE EXISTING PHASES OF MATTER
Determination of phases and coexisting phases (143).
The number of independent changes possible in a system of coexisting phases (144).
Case of n + 1 coexisting phases (144).
The case when the number of coexisting phases is less than n + 1 (146).
INTERNAL STABILITY OF HOMOGENEOUS LIQUIDS ACCORDING TO FUNDAMENTAL EQUATIONS
General condition for absolute stability (148).
Other forms of this condition (152).
Stability with respect to continuous phase changes (154).
Conditions characterizing the boundaries of stability in this regard (163).
GEOMETRIC ILLUSTRATIONS
Surfaces on which the composition of the depicted bodies is constant (166).
Surfaces and curves for which the composition of the depicted body changes, but its temperature and pressure are constant (169).
CRITICAL PHASES
Definition (182).
The number of independent changes that the critical phase is capable of while remaining so (183).
Analytical expression of conditions characterizing critical phases. Position of critical phases relative to stability boundaries (183).
Changes that are possible under different circumstances for a mass that was originally a critical phase (185).
About the values of potentials when the amount of one of the components is very small (189).
ON SOME QUESTIONS RELATING TO THE MOLECULAR STRUCTURE OF BODIES
Proximate and primary components (192).
Phases of dissipated energy (195).
Catalysis is a perfect catalytic agent (196).
The fundamental equation for the phases of dissipated energy can be derived from more general view fundamental equation (196).
Dissipated energy phases may sometimes be the only phases whose existence can be determined experimentally (197).
EQUILIBRIUM CONDITIONS FOR HETEROGENEOUS MASSES UNDER THE INFLUENCE OF GRAVITY
This problem is treated in two different ways:
The volume element is treated as variable (199).
The volume element is treated as fixed (203).
FUNDAMENTAL EQUATIONS OF IDEAL GASES AND GAS MIXTURES
Ideal gas (206).
Ideal gas mixture. Dalton's Law (210).
Some conclusions related to the potentials of liquids and solids (223).
Considerations regarding the increase in entropy caused by diffusion when mixing gases (225).
Phases of dissipated energy of an ideal gas mixture, the components of which chemically interact with each other (228).
Gas mixtures with converting components (232).
The case of nitrous peroxide (236).
Fundamental equations for equilibrium phases (244).
SOLIDS
Conditions of internal and external equilibrium for solids in contact with liquids, in relation to all possible states of deformation of solids (247).
Deformations are expressed by nine derivatives (248).
Energy change in a solid element (248).
Derivation of equilibrium conditions (250).
Discussion of the condition relating to the dissolution of a solid (258).
Fundamental equations for solids (267).
Solids absorbing liquids (283).
CAPILLARITY THEORY
Surfaces of discontinuity between liquid masses
Preliminary remarks. Fracture surfaces. Separating surface (288).
Discussion of the problem. Particular equilibrium conditions for adjacent masses related to temperature and potentials, obtained earlier, do not lose their significance under the influence of the discontinuity surface. Surface energy and entropy. Surface densities of constituent substances. General expression for variation of energy surfaces. Equilibrium condition relating to pressures in adjacent masses (289).
Fundamental equations for discontinuity surfaces between liquid masses (300).
On the experimental determination of fundamental equations for discontinuity surfaces between liquid masses (303).
Fundamental equations for flat surfaces of discontinuity between liquid masses (305).
On the stability of discontinuity surfaces:
1) in relation to changes in the nature of the surface (310).
2) in relation to changes in which the shape of the surface changes (316).
On the possibility of the formation of a liquid of a different phase inside a homogeneous liquid (328).
On the possibility of formation at the surface where two different homogeneous liquids come into contact, a new liquid phase different from them (335).
Replacing potentials with pressures in the fundamental equations of surfaces (342).
Thermal and mechanical relationships related to the tensile strength of the fracture surface (348).
Impermeable films (354).
Internal equilibrium conditions for a system of heterogeneous liquid masses, taking into account the influence of discontinuity surfaces and gravitational force (356).
Conditions for stability (367).
On the possibility of the formation of a new discontinuity surface in the place where several discontinuity surfaces meet (369).
Conditions for stability of liquids with respect to the formation of a new phase at the line where three discontinuity surfaces meet (372).
Conditions for stability of liquids with respect to the formation of a new phase at the point where “the vertices of four different masses meet (381).
Liquid films (385).
Film element definition (385).
Each element can generally be considered as being in a state of equilibrium. The properties of an element in such a state and thick enough that its interior has the properties of a substance in bulk. Conditions under which stretching the film will not cause an increase in tension. If the film has more than one component that does not belong to adjacent masses, then stretching will, generally speaking, cause an increase in tension. The value of film elasticity derived from the fundamental equations of surfaces and masses. Observable elasticity (385).
The elasticity of the film does not vanish at the boundary at which its inner part loses the properties of a substance in the mass, but a certain kind of instability appears (390).
Application of equilibrium conditions already derived for a system subject to the influence of gravity (pp. 361-363) to the case of a liquid film (391).
Regarding the formation of liquid films and processes leading to their destruction. Black spots in films of soapy water (393).
TERMINAL SURFACES BETWEEN SOLIDS AND LIQUIDS
Preliminary remarks (400).
Equilibrium conditions for isotropic solids (403).
The influence of gravity (407).
Equilibrium conditions in the case of crystals (408).
The influence of gravity (411).
Restrictions (413).
Equilibrium conditions for a line in which three different masses occur, one of which is solid (414).
General relations (418).
Different method and different notation (418).
ELECTROMOTIVE FORCE
Changes in equilibrium conditions under the influence electromotive force (422).
Flow equation. Ions. Electrochemical equivalents (422).
Equilibrium conditions (423).
Four cases (425).
Lippmann electrometer (428).
Limitations caused by passive resistance (429).
General properties of a perfect electrochemical device (430).
Reversibility as a test of ideality. Determination of electromotive force from changes that occur in the cell. Modification of the formula for the case of a non-ideal device (430).
When the cell temperature is considered constant, the change in entropy caused by the absorption or release of heat cannot be neglected; proof of this for a Grove gas battery charged with hydrogen and nitrogen, by currents caused by differences in the concentrations of the electrolyte, and for electrodes of zinc and mercury in a solution of zinc sulfate (431).
That the same is true when they take place chemical processes in certain respects, is shown by reasoning a priori, based on the phenomenon occurring by the direct combination of the elements of water or the elements of hydrochloric acid and by the absorption of heat, which Favre has many times observed in galvanic or electrolytic cells (434).
The different physical states in which the ion is deposited do not affect the magnitude of the electromotive force if the phases are coexisting. Raoul's experiments (441).
Other formulas for electromotive force (446).
Editor's Notes (447).
From the editor's preface: The main thermodynamic works of Gibbs, the translation of which is given in this book, appeared in 1873-1878, but getting to know them is of not only historical interest for the modern reader...
