Lecture

Thermodynamics: Understanding State Variables and Functions

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In course

PHYS-106(i): General physics : thermodynamics

Le but du cours de Physique générale est de donner à l'étudiant les notions de base nécessaires à la compréhension des phénomènes physiques. L'objectif est atteint lorsque l'étudiant est capable de prévoir quantitativement les conséquences de ces phénomène ...

Description

This lecture provides an overview of thermodynamic systems, focusing on state variables and state functions. The instructor begins by defining what constitutes a thermodynamic system and its environment, emphasizing the importance of understanding the types of exchanges that can occur. Three types of systems are introduced: open, closed, and isolated, each characterized by their ability to exchange matter and energy with their surroundings. The lecture then delves into state variables, distinguishing between intensive and extensive variables, and explaining their significance in defining the state of a system. The instructor discusses the ideal gas equation and its implications, illustrating how pressure, volume, and temperature are interrelated. The concept of state functions is also introduced, highlighting their independence from the path taken during a transformation. The lecture concludes with practical examples, including Boyle's Law and Charles' Law, demonstrating how these principles apply to real-world scenarios in thermodynamics.

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Ontological neighbourhood

Physics

Thermodynamics: Statistical mechanics

Related concepts (32)

Non-equilibrium thermodynamics

Non-equilibrium thermodynamics is a branch of thermodynamics that deals with physical systems that are not in thermodynamic equilibrium but can be described in terms of macroscopic quantities (non-equilibrium state variables) that represent an extrapolation of the variables used to specify the system in thermodynamic equilibrium. Non-equilibrium thermodynamics is concerned with transport processes and with the rates of chemical reactions.

Closed system

A closed system is a natural physical system that does not allow transfer of matter in or out of the system, although - in the contexts of physics, chemistry, engineering, etc. - the transfer of energy (e.g. as work or heat) is allowed. In nonrelativistic classical mechanics, a closed system is a physical system that doesn't exchange any matter with its surroundings, and isn't subject to any net force whose source is external to the system. A closed system in classical mechanics would be equivalent to an isolated system in thermodynamics.

Chemical thermodynamics

Chemical thermodynamics is the study of the interrelation of heat and work with chemical reactions or with physical changes of state within the confines of the laws of thermodynamics. Chemical thermodynamics involves not only laboratory measurements of various thermodynamic properties, but also the application of mathematical methods to the study of chemical questions and the spontaneity of processes. The structure of chemical thermodynamics is based on the first two laws of thermodynamics.

Intensive and extensive properties

Physical properties of materials and systems can often be categorized as being either intensive or extensive, according to how the property changes when the size (or extent) of the system changes. According to IUPAC, an intensive quantity is one whose magnitude is independent of the size of the system, whereas an extensive quantity is one whose magnitude is additive for subsystems. The terms "intensive and extensive quantities" were introduced into physics by German writer Georg Helm in 1898, and by American physicist and chemist Richard C.

Thermodynamics

Thermodynamics is a branch of physics that deals with heat, work, and temperature, and their relation to energy, entropy, and the physical properties of matter and radiation. The behavior of these quantities is governed by the four laws of thermodynamics which convey a quantitative description using measurable macroscopic physical quantities, but may be explained in terms of microscopic constituents by statistical mechanics.

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