Lecture

Phase Diagrams: Eutectic Type and Liquidus Slope

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In course

ME-212: Mechanical Design I: Manufacturing Processes

Application des principales catégories de procédés de production. Modèles physiques élémentaires décrivant le comportement des principaux procédés de production. Compréhension de base des aspects économiques des procédés de production. Méthodologie de ...

Description

This lecture covers the concept of phase diagrams, focusing on eutectic type phase diagrams and the liquidus slope. It explains how different concentrations of solute affect the phases present in a system, and how to determine the liquidus and solidus curves. The lecture also discusses the segregation coefficient, liquid and solid fractions, and the law of levers in equilibrium conditions. Additionally, it explores the construction of phase diagrams based on the minimization of Gibbs free energy. The indeterminacy of solid and liquid fractions at certain points is addressed, along with Scheil's law for estimating solute distribution during phase transitions.

Instructor

Eric Boillat

Contact Microcity Phone: 41 21 69 54456 Teaching & PhD Past EPFL PhD Students as codirector Serguei Kolossov, Cédric André, Jamasp Jhabvala, Christoph Van Gestel, Tatiana Polivnikova, Nikola Kalentics Courses Industrial production processes ME-212 Application windows of the main manufacturing process categories. Implementation of simple models describing the behavior of the main manufacturing processes. Basic understanding of the economic aspects of production processes. Manufacturing proc

Official source

Related concepts (32)

Phase diagram

A phase diagram in physical chemistry, engineering, mineralogy, and materials science is a type of chart used to show conditions (pressure, temperature, volume, etc.) at which thermodynamically distinct phases (such as solid, liquid or gaseous states) occur and coexist at equilibrium. Common components of a phase diagram are lines of equilibrium or phase boundaries, which refer to lines that mark conditions under which multiple phases can coexist at equilibrium. Phase transitions occur along lines of equilibrium.

Phase (matter)

In the physical sciences, a phase is a region of material that is chemically uniform, physically distinct, and (often) mechanically separable. In a system consisting of ice and water in a glass jar, the ice cubes are one phase, the water is a second phase, and the humid air is a third phase over the ice and water. The glass of the jar is another separate phase. (See .) More precisely, a phase is a region of space (a thermodynamic system), throughout which all physical properties of a material are essentially uniform.

Gibbs free energy

In thermodynamics, the Gibbs free energy (or Gibbs energy as the recommended name; symbol ) is a thermodynamic potential that can be used to calculate the maximum amount of work, other than pressure-volume work, that may be performed by a thermodynamically closed system at constant temperature and pressure. It also provides a necessary condition for processes such as chemical reactions that may occur under these conditions. The Gibbs free energy is expressed as where p is pressure, T is the temperature, U is the internal energy, V is volume, H is the enthalpy, and S is the entropy.

Phase transition

In chemistry, thermodynamics, and other related fields, a phase transition (or phase change) is the physical process of transition between one state of a medium and another. Commonly the term is used to refer to changes among the basic states of matter: solid, liquid, and gas, and in rare cases, plasma. A phase of a thermodynamic system and the states of matter have uniform physical properties. During a phase transition of a given medium, certain properties of the medium change as a result of the change of external conditions, such as temperature or pressure.

Thermodynamic free energy

In thermodynamics, the thermodynamic free energy is one of the state functions of a thermodynamic system (the others being internal energy, enthalpy, entropy, etc.). The change in the free energy is the maximum amount of work that the system can perform in a process at constant temperature, and its sign indicates whether the process is thermodynamically favorable or forbidden. Since free energy usually contains potential energy, it is not absolute but depends on the choice of a zero point.

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