The document introduces phase diagrams, which graphically represent the relationship between temperature, pressure, and composition of engineering materials and their properties. It classifies phase diagrams based on the number of components (unary, binary, tertiary, and quaternary) and discusses Gibbs's phase rule, which calculates the coexistence of phases in equilibrium systems. The content includes details on how to interpret unary phase diagrams for one-component systems, highlighting equilibrium conditions, phase boundaries, and critical points.

1. PHASE DIAGRAMS
INTRODUCTION
 Engineering materials are known by their set of properties.
 The properties depends to a large extent on microstructure and macrostructure.
 Macrostructure, it can be observed with the naked eye or maybe even upto 15 times magnification.
 The macrostructure gives information on the material’s grain size, shape and defects present like blow
holes.
 Microstructure, refers to the internal structure.
 It reveals the distribution of phases present in it, each of these phases have their own unique
properties, crystal structures.
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2.  The nature and occurrence of these phases depends on:
i. Temperature
ii. Pressure
iii. Composition
A PHASE DIAGRAM IS ESSENTIALLY A GRAPHICALLY REPRESENTATION OF AN ALLOY
DIAGRAMS ARE ALSO CALLED AS “EQUILIBRIUM DIAGRAMS” OR “CONSTITUTIONAL DIAGRAMS”.
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3. CLASSIFICATION OF PHASE DIAGRAMS
Based on the number of components in the system
 Unary phase diagrams - 1 component systems
 Binary phase diagrams - 2 component systems
 Tertiary phase diagrams - 3 component systems
 Ternary phase diagrams – 4 component systems
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4. GIBB’S PHASE RULE
 Josiah Willard Gibbs (1839–1903)
 Gibbs developed the phase rule in 1875–1876.
 This rule enables to compute the number of phases that can co-exist in equilibrium in a chosen
system.
n + C = F + P
Where P = Number of Phases
F = Number of degrees of freedom
C = Number of components in the system
n = Number of external factors used for the study
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5.  Degrees of Freedom, F: The number of degrees of freedom of a system is the number of
variables that can be changed independently without causing disappearance of phase.
 Components, C: The elements or compounds that constitute the alloy system.
Ex: Fe-Ni alloy system is a two component (binary) system
Cu-Ni-Zn in German Silver is a three component (tertiary) system
Al-Cu-Mn-Mg in Duralumin is a four component (ternary) system.
 Number of External Factors, n: It is simply an integral number which represents the number of
external factors like temperature and pressure used during construction (study) of phase
Generally n = 2.
So, the phase rule is written as 2+C = F+P
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6.  If the effect of pressure is ignored and assumed to be 1atm (as it remains constant), only temperature is
the external factor. So, n=1.
 The Phase Rule becomes P+F = C+1 (Modified Gibb’s Phase Rule)
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7. UNARY PHASE DIAGRAM (ONE COMPONENT SYSTEM)
 The simplest and easiest type of phase diagram to understand is that for a one-component system, in
which composition is held constant (i.e., the phase diagram is for a pure substance); this means that
pressure and temperature are the variables.
 This one-component phase diagram (or unary phase diagram) [sometimes also called a pressure–
temperature (or P–T) diagram] is represented as a two-dimensional plot of pressure (ordinate, or
vertical axis) versus temperature (abscissa, or horizontal axis).
 Illustration and demonstration of this phase diagram is done taking example of H₂O .
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8. MTE/III SEMESTER/MSE/MTE 2101 8
Pic Courtesy:
Material Science
and Engineering,
Callister

9. DESCRIPTION
 Three different phases—solid, liquid, and vapour—are delineated on the plot.
 Each of the phases will exist under equilibrium conditions over the temperature–pressure ranges of its
corresponding area.
 The three curves shown on the plot (labelled aO, bO, and cO) are phase boundaries; at any point on
of these curves, the two phases on either side of the curve are in equilibrium (or coexist) with one
another.
 That is, equilibrium between solid and vapour phases is along curve aO—likewise for the solid-liquid,
curve bO, and the liquid-vapour, curve cO.
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10.  Also, upon crossing a boundary (as temperature and/or pressure is altered), one phase transforms to
another.
 All three of the phase boundary curves intersect at a common point, which is labelled O (and for H₂O
system, at a temperature of 273.16 K and a pressure of 6.04×10⁻³atm).
 This means that at this point only, all of the solid, liquid, and vapour phases are simultaneously in
equilibrium with one another. This point is called as “Triple Point” or “Invariant Point”.
 Point c is called as “critical point”.
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11. APPLICATION OF GIBB’S PHASE RULE FOR A ONE-COMPONENT SYSTEM
 For one-component system, C = 1, n = 2 (pressure & temperature). Hence, the Gibb’s phase rule
becomes:
P + F = C + n
P + F = 1 + 2
 F = 3 – P
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12. Gibb’s phase rule applied to single-phase region (P = 1)
 Let a point “A” be marked in a single phase region.
 The temperature and pressure at ‘A’ are ‘TA’ & ‘PA’
respectively.
 Degrees of Freedom = 2 (as both temperature and
pressure can be varied without any change in the phase).
 Applying Gibb’s Phase Rule: F = 3 – P = 3 – 1 = 2
 Number of degrees of freedom = 2.
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Fig: Schematic unary phase diagram for magnesium,
showing the melting and boiling temperatures at one
atmosphere pressure. On this diagram, point X is the
triple point.
Pic courtesy: Science and Engineering of Materials, Donald Askeland, Pradeep Phule

13.  In the same way, Gibb’s phase rule can be applied to two phase region (Point B) and three phase
region (Point X) .
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