Podcast
Questions and Answers
Is the application of the principles of
thermodynamics to the study of
equilibrium relationships within or
between phases, corresponding to
homogeneous and heterogeneous
phase equilibria, respectively.
Is the application of the principles of thermodynamics to the study of equilibrium relationships within or between phases, corresponding to homogeneous and heterogeneous phase equilibria, respectively.
PHASE EQUILIBRIA
__________ in physics is a branch that deals with
heat, work and temperature, and their relation to energy,
radiation and physical properties of matter.
__________ in physics is a branch that deals with heat, work and temperature, and their relation to energy, radiation and physical properties of matter.
THERMODYNAMICS
It explains
how thermal energy is converted to or from other forms
of energy and how matter is affected by this process.
It explains how thermal energy is converted to or from other forms of energy and how matter is affected by this process.
THERMODYNAMICS
Is the term used to describe with two or more
phases co-exist
Is the term used to describe with two or more phases co-exist
The stability of phases can be predicted by the
__________, in that the most stable form of
the substance will have the __________ at the given &.
The stability of phases can be predicted by the __________, in that the most stable form of the substance will have the __________ at the given &.
A key tool in exploring phase equilibria is a _________ which is used to show conditions
at which thermodynamically distinct phases occur and coexist at
equilibrium.
A key tool in exploring phase equilibria is a _________ which is used to show conditions at which thermodynamically distinct phases occur and coexist at equilibrium.
The three primary phases of matter are
often defined individually under
different conditions but in most
systems, we usually encounter phases
in coexistence.
The three primary phases of matter are often defined individually under different conditions but in most systems, we usually encounter phases in coexistence.
[glass of ice water on a hot summer day, with a focus on the solid ice, liquid water, and gas phases.]
As the drink is exposed to warm air, the ice
melts, increasing the water level. However,
evaporation reduces the liquid volume as vapor
is released into the surrounding air.
[glass of ice water on a hot summer day, with a focus on the solid ice, liquid water, and gas phases.]
As the drink is exposed to warm air, the ice melts, increasing the water level. However, evaporation reduces the liquid volume as vapor is released into the surrounding air.
A series of independent
variables (e.g., temperature) and
their coexistence can only occur
over a limited range.
A series of independent variables (e.g., temperature) and their coexistence can only occur over a limited range.
[THE PHASE RULE] ice does not last
as long in boiling water as it
does in cold water. Therefore, to
understand and define the state
of each phase, knowledge of
several variables is required.
[THE PHASE RULE] ice does not last as long in boiling water as it does in cold water. Therefore, to understand and define the state of each phase, knowledge of several variables is required.
formulated the
phase rule.
formulated the phase rule.
Which is the relationship for
determining the least number of
intensive variables (temperature,
pressure, density, and
concentration) that can be
changed without changing the
equilibrium state of the system, or,
alternately, the least number is
required to define the state of the
system.
Which is the relationship for determining the least number of intensive variables (temperature, pressure, density, and concentration) that can be changed without changing the equilibrium state of the system, or, alternately, the least number is required to define the state of the system.
The following plot shows the _______ as a function of temperature,
including phase changes from solid to liquid (melting) and liquid to gas
(boiling).
The following plot shows the _______ as a function of temperature, including phase changes from solid to liquid (melting) and liquid to gas (boiling).
determines the least # of intensive variable that can be altered without affecting the equilibrium of the system
determines the least # of intensive variable that can be altered without affecting the equilibrium of the system
Formula for 1 component system
Formula for 1 component system
Formula for 2 component system
Formula for 2 component system
Formula for 3 component system
Formula for 3 component system
Maximum number of intensive variables that can be varied independently while the system remains in an equilibrium state
Maximum number of intensive variables that can be varied independently while the system remains in an equilibrium state
The smallest number of constituents by which the phase of equilibrium system can be expressed as a chemical formula or equation
The smallest number of constituents by which the phase of equilibrium system can be expressed as a chemical formula or equation
Homogenous physically distinct portion of the system by which is separated from other parts of the system by bounding surfaces
Homogenous physically distinct portion of the system by which is separated from other parts of the system by bounding surfaces
Phase diagrams are tools used by
engineers to analyze and solve
problems related to different
phases, including hydrates. They
provide rules for constructing
diagrams and reveal interesting
results, such as the fact that free-
water is not necessary for hydrate
formation and excess water can
actually inhibit it.
Phase diagrams are tools used by engineers to analyze and solve problems related to different phases, including hydrates. They provide rules for constructing diagrams and reveal interesting results, such as the fact that free- water is not necessary for hydrate formation and excess water can actually inhibit it.
summarizes the condition at
which a substance exists as a
solid, liquid, or gas.
where the relationships
between T, compositions, and
the quantities of phases
present at equilibrium are
represented.
summarizes the condition at which a substance exists as a solid, liquid, or gas. where the relationships between T, compositions, and the quantities of phases present at equilibrium are represented.
vapor pressure curve; where liquid and gas are in equilibrium.
vapor pressure curve; where liquid and gas are in equilibrium.
sublimation curve; where solid and gas are in equilibrium.
sublimation curve; where solid and gas are in equilibrium.
melting point curve; where solid and liquid are in equilibrium.
melting point curve; where solid and liquid are in equilibrium.
point where solid, liquid, and gas exist in equilibrium
point where solid, liquid, and gas exist in equilibrium
end point of phase equilibrium; highest point where a regular substance can exist.
end point of phase equilibrium; highest point where a regular substance can exist.
maximum temp at which 2 phase region exists
maximum temp at which 2 phase region exists
curve that separates two phase area from one phase.
curve that separates two phase area from one phase.
line drawn across the region of 2 phases or conjugate phases
line drawn across the region of 2 phases or conjugate phases
test tubes consisting of 2 phases
test tubes consisting of 2 phases
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Study Notes
Thermodynamics and Phase Equilibria
- Application of thermodynamics to study phase relationships includes homogeneous and heterogeneous equilibria.
- Thermodynamics examines the interactions of heat, work, temperature, energy, radiation, and physical properties of matter.
- Stability of phases is determined by their Gibbs free energy; the most stable phase has the lowest Gibbs free energy at given temperature and pressure.
Phase Diagrams and Tools
- A phase diagram visually represents conditions under which distinct phases coexist in equilibrium.
- The primary phases of matter include solid, liquid, and gas, and they can be present together in various systems.
- For example, a glass of ice water shows coexistence of solid ice, liquid water, and vapor as it interacts with warm air.
Changes in Phases
- As the ice melts in warm air, the water level rises, but evaporation decreases liquid volume.
- Phase coexistence is limited by independent variables such as temperature; e.g., ice melts slower in cold water than in boiling water.
Phase Rule
- The phase rule defines the least number of intensive variables (temperature, pressure, density, concentration) needed to characterize a system's equilibrium state.
- Formulated by Josiah Willard Gibbs, it indicates how variables can change without affecting equilibrium.
Phase Equilibrium Characteristics
- A phase diagram plots phase changes relative to temperature, including transitions such as melting and boiling.
- The maximum number of independent intensive variables varies while keeping the system in equilibrium.
- The smallest constituent number required to express a phase equilibrium system is represented as a chemical formula.
Types of Phase Relationships
- Vapor pressure curve: equilibrium between liquid and gas phases.
- Sublimation curve: equilibrium between solid and gas phases.
- Melting point curve: equilibrium between solid and liquid phases.
- The critical point indicates the highest temperature and pressure where distinct liquid and gas phases coexist.
Applications of Phase Diagrams
- Engineers use phase diagrams to analyze problems related to various phases, including hydrates.
- Diagrams reveal insights such as free-water not being required for hydrate formation and that excess water can inhibit it.
- The conditions for a substance to exist as a solid, liquid, or gas are detailed in phase diagrams, mapping the relationships between temperature, composition, and phase quantities.
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