5.8
The Phase Rule
The phase rule is the relationship between the variance, the number of components, and the number of phases at equilibrium for a system at any composition.
Here, the variance or number of degrees of freedom is the number of intensive variables that can be changed independently without altering the number of phases in equilibrium.
For example, in a single-component system, if only one phase is present, there are two degrees of freedom. This means that both pressure and temperature can be varied independently.
Suppose both solid and liquid phases are present at equilibrium. In that case, the degree of freedom equals one, suggesting that either pressure or temperature can be varied independently, allowing the other variable to adjust to maintain equilibrium. However, changing both pressure and temperature simultaneously would disturb the phase equilibrium.
When a system experiences equilibrium across its three phases, it has a variance value of zero, which implies that the system is invariant.
This exclusive state can only be achieved at a precise temperature and pressure distinct to the system, represented by the triple point.
The phase rule describes the relationship between the variance (degrees of freedom), the number of components, and the number of phases in a system at equilibrium.
Variance is a concept that denotes the number of independent intensive properties (properties are those that do not depend on the amount of material in the system), such as temperature, pressure, and composition, that can be altered without impacting the number of phases in equilibrium.
In a single-component system, such as pure water, if only one phase (e.g., liquid) is present, there are two degrees of freedom. This means that both pressure and temperature can be varied independently without altering the number of phases. Increasing the temperature or decreasing the pressure, for example, wouldn't necessarily cause the water to evaporate or freeze.
However, if both solid and liquid phases are present at equilibrium (for example, an ice-water mixture), the degree of freedom decreases to one. This means that either the pressure or the temperature can be varied independently, but not both, without changing the number of phases. If the temperature is raised while keeping the pressure constant, the ice will melt, altering the number of phases.
A system experiencing equilibrium across its three phases (solid, liquid, and gas), such as water existing as ice, liquid, and steam simultaneously, has a variance value of zero. This means the system is invariant or fixed, and neither temperature nor pressure can be altered independently without changing the number of phases. This unique state, known as the triple point, can only occur at a specific temperature and pressure unique to the system.
The phase rule is the relationship between the variance, the number of components, and the number of phases at equilibrium for a system at any composition.
Here, the variance or number of degrees of freedom is the number of intensive variables that can be changed independently without altering the number of phases in equilibrium.
For example, in a single-component system, if only one phase is present, there are two degrees of freedom. This means that both pressure and temperature can be varied independently.
Suppose both solid and liquid phases are present at equilibrium. In that case, the degree of freedom equals one, suggesting that either pressure or temperature can be varied independently, allowing the other variable to adjust to maintain equilibrium. However, changing both pressure and temperature simultaneously would disturb the phase equilibrium.
When a system experiences equilibrium across its three phases, it has a variance value of zero, which implies that the system is invariant.
This exclusive state can only be achieved at a precise temperature and pressure distinct to the system, represented by the triple point.
From Chapter 5:
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5.8 : The Phase Rule
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5.9 : Phase Diagram
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