Gibbs phase rule: Difference between revisions
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[[File:Water phase diagram.svg|thumb|Water phase diagram]] | [[File:Water phase diagram.svg|thumb|Water phase diagram]] | ||
'''A dispersion system''' is a system containing at least two phases or two components (one – the proportion is dispersed in the other – the environment). A two-phase dispersion system is '''heterogeneous''' because there are clear boundaries between the dispersion fractions in the dispersion medium. Conversely, a system consisting of two components in one phase is '''homogeneous''' (sugar dissolved in water) and its components are not optically distinguishable. | '''A [[Dispersion systems|dispersion system]]''' is a system containing at least two phases or two components (one – the proportion is dispersed in the other – the environment). A two-phase dispersion system is '''heterogeneous''' because there are clear boundaries between the dispersion fractions in the dispersion medium. Conversely, a system consisting of two components in one phase is '''homogeneous''' (sugar dissolved in water) and its components are not optically distinguishable. | ||
'''Gibbs phase rule: f + v = s + 2''' | '''Gibbs phase rule: f + v = s + 2''' | ||
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===Reference=== | ===Reference=== | ||
</noinclude>[[Category:Thermodynamics]] [[Category:Biochemistry]]<references /> | </noinclude> | ||
[[Category:Thermodynamics]] [[Category:Biochemistry]]<references /> | |||
Latest revision as of 22:37, 22 December 2022
A dispersion system is a system containing at least two phases or two components (one – the proportion is dispersed in the other – the environment). A two-phase dispersion system is heterogeneous because there are clear boundaries between the dispersion fractions in the dispersion medium. Conversely, a system consisting of two components in one phase is homogeneous (sugar dissolved in water) and its components are not optically distinguishable.
Gibbs phase rule: f + v = s + 2
- s = number of components of the system, f = number of phases of the system, v = degrees of freedom (temperature, pressure)
- The liquid and its vapor (s = 1, f = 2) have one degree of freedom - only the pressure or only the temperature can be changed.
- If we want to change both temperature and pressure, there can only be one phase.
- If phase three is to be maintained in equilibrium, it will only happen at a given temperature and pressure (v = 0) – at the so-called triple point.
- For water, the triple point is 273.16 K[1] (0,01 °C) at a pressure of 610.6 Pa
Links[edit | edit source]
Source[edit | edit source]
- KUBATOVA, Senta. Biofot [online]. [cit. 2011-01-31]. <https://uloz.to/!CM6zAi6z/biofot-doc>.
