In: Chemistry
Gibbs phase rule applies to non-reactive multi-component heterogeneous systems in thermodynamic equilibrium.
The phase rule is given as:
F= C-P+2
F= Intensive degrees of freedom i.e. the number of intensive variables that can be changed independently without disturbing the number of phases in equilibrium
P= number of phases i.e. gas, homogeneous liquid phases, homogeneous solid phases
C= components i.e. minimum number of independent constituents
For a glass of liquid water,
F= 2 since, temperature and pressure are independant variables.
i.e. F= C-P+2
C=1, P=1
F= 1 -1 +2 =2
For a glass of boiling water in equilibrium with saturated steam.
F= C-P+2 = 1-2+2= 1
In this case, one of the independent intensive variables i.e. pressure is defined, for eg. 1 atm. At this pressure, the temperature has to be 100 degrees for water to boil. So, temperature cannot be chosen independently of pressure when iquid and vapor are present.
Vapor, solid and liquid state of water
At the triple point; vapor, liquid and solid states coexist. The triple point occurs only at one specific pair of temperature and pressure for any given substance. Once the triple point is stated, its values can be obtained from a graph. So, thermodynamic properties cannot be chosen independently.
i.e. F= C-P+2 = 1-3+2 = 0
Solid forms of SO2
F= 2, since it is given that temperature and pressure can be varied to any desired value
P=1
From phase rule,
F= C-P+2 i.e. C= F+P-2
So, C= 2+1-2=1
Solid and liquid SO2 exist.
C= 2 +2-2= 2
Vapour and solid SO2 exist.
C= 2+2-2= 2
Vapour and solid SO2 exist.
C= 2+2-2= 2
Solid SO2 coexit with vapour and liquid.
C= 2+3-2= 3