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Question 12.10.1: Apply the Gibbs equilibrium phase rule to the oxidation of C...

Apply the Gibbs equilibrium phase rule to the oxidation of Cu to form cuprous oxide (Figure 12.1).

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4Cu_{(s)}+O_{2_{(g)}}=2Cu_2O_{(s)}

We use the equation

Φ + F = (C – r) + 2

where:
Φ  is the number of phases in equilibrium
F  is the thermodynamic degrees of freedom
C  is the number of components
r  is the number of chemical reactions needed to specify equilibrium
2  accounts for the intensive variables pressure and temperature

For this case:
r  = 1
Φ  = 3 (2 solids and one gaseous)
3  + F = (3– 1) + 2 or F = 1

We can see from Figure 12.1 that when the temperature is specified, there is only one possible partial pressure of oxygen gas that allows for the equilibrium of the given reaction. Or, if a specific partial pressure is desired, it can be found at but one temperature.

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