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Question:

The choice of a reducing agent in a particular case depends on thermodynamic factor. How far do you agree with this statement? Support your opinion with two examples.

Answer:

 

The above figure is a plot of Gibbs energy ΔGø vs. T for formation of some oxides.

It can be observed from the above graph that a metal can reduce the oxide of other metals, if the standard free energy of formation ΔfGø of the oxide of the former is more negative than the latter. For example, since ΔfGø(Al,Al2,O3) is more negative than ΔfGø(Cu,Cu2,O) , Al can reduce Cu2O to Cu, but Cu cannot reduce Al2O3. Similarly, Mg can reduce ZnO to Zn, but Zn cannot reduce MgO because ΔfGø(Mg,MgO) is more negative thanΔfGø(Zn,ZnO) .


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