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13/02/2022 4:54 pm
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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.
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13/02/2022 5:02 pm
The above figure is a plot of Gibbs energy (ΔG⊖)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 (ΔfG⊖) of the oxide of the former is more negative than the latter. For example, since ΔfG⊖(Al, Al2,O3) is more negative than ΔfG⊖(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 ΔfG⊖(Mg, MgO) is more negative than ΔfG⊖(Zn, ZnO).