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.

Explanation

Thermodynamic factors are helpful in choosing a suitable reducing agent for the reduction of a particular metal oxide to the metallic state as described below. Metals for which the standard free energy of formation `triangle_(f)G^(ɵ)` of their oxides is more negative can reduce those metal oxides for which the standard free energy of formation `triangle_(f)G^(ɵ)` of their respective oxides is less negative. in other words, any metal will reduce the oxides of other metals which lie above it in the ellingham diagram because the standard free energy change `triangle_(f)G^(ɵ)` of the combined redox reaction will `-ve` by an amound wqual to the difference in `triangle_(f)G^(ɵ)` by an amount equal to the difference in `triangle_(f)G^(ɵ)` of the two metal oxides. Thus both Al and Zn can reduce FeO to Fe but Fe cannot reduce `Al_2O_3` to Al an ZnO to Zn. Similarly, C can reduce ZnO to Zn but not CO.