Question

What happens to an oxidizing agent during a redox reactions?

Answer 1

The oxidizing reagent is FORMALLY reduced.......

Explanation:

Redox reactions are conceived to occur on the basis of CONCEPTUAL electron transfer, and typically we write out separate redox processes.........

For oxidation of methane we could write...........

`stackrel(-IV)" CH"_4(g) +2H_2O rarrstackrel(+IV)"CO"_2(g)+"4H"^+ +8e^(-)` `(i)`

And for every oxidation, there must be a corresponding reduction; here of dioxygen gas to water..........

`stackrel(0)O_2(g) + 4H^+ +4e^(-)rarr2H_2stackrel(-II)O` `(ii)`

And this is the FORMAL reduction reaction. Oxygen decreases in oxidation number, and it has FORMALLY GAINED electrons.....

`stackrel(0)O_2+4e^(-) rarr 2stackrel(-II)O""^(2-)`

And add the two half equation together.......so that we eliminate the electrons: `(i) + 2xx(ii)`

`stackrel(0)CH_4(g) +2stackrel(0)O_2(g) rarrstackrel(+IV)"CO"_2(g)+2H_2O(g)`

Of course, I am making a meal of it here; I could simply follow the usual rigmarole and (i) balance the carbons, (ii) balance the hydrogens as water, and (iii) balance the oxygens.