How would MnO_4^(-)MnO4, and SO_2(g)SO2(g) interact?

1 Answer
Mar 2, 2017

We would assume that the permanganate ion, which is a potent oxidant...............

Explanation:

We would assume that the permanganate ion, which is potent oxidant, oxidizes the SO_2(g)SO2(g) up to S(VI+)S(VI+). Let's assume such oxidation:

"Oxidation rxn (i):"Oxidation rxn (i):

SO_2(g) +2H_2O(l) rarr SO_4^(2-) +4H^+ + 2e^(-)SO2(g)+2H2O(l)SO24+4H++2e

"Reduction rxn (ii):"Reduction rxn (ii):

MnO_4^(-) +8H^(+) + 5e^(-) rarr Mn^(2+) +4H_2O MnO4+8H++5eMn2++4H2O

"Overall rxn:"Overall rxn: == 5xx(i)+2xx(ii)5×(i)+2×(ii) ==

2MnO_4^(-) + 5SO_2(g) +2H_2O(l) rarr 2Mn^(2+) +5SO_4^(2-) +4H^+ 2MnO4+5SO2(g)+2H2O(l)2Mn2++5SO24+4H+

I would recheck this question. They should give you a bit of context (I am guessing that you are an undergrad). Namely, that the reaction proceeds with the disappearance of the deep purple colour of permanganate to give the almost colourless Mn^(2+)Mn2+ ion. The redox equation is as far as I know stoichiometrically balanced; i.e. garbage out equals garbage in, including electronic charge.