Question

What is the oxidizing agent in the following reaction?

Pb (s) + PbO2 (s) + 2SO4 ^2- (aq) +4H (aq) --> 2PbSO4 (s) + 2 H2O

a) Pb
b) PbO2
c) SO4^2-
d) H
e) PbSO4

Answer 1

The oxidizing agent in the given reaction is PbO2, as it is the species that gains electrons and gets reduced from Pb(IV) to Pb(II) in the product PbSO4.

Step-by-step explanation:

The oxidizing agent in the reaction Pb (s) + PbO2 (s) + 2SO42- (aq) +4H+ (aq) → 2PbSO4 (s) + 2 H2O is PbO2 (lead (IV) oxide). This is because PbO2 gains electrons (is reduced) during the reaction, changing from an oxidation state of +4 in PbO2 to +2 in PbSO4. The species that is reduced in a reaction is the oxidizing agent, as it accepts electrons from the species that gets oxidized. In this case, Pb (s) is oxidized as it loses two electrons, transforming from elemental lead (oxidation state 0) to lead (II) in PbSO4 (oxidation state +2).