Explanation:
8H+(aq) + MnO4-(aq) + 5Fe2+(aq) → Mn2+(aq) + 5Fe3+(aq) + 4H2O(l)
To determine if a substance was reduced or oxidized, the oxidation number at the reactant and product side is compared.
When oxidation occurs, an element loses electrons and its oxidation number increases (becomes more positive). When reduction occurs, an element gains electrons and its oxidation number decreases or is reduced (becomes more negative).
H+ (oxidized or reduced) Answer 1 Choose...
There is an increase in oxidation number from 0 to 1. This means H+ was oxidized.
MnO4- (oxidizing or reducing agent) Answer 2 Choose...
In chemistry, an oxidizing agent is a substance that has the ability to oxidize other substances — in other words to accept their electrons
MnO4- is a strong oxidizing agent.
Fe2+ (oxidizing or reducing agent) Answer 3 Choose...
A reducing agent means it will itself get oxidized. In this reaction, Fe2+ is the reducing agent.
Fe2+ (oxidized or reduced) Answer 4 Choose...
Oxidized
O in MnO4- (oxidized or reduced) Answer 5 Choose...
There is no change in oxidation number of , so it was neither reduced nor was it oxidized.
Mn in MnO4- (oxidized or reduced) Answer 6 Choose...
There is a decreaase in oxidation number from +7 to +2. This means reduction.
