In Sn4+ + 2Fe2+ _____ Sn2+ + 2Fe3+ equation the specie reduced is
a.
Fe2+
b.
both Sn4+ and Fe2+
c.
None of the above.
d.
Sn4+
d. Sn4+
To determine the species that is reduced in the equation Sn4+ + 2Fe2+ → Sn2+ + 2Fe3+, we need to understand the concept of reduction and oxidation in redox reactions.
In a redox reaction, reduction and oxidation occur simultaneously. Reduction is the gain of electrons by a species, while oxidation is the loss of electrons by a species. To identify the species that is reduced, we need to look for the one that gains electrons.
In the given equation, Sn4+ (tin in the +4 oxidation state) is on the reactant side and Sn2+ (tin in the +2 oxidation state) is on the product side. Since tin goes from a higher oxidation state (+4) to a lower oxidation state (+2), it gains electrons and is therefore reduced.
Fe2+ (iron in the +2 oxidation state) on the reactant side is being oxidized to Fe3+ (iron in the +3 oxidation state) on the product side. It loses electrons, which means it is being oxidized and not reduced.
Therefore, the specie that is reduced in the equation Sn4+ + 2Fe2+ → Sn2+ + 2Fe3+ is:
d. Sn4+
The specie reduced in the equation Sn4+ + 2Fe2+ → Sn2+ + 2Fe3+ is:
a. Fe2+