Answer:
C) Ce is getting reduced while Fe is getting oxidized
Step-by-step explanation:
Currently, redox reactions, or oxidation reduction, are considered to be those in which the state or degree of oxidation of the reactant species changes because there is an exchange of electrons between the reagents, although neither oxygen nor hydrogen intervenes in them.
For a redox reaction to occur, the presence of a species that yields electrons (reducer) and another species that accepts electrons (oxidant) are necessary. After the redox reaction, the reductant is transformed into its oxidized form and the oxidant into its reduced form:
Oxidant 1 + n e- = reduced form of oxidant 1 (reduction)
Reducer 2 + n e- = oxidized form of the reducer (oxidation)
Global reaction:
Oxidant 1 + Reducer 2 = Reducer 1 + Oxidant 2
The concept of redox reactions resembles that of Bronsted-Lowry acid base reactions. Both involve the transfer of one or more charged particles from a donor to an acceptor, these being the electrons in the redox and the protons in the neutralization
In this example, the parcial reactions are:
Ce+4 + e- ⇌ Ce+3 reduction of Ce+4
Fe+2 ⇌ Fe+3 + e- oxidation of Fe+2
Global reaction:
Fe+2 + Ce+4 --> Fe+3 + Ce+3