The reducing agent is the element that gets oxidized. Therefore, Zn(s) is the correct choice. It goes from 0 charge to 2+
Zn(s) is the reducing agent in the redox reaction below.
[tex]Zn(s)+Fe^{+2}(aq)\to \ Zn^{+2}(aq)+Fe(s)[/tex]
A reducing agent (also known as a reductant, reducer, or electron donor) is a chemical species that "donates" an electron to an electron recipient (called the oxidizing agent, oxidant, oxidizer, or electron acceptor).
In this reaction,
[tex]Zn(s)+Fe^{+2}(aq)\to \ Zn^{+2}(aq)+Fe(s)[/tex]
Zn gets oxidized 0 charges to 2+ and [tex]Fe^{+2}[/tex] is getting reduced. So, Zn is the reducing agent.
Hence, Zn(s) is the reducing agent.
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