Sn is the only form of tin that can act as a reducing agent.
Reduction: Sn²⁺ + 2e⁻ ⟶ Sn; E° = -0.15 V
The Sn²⁺ is being reduced, so it is acting as an oxidizing agent.
Oxidation: Sn ⟶ Sn²⁺ + 2e⁻; E° = +0.15 V
The Sn is being oxidized, so it is acting as a reducing agent.
Answer: The stronger reducing agent will be [tex]Sn^{2+}[/tex]
Explanation:
Reducing agent is defined as the agent which helps the other substance to reduce and itself gets oxidized. Thus, it will undergo oxidation reaction.
We are given:
[tex]E_o(Sn)=0.14V\\E_o(Sn^{2+})=-0.15V[/tex]
The electrode potential values of given substances determine the tendency to gain electrons. Higher value of positive electrode potential means that it will gain more and hence, will be a stronger oxidizing agent.
If the specie has negative electrode potential, it means that it will easily loose electrons and hence, will be considered as a stronger reducing agent.
Thus, the stronger reducing agent among the given species will be [tex]Sn^{2+}[/tex]
