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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]

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