Question

Which substance is the oxidizing agent in the following reaction? Fe(s) + Ni⁽²⁺⁾ (aq) → Fe⁽²⁺⁾(aq) + Ni(s)

1) Fe
2) Ni
3) Fe⁽²⁺⁾
4) Ni⁽²⁺⁾

Answer 1

In the reaction Fe(s) + Ni²⁺(aq) → Fe²⁺(aq) + Ni(s), the oxidizing agent is Ni²⁺(aq) since it is the species that gains electrons and is reduced.

Step-by-step explanation:

To determine which substance is the oxidizing agent in the reaction Fe(s) + Ni²⁺(aq) → Fe²⁺(aq) + Ni(s), we need to examine the changes in oxidation numbers of the elements involved.

Iron (Fe) starts as a solid with an oxidation number of 0 and becomes Fe²⁺ with an oxidation number of +2, indicating that Fe is oxidized. Nickel (Ni²⁺) starts with an oxidation number of +2 and becomes Ni(s) with an oxidation number of 0, indicating that Ni²⁺ is reduced. Remember that the reducing agent is the species that is oxidized and the oxidizing agent is the one that is reduced. In this case, Fe is the reducing agent, and Ni²⁺ is the oxidizing agent because it undergoes reduction by gaining electrons.

Answer 2

The oxidizing agent in the reaction Fe(s) + Ni²⁺ (aq) → Fe²⁺(aq) + Ni(s) is Ni²⁺ because it gains electrons and is reduced (Option 4).

Step-by-step explanation:

The question asks which substance is the oxidizing agent in the reaction Fe(s) + Ni²⁺ (aq) → Fe²⁺(aq) + Ni(s). To determine the oxidizing agent, we must look at which substance is reduced. The substance that is reduced gains electrons during the reaction. In this case, nickel (Ni²⁺) gains two electrons to become nickel metal (Ni), thus it is reduced.

The substance that causes another to be reduced (and is itself oxidized) is the reducing agent, which is iron (Fe). Therefore, the reducing agent Fe is oxidized.

Since nickel was reduced, Ni²⁺ is the oxidizing agent, making choice 4) Ni²⁺ the correct answer.