A battery is constructed from iron, Fe, and silver, \(\mathrm{Ag}\), by dipping a strip of each metal into a solution of its ions \(\left(\mathrm{Fe}^{3+}\right.\) and \(\mathrm{Ag}^{+}\), respectively). As the battery operates, the \(\mathrm{Fe}^{3+}\) concentration increases while the \(\mathrm{Ag}^{+}\) concentration decreases. (a) What is getting oxidized? (b) What is getting reduced? (c) Draw a battery similar to the one you drew for WorkPatch \(10.7\), label which way the electrons flow, and label cathode, \(+\), and anode, \(=\).

Short Answer

Expert verified
In the given battery, iron (Fe) gets oxidized, as seen in the oxidation half-reaction: \(Fe \rightarrow Fe^{3+} + 3e^{-}\). Meanwhile, silver ions (Ag⁺) get reduced, as seen in the reduction half-reaction: \(Ag^{+} + e^{-} \rightarrow Ag\). In the battery diagram, the anode (-) is a strip of iron (Fe) and the cathode (+) is a strip of silver (Ag) with an external wire connecting them, directing electron flow from the anode to the cathode. The solution contains both Fe³⁺ and Ag⁺ ions.

Step by step solution

01

Oxidation half-reaction

In an oxidation half-reaction, the species loses electrons and its oxidation state increases. Since Fe³⁺ concentration increases, it implies that the reaction involves Fe turning into Fe³⁺. The oxidation half-reaction can be written as: \[ Fe \rightarrow Fe^{3+} + 3e^{-} \] Thus, iron (Fe) is getting oxidized. (b) Identify the substance that gets reduced
02

Reduction half-reactions

In a reduction half-reaction, the species gains electrons and its oxidation state decreases. Since Ag⁺ concentration decreases, it means that Ag⁺ is accepting electrons and turning into Ag. The reduction half-reaction can be written as: \[ Ag^{+} + e^{-} \rightarrow Ag \] Therefore, silver ions (Ag⁺) are getting reduced. (c) Drawing a battery diagram
03

Battery diagram

Find a piece of paper and draw the following components: 1. An anode (-) on the left, which consists of a strip of iron (Fe). Label it as "Fe". 2. A cathode (+) on the right, which consists of a strip of silver (Ag). Label it as "Ag". 3. A solution containing ions of each metal in the middle. Label it as "Fe³⁺ and Ag⁺". 4. Connect the anode and the cathode with an external wire, indicating the flow of electrons from the anode (Fe) to the cathode (Ag). In summary, the iron (Fe) strip acts as the anode and gets oxidized, losing electrons that flow through the wire towards the silver (Ag) strip. The silver (Ag) strip acts as the cathode, where silver ions (Ag⁺) gain these electrons and get reduced to form metallic silver.

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