Question

Which of the following cells is most likely to be an example of a galvanic cell?

A. Au(s) | Au || Ag | Ag(s)

B. Cu(s) | Cu²⁺ || Fe²⁺ | Fe(s)

C. Sn(s) | Sn²⁺ || Fe²⁺ | Fe(s)

D. Zn(s) | Zn²⁺ || Cu²⁺ | Cu(s)

Answer 1

Option D, Zn(s) | Zn²⁺ || Cu²⁺ | Cu(s), most accurately represents a galvanic cell, where zinc and copper engage in spontaneous redox reactions to produce electrical energy.

Step-by-step explanation:

The question asks which of the following cells is most likely to be an example of a galvanic cell. A galvanic cell, also known as a voltaic cell, is an electrochemical cell that derives electrical energy from spontaneous redox reactions taking place within the cell. Zn(s) | Zn²⁺ || Cu²⁺ | Cu(s) is the correct representation of a galvanic cell where a zinc rod is dissolved in an aqueous solution containing Cu²⁺ ions, which results in copper metal being deposited and Zn²⁺ ions being released into the solution. This process is spontaneous and generates electrical energy.

An example demonstrating the principle of a galvanic cell is the reaction between metallic zinc and cupric ion (Cu²⁺) to give copper metal and Zn²⁺ ion. The balanced chemical equation for this reaction is Zn(s) + Cu²⁺ (aq) → Zn²⁺ (aq) + Cu(s). Hence, option D represents a typical galvanic cell scenario.