Chemistry Problem (3)

Studying the Galvanic Cell

Oxidation-Reduction reactions can be used to provide electricity. Various forms of cells and batteries produce electricity through a redox reaction. A device that converts chemical energy into electric energy is called a galvanic cell. In order to build a galvanic cell, we need two metal strips, one being more reactive than the other. Each of the two metals is dipped in a solution containing the ion specific to that metal. Then, the solutions are connected to each other by a salt bridge. The two metal strips are connected to the terminals of a voltmeter or a bulb. The figure above displays a galvanic cell.
1) Why can redox reactions produce electricity?
2) Using the passage:
- write examples of uses of redox reactions in daily life.

- define the galvanic cell

3) Can we use two metals of the same nature? Justify your answer.
4) The sketch above shows the direction of transfer of electrons. Label the anode and the cathode of the cell justifying your answer.

5) Given: the other electrode is Ag, the ion of Ag is Ag+, the ion of Zn is Zn2+. - Write the oxidation and reduction half reactions, and write the overall redox reaction.
6) Give the representation of this cell.
7) Which electrode becomes thinner? Which electrode becomes thicker? Justify your answer.