The following reaction occurs at 298 K: Zn(s) + 2Ag+(aq)  Zn2+(aq) + 2Ag(s)

Question

Topic: REDOX AND ELECTROCHEMISTRY

Question:

Sketch a diagram that shows how this cell could be set up. A voltmeter and two beakers, with some labels, are provided to give you a start. Add and label any items you think are necessary for a complete cell.

Answer 1

Zn is being oxidized.

Ag is being reduced.

By convention, we place the anode (oxidation) on the left, and the cathode (reduction) on the right, with a salt bridge in between.

Zn(s) l Zn²⁺(aq) ll Ag⁺(aq) l Ag(s)

s

Since you didn’t include the diagram with the beakers, the above is the best I can do. In one beaker (left) place a solid Zn electrode in a solution of Zn²⁺ ions. In another beaker on the right, place a sold Ag electrode in a solution of Ag⁺ ions. Connect the 2 beakers with a salt bridge containing KNO₃. Also connect the two electrodes with a voltmeter.