Question

On the sketch below for a spontaneous voltaic cell:

i. Label the anode and cathode
ii. Write the half-reaction that occurs at each electrode
iii. Show the direction of electron flow and ion flow

Answer 1

• Zn is the anode and the Cu is the cathode
• At the anode; Zn(s) --->
  `Zn^{2+`(aq) + 2e. At the cathode;
  `Cu^{2+`(aq) + 2e --> Cu(s)

• Electrons flows from the Zn to the Cu electrode

What is a voltaic cell

A voltaic cell, sometimes called a galvanic cell, is a clever device that uses spontaneous redox reactions to transform chemical energy into electrical energy. Put simply, oxidation is the loss of electrons by one substance and reduction is the gain of electrons by another.

Two electrodes—the cathode for reduction and the anode for oxidation—an electrolyte solution for ion flow, and a salt bridge to preserve electrical neutrality are all involved in this process. Imagine that at the anode, a metal dissolves, releasing electrons that flow as electricity through an external circuit. Via the salt bridge, positive ions from the anode move to the cathode, where they pick up electrons and deposit as metal.