Construction of a voltaic cell Consider a cobalt-silver voltaic cell that is constructed such that one half-cell consists of the cobalt, CoCo, electrode immersed in a Co(NO3)3Co(NO3)3 solution, and the other half-cell consists of the silver, AgAg, electrode immersed in a AgNO3AgNO3 solution. The two electrodes are connected by a copper wire. The CoCo electrode acts as the anode, and the AgAg electrode acts as the cathode. To maintain electric neutrality, you add a KNO3KNO3 salt bridge separating the two half-cells.
The half-cell is a chamber in the voltaic cell where one half-cell is the site of the oxidation reaction and the other half-cell is the site of the reduction reaction. Type the half-cell reaction that takes place at the anode for the cobalt-silver voltaic cell. Indicate the physical states of atoms and ions using the abbreviation (s), (l), or (g) for solid, liquid, or gas, respectively.

A voltaic cell produces energy by spontaneous chemical processes. A voltaic cell contains an anode and a cathode. Oxidation (electron loss) occurs at the anode while reduction (electron gain) occurs at the cathode.

For the cobalt-silver voltaic cell, the reaction equation of the cobalt and silver voltaic anode half cell is shown;

At the anode;

Co(s) ------> Co^3+(aq) + 3e

Note that the anode is the electrode where oxidation occurs hence electrons are lost at the anode.