Consider a iron-silver voltaic cell that is constructed such that one half-cell consists of the iron, \rm Fe , electrode immersed in a \rm Fe(NO_3)_3 solution, and the other half-cell consists of the silver, \rm Ag, electrode immersed in a \rm AgNO_3 solution. The two electrodes are connected by a copper wire. The \rm Fe electrode acts as the anode, and the \rm Ag electrode acts as the cathode. To maintain electric neutrality, you add a \rm KNO_3 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 an oxidation reaction and the other half-cell is the site of a reduction reaction.
Type the half-cell reaction that takes place at the cathode for the iron-silver voltaic cell. Indicate physical states using the abbreviation (s), (l), or (g) for solid, liquid, or gas, respectively. Use (aq) for an aqueous solution. Do not forget to add electrons in your reaction.