Question

Consider a aluminum-silver voltaic cell that is constructed such that one half-cell consists of the aluminum, Al, electrode immersed in a Al(NO3)3 solution, and the other half-cell consists of the silver, Ag, electrode immersed in a AgNO3 solution. The two electrodes are connected by a copper wire. The Al electrode acts as the anode, and the Agelectrode acts as the cathode. To maintain electric neutrality, you add a KNO3 salt bridge separating the two half-cells. Use this information to solve Parts B.
B) 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 aluminum-silver voltaic cell. Indicate the physical states of atoms and ions using the abbreviation (s), (l), or (g) for solid, liquid, or gas, respectively. Use (aq) for an aqueous solution. Do not include phases for electrons.
Express your answer as a chemical equation.

Answer 1

Answer:

Overall reaction equation

Al(aq) + 3Ag^+(aq)--------> Al^3+(aq) + 3Ag(s)

Explanation:

A voltaic cell consists of two half cells; the oxidation half cell( anode) and the reduction half cell(cathode)

Anode:

Al(aq) --------> Al^3+(aq) +3e

Cathode:

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

Overall reaction equation

Al(aq) + 3Ag^+(aq)--------> Al^3+(aq) + 3Ag(s)

The overall reaction equation shows the complete redox reaction taking place in the voltaic cell.