Question

Consider a chromium-silver voltaic cell that is constructed such that one half-cell consists of the chromium, Cr, electrode immersed in a Cr(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 Cr electrode acts as the anode, and the Ag electrode acts as the cathode. To maintain electric neutrality, you add a KNO3 salt bridge separating the two half-cells. Use this information to answer the following 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 chromium-silver voltaic cell. Indicate the 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.

Answer 1

Anode: Cr(s) ⇒ Cr³⁺(aq) + 3 e⁻

Step-by-step explanation:

In the anode takes place the oxidation, in which the reducing agent loses electrons.

In the cathode takes place the reduction, in which the oxidizing agent gains electrons.

The corresponding half-reactions are:

Anode: Cr(s) ⇒ Cr³⁺(aq) + 3 e⁻

Cathode: Ag⁺(aq) + 1 e⁻ ⇒ Ag(s)