Answer:
Cathode: Ag
Anode: Br₂
Explanation:
In the cathode must occur a reduction, so it's more likely to a metal atom be in the cathode. For the metals given the reduction reactions and the potential of reduction are:
Ag⁺ + e⁻ ⇒ Ag⁰ E° = + 0.80 V
Fe⁺² + 2e⁻ ⇒ Fe⁰ E° = - 0.44 V
Al⁺³ + 3e⁻ ⇒ Al⁰ E° = -1.66 V
As the potential for Ag is the higher, the reduction will occur for it first, so in the cathode will produce Ag.
For the anode an oxidation must occurs, so the reactions for the nonmetals are:
F₂ + 2e⁻ ⇒ 2F⁻ E° = +2.87 V
Cl₂ + 2e⁻ ⇒ 2Cl⁻ E° = +1.36 V
Br₂ + 2e⁻ ⇒ 2Br⁻ E° = +1.07 V
For oxidation, the less the E°, the faster the reaction will occur, so Br₂ will be formed in the anode.
Based on the reduction potential, Ag is produced at the cathode while Br₂ is produced at the anode.
When electric current is passed through electrolytes, ions are discharged according to their electrode potential.
Reduction occurs at the cathode.
The metals and their reduction potential are as follows:
Since the reduction potential for Ag is highest, Ag is produced at the cathode
At the anode, reduction occurs.
The nonmetallic ions and their reduction potential are as follows:
For oxidation, the smaller the E°, the faster the reaction will occur.
Therefore, Br₂ is formed at the anode.
Learn more about reduction potential at: https://brainly.com/question/19036092
