The full inoic equation for an electrochemical cell is Br2 + Zn yields 2Br- + Zn2+. write the half reaction that occurs at the anode and the half reaction that occurs at the cathode
Br2 + 2e ==> 2Br^-
Zn ==> Zn^+ + 2e
Can you figure which is the anode and which the cathode? Remember, the anode is where oxidation occurs.
To determine the half-reactions that occur at the anode and cathode, we need to identify the oxidation and reduction processes.
In the given reaction, Br2 is being reduced to 2Br-. This indicates that Br2 gains electrons, which is a reduction process, and occurs at the cathode.
The half-reaction that occurs at the cathode is:
Br2 + 2e- -> 2Br-
On the other hand, Zn is being oxidized to Zn2+. This indicates that Zn loses electrons, which is an oxidation process, and occurs at the anode.
The half-reaction that occurs at the anode is:
Zn -> Zn2+ + 2e-
To determine the half-reactions occurring at the anode and cathode in an electrochemical cell, we need to identify the species that is oxidized (loses electrons) at the anode and the species that is reduced (gains electrons) at the cathode.
In this case, the species that is oxidized is Zn (zinc) because it forms Zn2+ ions. The species that is reduced is Br2 (bromine) because it forms 2Br- ions.
Therefore, the half-reaction occurring at the anode (oxidation) is:
Zn → Zn2+ + 2e-
And the half-reaction occurring at the cathode (reduction) is:
Br2 + 2e- → 2Br-
These half-reactions represent the electron transfer that takes place in the cell.