2 Ag+(aq) + Fe(s) --> 2 Ag(s) + Fe2+(aq)
Which electrode is the anode, and which is the cathode.
and
In which directions do the cations and anions migrate through the solution?
cations
thanks
Write the two half equations.
Ag^+ + e ==> Ag
Fe==> Fe^+2 + 2e
Which one loses electrons. That is oxidation. Oxidation occurs at the anode.
The anode is - charge. Fe^2+ are increasing (which means more negative ions migrate to that half cell). Ag^+ is decreasing which means fewer negative ions needed in that half cell.
To determine the anode and cathode in a redox reaction, we need to identify the species that is being oxidized and reduced.
In the given reaction: 2 Ag+(aq) + Fe(s) -> 2 Ag(s) + Fe2+(aq)
The species Ag+(aq) is being reduced to Ag(s), gaining electrons and getting reduced from +1 to 0 oxidation state. On the other hand, Fe(s) is being oxidized to Fe2+(aq), losing electrons and getting oxidized from 0 to +2 oxidation state.
According to the general rules of redox reactions, oxidation occurs at the anode, and reduction occurs at the cathode.
Therefore, in this reaction:
- The anode is Fe(s)
- The cathode is Ag+(aq)
Regarding the migration of cations and anions through the solution, we need to consider the movement of ions based on their charge.
In the given reaction, Ag+ ions (cations) are gaining electrons and getting reduced to Ag(s), so they are being attracted to the cathode. Therefore, cations (Ag+) migrate towards the cathode.
Fe2+ ions (also cations) are produced during the oxidation of Fe(s) and are released into the solution. As a result, Fe2+ ions are being attracted to the anode. Thus, cations (Fe2+) migrate towards the anode.
In summary:
- Cations (Ag+ and Fe2+) migrate towards the cathode,
- Anions would typically migrate towards the anode, but in this reaction, there are no anions involved.
I hope this helps! Let me know if you have any further questions.
To determine which electrode is the anode and which is the cathode, we need to consider the standard reduction potentials of the half-reactions involved.
In the given reaction: 2 Ag+(aq) + Fe(s) -> 2 Ag(s) + Fe2+(aq)
The half-reaction for Ag+ reduction is: Ag+(aq) + e- -> Ag(s)
The half-reaction for Fe oxidation is: Fe(s) -> Fe2+(aq) + 2 e-
The half-reaction with the more positive reduction potential is the reduction reaction, and the other is the oxidation reaction. So, in this case, the Ag+ reduction half-reaction has a more positive reduction potential, and therefore, it occurs at the cathode. The Fe oxidation half-reaction occurs at the anode.
Therefore, the cathode is where the reduction occurs, and in this reaction, it is where Ag+ ions gain electrons to form Ag(s). The anode is where the oxidation occurs, and it is where Fe(s) loses electrons to form Fe2+(aq).
Regarding the migration of cations (positive ions) and anions (negative ions) through the solution, cations are attracted towards the cathode (where reduction occurs) and migrate towards it. In this case, Ag+ ions are cations and will migrate towards the cathode. Anions, on the other hand, are attracted towards the anode (where oxidation occurs) and migrate towards it. However, there are no anions present in the given equation, so we cannot determine their migration direction.