Consider an electrochemical cell where the following reaction takes place: 3 Sn²⁺(aq) + 2 Al(s) → 3 Sn(s) + 2 Al³⁺(aq) Which of the following is the correct cell notation for this cell?
You didn't list the choices; however, see your first post where I wrote the notation for a cell.
See your first post where I wrote the notation for that cell.
whoops haha!
Al | Al³⁺ || Sn²⁺ | Sn
Al³⁺ | Al || Sn | Sn²⁺
Sn | Sn²⁺ || Al³⁺ | Al
Sn | Al³⁺ || Al | Sn²⁺
To find the correct cell notation for this electrochemical cell, we need to understand the conventions used. The cell notation consists of several components:
1. The anode (oxidation half-reaction) on the left side of the vertical line.
2. The vertical line "|" representing the phase boundary between the anode and the cathode.
3. The cathode (reduction half-reaction) on the right side of the vertical line.
4. The double vertical lines "||" representing the salt bridge or porous barrier between the two half-cells.
5. The phase symbols (s, l, g, or aq) for solid, liquid, gas, or aqueous species.
In this given electrochemical cell, the Sn²⁺(aq) ions are being reduced to Sn(s) at the cathode (reduction half-reaction), while Al(s) is being oxidized to Al³⁺(aq) at the anode (oxidation half-reaction).
The correct cell notation for this reaction is:
Anode: Al(s) | Al³⁺(aq) || Sn²⁺(aq) | Sn(s) : Cathode
The anode is written on the left side of the vertical line, and the cathode is written on the right side. The "|" separates the anode and cathode, and the "||" represents the salt bridge or porous barrier. The phase symbols are included for the appropriate species (s for solid, aq for aqueous).
So, the correct cell notation for this electrochemical cell is:
Al(s) | Al³⁺(aq) || Sn²⁺(aq) | Sn(s)