write the cell notation of Zn°(s)|Zn 2+ (aq),Cl − (aq)|AgCl(s)|Ag°(s)

To write the cell notation for the given electrochemical cell, we need to understand the components and their arrangement within the cell. Let's break it down step by step.

1. Identify the half-reactions:
In this cell, we have two half-reactions:
- Zinc half-reaction: Zn°(s) → Zn2+(aq) + 2e−
- Silver half-reaction: AgCl(s) + e− → Ag°(s) + Cl−(aq)

2. Determine the electrode compositions:
The oxidized form (lost electrons) is on the left side of the vertical line (|), while the reduced form (gained electrons) is on the right side.
- The Zinc electrode: Zn°(s) on the left side loses electrons, which makes it the anode (the negative electrode).
- The Silver electrode: Ag°(s) on the right side gains electrons, which makes it the cathode (the positive electrode).

3. Include the ions present:
In this cell, both Zinc and Chloride ions are present as aqueous solutions, so we need to include them in the cell notation.
- The Zinc ion (Zn2+) is represented as Zn2+(aq).
- The Chloride ion (Cl−) is represented as Cl−(aq).

Putting it all together, the cell notation for the given electrochemical cell is:

Zn°(s) | Zn2+(aq) || Cl−(aq) | AgCl(s) | Ag°(s)

Here, the double line (||) represents the salt bridge or porous barrier that allows ion flow between the two half-cells to balance the charges and maintain electrical neutrality.