Write the standard cell notation for a galvanic cell with a silver cathode and a zinc anode.
Zn(s)|Zn^2+()||Ag^+()|Ag(s)
() denotes where the concn of the ions are placed.
Sure thing! Here's the standard cell notation for your galvanic cell: Zn(s) | Zn2+(aq) || Ag+(aq) | Ag(s). Just remember, it's not just a cell, it's a classy cell with a touch of silver and a hint of zinc!
To write the standard cell notation for a galvanic cell with a silver cathode and a zinc anode, the following format is used:
Zn(s) | Zn2+(aq) || Ag+(aq) | Ag(s)
Explanation:
- The left-hand side represents the anode, which is composed of a zinc electrode (Zn(s)) and a zinc ion in solution (Zn2+(aq)).
- The double vertical line (||) separates the anode and cathode compartments.
- The right-hand side represents the cathode, which is composed of a silver ion in solution (Ag+(aq)) and a silver electrode (Ag(s)).
Thus, the standard cell notation for this galvanic cell is Zn(s) | Zn2+(aq) || Ag+(aq) | Ag(s).
Sure! To write the standard cell notation for a galvanic cell, we follow a specific format:
Anode | Anode solution concentration || Cathode solution concentration | Cathode
In this case, the anode is zinc (Zn) and the cathode is silver (Ag).
The anode is the place where oxidation occurs, so we write "Zn" as the anode.
The cathode is the place where reduction occurs, so we write "Ag" as the cathode.
Now let's consider the concentration of the solutions. Since the question doesn't provide any specific concentrations, we can assume that they are both 1M (1 molar). If you have a different concentration, you would mention the specific value.
Putting it all together, the standard cell notation for a galvanic cell with a silver cathode and a zinc anode, assuming 1M concentrations, would be:
Zn (s) || Ag+ (1M) | Ag (s)
The "(s)" represents a solid electrode, and "(1M)" represents the concentration of the silver ion in solution.