Consider an electrochemical cell where the following reaction takes place: 2 Au³⁺(aq) + 3 Zn(s) → 2 Au(s) + 3 Zn²⁺(aq)
What is the correct cell notation for this cell?
Au³⁺(aq) + 3 Zn(s) → 2 Au(s) + 3 Zn²⁺(aq)
Zn|Zn^2+||Au^3+|Au
To determine the correct cell notation for the given electrochemical cell, we need to follow a specific format, which includes:
1. Identifying the half-reactions:
- The oxidation half-reaction occurs at the anode (the electrode where oxidation takes place), which involves the oxidation of Zn to Zn²⁺ ions: Zn(s) → Zn²⁺(aq) + 2e⁻
- The reduction half-reaction occurs at the cathode (the electrode where reduction takes place), which involves the reduction of Au³⁺ ions to Au atoms: Au³⁺(aq) + 3e⁻ → Au(s)
2. Writing the cell notation:
- The anode (oxidation) is written on the left side and the cathode (reduction) is written on the right side.
- A single vertical line (|) represents the phase boundary between the two electrodes.
- The salt bridge is indicated with a double vertical line (||).
Based on the given information, the correct cell notation for this electrochemical cell would be:
Zn(s) | Zn²⁺(aq) || Au³⁺(aq) | Au(s)
Keep in mind that the anode is always written on the left and the cathode on the right, separated by a single vertical line, and the salt bridge is represented by a double vertical line.