To write the shorthand notation for the given galvanic cell, we need to follow these steps: 1. **Identify the anode and cathode reactions:** - **Anode (oxidation):** Lead (Pb) is oxidized to lead ions (Pb²⁺). \[ \text{Pb(s)} \rightarrow \text{Pb}^{2+}(\text{aq}) + 2\text{e}^- \] - **Cathode (reduction):** Ferric ions (Fe³⁺) are reduced to ferrous ions (Fe²⁺). \[ \text{Fe}^{3+}(\text{aq}) + \text{e}^- \rightarrow \text{Fe}^{2+}(\text{aq}) \] 2. **Write the cell notation:** - The anode (oxidation) half-cell is written on the left. - The cathode (reduction) half-cell is written on the right. - A single vertical line (|) separates different phases within the same half-cell. - A double vertical line (||) represents the salt bridge between the two half-cells. Given the reactions: - Anode: \(\text{Pb(s)} \rightarrow \text{Pb}^{2+}(\text{aq}) + 2\text{e}^-\) - Cathode: \(\text{Fe}^{3+}(\text{aq}) + \text{e}^- \rightarrow \text{Fe}^{2+}(\text{aq})\) The shorthand notation for the galvanic cell is: \[ \text{Pb(s)} | \text{Pb}^{2+}(\text{aq}) || \text{Fe}^{3+}(\text{aq}), \text{Fe}^{2+}(\text{aq}) | \text{Pt(s)} \] Here: - \(\text{Pb(s)}\) is the solid lead electrode. - \(\text{Pb}^{2+}(\text{aq})\) is the lead ion in solution. - \(\text{Fe}^{3+}(\text{aq})\) and \(\text{Fe}^{2+}(\text{aq})\) are the ferric and ferrous ions in solution. - \(\text{Pt(s)}\) is the platinum electrode used as an inert conductor for the cathode reaction

To write the shorthand notation for the given galvanic cell, we need to follow these steps: 1. Identify the anode and cathode reactions: - Anode (oxidation): Lead (Pb) is oxidized to lead ions (Pb²⁺). $\text{Pb(s)} \rightarrow \text{Pb}^{2+}(\text{aq}) + 2\text{e}^-$ - Cathode (reduction): Ferric ions (Fe³⁺) are reduced to ferrous ions (Fe²⁺). $\text{Fe}^{3+}(\text{aq}) + \text{e}^- \rightarrow \text{Fe}^{2+}(\text{aq})$ 2. Write the cell notation: - The anode (oxidation) half-cell is written on the left. - The cathode (reduction) half-cell is written on the right. - A single vertical line (|) separates different phases within the same half-cell. - A double vertical line (||) represents the salt bridge between the two half-cells. Given the reactions: - Anode: $\text{Pb(s)} \rightarrow \text{Pb}^{2+}(\text{aq}) + 2\text{e}^-$ - Cathode: $\text{Fe}^{3+}(\text{aq}) + \text{e}^- \rightarrow \text{Fe}^{2+}(\text{aq})$ The shorthand notation for the galvanic cell is: $\text{Pb(s)} | \text{Pb}^{2+}(\text{aq}) || \text{Fe}^{3+}(\text{aq}), \text{Fe}^{2+}(\text{aq}) | \text{Pt(s)}$ Here: - $\text{Pb(s)}$ is the solid lead electrode. - $\text{Pb}^{2+}(\text{aq})$ is the lead ion in solution. - $\text{Fe}^{3+}(\text{aq})$ and $\text{Fe}^{2+}(\text{aq})$ are the ferric and ferrous ions in solution. - $\text{Pt(s)}$ is the platinum electrode used as an inert conductor for the cathode reaction