Give the standard line notation for a galvanic cell based on the following unbalanced equation

Give the standard line notation for a galvanic cell based on the following unbalanced equation: Cr3+ + Cl2 → Cr2O72- + Cl-

The Correct Answer and Explanation is:

To begin, let’s break down the given unbalanced reaction:
Cr3++Cl2→Cr2O72−+Cl−\text{Cr}^{3+} + \text{Cl}_2 \rightarrow \text{Cr}_2\text{O}_7^{2-} + \text{Cl}^-Cr3++Cl2​→Cr2​O72−​+Cl−

Step 1: Identify the Oxidation and Reduction Half-Reactions

• Oxidation half-reaction: Chlorine (Cl2_22​) is reduced to chloride ions (Cl−^-−). Cl2→Cl−\text{Cl}_2 \rightarrow \text{Cl}^-Cl2​→Cl− In this reaction, chlorine gains electrons (is reduced).
• Reduction half-reaction: Chromium (Cr3+^3+3+) is oxidized to chromium in the chromium oxide form (Cr2_22​O72−_7^{2-}72−​). Cr3+→Cr2O72−\text{Cr}^{3+} \rightarrow \text{Cr}_2\text{O}_7^{2-}Cr3+→Cr2​O72−​

Step 2: Balance the Half-Reactions

Let’s balance each half-reactionTools