Determine the cell diagram for the reaction below.Assume platinum electrodes are used when no other solid is present. Cl₂(g)+ Sn²⁺(aq)$\rarr$Sn⁴⁺(aq)+ 2Cl^-(aq)

Question

Quizplus · Accepted Answer

The cell diagram is written with the anodes on the left and cathodes on the right, separated by a double vertical line indicating the phase boundary. The electrons move from left to right in the diagram. The given balanced redox half-reactions are: Sn4+ + 2e- -> Sn2+ 2Cl- -> Cl2 + 2e- The half-reactions can be combined to give the overall reaction: 2Cl- + Sn4+ -> Cl2 + Sn2+ The reactants and products are listed in the order of the half-reactions, so the anode is Sn²⁺(aq) and the cathode is Cl^-(aq). The platinum electrodes are used when no other solid is present. Therefore, the correct cell diagram is: Pt(s) | Sn²⁺(aq), Sn⁴⁺(aq) || Cl₂(g) | Cl^-(aq) | Pt(s)

Determine the Cell Diagram for the Reaction Below →\rarr→ Sn4+(aq)+ 2Cl-(aq) A)Pt(s)| Cl2(g)| Cl-(aq)|| Sn2+(aq), Sn4+(aq)| Pt(s) B)Pt(s)| Sn2+(aq)

Determine the Cell Diagram for the Reaction Below $\rarr$ Sn⁴⁺(aq)+ 2Cl^-(aq)
A)Pt(s)| Cl₂(g)| Cl^-(aq)|| Sn²⁺(aq), Sn⁴⁺(aq)| Pt(s)
B)Pt(s)| Sn²⁺(aq)