The balanced overall redox equation for the following cell diagram:
Cr(s) | Cr³⁺(aq) || Sn⁴⁺(aq),Sn²⁺(aq) | Pt(s) is:
2Cr(s) + 3Sn⁴⁺(aq) $\rarr$ 2Cr³⁺(aq) + 3Sn²⁺(aq)

Question

The balanced overall redox equation for the following cell diagram: Cr(s) | Cr³⁺(aq) || Sn⁴⁺(aq),Sn²⁺(aq) | Pt(s) is: 2Cr(s) + 3Sn⁴⁺(aq) $\rarr$ 2Cr³⁺(aq) + 3Sn²⁺(aq)

Quizplus · Accepted Answer

To balance the redox equation, we need to write the half-reactions for oxidation and reduction. Oxidation half-reaction: Cr(s) → Cr³⁺(aq) + 3e- Reduction half-reaction: 3Sn⁴⁺(aq) + 4e- → 3Sn²⁺(aq) Multiplying the oxidation half-reaction by 3 and adding it to the reduction half-reaction, we get: 2Cr(s) + 3Sn⁴⁺(aq) → 2Cr³⁺(aq) + 3Sn²⁺(aq) Including the double vertical line (||) to separate the half-cells and the solid electrodes (Pt(s) and Cr(s)), we get the cell diagram: Cr(s) | Cr³⁺(aq) || Sn⁴⁺(aq),Sn²⁺(aq) | Pt(s)

The Balanced Overall Redox Equation for the Following Cell Diagram →\rarr→

The Balanced Overall Redox Equation for the Following Cell Diagram $\rarr$