A galvanic cell is constructed from the Sn4+/Sn2+ and Zn2+/Zn half cells. With reference to the Standard Reduction Potential Table the formula sheet, which of the following statements is correct about this cell?

Question

A galvanic cell is constructed from the Sn4+/Sn2+ and Zn2+/Zn half cells. With reference to the Standard Reduction Potential Table  the formula sheet, which of the following statements is correct about this cell?

BlackTom AI · Accepted Answer

We start by identifying the two half-cells involved: Sn4+/Sn2+ and Zn2+/Zn. To predict the cell behavior, compare their standard reduction potentials. The higher (more positive) reduction potential is the species that will be reduced at the cathode, while the lower (more negative) reduction potential will be oxidized at the anode.

Option 1: 'Sn is oxidized and E°(cell) = 0.91' — This would require Sn to be the anode and oxidize Sn2+ to Sn4+, which contradicts the fact that Sn4+/Sn2+ has a higher tendency to stay reduced relative to Zn2+/Zn; in this setup Sn is actually reduced, not oxidized. The E° value being 0.91 is tied to the overall cell potential, not to Sn being oxidized here, so this statement is inconsistent.

Option 2: 'Sn is reduced and E°(cell) = 0.61' — While Sn is indeed reduced in this cell, the reported cell potential is incorrect. The standard cell potential is not 0.61 V for this combination; it is determined by E°cell = E°cathode − E°anode, which yields 0.91 V when Sn4+/Sn2+ is the cathode and Zn2+/Zn is the anode.

Option 3: 'Zn is reduced and E°(cell) = 0.61' — Zn2+/Zn has a relatively low (negative) reduction potential, so Zn would not be reduced at the cathode of this cell; this option incorrectly assigns reduction to Zn and also uses an incorrect E°cell value.

Option 4: 'Zn is oxidized and E°(cell) = 0.91' — This matches the expected thermodynamics: Zn2+/Zn has the lower reduction potential, so Zn is oxidized at the anode (Zn → Zn2+ + 2e−). The Sn4+/Sn2+ couple serves as the cathode, where reduction occurs (Sn4+ + 2e− → Sn2+). The standard cell potential is E°cell = E°cathode − E°anode = (+0.15 V) − (−0.76 V) = +0.91 V, which aligns with the stated E°cell. This option correctly identifies both the oxidation at the anode and the correct E°cell value.

Option 5: 'Zn is oxidized and E°(cell) = 0.61' — Although the oxidation part is correct, the reported E°cell is incorrect for this pair of half-reactions; the actual E°cell is 0.91 V, not 0.61 V.

In summary, the correct understanding is that Zn is oxidized at the anode while Sn4+/Sn2+ is reduced at the cathode, giving a standard cell potential of 0.91 V. The other options either flip which metal is oxidized/reduced or assign an incorrect cell potential, or both.

A galvanic cell is constructed from the Sn4+/Sn2+ and Zn2+/Zn half cells. With reference to the Standard Reduction Potential Table the formula sheet, which of the following statements is correct about this cell? Single choice

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