Question

Consider a galvanic cell with a beaker of sulfuric acid and a beaker of nitric acid. The sulfuric acid beaker contains a strip of tin, and the nitric acid cell contains a strip of platinum. A wire runs between the strips. The reaction that occurs is as follows:

3Sn(s) + 2NO3–(aq) + 8H+(aq) → 3Sn2+(aq) + 2NO(g) + 4H2O(l)

In three to five sentences, list which electrode is the anode and which is the cathode and the half reactions that occur at each electrode.

Answer 1

I wrote, The platinum electrode is the cathode in this reaction. The tin electrode is the anode in this reaction. In the half reactions that occur the nitrate is reduced to nitric oxide(NO) while the tin electrode is oxidized to Sn2+.

Answer 2

Oxidation occurs at the tin half cell(anode) while reduction occurs at the nitrate half cell(cathode).

A galvanic cell refers to a cell that produces electrical energy spontaneously by redox reaction. Oxidation occurs at the anode while reduction occurs at the cathode in a galvanic cell.

The oxidation half equation at the anode occurs as follows;

3Sn(s) → 3Sn^2+(aq) + 6e

The reduction half equation that occurs at the cathode is;

2NO3–(aq) + 8H+(aq) + 6e→  2NO(g) + 4H2O(l)

We can see that electron loss occurs at the cathode while electron gain occurs at the anode as we can see in the equations above.

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