Consider a galvanic cell with a beaker of Chromium(III) nitrate Cr(NO3)3 and a beaker of Copper(II) nitrate Cu(NO3)2. The Chromium(III) nitrate beaker contains a strip of chromium, and the Copper(II) nitrate cell contains a strip of copper. A wire runs between the strips. The reaction that occurs is as follows: 2Cr(s) + 3Cu2+(aq) → 2Cr3+(aq) + 3Cu(s) 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. (4 points)

Question

Consider a galvanic cell with a beaker of Chromium(III) nitrate Cr(NO3)3 and a beaker of Copper(II) nitrate Cu(NO3)2. The Chromium(III) nitrate beaker contains a strip of chromium, and the Copper(II) nitrate cell contains a strip of copper. A wire runs between the strips. The reaction that occurs is as follows: 2Cr(s) + 3Cu2+(aq) → 2Cr3+(aq) + 3Cu(s) 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. (4 points)

Answer 1

In this galvanic cell, the anode is the electrode where oxidation occurs, while the cathode is the electrode where reduction occurs. In this case, the chromium strip is the anode and the copper strip is the cathode.

At the anode (Cr strip), the half-reaction that occurs is the oxidation of chromium:

2Cr(s) -> 2Cr3+(aq) + 6e-

At the cathode (Cu strip), the half-reaction that occurs is the reduction of copper:

3Cu2+(aq) + 6e- -> 3Cu(s)