Consider a galvanic cell with a beaker of Chromium(III) nitrate Cr(NO3)3 and a beaker of Copper (Il) nitrate Cu(NO3)2•
The Chromium(III) nitrate beaker contains a strip of chromium, and the Copper(Il) nitrate cell contains a strip of copper. A wire runs between the strips. The reaction that occurs is as follows:
2Cr(s) + 3Cu?+(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.
In this galvanic cell, the copper electrode is the cathode, and the chromium electrode is the anode. At the copper cathode, the reduction half-reaction occurs: Cu2+(aq) + 2e- → Cu(s). At the chromium anode, the oxidation half-reaction occurs: Cr(s) → Cr3+(aq) + 3e-.
Overall, the net reaction is: 2Cr(s) + 3Cu2+(aq) → 2Cr3+(aq) + 3Cu(s).