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).
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.
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