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
In this galvanic cell, the strip of chromium (Cr) is the anode, while the strip of copper (Cu) is the cathode. At the anode (Cr strip), the half-reaction occurring is the oxidation of Cr(s) to Cr3+(aq): 2 Cr(s) → 2 Cr3+(aq) + 6 e-. At the cathode (Cu strip), the half-reaction occurring is the reduction of Cu2+(aq) to Cu(s): 3 Cu2+(aq) + 6 e- → 3 Cu(s).
