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:

Question

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.%0D%0A%0D%0A(4 points)

Answer 1

The anode is the electrode at which oxidation occurs, and the cathode is the electrode at which reduction occurs. In this galvanic cell, chromium is oxidized from Cr(s) to Cr3+(aq) at the anode, while copper(II) ions, Cu2+(aq), are reduced to Cu(s) at the cathode. The half-reaction at the anode is: 2Cr(s) → 2Cr3+(aq) + 6e^-, and the half-reaction at the cathode is: 3Cu2+(aq) + 6e^- → 3Cu(s).