In the zinc-copper cell, Zn(s) | Zn^+2(1M) || Cu^+2(1M) | Cu(s), which electrode is negative
Cu^+2
Cu(s)
Zn(s)
Zn^+2***
No. The Zn^2+ is not an electrode. That's a solution. The two electrons are copper and Zinc.
To determine which electrode is negative in the zinc-copper cell, you'll need to identify the oxidation and reduction reactions occurring at each electrode. The oxidation reaction occurs at the anode, where electrons are lost, while the reduction reaction occurs at the cathode, where electrons are gained.
In the given cell configuration, the zinc electrode is on the left side (anode) and the copper electrode is on the right side (cathode). The overall cell reaction can be broken down into two half-reactions:
1. At the zinc electrode (anode): Zn(s) → Zn^+2(aq) + 2e^-
This half-reaction represents the oxidation of zinc metal, where it loses two electrons and forms zinc ions (Zn^+2) in the solution.
2. At the copper electrode (cathode): Cu^+2(aq) + 2e^- → Cu(s)
This half-reaction represents the reduction of copper ions (Cu^+2) in the solution, where they gain two electrons and deposit as copper metal on the electrode.
Now, let's compare the two half-reactions. In the oxidation half-reaction, electrons are lost, indicating oxidation. In the reduction half-reaction, electrons are gained, indicating reduction.
Based on the half-reactions, we can conclude that the zinc electrode is negative (anode), and the copper electrode is positive (cathode). So, the answer is Zn^+2 electrode, which is the zinc electrode.