In a zinc-copper cell, Zn | Zn+2(1M) || Cu+2(1M) | Cu, which electrode is negative?
a. Cu(s)
b. Zn(s)
c. Zn+2(aq)
d. Cu+2(aq)
Its A or C.
Not sure.
Please help.
wooooooo ZN it is mutha
ZN(s)
To determine which electrode is negative in a zinc-copper cell, we need to understand the concept of the standard electrode potential (E°). The standard electrode potential is a measure of the tendency of an electrode to undergo reduction (gain of electrons) or oxidation (loss of electrons).
In a cell notation, the thicker line represents the phase boundary, and the double vertical lines indicate a salt bridge or a porous barrier. The anode (oxidation) is written on the left and the cathode (reduction) is written on the right.
In the given cell notation, Zn | Zn+2(1M) || Cu+2(1M) | Cu:
- The half-cell on the left side (anode) is Zn | Zn+2(1M).
- The half-cell on the right side (cathode) is Cu+2(1M) | Cu.
To determine which electrode is negative, we compare the reduction potential values of Zn and Cu. The half-cell with the higher reduction potential value will be the cathode (negative electrode), while the half-cell with the lower reduction potential value will be the anode (positive electrode).
Standard reduction potential values can be found in tables, such as the Standard Electrode Potentials table.
By looking up the standard reduction potential values for Zn and Cu, we can find that the reduction potential for Cu is greater than that of Zn. Therefore, Cu is reduced more easily and is the cathode (negative electrode). The correct answer is option a. Cu(s).
As a general rule, the cell potential (E cell) is positive when the reduction potential of the cathode is greater than that of the anode.
Nope. Zn(s) + Cu^2+ ==> Zn^2+ + Cu(s)
Zn is the negative electrode (and the anode) while Cu is positive (and the cathode).