Question

Part A:
Calculate the standard potential for the following galvanic cell:
Zn(s) l Zn2+(aq) ll Ag+(aq) l Ag(s)
Express your answer to 3 significant figures.
(I'll post the picture of more information)

Part B:
In the context of the zinc-silver cell described in Part A, match each of the following descriptions to the anode or cathode.

Zn, Ag, gains mass, loses mass, attracts electrons, positive electrode, negative electrode, stronger reducing agent.

Answer 1

Could you write your half equations please.
HINT: Using your activity series, the metal that is more active, is the Anode and thus the other metal would be the cathode.

Answer 2

Activity Series:
The metals are listed in order of decreasing activity or decreasing strength as reductants. The list is:
\[\large K>Ca>Na>Mg>Al>Zn>Fe>Pb>H_{2}>Cu>Ag>Au\]

Answer 3

\[\large Ag^{+}(aq)+e^{-} \rightarrow Ag(s)\]
\[\large Zn(s)\rightarrow Zn^{2+}(aq)+2e^{-}\]
There are your half equations. Using your table of standard potentials, the oxidation potentials can be determined by reversing the sign. SO therefore cell potential for this galvanic cell is:
\[\large E^{o} = E^{o}(reduction)+E^{o}(oxidation)\]
\[\large E^{o}=-(-0.76)+(0.8)\]
\[\large =0.76+0.8\]
\[\large =1.56V\]

Answer 4

Thank you for your help!