alt=\"Image for The voltage generated by the zinc concentration cell described b
ID: 869044 • Letter: A
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alt="Image for The voltage generated by the zinc concentration cell described by, Zn(s)|Zn2+(aq, 0.100 M)||Zn2+(aq, ? M)|Zn(salt="Image for The voltage generated by the zinc concentration cell described by, Zn(s)|Zn2+(aq, 0.100 M)||Zn2+(aq, ? M)|Zn(salt="Image for The voltage generated by the zinc concentration cell described by, Zn(s)|Zn2+(aq, 0.100 M)||Zn2+(aq, ? M)|Zn(salt="Image for The voltage generated by the zinc concentration cell described by, Zn(s)|Zn2+(aq, 0.100 M)||Zn2+(aq, ? M)|Zn(salt="Image for The voltage generated by the zinc concentration cell described by, Zn(s)|Zn2+(aq, 0.100 M)||Zn2+(aq, ? M)|Zn(salt="Image for The voltage generated by the zinc concentration cell described by, Zn(s)|Zn2+(aq, 0.100 M)||Zn2+(aq, ? M)|Zn(salt="Image for The voltage generated by the zinc concentration cell described by, Zn(s)|Zn2+(aq, 0.100 M)||Zn2+(aq, ? M)|Zn(s The voltage generated by the zinc concentration cell described by, Zn(s)|Zn2+(aq, 0.100 M)||Zn2+(aq, ? M)|Zn(s) is 17.0 mV at 25 degree C. Calculate the concentration of the Zn2+(aq) ion at the cathode.Explanation / Answer
Zn(s) | Zn2+ (0.100 M ) || Zn2+ (? M) | Zn(s)
Anode .............................. ....................... cathode
Oxidation ......................... ....................... reduction
This is what is called a "concentration cell." It produces a voltage because of the two different concentrations of zinc ions.
Zn(s) --> Zn2+ + 2e- ....... E = +0.763V
Zn2+ + 2e- --> Zn2+ ........E = -0.763V
The standard cell potential must be zero. But since the zinc ions are each at different concentrations, and neither is 1M, then there is a potential difference between the anode and cathode, albeit, rather small.
The Nernst equation...
.............. RT..... [C]^c [D]^d
E = E
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