Question

1. Write the half reactions that occur at the anode and cathode in these electrochemical cells. Annotate which half reaction occurs at the anode and the cathode.

2. Write the overall balance reaction for the following electrochemical cells.

Ag(s), Ag(NO3)2 (1.0 M) || Cu (s), CuCl2 (1.0M)

Zn(s), Zn(NO3)2 (1.0M) || Ni (s), Ni(NO3)2 (1.0M)

Zn(s), Zn(NO3)2 (0.3 M) || Cu(s), CuCl2 (0.5M)

Ag(s), Ag(NO3)2 (0.3 M) || Cu(s), CuCl2 (0.5 M)

Ag(s), Ag(NO3)2 (0.3 M) || Ni(s), Ni(NO3)2 (0.5 M)

Cu(s), CuCl2 (.001 M) || Cu(s), CuCl2 (1.0 M)

Thank you!!!

Answer 1

(i) Ag(s), Ag(NO3)2 (1.0 M) || Cu (s), CuCl2 (1.0M)
1.
Anode half reaction: Ag(s) -> Ag(+2) + 2e-
cathode half reaction: Cu(+2) + 2e- -> Cu(s)

2. overall balanced redox reaction
Ag(s) + Cu(+2) -> Ag(+2) + Cu(s)

(ii) Zn(s), Zn(NO3)2 (1.0M) || Ni (s), Ni(NO3)2 (1.0M)
1.
Anode half reaction:   Zn(s) -> Zn(+2) + 2e-
cathode half reaction: Ni(+2) + 2e- -> Ni(s)

2. overall balanced redox reaction
Zn(s) + Ni(+2) -> Zn(+2) + Ni(s)

(iii) Zn(s), Zn(NO3)2 (0.3 M) || Cu(s), CuCl2 (0.5M)
1.
Anode half reaction: Zn(s) -> Zn(+2) + 2e-
cathode half reaction: Cu(+2) + 2e- -> Cu(s)

2. overall balanced redox reaction
Zn(s) + Cu(+2)   -> Zn(+2) + Cu(s)

(iv) Ag(s), Ag(NO3)2 (0.3 M) || Cu(s), CuCl2 (0.5 M)
1.
Anode half reaction: Ag(s) -> Ag(+2) + 2e-
cathode half reaction: Cu(+2) + 2e- -> Cu(s)

2. overall balanced redox reaction
Ag(s) + Cu(+2)   -> Ag(+2) + Cu(s)

(v) Ag(s), Ag(NO3)2 (0.3 M) || Ni(s), Ni(NO3)2 (0.5 M)
1.
Anode half reaction: Ag(s) -> Ag(+2) + 2e-
cathode half reaction: Ni(s) -> Ni(+2) + 2e-

2. overall balanced redox reaction
Ag(s) + Cu(+2)   -> Ag(+2) + Cu(s)

(vi) Cu(s), CuCl2 (.001 M) || Cu(s), CuCl2 (1.0 M)
1.
Anode half reaction: Cu(s) -> Cu(+2) + 2e- -> Cu(s)
cathode half reaction: Cu(+2) + 2e- -> Cu(s)

2. overall balanced redox reaction
Cu(s) + Cu(+2)   -> Cu(+2) + Cu(s)