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Wize University Chemistry Textbook > Electrochemistry

Cell Notation

Galvanic Cells Previous Section
Important Equations + Nonstandard conditions (Nernst Equation) Next Section
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Cell Diagram

  • The cell diagram aka standard cell notation is as follows:
| Anode | Ions from anode || Ions to cathode | Cathode |\text{| Anode | Ions from anode || Ions to cathode | Cathode |}

If we wanted to write this notation for the galvanic cell we just drew...
  • These were the 2 half reactions that were involved:
Zn(s) -> Zn2+ (aq) + 2e- Eoox=+0.76
Cu2+(aq) + 2e- -> Cu(s) Eored=+0.34

| Zn(s) | Zn2+(aq) || Cu2+(aq) | Cu(s) |

  • It can also be called standard cell notation because it is describing SATP:
    25
    C,
    1
    atm, [
    1
    M]
  • Note that if a half cell does not contain a solid species then an inert electrode must be used. eg. Pt(s)
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Write the cell notation for the voltaic (or galvanic) cell that incorporates the following redox reaction:

Al(s)+Cr(aq)3+→Al(aq)3++Cr(s)Al_{(s)}+Cr^{3+}_{(aq)} \to Al^{3+}_{(aq)}+Cr_{(s)}
Al3+ +3e -> Al(s) Eored=-1.66V
Cr3+ + 3e- -> Cr(s) Eored=-0.73V
In a zinc-lead cell the reaction is:

Pb2+(aq)+Zn(s)→Pb(s)+Zn2+(aq)       E°=0.637VPb^{2+}\left(aq\right)+Zn\left(s\right)\to Pb\left(s\right)+Zn^{2+}\left(aq\right)\ \ \ \ \ \ \ E\degree=0.637V

Which of the following statements about this cell is FALSE?