Standard Electrode Potentials in Aqueous Solutions at 25◦ C and 1 atm

Cathode Half-Reaction Std Potential(V) Cathode Half-Reaction Std Potential(V)
Li+(aq) + e–   = Li(s)         -3.04 IO–(aq) + H2O(l) + 2 e– = I–(aq) + 2 OH–(aq) 0.49
Na+(aq) + e– = Na(s)         -2.71 Cu+(aq) + e– = Cu(s) 0.52
Mg2+(aq) + 2 e– = Mg(s)         -2.38 I2(s) + e– = 2 I–(aq) 0.54
Al3+(aq) + 3 e– = Al(s)         -1.66 Fe3+(aq) + e– = Fe2+(aq)         0.77
2 H2O(l) + 2 e– = H2(g) + 2 OH–(aq) -0.83 Hg22+(aq) + 2 e– = 2 Hg(l) 0.80
Zn2+(aq) + 2 e– = Zn(s)         -0.76 Ag+(aq) + e– = Ag(s)  0.80
Cr3+(aq) + 3 e– = Cr(s)         -0.74 Hg2+(aq) + 2 e– = Hg(l) 0.85
Fe2+(aq) + 2 e– = Fe(s)         -0.41 ClO–(aq) + H2O(l) + 2 e– = Cl–(aq) + 2 OH–(aq) 0.90
Cd2+(aq) + 2 e– = Cd(s)         -0.40 2 Hg2+(aq) + 2 e– = Hg22+(aq) 0.90
Ni2+(aq) + 2 e– = Ni(s)         -0.23 NO3–(aq) + 4 H+(aq)  + 3 e– = NO(g) + 2  H2O(l) 0.96
Sn2+(aq) + 2 e– = Sn(s)         -0.14 Br2(l) + 2 e– = 2 Br–(aq) 1.07
Pb2+(aq) + 2 e– = Pb(s)         -0.13 O2(g) +  4 H+(aq)  + 4 e– =   2  H2O(l) 1.23
Fe3+(aq) + 3 e– = Fe(s)         -0.04 Cr2O72-(aq) + 14 H+(aq) + e– = 2 Cr3+(aq) + 7 H2O(l) 1.33
2 H+(aq) + 2 e– = H2(g)         0.00 Cl2(g) + e– = 2 Cl–(aq) 1.36
Sn4+(aq) + 2 e– = Sn2+(aq)         0.15 MnO4–(aq) + 8 H+(aq)  + 5 e– = Mn2+(aq) + 4  H2O(l) 1.49
Cu2+(aq) + e– = Cu+(aq)         0.16 H2O2(aq) +  2 H+(aq)  + 2 e– =   2  H2O(l)   1.78
Cu2+(aq) + 2 e– = Cu(s)         0.34 S2O82-(aq) + 2 e– = 2 SO42-(aq) 2.01
    F2(g) + 2 e– = 2 F–(aq) 2.87

 

  1. A voltaic cell is constructed from the following half-cells: A nickel electrode in a 1.00 M solution of nickel(II) nitrate, and a zinc electrode in a 1.00 M solution of zinc nitrate solution. Which electrode is the cathode?
  2. Using standard electrode potentials provided in the link below, decide if the following reaction is spontaneous. The aqueous solutions are 1.00 M. To enter your answer click in the small circle in front of your choice.
    Sn(s) + Cd2+(aq) ==> Sn2+(aq) + Cd(s)
  3. A voltaic cell is constructed from the following half-cells: A chromium electrode in a 1.00 M solution of chromium(III) nitrate, and a silver electrode in a 1.00 M solution of silver nitrate solution. Cations in this cell will move towards which electrode?
  4. Using standard electrode potentials provided in the link below, decide if the following reaction is spontaneous. The aqueous solutions are 1.00 M. To enter your answer click in the small circle in front of your choice.
    Pb(s) + Ni2+(aq) ==> Pb2+(aq) + Ni(s)
  5. A voltaic cell is constructed from the following half-cells: A nickel electrode in a 1.00 M solution of nickel(II) nitrate, and a chromium electrode in a 1.00 M solution of chromium(III) nitrate solution. Which electrode is the anode?
  6. Using standard electrode potentials provided in the link below, decide if the following reaction is spontaneous. The aqueous solutions are 1.00 M. To enter your answer click in the small circle in front of your choice.
    Cd(s) + Ni2+(aq) ==> Cd2+(aq) + Ni(s)
  7. A voltaic cell is constructed from the following half-cells: A nickel electrode in a 1.00 M solution of nickel(II) nitrate, and a silver electrode in a 1.00 M solution of silver nitrate solution. Anions in this cell will move towards which electrode?
  8. Using standard electrode potentials provided in the link below, decide if the following reaction is spontaneous. The aqueous solutions are 1.00 M.

                   Ni(s) + Zn2+(aq) ==> Ni2+(aq) + Zn(s)

     9.  Using standard electrode potentials provided in the link below, decide if the following reaction is spontaneous. The aqueous solutions are 1.00 M.

                Cd(s) + Sn2+(aq) ==> Cd2+(aq) + Sn(s)

    10.  A voltaic cell is constructed from the following half-cells: A silver electrode in a 1.00 M solution of silver nitrate, and a copper electrode in a 1.00 M solution of copper(II) nitrate solution. Cations in this cell will move towards which electrode?

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