Standard Reduction (Electrode) Potentials at 25 o C Standard Reduction (Electrod

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Standard Reduction (Electrode) Potentials at 25 oC

Standard Reduction (Electrode) Potentials at 25 oC

Standard Reduction (Electrode) Potentials at 25 oC

Half-Cell Reaction Eo (volts)

Standard Reduction (Electrode) Potentials at 25 oC

Half-Cell Reaction Eo (volts) F2(g) + 2 e- 2 F-(aq) 2.87 Ce4+(aq) + e- Ce3+(aq) 1.61 MnO4-(aq) + 8 H+(aq) + 5 e- Mn2+(aq) + 4 H2O(l) 1.51 Cl2(g) + 2 e- 2 Cl-(aq) 1.36 Cr2O72-(aq) + 14 H+(aq) + 6 e- 2 Cr3+(aq) + 7 H2O(l) 1.33 O2(g) + 4 H+(aq) + 4 e- 2 H2O(l) 1.229 Br2(l) + 2 e- 2 Br-(aq) 1.08 NO3-(aq) + 4 H+(aq) + 3 e- NO(g) + 2 H2O(l) 0.96 2 Hg2+(aq) + 2 e- Hg22+(aq) 0.920 Hg2+(aq) + 2 e- Hg(l) 0.855 O2(g) + 4 H+(aq, 10-7 M) + 4 e- 2 H2O(l) 0.82 Ag+(aq) + e- Ag(s) 0.799 Hg22+(aq) + 2 e- 2 Hg(l) 0.789 Fe3+(aq) + e- Fe2+(aq) 0.771 I2(s) + 2 e- 2 I-(aq) 0.535 Fe(CN)63-(aq) + e- Fe(CN)64-(aq) 0.48 Cu2+(aq) + 2 e- Cu(s) 0.337 Cu2+(aq) + e- Cu+(aq) 0.153 S(s) + 2 H+(aq) + 2 e- H2S(aq) 0.14 2 H+(aq) + 2 e- H2(g) 0.0000 Pb2+(aq) + 2 e- Pb(s) -0.126 Sn2+(aq) + 2 e- Sn(s) -0.14 Ni2+(aq) + 2 e- Ni(s) -0.25 Co2+(aq) + 2 e- Co(s) -0.28 Cd2+(aq) + 2 e- Cd(s) -0.403 Cr3+(aq) + e- Cr2+(aq) -0.41 2 H2O(l) + 2 e- H2(g) + 2 OH-(aq, 10-7 M) -0.41 Fe2+(aq) + 2 e- Fe(s) -0.44 Cr3+(aq) + 3 e- Cr(s) -0.74 Zn2+(aq) + 2 e- Zn(s) -0.763 2 H2O(l) + 2 e- H2(g) + 2 OH-(aq) -0.83 Mn2+(aq) + 2 e- Mn(s) -1.18 Al3+(aq) + 3 e- Al(s) -1.66 Mg2+(aq) + 2 e- Mg(s) -2.37 Na+(aq) + e- Na(s) -2.714 K+(aq) + e- K(s) -2.925 Li+(aq) + e- Li(s) -3.045 A voltaic cell is constructed from a standard H^+|H_2 half cell and a standard Ni^2+|Ni half cell The anode reaction is: The cathode reaction is: The spontaneous cell reaction is: The cell voltage is V.

Explanation / Answer

The half cell which is having less reduction potential undergoes oxidation at anode and the other undergoes reduction at cathode.

The reduction potential of H+/H2 is more than Ni2+/Ni ,

Anode Half Reaction:

Ni (s) ------------> Ni2+ (aq.) + 2 e-

Cathode Half Reaction :

2 H+ (aq.) + 2 e- -----------> H2 (g)

Spontaneous cell reaction:

2 H+ (aq.) + Ni (s) -----------> Ni2+ (aq.) + H2 (g)

E0cell = E0cathode - E0anode

E0cell = 0.000 - ( - 0.250)

E0cell = + 0.250 V

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