Step 1. Write the two half-cell reactions and determine the half-cell potentials (refer to the Standard Reduction Potential Table)
Ni2+(aq) + 2 e-→ Ni(s) E° = -0.230 V
Co2+(aq) + 2 e- → Co(s) E° = -0.277 V
Step 2. Identify the reduction half-reaction (cathode) and the anode half-reaction (anode)
Co2+(aq) + 2 e- → Co(s) E° = -0.277 V ↓ E° → oxidation → anode
Ni2+(aq) + 2 e-→ Ni(s) E° = -0.230 V ↑ E° → reduction → cathode
Step 3. Get the overall reaction by balancing the number of electrons transferred then adding the oxidation half-reaction and reduction half-reaction.
lose electrons → oxidation → anode
gain electrons → reduction → cathode
A voltaic cell with Ni/Ni 2+ and Co/Co2+ half-cells has the following initial concentrations: [Ni2+] = 0.80 M; [Co 2+] = 0.20 M.
(a) What is the initial Ecell?
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Our data indicates that this problem or a close variation was asked in Chemistry: The Molecular Nature of Matter and Change - Silberberg 8th Edition. You can also practice Chemistry: The Molecular Nature of Matter and Change - Silberberg 8th Edition practice problems.