Question

Write the cell notation for an electrochemical cell consisting of an anode where Ni(s) is oxidized to Ni2+(aq) and a cathode where Fe3+(aq) is reduced to Fe2+(aq) at a platinum electrode. Assume all aqueous solutions have a concentration of 1 mol/L and gases have a pressure of 1 bar.

Write the cell notation for an electrochemical cell consisting of an anode where Zn (s) is oxidized to Zn²⁺(aq) and a cathode where Ag⁺(aq) is reduced to Ag (s) . Assume all aqueous solutions have a concentration of 1 mol/L.

Write the cell notation for an electrochemical cell consisting of an anode where Cr²⁺(aq) is oxidized to Cr³⁺(aq) at a platinum electrode and a cathode where Ni²⁺(aq) is reduced to Ni (s) . Assume all aqueous solutions have a concentration of 1 mol/L and gases have a pressure of 1 bar.

Answer 1

General cell notation : M/M^+n // M^+n/M

                         oxidation(anode) // reduction(cathode)                         ( // inidicates salt bridge)

1. Ni(s)/Ni^2+(aq)//Fe^3+(aq)/Fe(s)

2. Zn(s)/Zn^2+(aq)//Ag^+(aq)/Ag(s)

3. Cr^2+(aq)/Cr^3+(aq)/Ni^2+(aq)/Ni(s)