Write the cell notation for each of the electrochemical cells described below. Remember to include passive electrodes if gases are present.a. 2 Ag^+ (aq) + Pb (s) → 2 Ag (s) + Pb^2+ (aq)b. 2 ClO2 (g) + 2 I^- (aq) → 2 ClO2^- (aq) + I2 (s)c. Ni^2+ (aq) + Mg (s) → Ni (s) + Mg^2+ (aq)
a. Pb(s)|Pb^2+(aq)||Ag^+(aq)|Ag(s)b. Pt(s)|I^-(aq)|I(s)||ClO2(g)|ClO2^-(aq)|Pt(s)c. Mg(s)|Mg^2+(aq)||Ni^2+(aq)|Ni(s)
a. The cell notation for the given electrochemical cell is:
Pb(s) | Pb^2+(aq) || Ag^+(aq) | Ag(s)
Note that the anode is Pb(s) and the cathode is Ag(s).
b. The cell notation for the given electrochemical cell is:
Pt(s) | I^-(aq) || ClO2(g) | ClO2^-(aq), I2(s)
Note that since ClO2(g) is a gas, it is represented by a Pt electrode as a passive electrode. The anode is I^-(aq) and the cathode is ClO2^-(aq) on the Pt electrode.
c. The cell notation for the given electrochemical cell is:
Mg(s) | Mg^2+(aq) || Ni^2+(aq) | Ni(s)
Note that the anode is Mg(s) and the cathode is Ni(s).
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