Write the cell reaction and electrode half-reactions and calculate the standard potential of each the following cells:(i) Pt(s)|Cl2(g)| HCl(aq)||K2CrO4(aq)|Ag2CrO4(s)|Ag(s)(ii) Pt(s)|Fe3+(aq),Fe2+(aq)||Sn4+(aq),Sn2+(aq)|Pt(s)(iii) Cu(s)|Cu2+(aq)||Mn2+(aq),H+(aq)|MnO2(s)|Pt(s)

For the cell shown, the measured cell potential, Ecell, is –0.3521 V at 25 °C. Pt(s) | H,(g, 0.785 atm) | H* (aq, ? M) || Cd²*(aq, 1.00 M) | Cd(s) The balanced reduction half-reactions for the cell, and their respective standard reduction potential values, E°, are 2H* (aq) + 2e- - H, (g) E° = 0.00 V Cd²* (aq) + 2e" - Cd(s) E° = -0.403 V Calculate the H* concentration. [H*] = M

The standard cell potential for the reactions Sn(s) + CuSO4(aq) → Cu(s) + SnSO4(aq) at 25 °C exceeds +0.20V

A galvanic cell Mn(s)|Mn2+(aq) || Pb2+(aq)|Pb(s) is constructed using a completely immersed Mn electrode that weighs 34.9 g and a Pb electrode immersed in 532 mL of 1.00 M Pb2+(ag) solution. A steady current of 0.0519 A is drawn from the cell as the electrons move from the Mn electrode to the Pb electrode. (a) Which reactant is the limiting reactant in this cell? Enter symbol (b) How long does it take for the cell to be completely discharged? (c) How much mass has the Pb electrode gained when the cell is completely discharged? g (d) What is the concentration of the Pb2+(aq) when the cell is completely discharged? (Assume that the limiting reactant is 100% reacted.) M