33. Calculate the copper(II) ion concentration at 25 °C in the cell Zn(s) + Cu²*(aq) → Zn²"(aq, 1.0 M) + Cu(s) if the measured cell potential is 1.06 V. The standard cell potential of the above electrochemical reaction is 1.10 V. The concentration of Zn2"(aq) is 1.0 M. a) 0.044 M b) 0.21 M c) 1.0 M d) 4.74 M e) 22.7 M f) none of the above

8. Suppose that the concentrations of NaF and KCI were each 0.10 M in the cell Pb(s) PbF₂(s) F (aq)||Cl(aq)| AgCl(s) Ag(s) Using the half-reactions 2 AgCl(s) + 2e = 2Ag(s) + 2Cl and PbF2(s) +2e = Pb(s) + 2F- and, calculate the cell voltage.

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

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