1. Given the following notation for an electrochemical cell Pt(s) | H2(g) | H+(aq) || Ag+(aq) | Ag(s), what is the balanced overall (net) cell reaction? a. 2H+(aq) + 2Ag+(aq) →H2(g) + 2Ag(s) b. H2(g) + 2Ag(s) →H+(aq) + 2Ag+(aq) c. 2H+(aq) + 2Ag(s) →H2(g) + 2Ag+(aq) d. H2(g) + Ag+(aq) →H+(aq) + Ag(s) E. H2(g) + 2Ag+(aq) →2H+(aq) + 2Ag(s) 2. Which choice lists all of the following species that can oxidize H2O to O2(g) under standard-state conditions? (2H2O(l) →O2(g) + 4H+(aq) + 4e-) MnO4-(aq), Cl2(g), Pb2+(aq), Cl-(aq), Ag+(aq) a. Cl-(aq) only b. Cl2(g) only c. Pb2+(aq) and Ag+(aq) d. Cl-(aq) andMnO4-(aq) E. E.MnO4-(aq) and Cl2(g) 3. Consider the following standard reduction potentials in acid solution: The strongest oxidizing agentlisted above is a. Cr3+. b. Cr. c. C.Mn2+. d. Co2+. E. E.MnO4-. 4. A battery is constructed by placing copper and lead electrodes in contact with 1.0 molar CuSO4(aq) and Pb(NO3)2(aq) solutions, respectively. If sulfuric acid is then added to the Pb(NO3)2solution, thereby forming a precipitate of PbSO4, what will happen to the cell potential? The cell potential will increase. 5. A current of 2.50 A was passed through an electrolytic cell containing molten CaCl2for 4.50 hours. How many moles of calcium metal should be deposited? a. 5.83 ×10-5mol B. 0.210 mol c. 0.420 mol d. 0.840 mol e. 1.95 ×109mol
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