Three voltaic cells can be constructed fromsolutionsPb(NO3)2(aq) and the corresponding metalelectrodes.ofCuso (aq),ZnSOa(aq),andReactionEZn?daa) + 2e s zn(s)-0,7626VPbaas +2e 5 Pb (S)- 0.1251 VCalculate the standard cell potential for eachvoltaic cell combination. For a spontaneousreaction, E'cell must be positive when E'anode issubtracted from E'cathode. Use the standardpotentlals from p. 119 for calculations.1.* 2e- ニ Cucs)0. 340 VAgčaa)e- 5 Ag(s)0.79912. Identify which metal electrode serves as thecathode and which metal electrode serves asthe anode.Tabulate the results from questions 1 and 2:E'cellCellAnodeCathodeCu/ZnCu/PbPb/Zn3.a. Using the Nernst Equation, calculate theexpected voltage (Etheo) for a cell whichconsists of 0.0300 M Pb(NOs)2(aq) and 0.0400M CuSO (aq).b. Glve the conventional cell notation for this cell,assuming a salt bridge separates the two half-cells.

Answered: Image /qna-images/answer/e1249205-60a8-4dc5-a026-1909d2dfa291.jpg

Three voltaic cells can be constructed from solutions of Cusoa(aq), ZnSOa(aq), and Reaction E Pb(NOs)2(aq) and the corresponding metal electrodes. Znaa) + 2e" s zn(s) - 0. 24 Pbaa) + 2e 5 Pb(s) 1. Calculate the standard cell potential for each voltaic cell combination. For a spontaneous reaction, E'cell must be positive when E'anode is subtracted from E'cathode. Use the standard potentlals from p. 119 for calculations. + 2e- ら Cu(s) Agiaa) + t- S Ag(s) 2. Identify which metal electrode serves as the cathode and which metal electrode serves as the anode. Tabulate the results from questions 1 and 2: Cathode Cell E'cll Anode Cu/Zn Cu/Pb Pb/Zn 3.a. Using the Nernst Equation, calculate the expected voltage (Etheo) for a cell which consists of 0.0300 M Pb(NO)z(aq) and 0.0400 M CuSO(aq). b. Glve the conventional cell notation for this cell, assuming a salt bridge separates the two half- cells.

Three voltaic cells can be constructed from solutions of Cusoa(aq), ZnSOa(aq), and Reaction E Pb(NOs)2(aq) and the corresponding metal electrodes. Znaa) + 2e" s zn(s) - 0. 24 Pbaa) + 2e 5 Pb(s) 1. Calculate the standard cell potential for each voltaic cell combination. For a spontaneous reaction, E'cell must be positive when E'anode is subtracted from E'cathode. Use the standard potentlals from p. 119 for calculations. + 2e- ら Cu(s) Agiaa) + t- S Ag(s) 2. Identify which metal electrode serves as the cathode and which metal electrode serves as the anode. Tabulate the results from questions 1 and 2: Cathode Cell E'cll Anode Cu/Zn Cu/Pb Pb/Zn 3.a. Using the Nernst Equation, calculate the expected voltage (Etheo) for a cell which consists of 0.0300 M Pb(NO)z(aq) and 0.0400 M CuSO(aq). b. Glve the conventional cell notation for this cell, assuming a salt bridge separates the two half- cells.

Principles of Modern Chemistry

8th Edition

ISBN:9781305079113

Author:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler

Publisher:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler

Chapter17: Electrochemistry

Section: Chapter Questions

Problem 77AP

See similar textbooks

Similar questions

The half-cells Ag+(aq. 1.0 M)|Ag(s) and H+(aq, ? M)|H2(1.0 bar) are linked by a salt bridge to create a voltaic cell. With the silver electrode as the cathode, a value of 0.902 V is recorded tor kcell at 298 K. Determine the concentration of H+ and the pH of the solution.
At 298 K, the solubility product constant for PbC2O4 is 8.5 1010, and the standard reduction potential of the Pb2+(aq) to Pb(s) is 0.126 V. (a) Find the standard potential of the half-reaction PbC2O4(s)+2ePb(s)+C2O42(aq) (Hint: The desired half-reaction is the sum of the equations for the solubility product and the reduction of Pb2+. Find G for these two reactions and add them to find G for their sum. Convert the G to the potential of the desired half-reaction.) (b) Calculate the potential of the Pb/PbC2O4 electrode in a 0.025 M solution of Na2C2O4.
At 298 K, the solubility product constant for Pb(IO3)2 is 2.6 1013, and the standard reduction potential of the Pb2+(aq) to Pb(s) is 0.126 V. (a) Find the standard potential of the half-reaction Pb(IO3)2(s)+2ePb(s)+2IO3(aq) (Hint: The desired half-reaction is the sum of the equations for the solubility product and the reduction of Pb2+. Find G for these two reactions, and add them to find G for their sum. Convert the G to the potential of the desired half-reaction.) (b) Calculate the potential of the Pb/Pb(IO3)2 electrode in a 3.5 103 M solution of NaIO3.
a Calculate G for the following cell reaction: Tl(s)Tl+(aq)Pb2+(aq)Pb(s) The Gf for Tl+(aq) is 32.4 kJ/mol. b From G, calculate the standard cell potential for the cell reaction and from this, determine the standard potential for Tl2+(aq)+eTl(s).
At 298 K, the solubility product constant for solid Ba(IO3)2 is 1.5 109. Use the standard reduction potential of Ba2+(aq) to find the standard potential for the half-reaction Ba(IO3)2(s)+2eBa(s)+2IO3(aq)
Halide ions can he deposited at a silver anode, the reaction being Ag(s) + X- AgX(s) +e- Suppose that a cell was formed by immersing a silver anode in an analyte solution that was 0.0250 M Cl-,Br-, and I -ions and connecting the half-cell to a saturated calomel cathode via a salt bridge. (a) Which halide would form first and at what potential? Is the cell galvanic or electrolytic? (b) Could I- and Br- be separated quantitatively? (Take 1.00 l0-5 M as the criterion for quantitative removal of an ion.) If a separation is feasible, what range of cell potential could he used? (c) Repeat part (b) for I- and Cl-. (d) Repeat part (b) for Br- and Cl-.
Calculate the theoretical potential of each of the following cells. Is the cell reaction spontaneous as written or spontaneous in the opposite direction? (a) Pt|Cr3+(2.00 10-4M),Cr2+(1.50 10-3 M)||Pb2+ (5.60 0215 10-2M)|Pb (b) Hg|Hg22+(2.00 10-2 M)||H+(1.50 10-2 M),V3+ (2.00 10-2M),VO2+(3.00 10-3M)|Pt (e) Pt|Fe3+(3.00 10-2 M), Fe2+ (4.00 10-5M)||Sn2+ (3.50 10-2M), Sn4+ (5.50 10-4 M)|Pt
Calculate the electrode potentials of the following half-cells. (a) Ag+(0.0436 M)|Ag (b) Fe3+ (5.34 10-4M),Fe2+ (0.090 M)|Pt (c) AgBr(sat’d),Br- (0.037 M)|Ag
For each of the reactions, calculate E from the table of standard potentials, and state whether the reaction is spontaneous as written or spontaneous in the reverse direction under standard conditions. (a) Zn(s)+Fe2+(aq)Zn2+(aq)+Fe(s) (b) AgCl(s)+Fe2+(aq)Ag(s)+Fe3+(aq)+Cl(aq) (c) Br2(l)+2Cl(aq)Cl2(g)+2Br(aq)
The standard potential of the cell reaction Ag+(aq)+Eu2+(aq)Ag(s)+Eu3+(aq) is E = +1.23 V. Use the tabulated standard potential of the silver half-reaction to find the standard reduction potential for the europium half-reaction.