Four voltaic cells are set up. In each, one half-cell contains a standard hydrogen electrode (SHE). The second half-cell is one of the following.2+• Sr" (ag, 1.0 M) | Sr(s)• Cr" (ag, 1.0 M)| Cr(s)(aq, 1.0 M) | V(8)Hg2 (ag, 1.0 M) | Hg(1)2+2+(a) In which of the voltaic cells does the hydrogen electrode serve as the cathode?2+SHE & Sr (aq, 1.0 M) | Sr(s)2+SHE & Cr (ag, 1.0 M) | Cr(s)2+SHE & V" (aq, 1.0 M) | V(s)2+SHE & Hg, (aq, 1.0 M) | Hg(1)(b) Which voltaic cell produces the highest voltage? Which produces the lowest voltage?- half-cell. The lowest voltage willThe highest voltage will be produced by combining the SHE and theSHE and thehalf-cell.O O O

Answered: Image /qna-images/answer/131abe28-d8fc-4e09-9c73-0ae3d97cfbc3.jpg

(a) In which of the voltaic cells does the hydrogen electrode serve as the cathode? 2+ SHE & Sr (aq, 1.0 M) | Sr(s) 2+ O SHE & Cr (aq, 1.0 M) | Cr(s) O SHE & V2+ (ag, 1.0 M) | V(s) 2+ O SHE & Hg, (aq, 1.0 M) | Hg(1) (b) Which voltaic cell produces the highest voltage? Which produces the lowest voltage? - half-cell. The lowest voltage will The highest voltage will be produced by combining the SHE and the SHE and the half-cell.

(a) In which of the voltaic cells does the hydrogen electrode serve as the cathode? 2+ SHE & Sr (aq, 1.0 M) | Sr(s) 2+ O SHE & Cr (aq, 1.0 M) | Cr(s) O SHE & V2+ (ag, 1.0 M) | V(s) 2+ O SHE & Hg, (aq, 1.0 M) | Hg(1) (b) Which voltaic cell produces the highest voltage? Which produces the lowest voltage? - half-cell. The lowest voltage will The highest voltage will be produced by combining the SHE and the SHE and the half-cell.

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

See similar textbooks

Similar questions

The following cell has a potential of 0.10 V at 25oC. Ni(s) | Ni2+(aq) (1.0 M) || H+ (? M) | H2(g) (1.0 atm) | Pt(s) What is the pH of the solution in the cathode compartment? Your answer should go to two places past the decimal (i.e. 9.22)
9) The standard cell potential (E°cell) for the voltaic cell based on the reaction below is_ 3Fe2+ (aq) + Cr³+ (aq) C) +1.57 Cr (s) + 3Fe3+ (aq) A) -1.45 B) +1.51 D) +2.99 V. E) +3.05
For a standard voltaic cell comprised of a Cu2+|Cu electrode and a Fe2+|Fe electrode, what is the cell potential, in volts?
A galvanic cell was constructed where one electrode was a Cu2+(aq)|Cu(s) electrode and the other was an M2+(aq)|M(s) electrode. The potential difference between the two electrodes was measured to be 1.65 V with the copper electrode being the more positive electrode. What is the potential of the M2+(aq)|M(s) electrode with respect to the standard hydrogen electrode? Data: E°(Cu2+(aq)|Cu(s)) = +0.34 V
The potential of the following voltaic cell is 0.55 V. Given this information, determinethe Kb for the organic base (RNH2) dissolved in the left cell.
Consider the reaction corresponding to a voltaic cell and its standard cell potential. Zn(s)+Cu2+(aq)⟶Cu(s) +Zn2+(aq) Eocell=1.1032 V What is the cell potential for a cell with a 2.214 M solution of Zn2+(aq) and 0.1456 M solution of Cu2+(aq) at 437.7 K?
Four voltaic cells are set up. In each, one half-cell contains a standard hydrogen electrode (SHE). The second half-cell is one of the following. 2+ • Cr" (aq, 1.0 M) | Cr(s) 3+ Al" (ag, 1.0 M) | Al(s) 2+ • Ca" (aq, 1.0 M) | Ca(s) 2+ Hg2" (aq, 1.0 M) | Hg(1) (a) In which of the voltaic cells does the hydrogen electrode serve as the cathode? 2+ O SHE & Cr´" (aq, 1.0 M) | Cr(s) ,3+ O SHE & Alº" (aq, 1.0 M) | Al(s) 2+ O SHE & Ca" ' (aq, 1.0 M) | Ca(s) 2+ O SHE & Hg," (aq, 1.0 M) | Hg(1) (b) Which voltaic cell produces the highest voltage? Which produces the lowest voltage? The highest voltage will be produced by combining the SHE and the half-cell. The lowest voltage will be produced by combining the SHE and the v half-cell.
A student wishes to determine the chloride ion concentration in a water sample at 25 \deg C using a galvanic cell constructed with a graphite electrode and a half - cell of AgCl(s) + e¯ - > Ag(s ) + Cl(aq) E\deg red = 0.2223 V And a copper electrode with 0.500 M Cu^2+ as the second half cell Cu^2+ (aq) + 2 e¯ - > Cu(s) E\deg red = 0.337 V The measured cell potential when the water sample was placed into the silver side of the cell was 0.0781 V. Given the standard cell potential for this cell is 0.115 V, and the measured cell potential is 0.0781, what is the concentration of chloride ions in the solution?
+2 t- 4) Consider the following redox reactions and their standard cell potentials: (acidic conditions) (basic conditions) S,0, (aq) + Cl2(g) = HCI0(aq) + So,"(aq) (acidic conditions) cell =-1.31 V E°cell = +0.10 V E° cell = +0.37 V E°. C2(g) + Bio*(aq) = Bi(s)+ HCIO(aq) So(aq) + 03(g) = S20 (aq) + 02(g) a) Using the ½ rxn method, balance the three redox reactions under the conditions indicated. b) Write each balanced redox reaction in the spontaneous direction and indicate its corresponding standard cell potential. c) Between these 3 redox reactions there are FOUR oxidizing agents and FOUR reducing agents. (Hint: You may need to consider the balanced equations.) i) Place the FOUR oxidizing agents in order of decreasing oxidizing strength. (From the strongest OA to the weakest OA.) ii) Place the FOUR reducing agents in order of decreasing reducing strength. ( (From the strongest RA to the weakest RA.)