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+Pd" (aq, 1.0 M) | Pd(s)2+Sr" (ag, 1.0 M) | Sr(s)3+Al" (ag, 1.0 M) | Al(s)3+. Ст (ад, 1.0 м) | Cr(s)(a) In which of the voltaic cells does the hydrogen electrode serve as the cathode?2+O SHE & Pd´" (aq, 1.0 M) | Pd(s)2+O SHE & Sr°' (aq, 1.0 M) | Sr(s)O SHE & Al°™ (aq, 1.0 M) | Al(s)3+O SHE & Cr" (aq, 1.0 M) | Cr(s)(b) Which voltaic cell produces the highest voltage? Which produces the lowest voltage?The highest voltage will be produced by combining the SHE and thehalf-cell. The lowest voltage will be produced by combining the SHE and the- half-cell.

Answered: Image /qna-images/answer/244a58ab-f0a3-432f-ba75-c6342b59b650.jpg

roltaic 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+ Pd" (aq, 1.0 M) | Pd(s) 2+ Sr* (aq, 1.0 M) | Sr(s) Al* (aq, 1.0 M) | Al(s) (aq, 1.0 M) | Cr(s) In which of the voltaic cells does the hydrogen electrode serve as the cathode? O SHE & Pd*+* (aq, 1.0 M) | Pd(s) 2+ O SHE & Sr* (aq, 1.0 M) | Sr(s) O SHE & AI+ (aq, 1.0 M) | Al(s) 3+ O SHE & Cr" (aq, 1.0 M) | Cr(s) 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 - half-cell.

roltaic 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+ Pd" (aq, 1.0 M) | Pd(s) 2+ Sr* (aq, 1.0 M) | Sr(s) Al* (aq, 1.0 M) | Al(s) (aq, 1.0 M) | Cr(s) In which of the voltaic cells does the hydrogen electrode serve as the cathode? O SHE & Pd+ (aq, 1.0 M) | Pd(s) 2+ O SHE & Sr* (aq, 1.0 M) | Sr(s) O SHE & AI+ (aq, 1.0 M) | Al(s) 3+ O SHE & Cr" (aq, 1.0 M) | Cr(s) 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 - half-cell.

Fundamentals Of Analytical Chemistry

9th Edition

ISBN:9781285640686

Author:Skoog

Publisher:Skoog

Chapter18: Introduction To Electrochemistry

Section: Chapter Questions

Problem 18.18QAP

See similar textbooks

Similar questions

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)
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-.
Consider the following galvanic cell: A 15 0-mole sample of NH is added to the Ag compartment (assume 1.00 L of total solution after the addition). The silver ion reacts with ammonia to form complex ions as shown: Ag+(aq)+NH3(aq)AgNH3+(aq)K1=2.1103AgNH3+(aq)+NH3(aq)Ag(NH3)2+(aq)K2=8.2103 Calculate the cell potential after the addition of 15.0 moles of NH3.
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
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).
From the information provided, use cell notation to describe the following systems: (a) In one half-cell, a solution of Pt(NO3)2 forms Pt metal, while in the other half-Cell, Cu metal goes into a.Cu(NO3)2 solution with all solute concentrations 1 M. (b) The cathode consists of a gold electrode in a 0.55 M Au(NO3)3 solution and the anode is a magnesium electrode in 0.75 M Mg(NO3)2 solution. (c) One half-cell consists of a silver electrode in a 1 M AgNO3 solution, and in the other half-cell, a copper Electrode in 1 M Cu(NO3)2 is oxidized.
Calculate the standard cell potential of the following cell at 25C. Cr(s)Cr3(aq)Hg22(aq)Hg(l)
The cell potential of the following cell at 25C is 0.480 V. ZnZn2+(1M)H+(testsolution)H2(1atm)Pt What is the pH of the test solution?