4 Consider the hydrogen-oxygen fuel cell whereH2(g) + O2(g) = H20() DG° = -237.18 kJ/mol H2Which of the following statements is(are) true?1.At standard conditions, the maximum work the fuel cell could do on thesurroundingsis 237.18 kJ/mol.II.In the real world, the actual amount of useful work the cell can do is less than237.18 kJ.I.More energy is dissipated as waste heat in the fuel cell than in the reversiblepathway.Select one:O a. Ib. IIO c. None of the statements is true.d. IO e. I, II, and IIIn which of the following cases can E° be equal to zero?1.In any cell at equilibriumII. In a concentration cellI. E° can never be equal to zero.Select one:a. I onlyO b. IIO c. I and ||O d. Il only The standard free energies of formation of several aqueous species arekJ/molH*(aq)H20()CH;OH(aq)HCOOH(aq)-237-163-351eWhat is the standard reduction potential of methanoic acid in aqueous solution (that is,for HCOOH + 4H* + 4e ® CH;OH + H;O)?Select one:О а. +0.13 VO b. -0.13 VO c. +0.17 VO d. -0.25 VO e. +0.25 VWhich of the following is the best reducing agent?Cl, + 2e ® 2CrMg? + 2e ® MgE° = 1.36 VE = -2.37 V2H* + 2e ® H2E° = 0.00 VSelect one:O a. MgO b. Cl2Oc. Mg?+O d. crO e. H2How many minutes will take to plate out 140.00 g of Ni form a solution of NISO, using acurrent of 2.250 amp? (1C = 1Ax1s)Select one:O a. 3409 minO b. 478 minO c. 2226 minO d. 461 min

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Consider the hydrogen-oxygen fuel cell where H2(g) + O2(g) = H20() DG° = -237.18 kJ/mol H2 Which of the following statements is(are) true? 1. At standard conditions, the maximum work the fuel cell could do on the surroundings is 237.18 kJ/mol. II. In the real world, the actual amount of useful work the cell can do is less than 237.18 kJ. More energy is dissipated as waste heat in the fuel cell than in the reversible pathway. II. Select one: O a. I O b. II O c. None of the statements is true. O d.I O e. 1, II, and II In which of the following cases can E° be equal to zero? In any cell at equilibrium II. In a concentration cell II. E° can never be equal to zero. 1. Select one: O a. T only O b. II O c. I and || O d. Il only

Consider the hydrogen-oxygen fuel cell where H2(g) + O2(g) = H20() DG° = -237.18 kJ/mol H2 Which of the following statements is(are) true? 1. At standard conditions, the maximum work the fuel cell could do on the surroundings is 237.18 kJ/mol. II. In the real world, the actual amount of useful work the cell can do is less than 237.18 kJ. More energy is dissipated as waste heat in the fuel cell than in the reversible pathway. II. Select one: O a. I O b. II O c. None of the statements is true. O d.I O e. 1, II, and II In which of the following cases can E° be equal to zero? In any cell at equilibrium II. In a concentration cell II. E° can never be equal to zero. 1. Select one: O a. T only O b. II O c. I and || O d. Il only

Chemistry: An Atoms First Approach

2nd Edition

ISBN:9781305079243

Author:Steven S. Zumdahl, Susan A. Zumdahl

Publisher:Steven S. Zumdahl, Susan A. Zumdahl

Chapter17: Electrochemistry

Section: Chapter Questions

Problem 135CWP: Consider a galvanic cell based on the following half-reactions: a. What is the expected cell...

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Consider a galvanic cell based on the following half-reactions: a. What is the expected cell potential with all components in their standard states? b. What is the oxidizing agent in the overall cell reaction? c. What substances make up the anode compartment? d. In the standard cell, in which direction do the electrons flow? e. How many electrons are transferred per unit of cell reaction? f. If this cell is set up at 25C with [Fe2+] = 2.00 104 M and [La3+] = 3.00 103 M, what is the expected cell potential?
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).
The mass of three different metal electrodes, each from a different galvanic cell, were determined before and after the current generated by the oxidation-reduction reaction in each cell was allowed to flow for a few minutes. The first metal electrode, given the label A, was found to have increased in mass; the second metal electrode, given the label B, did not change in mass; and the third metal electrode, given the label C, was found to have lost mass. Make an educated guess as to which electrodes were active and which were inert electrodes, and which were anode(s) and which were the cathode(s).
Consider the following galvanic cell at 25C: Pt|Cr2+(0.30M),Cr3+(2.0M)||Co2+(0.20M)|Co The overall reaction and equilibrium constant value are 2Cr2+(aq)+Co2+(aq)2Cr3+(aq)+Co(s)K=2.79107 Calculate the cell potential, for this galvanic cell and G for the cell reaction at these conditions.
An aqueous solution of an unknown salt of gold is electrolyzed by a current of 2.75 amps for 3.39 hours. The electroplating is carried out with an efficiency of 93.0%, resulting in a deposit of 21.221 g of gold. a How many faradays are required to deposit the gold? b What is the charge on the gold ions (based on your calculations)?
For each reaction listed, determine its standard cell potential at 25 C and whether the reaction is spontaneous at standard conditions. (a) Mg(s)+Ni2+(aq)Mg2+(aq)+Ni(s) (b) 2Ag+(aq)+Cu(s)Cu2+(aq)+2Ag(s) (c) Mn(s)+Sn(NO3)2(aq)Mn(NO3)2(aq)+Sn(s) (d) 3Fe(NO3)2(aq)+Au(NO3)3(aq)3Fe(NO3)3(aq)+Au(s)
Consider a voltaic cell in which the following reaction takes place in basic medium at 25°C. 2NO3-(aq)+3S2(aq)+4H2O3S(s)+2NO(g)+8OH(aq) (a) Calculate E°. (b) Write the Nernst equation for the cell E. (c) Calculate E under the following conditions: PNO=0.994atm,ph=13.7,[S2]=0.154M,[NO3-]=0.472M, .
Consider the voltaic cell 2 Ag+(aq) + Cd(s) 2 Ag(s) + Cd2+(aq) operating at 298 K. (a) Calculate the Ecell for this cell. (b) If (cone. Cd2+) = 2.0 M and (cone. Ag+) = 0.25 M, calculate Ecell. (c) If Ecell = 1.25 V and (cone. Cd2+) = 0.100 M, calculate(cone. Ag+).