Consider the following half-reactions:F2(g) + 2 e ® 2 F"(aq)Cu2+(aq) + 2 e ® Cu(s)Sn2E° = +2.87 VE° = +0.337 VE° = -0.14 V*(aq) + 2 e ® Sn(s)AI3+(aq) + 3 e ® Al(s)E° = -1.66 VNa*(aq) + e¯ ® Na(s)E° = -2.714 VWhich of the above compounds or ions are able to reduce Al 3+?O a. F2 and F"O b. F2, Cu2+ and Sn2+c. Na onlyO d. F", Cu, and Sne. Nat and Na Consider the reaction:NH3 (g) + HCI (g)NH4CI (s)Given the following table of thermodynamic data,Substance AHf (kJ/mol) S° (J/mol - K)NH 3 (g)HCI (g)NH4C1 (s) -314.4-46.19192.5-92 30186.6994.6determine the temperature (in °C) above which the reaction is nonspontaneous.This reaction is spontaneous at all temperatures.618.1432.8345.01235

You have asked multiple type questions, we will solve only first questions for you. If you want any…

Consider the following half-reactions: F2(g) + 2 e ® 2 F(aq) E° = +2.87 V Cu2+(aq) + 2 e ® Cu(s) Sn2*(aq) + 2 e" ® Sn(s) Al3+(aq) + 3 e¯ ® Al(s) Na*(aq) + e ® Na(s) E° = +0.337 V E° = -0.14 V E° = -1.66 V E° = -2.714 V Which of the above compounds or ions are able to reduce Al 3+*? O a. F2 and F" b. F2, Cu2+ and Sn2+ c. Na only d. F", Cu, and Sn e. Nat and Na

Consider the following half-reactions: F2(g) + 2 e ® 2 F(aq) E° = +2.87 V Cu2+(aq) + 2 e ® Cu(s) Sn2(aq) + 2 e" ® Sn(s) Al3+(aq) + 3 e¯ ® Al(s) Na(aq) + e ® Na(s) E° = +0.337 V E° = -0.14 V E° = -1.66 V E° = -2.714 V Which of the above compounds or ions are able to reduce Al 3+*? O a. F2 and F" b. F2, Cu2+ and Sn2+ c. Na only d. F", Cu, and Sn e. Nat and Na

Chemistry

9th Edition

ISBN:9781133611097

Author:Steven S. Zumdahl

Publisher:Steven S. Zumdahl

Chapter18: Electrochemistry

Section: Chapter Questions

Problem 59E: Answer the following questions using data from Table 17-1 (all under standard conditions). a. Is...

See similar textbooks

Similar questions

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)?
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?
Answer the following questions using data from Table 17-1 (all under standard conditions). a. Is H+(aq) capable of oxidizing Cu(s) to Cu2+(aq)? b. Is Fe3+ (aq) capable of oxidizing I (aq)? c. Is H2(g) capable of reducing Ag+(aq)?
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+).
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, .
Calculate the theoretical potential of each of the following cells.Is the cell reaction spontaneous as written or spontaneous in the opposite direction? (a) Bi|BiO+ (0.0300 M),H+ (0.100 M)||I- (0.100 M), AgI(sat’d)|Ag (b) Zn|Zn2+(5.75 10-4M)||Fe(CN)64-(530 10-2 M),Fe(CN)63-(6.75 10-2M)|Pt (c) Pt,H2O (0.200 atm)|HCI(8.25 10-4M), AgCI(sat’d)| Ag
Consider a voltaic cell in which the following reaction occurs. Zn(s)+Sn2+(aq)Zn2+(aq)+Sn(s) (a) Calculate E° for the cell. (b) When the cell operates, what happens to the concentration of Zn2+? The concentration of Sn2+? (c) When the cell voltage drops to zero, what is the ratio of the concentration of Zn2+ to that of Sn2+? (d) If the concentration of both cations is 1.0 M originally, what are the concentrations when the voltage drops to zero?
An electrolysis experiment is performed to determine the value of the Faraday constant (number of coulombs per mole of electrons). In this experiment, 28.8 g of gold is plated out from a AuCN solution by running an electrolytic cell for two hours with a current of 2.00 A. What is the experimental value obtained for the Faraday Constant?
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.

Recommended textbooks for you

Chemistry

ISBN:

9781133611097

Author:

Steven S. Zumdahl

Publisher:

Cengage Learning

Chemistry

ISBN:

9781305957404

Author:

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

Publisher:

Cengage Learning

Chemistry: An Atoms First Approach

Chemistry

ISBN:

9781305079243

Author:

Steven S. Zumdahl, Susan A. Zumdahl

Publisher:

Cengage Learning

General Chemistry - Standalone book (MindTap Cour…

Chemistry

ISBN:

9781305580343

Author:

Steven D. Gammon, Ebbing, Darrell Ebbing, Steven D., Darrell; Gammon, Darrell Ebbing; Steven D. Gammon, Darrell D.; Gammon, Ebbing; Steven D. Gammon; Darrell

Publisher:

Cengage Learning

Chemistry: Principles and Reactions

Chemistry

ISBN:

9781305079373

Author:

William L. Masterton, Cecile N. Hurley

Publisher:

Cengage Learning

Chemistry: The Molecular Science

Chemistry

ISBN:

9781285199047

Author:

John W. Moore, Conrad L. Stanitski

Publisher:

Cengage Learning

Chemistry

ISBN:

9781133611097

Author:

Steven S. Zumdahl

Publisher:

Cengage Learning

Chemistry

ISBN:

9781305957404

Author:

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

Publisher:

Cengage Learning

Chemistry: An Atoms First Approach

Chemistry

ISBN:

9781305079243

Author:

Steven S. Zumdahl, Susan A. Zumdahl

Publisher:

Cengage Learning

General Chemistry - Standalone book (MindTap Cour…

Chemistry

ISBN:

9781305580343

Author:

Steven D. Gammon, Ebbing, Darrell Ebbing, Steven D., Darrell; Gammon, Darrell Ebbing; Steven D. Gammon, Darrell D.; Gammon, Ebbing; Steven D. Gammon; Darrell

Publisher:

Cengage Learning

Chemistry: Principles and Reactions

Chemistry

ISBN:

9781305079373

Author:

William L. Masterton, Cecile N. Hurley

Publisher:

Cengage Learning

Chemistry: The Molecular Science

Chemistry