A electrochemical cell is made by considering the following unbalanced redoxreaction:Pb2+(aq) + Fe(s) → Fe3+(aq) + Pb(s)The cell voltage, Ecell, at 298 K, when [Pb2+] = 0.25 M and [Fe3+] = 0.15 M, isnonspontaneous?Is the reaction spontaneous or

Thank you,Please rate my response.

Answered: A electrochemical cell is made by…

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

Calculate the cell potential, at 298 K, for the following reaction under the conditions given.Pb(s) + Fe2+(aq, 0.0100 M) → Pb2+(aq, 0.150 M) + Fe(s) Pb2+(aq) + 2 e‒ → Pb(s) E°red = ‒0.13 VFe2+(aq) + 2 e‒ → Fe(s) E°red = ‒0.44 V Group of answer choices: ‒0.75 V ‒0.80 V ‒0.34 V ‒0.27 V ‒0.44 V ‒0.50 V
A galvanic cell at a temperature of 25.0 °C is powered by the following redox reaction: 3Cu2+ +2Al(s). (aq) + 2Al (s) 3Cu (s) + 2 Al³+ (aq) Suppose the cell is prepared with 5.70 M Cu2+ in one half-cell and 5.24 M A13+ in the other. Calculate the cell voltage under these conditions. Round your answer to 3 significant digits. ☐ x10 μ ロ・ロ

The chemical reaction that causes iron to corrode in air is given by: 4Fe+3O2→2Fe2O3 in which at 298 K, ΔHorxn = −1684 kJ and ΔSorxn = −543.7 J/K At what temperature Teq do the forward and reverse corrosion reactions occur in equilibrium?
Consider a galvanic electrochemical cell constructed using Cr/Cr³⁺ and Zn/Zn²⁺ at 25 °C. The following half-reactions are provided for each metal: Cr³⁺(aq) + 3 e⁻ → Cr(s) E°red = -0.744 V Zn²⁺(aq) + 2 e⁻ → Zn(s) E°red = -0.763 V Given that the standard cell potential is 0.019 V and the overall equation is 2 Cr³⁺ (aq) + 3 Zn (s) → 2 Cr (s) + 3 Zn²⁺ (aq), what is the cell potential for this cell at 25 °C when [Zn²⁺] = 0.0323 M and [Cr³⁺] = 0.1736 M?
The free energy change for the following reaction at 25 °C, when [Pb2+] = 3.82×10-3 M and [Cu2+] = 1.20 M, is 68.1 kJ: Pb2+(3.82×10-3 M) + 2Cu+(aq)Pb(s) + 2Cu2+(1.20 M) ΔG = 68.1 kJ What is the cell potential for the reaction as written under these conditions? Answer: V Would this reaction be spontaneous in the forward or the reverse direction?
The cell potential for a voltaic cell composed of zinc and copper is 1.0 V under standard conditions. Zn(s) + Cu2+(aq) => Cu(S) + Zn2+(aq) What is the cell potential when one of the following deviations from standard conditions are made? A) [Zn2+] = 0.25 M; [Cu2+] = 0.25 M B) [Zn2+] = 0.25 M; [Cu2+] = 0.50 M C) [Zn2+] = 0.75 M; [Cu2+] = 0.75 M D) [Zn2+] = 0.75 M; [Cu2+] = 0.25 M E) [Zn2+] = 0.25 M; [Cu2+] = 0.75 M
What is the equilibrium constant K at 25 °C for an electrochemical cell when E° = +0.0235 V and n = 2?(F = 96,500 J/(V･mol), R = 8.314 J/(mol･K))
The oxidation of methanol, as described by the equation below, has a ΔG° value of -938 kJ/mol. What is the standard cell potential (in V) for a methanol fuel cell? 2 CH3OH (l) + 3 O2 (g) → 2 CO2 (g) + 4 H2O (l)

Recommended textbooks for you

Chemistry

ISBN:

9781305957404

Author:

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

Publisher:

Cengage Learning

Chemistry

ISBN:

9781259911156

Author:

Raymond Chang Dr., Jason Overby Professor

Publisher:

McGraw-Hill Education

Principles of Instrumental Analysis

Chemistry

ISBN:

9781305577213

Author:

Douglas A. Skoog, F. James Holler, Stanley R. Crouch

Publisher:

Cengage Learning

Chemistry

ISBN:

9781305957404

Author:

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

Publisher:

Cengage Learning

Chemistry

ISBN:

9781259911156

Author:

Raymond Chang Dr., Jason Overby Professor

Publisher:

McGraw-Hill Education

Principles of Instrumental Analysis

Chemistry

ISBN:

9781305577213

Author:

Douglas A. Skoog, F. James Holler, Stanley R. Crouch

Publisher:

Cengage Learning

Organic Chemistry

Chemistry

ISBN:

9780078021558

Author:

Janice Gorzynski Smith Dr.

Publisher:

McGraw-Hill Education

Chemistry: Principles and Reactions

Chemistry

ISBN:

9781305079373

Author:

William L. Masterton, Cecile N. Hurley

Publisher:

Cengage Learning

Elementary Principles of Chemical Processes, Bind…

Chemistry

ISBN:

9781118431221

Author:

Richard M. Felder, Ronald W. Rousseau, Lisa G. Bullard

Publisher:

WILEY

SEE MORE TEXTBOOKS

A electrochemical cell is made by considering the following unbalanced redox reaction: Pb2+(aq) + Fe(s) → Fe3+(aq) + Pb(s) The cell voltage, Ecell, at 298 K, when [Pb2+] = 0.25 M and [Fe3+] = 0.15 M, is nonspontaneous? Is the reaction spontaneous or