Sketch the cell and write the line notation.• 2Ag+ + Cu → Cu2+ + 2AgAg (aq) + eFe3+(aq) + eO2(g) +2 H(aq) + 2eMnO4 (aq) + e2(s) + 2eCu+(aq) + e→Ag(s)0.80Fe2+(aq)0.77→H₂O₂(aq)0.70MnO4(aq)0.56→2(aq)0.54→Cu(s)0.52→→→→4 OH(aq)0.40→ Cu(s)0.3402(g) + 2 H2O(l) + 4 e¯¯Cu2+(aq) + 2eE cell1 = E° SRPcathode - E° SRPanode or E° cell = E° SRPred - E° SRPOX

To sketch the electrochemical cell and write the line notation for the given reaction:2Ag+ + Cu →…

Answered: Sketch the cell and write the line…

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

An electrochemical cell is based on these two half-reactions: Oxidation: Cu(s) → Cu2+(aq, 0.010 M) + 2 e− Reduction: MnO4 −(aq, 2.0 M) + 4 H+(aq, 1.0 M) + 3 e− → MnO2(s) + 2 H2O(l) Calculate the cell potential.
Select each of the following electrons that are more likely than that of the standard hydrogen electrode Cu²+ (aq) + 2e → Cu (s) Fe³+ (aq) + e → Fe²+ (aq) Ni²+ (aq) + 2e → Ni (s) F2 (g) + 2e → 2 F¯ (aq) Li+ (aq) + e Li (s)
Consider a cell that uses the redox reaction: 3 Na (s) + La3+ (aq) → 3 Na+ (aq) + La (s). Calculate the equilibrium constant (K) for this reaction at 25 ºC, given the following standard reduction potentials: La3+ (aq) + 3 e- → La (s) E° = -2.37 V Na+ (aq) + e- → Na (s) E° = -2.71 V 1.8 x 10-6 5.7 x 10-18 5.6 x 105 1.7 x 1017
Using standard reduction potentials from the ALEKS Data tab, calculate the standard reaction free energy ΔG^0 for the following redox reaction. 2Br-(aq) + 2H2O(l) -> Br2(l) + H2(g) + 2OH−(aq) Be sure your answer has the correct number of significant digitss
Based on standard reduction potentials (in second table below), will each of these reactions (in table 1) take place? How to calculate this?
Use the standard reduction potentials located in the 'Tables' linked above to calculate the standard free energy change in kJ for the reaction: Cd2+ (aq) + Zn(s)→→→→→→ Cd(s) + Zn²+ (aq) Answer: kJ K for this reaction would be than one.
Balance the following redox equation to its lowest integer ratio. (Under Acidic Conditions) Te(s) + Ru(NO3)3(aq) + NO2(g) ↔ Ru2Te3(s) + HNO3(aq) Note that H2O and H+ are not shown in the equation above. If it is required to balance the equation, then add these.Fill in the coefficient for each chemical after you finish balancing the equation. If the chemical is not needed in the equation then mark a zero next to it Te(s) HNO3(aq) H2O(l) Ru2Te3(s) NO2(g) Ru(NO3)3(aq) H+ (aq)
Suppose the galvanic cell sketched below is powered by the following reaction: Cu(s)+2 A£NO3(aq) → Cu(NO,),(aq)+2 Ag(s) E1 E2 sí S2 Write a balanced equation for the half-reaction that happens at the cathode of this cell. O-0 Write a balanced equation for the half-reaction that happens at the anode of this cell. Of what substance is E1 made? Of what substance is E2 made? What are the chemical species in solution S1? What are the chemical species in solution S2? O DD
Calculate the cell potential given the standard reduction potentials for the half reactions of the following hypothetical elements: X3+(aq) + e- → X2+(aq) SRP: +0.64 V Y2(ℓ) + 2e- → 2Y-(aq) SRP: +0.44 V
Using standard reduction potentials from the ALEKS Data tab, calculate the standard reaction free energy following redox reaction. Be sure your answer has the correct number of significant digits. H₂(g) + 2OH¯(aq) + 2Fe³+ (aq) → 2H₂O (1) + 2Fe²+ (aq) kJ x10 X Ś AGO for the
Use standard reduction potentials to calculate the standard free energy change in kJ for the reaction: Cu²+ (aq) + 2Cu+ (aq) → Cu(s) + 2Cu²+ (aq) 2+ Cu²+ (aq) + 2e → Cu(s) Ee = 0.337 V red 0.153 V = 2+ Cu²+ (aq) +e → Cut (aq) E red AG° kJ K for this reaction would be than one.
Copper(I) ion can act as both an oxidizing agent and a reducing agent. Hence, it can react with itself. 2Cu+(aq) → Cu(s) + Cu2+(aq) Calculate the equilibrium constant at 25°C for this reaction, using appropriate values of electrode potentials.

SEE MORE QUESTIONS

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