Calculate the E° for both reactions and determine which reaction iscellspontaneous.• Cu2+ + 2Ag → 2Ag+ + Cu• 2Ag+ + Cu → Cu2+ + 2AgA. Reaction 1B. Reaction 2C. No ClueAg+ (aq) + eFe3+(aq) + eO2(g) +2 H(aq) + 2eMnO4 (aq) + e2(s) + 2e→ 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)0.34= E° SRPcathode - E° SRPanode or E° cell = E SRPred - E° SRPOXCu+(aq) + eO2(g) + 2 H2O(l) + 4 e¯Cu2+(aq) + 2eE cell

Step 1: Step 2: Step 3: Step 4:

Answered: Calculate the E° for both reactions and…

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...

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Find K for the following reaction at 25°C. E cell = 0.45 V Pb2+ + Fe(s) ----> Pb(s) + Fe²+ (aq) 8.6 x 10-6 1.4 x 1015 7.1 x 10-11 1.6 x 1015
What is the pH in the cathode for the following galvanic cell made from the following two half reactions? The initial concentration of gold ion is 3.5x10 3 M, the initial concentration of permanganate is 6.07 M, and the Ecell is 0.15 V. Assume the temperature is 298K. Au³+ (aq) + 3e-→ Au(s) E° = 1.52 V MnO4 (aq) + 4H* (aq) 3e-→ MnO2(s) + 2H₂O E° = 1.70 V Read more about this topic
19
Which of the following metals can be oxidized by H+ under standard conditions? Cu, Zn, Ag, Sn Ag+(aq) + e– → Ag(s) E° = 0.80 V Cu2+(aq) + 2e– → Cu(s) E° = 0.34 V Cu2+(aq) + e– → Cu+(aq) E° = 0.15 V Sn4+(aq) + 2e– → Sn2+(aq) E° = 0.13 V Sn2+(aq) + 2e– → Sn(s) E° = –0.14 V Zn2+(aq) + 2e– → Zn(s) E° = –0.76 V
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a Calculate E° values for the following cells. a. H2 (g) → H* (aq) + H¯(aq) Half-Reaction E° (V) 2H* + 2e + H2 0.00 H2 + 2e + 2H -2.23 b. Aut (ag) + Cu(s) → Cu+ (ag) + Au(s) Half-Reaction E° (V) Au+ + 3e + Au 1.50 Cu* +e + Cu 0.52 E°
Calculate the E° cell for both reactions and determine which reaction is spontaneous. • Cu2+ + 2Ag → 2Ag+ + Cu • 2Ag+ + Cu → Cu2+ + 2Ag A. Reaction 1 B. Reaction 2 C. No Clue Ag(aq) + e Fe3+(aq) + e 02(g) +2 H(aq) + 2e MnO4(aq) + e b(s) + 2e Cu+(aq) + e 02(g) +2 H₂O(1)+4e Cu2+(aq) + 2e E cell = E SRPcathode - Ag(s) 0.80 →Fe2(aq) 0.77 →H₂O₂(aq) 0.70 →MnO2 (aq) 0.56 →2(aq) 0.54 →Cu(s) 0.52 0.40 0.34 →4 OH (aq) Cu(s) E SRPanode or E° cell = = E° SRPred - E° SRPOX
Consider the following standard reduction potentials in acid solution: E°(V) Al⁺³ + 3e− → Al(s) −1.66 Ag⁺¹ + e− → Ag(s) +0.80 Sn⁺⁴ + 2e− → Sn⁺² +0.14 Fe⁺³ + e− → Fe⁺² +0.77 The strongest reducing agent among those shown above is A) Al⁰ B) Fe⁺³ C) Br⁻ D) Al⁺³

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