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Answer: Calculating E°red from E°cellFor the Zn–Cu2+

Chemistry: The Central Science | 13th Edition | ISBN: 9780321910417 | Authors: Theodore E. Brown; H. Eugene LeMay; Bruce E. Bursten; Catherine Murphy; Patrick Woodward; Matthew E. Stoltzfus ISBN: 9780321910417 77

Solution for problem 2PE Chapter 20.5SE

Chemistry: The Central Science | 13th Edition

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Chemistry: The Central Science | 13th Edition | ISBN: 9780321910417 | Authors: Theodore E. Brown; H. Eugene LeMay; Bruce E. Bursten; Catherine Murphy; Patrick Woodward; Matthew E. Stoltzfus

Chemistry: The Central Science | 13th Edition

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Problem 2PE

Calculating E°red from E°cell

For the Zn–Cu2+ voltaic cell shown in Figure, we have

How is electrical balance maintained in the left beaker as Zn2+ are formed at the anode?

Figure A voltaic cell that uses a salt bridge to complete the electrical circuit.

Zn(s) + Cu2+(aq, 1 M) → Zn2+(aq, 1 M) + Cu(s) E°cell = 1.10 V

Given that the standard reduction potential of Zn2+ to Zn(s) is –0.76 V, calculate the E°red for the reduction of Cu2+ to Cu:

Cu2+(aq, 1 M) + 2 e– → Cu(s)

The standard cell potential is 1.46 V for a voltaic cell based on the following half–reactions:

In+(aq) → In3+(aq) + 2 e–, Br2(l)+2 e– → 2 Br–(aq)

Using Table calculate E°red for the reduction of In3+ to In+.

Table Standard Reduction Potentials in Water at 25°c

Eºred(V)

Reduction Half–Reaction

+2.87

F2(g) + 2 e–→.2 F–(aq)

+1.51

MnO4–(aq) + 8 H+(aq) + 5 e–→.Mn2+(aq) + 4 H2O(l)

+1.36

Cl2(g) + 2 e–→.2 Cl–(aq)

+1.33

Cr2O72–(aq) + 14 H+(aq) + 6 e–→.2 Cr3+(aq) + 7 H2O(l)

+1.23

O2(g) + 4 H+(aq) + 4 e–→.2 H2O(l)

+1.06

Br2(l) + 2 e–→.2 Br–(aq)

+0.96

NO3–(aq) + 4 H+(aq) + 3 e–→.NO(g) + 2 H2O(l)

+0.80

Ag+(aq) + e–→.Ag(s)

+0.77

Fe3+(aq) + e–→.Fe2+(aq)

+0.68

O2(g) + 2 H+(aq) + 2 e–→.H2O2(aq)

+0.59

MnO4–(aq) + 2 H2O(l) + 3 e–→.MnO2(s) + 4 OH–(aq)

+0.54

l2(s) + 2 e–→.2 l–(aq)

+0.40

O2(g) + 2 H2O(l) + 4 e–→.4 OH–(aq)

+0.34

Cu2+(aq) + 2 e–→.Cu

0 [defined]

2 H+(aq) + 2 e–→.H2(g)

–0.28

Ni2+(aq) + 2 e–→.Ni(s)

–0.44

Fe2+ (aq) + 2 e–→.Fe(s)

–0.76

Zn2+(aq) + 2 e–→.Zn(s)

–0.83

2 H2O(l) + 2 e–→.H2(g) + 2 OH–(aq)

–1.66

Al3+(aq) + 3 e–→.Al(s)

–2.71

Na+(aq) + e–→.Na(s)

–3.05

Li+(aq) + e–→.Li(s)

Step-by-Step Solution:
Step 1 of 3
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Chapter 20.5SE, Problem 2PE is Solved
Step 3 of 3

Textbook: Chemistry: The Central Science
Edition: 13
Author: Theodore E. Brown; H. Eugene LeMay; Bruce E. Bursten; Catherine Murphy; Patrick Woodward; Matthew E. Stoltzfus
ISBN: 9780321910417

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Answer: Calculating E°red from E°cellFor the Zn–Cu2+

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