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# Answer: Calculating E°red from E°cellFor the Zn–Cu2+ ISBN: 9780321910417 77

## Solution for problem 2PE Chapter 20.5SE

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)
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##### ISBN: 9780321910417

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