A24Appendix 5Equilibrium Constants and Reduction PotentialsTable A5.5Standard Reduction Potentials at 25°C (298 K) for Many Common Half-ReactionsHalf-ReactionE° (V)Half-ReactionE° (V)F2 + 2e-Ag2+ + e → Ag*Соз+ + е —— Со2+О2 + 2H,0 + 4eCu2+ + 2e¯ → Cu→ 2F-2.87> 40H-0.401.990.34Hg2 Cl2 + 2e-AgCl + e- –→ Ag + Cl-SO,2- + 4H+ + 2e- → H,SO3 + H2OCu2+ + e- – → Cu+2H+ + 2eFe3+ + 3e1.822Hg + 2Cl-0.27>Н,О, + 2H+ + 2е —> 2H,0Се4+ + e — > Сез+PbO2 + 4H+ + SO,2- + 2eMnO4+ + 4H+ + 3e¯ → MnO2 + 2H2OI04- + 2H+ + 2eMnO4+ + 8H+ + 5e¯Au3+ + 3e- → Au1.780.221.700.20» PbSO4 + 2H2O1.690.161.68H20.00→ I03¯ + H2O→ Mn2+ + 4H2O1.60Fe-0.0361.51Pb2+ + 2e-Pb-0.131.50Sn2+ + 2e-Sn-0.14Ni2+ + 2ePbO2 + 4H+ + 2e- → Pb²+ + 2H2OCl2 + 2e- – → 2Cl-Cr202- + 14H+ + 6e¯ –→ 2Cr³+ + 7H2OO2 + 4H+ + 4e-MnO2 + 4H+ + 2e-IO3- + 6H+ + 5e-Br2 + 2e- – → 2B1¯VO2+ + 2H+ + e¯AuCl,- + 3e-NO3- + 4H+ + 3e¯ → NO + 2H2OCIO, + e- →2Hg²+ + 2eAg+ + e-Hg22+ + 2e- → 2HgFe3+ + e- –→ Fe2+1.46→ Ni-0.23PBSO4 + 2e-Cd2+ + 2e-→ Pb + SO,²-→ Cd→ Fe1.36-0.351.33-0.40Fe2+ + 2e-2H2O→ Mn2+I2 + 3H2O1.23-0.442H2O1.21Cr3+ + e-Cr2+-0.501.20Cr3+ + 3e-→ Cr-0.73Zn2+ + 2e2H2O + 2eMn2+ + 2e-1.09Zn-0.76» VO2+ + H2O→ Au + 4Cl-→ H2 + 20H-Mn1.00-0.830.99-1.180.96Al3+ + 3e-→ Al-1.66ClO,-» Hg,2+Н, + 2е-Mg2+ + 2e-La3+ + 3e-Na+ + e-0.9542H--2.23→ Mg→ La0.91-2.37→ Ag0.80-2.370.80→ Na-2.710.77Ca2+ + 2e-> Ca-2.76O2 + 2H+ + 2e- → H2O2MnO4- + e¯ → MnO,2-I2 + 2e- –Cut + e - → Cu0.68Вa2+ + 2e- — Ва-2.900.56K+ + e¯ –→ K-2.92→ 21-0.54Li+ + e¯ –→ Li- 3.050.52 1. Use the table of standard reduction potentials on page A24 of your textbook to picka reagent that is capable of each of the following reductions (under standardconditions in acidic solution).a) Reduces Cu²+ to Cu but does not reduce Cu2+ to Cu+b) Reduces Br2 to Br- but does not reduce I2 to I-

Answered: Image /qna-images/answer/3435d250-2417-452a-9be4-7965759f8536.jpg

1. Use the table of standard reduction potentials on page A24 of your textbook to pick a reagent that is capable of each of the following reductions (under standard conditions in acidic solution). a) Reduces Cu²+ to Cu but does not reduce Cu2+ to Cu* b) Reduces Br2 to Br- but does not reduce I2 to I-

1. Use the table of standard reduction potentials on page A24 of your textbook to pick a reagent that is capable of each of the following reductions (under standard conditions in acidic solution). a) Reduces Cu²+ to Cu but does not reduce Cu2+ to Cu* b) Reduces Br2 to Br- but does not reduce I2 to I-

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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Using data from the Standard Reduction Potentials table, place the following in order of increasing strength as oxidizing agents (all under standard conditions). (Use the appropriate symbol to separate substances in the list.) Cr³+, Ba²+, Au³+, Cu²+, K+, and Cd²+ Help chemPad XX → Greek
Use standard reduction potentials to calculate the standard free energy change in kJ for the reaction: Hg2+(aq) + Ni(s) Hg(1) + Ni2+(aq) Answer: kJ K for this reaction would be v than one. greater less
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Consider the following reaction and standard reduction potential data. 2Ag (aq) + Cu(s) 2Ag(s) + Cu*"(aq) Half reaction E°(V) Ag (aq) +eAg(s) 0.80 Cu2"(aq) + 2e → Cu(s) 0.34 a. As written, is the Keg of the reaction shown above greater than 1 or less than 17 (Select] b. Which species is the reducing agent? [Select ] c. Suppose a voltaic cell was constructed using a Cu and Ag electrode (pictured below). The Cu electrode was placed in a 0.01 M solution of Cu(NO;)2, and the Ag electrode was placed in a 1.00 M solution of AGNO3. What is the Ecell for this voltaic cell? Assume the temperature is 298 K. Also NO; is a spectator ion. ( Select ) Voltmeter Ag Cu sat bridge AgNO= 1.00 M -0.01 M >
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