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1a) Assuming standard conditions, answer the following questions. (Use the table of Standard Reduction Potentials for common Half-reactions i attached below If hydrogen is one of the reagents, assume acidic solution.). write yes or no beside each one.      Is Ag+(aq) capable of oxidizing H2(g)?     Is Fe2+(aq) capable of reducing VO2+(aq)?     Is Sn metal capable of reducing Fe3+(aq) to Fe2+(aq)?     Is Ni2+(aq) capable of oxidizing H2(g)?     Is Fe2+(aq) capable of reducing Sn2+(aq) to Sn metal?     Is Cr3+(aq) capable of oxidizing Fe2+(aq) to Fe3+(aq)?   1b) Assuming standard conditions, and considering the table of standard reduction potentials for half-reactions, attached below, rank the following species according to their relative strength as reducing agents. For example, the most powerful reducing agent would be given rank "1", and the least "6".          Al         Ca         H2 (acidic half-cell solution)         Fe         Pb2+ (acidic half-cell solution)         Fe2+

1a) Assuming standard conditions, answer the following questions. (Use the table of Standard Reduction Potentials for common Half-reactions i attached below If hydrogen is one of the reagents, assume acidic solution.). write yes or no beside each one.      Is Ag+(aq) capable of oxidizing H2(g)?     Is Fe2+(aq) capable of reducing VO2+(aq)?     Is Sn metal capable of reducing Fe3+(aq) to Fe2+(aq)?     Is Ni2+(aq) capable of oxidizing H2(g)?     Is Fe2+(aq) capable of reducing Sn2+(aq) to Sn metal?     Is Cr3+(aq) capable of oxidizing Fe2+(aq) to Fe3+(aq)?   1b) Assuming standard conditions, and considering the table of standard reduction potentials for half-reactions, attached below, rank the following species according to their relative strength as reducing agents. For example, the most powerful reducing agent would be given rank "1", and the least "6".          Al         Ca         H2 (acidic half-cell solution)         Fe         Pb2+ (acidic half-cell solution)         Fe2+

General Chemistry - Standalone book (MindTap Course List)
General Chemistry - Standalone book (MindTap Course List)
11th Edition
ISBN:9781305580343
Author:Steven D. Gammon, Ebbing, Darrell Ebbing, Steven D., Darrell; Gammon, Darrell Ebbing; Steven D. Gammon, Darrell D.; Gammon, Ebbing; Steven D. Gammon; Darrell
Publisher:Steven D. Gammon, Ebbing, Darrell Ebbing, Steven D., Darrell; Gammon, Darrell Ebbing; Steven D. Gammon, Darrell D.; Gammon, Ebbing; Steven D. Gammon; Darrell
Chapter19: Electrochemistry
Section: Chapter Questions
Problem 19.72QP: What is the standard cell potential you would obtain from a cell at 25C using an electrode in which...
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hello, i need hlep with part a and b.  last answers you provided were wrong . handwritten solutions are prefered. 

1a) Assuming standard conditions, answer the following questions.
(Use the table of Standard Reduction Potentials for common Half-reactions i attached below
If hydrogen is one of the reagents, assume acidic solution.). write yes or no beside each one. 


    Is Ag+(aq) capable of oxidizing H2(g)?
    Is Fe2+(aq) capable of reducing VO2+(aq)?
    Is Sn metal capable of reducing Fe3+(aq) to Fe2+(aq)?
    Is Ni2+(aq) capable of oxidizing H2(g)?
    Is Fe2+(aq) capable of reducing Sn2+(aq) to Sn metal?
    Is Cr3+(aq) capable of oxidizing Fe2+(aq) to Fe3+(aq)?

 

1b) Assuming standard conditions, and considering the table of standard reduction potentials for half-reactions, attached below, rank the following species according to their relative strength as reducing agents. For example, the most powerful reducing agent would be given rank "1", and the least "6". 


        Al
        Ca
        H2 (acidic half-cell solution)
        Fe
        Pb2+ (acidic half-cell solution)
        Fe2+

Standard Reduction Potentials at 25°C (298 K) for Many Common Half-reactions Half-reaction %° (V) Half-reaction F₂ +2e7 →2F- Ag²+ + e → Ag+ Co³+ + e→→ Co²+ H₂O₂ + 2H+ + 2e7 → 2H₂O Ce4+ + e→Ce³+ PbO₂ + 4H+ + SO4² +2e →→ PbSO4 + 2H₂O MnO4 + 4H+ + 3e7 → MnO₂ + 2H₂O IO4 + 2H+ + 2e → IO3 + H₂O MnO4 + 8H+ + 5e → Mn²+ + 4H₂O Au³+ + 3e7 → Au PbO₂ + 4H+ + 2e¯ → Pb²+ + 2H₂O Cl₂ +2e2C1- Cr₂O2 + 14H+ + 6e¯ → 2Cr³+ + 7H₂O O₂ + 4H+ + 4e → 2H₂O MnO₂ + 4H+ + 2e IO3 + 6H+ + 5e- Br₂ +2e7 → 2Br → Mn²+ + 2H₂O 1₂+ 3H₂O VO₂+ + 2H+ + e → VO²+ + H₂O AuCl4 + 3e → Au + 4Cl- NO3 + 4H+ + 3e → NO + 2H₂O CIO₂ + e→→ CIO₂ 2Hg2+ + 2c7 → Hg₂²+ Ag+ + e → Ag Hg₂+ + 2e →→ 2Hg Fe³+ + e Fe2+ O₂ + 2H+ + 2e → H₂O₂ MnO4 + e→→ MnO4²- 21- 1₂ +2e Cut + e → Cu 2.87 1.99 1.82 1.78 1.70 1.69 1.68 1.60 1.51 1.50 1.46 1.36 1.33 1.23 1.21 1.20 1.09 1.00 0.99 0.96 0.954 0.91 0.80 0.80 0.77 0.68 0.56 0.54 0.52 O₂ + 2H₂O + 4c→ 40H Cu²+ + 2e →→ Cu Hg₂Cl₂ + 2e →→ 2Hg + 2Cl- AgCleAg + Cl- SO4²- + 4H+ + 2e¯ → H₂SO3 + H₂O Cu²+ + e→ Cu+ 2H+ + 2e7 → H₂ →→ Fe →→ Pb → Sn → Ni Fe³+ + 3e Pb²+ + 2e Sn²+ + 2e7 Ni²+ + 2e7 PbSO4 + 2e Cr³+ + e→→ Cd²+ + 2e7 → Cd Fe2+ + 2e7 → Fe Cr²+ → Cr → Zn Cr3+ + 3e- Zn²+ + 2e7 2H₂O + 2e → H₂ + 2OH- Mn²+ + 2e7 → Mn Al³+ + 3e → Al H₂ +2e7 → 2H- Mg2+ + 2c→→ Mg La³+ + 3e7 → La Na+ + e- → Na Ca²+ + 2e7 → Ca Ba2+ + 2e7 → Ba K+ + e→→ K Lite Li →→ Pb + SO4²- 8° (V) 0.40 0.34 0.27 0.22 0.20 0.16 0.00 -0.036 -0.13 -0.14 -0.23 -0.35 -0.40 -0.44 -0.50 -0.73 -0.76 -0.83 -1.18 -1.66 - 2.23 -2.37 -2.37 -2.71 -2.76 -2.90 -2.92 -3.05
Transcribed Image Text:Standard Reduction Potentials at 25°C (298 K) for Many Common Half-reactions Half-reaction %° (V) Half-reaction F₂ +2e7 →2F- Ag²+ + e → Ag+ Co³+ + e→→ Co²+ H₂O₂ + 2H+ + 2e7 → 2H₂O Ce4+ + e→Ce³+ PbO₂ + 4H+ + SO4² +2e →→ PbSO4 + 2H₂O MnO4 + 4H+ + 3e7 → MnO₂ + 2H₂O IO4 + 2H+ + 2e → IO3 + H₂O MnO4 + 8H+ + 5e → Mn²+ + 4H₂O Au³+ + 3e7 → Au PbO₂ + 4H+ + 2e¯ → Pb²+ + 2H₂O Cl₂ +2e2C1- Cr₂O2 + 14H+ + 6e¯ → 2Cr³+ + 7H₂O O₂ + 4H+ + 4e → 2H₂O MnO₂ + 4H+ + 2e IO3 + 6H+ + 5e- Br₂ +2e7 → 2Br → Mn²+ + 2H₂O 1₂+ 3H₂O VO₂+ + 2H+ + e → VO²+ + H₂O AuCl4 + 3e → Au + 4Cl- NO3 + 4H+ + 3e → NO + 2H₂O CIO₂ + e→→ CIO₂ 2Hg2+ + 2c7 → Hg₂²+ Ag+ + e → Ag Hg₂+ + 2e →→ 2Hg Fe³+ + e Fe2+ O₂ + 2H+ + 2e → H₂O₂ MnO4 + e→→ MnO4²- 21- 1₂ +2e Cut + e → Cu 2.87 1.99 1.82 1.78 1.70 1.69 1.68 1.60 1.51 1.50 1.46 1.36 1.33 1.23 1.21 1.20 1.09 1.00 0.99 0.96 0.954 0.91 0.80 0.80 0.77 0.68 0.56 0.54 0.52 O₂ + 2H₂O + 4c→ 40H Cu²+ + 2e →→ Cu Hg₂Cl₂ + 2e →→ 2Hg + 2Cl- AgCleAg + Cl- SO4²- + 4H+ + 2e¯ → H₂SO3 + H₂O Cu²+ + e→ Cu+ 2H+ + 2e7 → H₂ →→ Fe →→ Pb → Sn → Ni Fe³+ + 3e Pb²+ + 2e Sn²+ + 2e7 Ni²+ + 2e7 PbSO4 + 2e Cr³+ + e→→ Cd²+ + 2e7 → Cd Fe2+ + 2e7 → Fe Cr²+ → Cr → Zn Cr3+ + 3e- Zn²+ + 2e7 2H₂O + 2e → H₂ + 2OH- Mn²+ + 2e7 → Mn Al³+ + 3e → Al H₂ +2e7 → 2H- Mg2+ + 2c→→ Mg La³+ + 3e7 → La Na+ + e- → Na Ca²+ + 2e7 → Ca Ba2+ + 2e7 → Ba K+ + e→→ K Lite Li →→ Pb + SO4²- 8° (V) 0.40 0.34 0.27 0.22 0.20 0.16 0.00 -0.036 -0.13 -0.14 -0.23 -0.35 -0.40 -0.44 -0.50 -0.73 -0.76 -0.83 -1.18 -1.66 - 2.23 -2.37 -2.37 -2.71 -2.76 -2.90 -2.92 -3.05
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