Part A) List the following ions according to their ability to oxidize H2 by undergoing reduction to form their parent me

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Part A) List the following ions according to their ability to oxidize H2 by undergoing reduction to form their parent metal. In other words list the strongest oxidizing agent to the weakest oxidizing agent, based on the chart provided, recall that stronger oxidizing agents have higher reduction potentials (E°)… they will be reduced, causing something else to be oxidized.
Ag+, Co2+, Cu2+, Cd2+, Cr3+, Sn2+
Highest reduction potential _____> ______ > ______> ______> _______> ______ lowest reduction potential
Part B) A researcher only interested in “relative” reduction potentials, selects Sn as a “standard” in preparing a table of reduction potentials of the above ions, assigning E° = 0.0 for the Sn2+/Sn cell.
According to the list of reduction potentials provided, which cells have a higher reduction potential (E°) than Sn2+/Sn cell?
Which have a lower reduction potential (E°) than Sn2+/Sn cell?
strong oxidizing agents. Standard Reduction Potentials at 298K, 1M, 1 atm HALF-REACTION E° (V) F29) + 2e → 2 F (3) +2.87 +2.07 O + 2H*) +2 e→Ozg) + H₂O Co+e→Co²+ H₂O2(g) + 2H+ (aq) +1.82 (Q) +2e → 2 H₂O +1.77 +1.70 PbO2(s) + 4 H*(aq) + SO4 (aq) +2 e→PbSO4(s) + 2 H₂O Ce ()+E→Ce³+ (aq) +1.61 +1.51 MnO4 (aq) + 8 H*(aq) + 5 e → Mn²-4 H₂00 Au²³)+3 e → AU(s) +1.50 +1.36 +1.33 Cl₂(g) + 2e → 2 CI Cr₂O7²¹ (9) + 14 Haq) + 6 e2 Cr³+ *(20) + 7 H₂O MnO₂ +4 H*+2 e→Mn²t) + 2H₂O O2(g) +4 H*(g) +4 e 2 H₂O +1 23 +1.23 Br20) +2 e 2 Br*(aq) ->> +1.07 NO3(aq) + 4H+ (aq) + 3 e→NO) + 2 H₂O +0.96 Hg₂²) 24 +0.92 2 Hg¹*() +2 e → Hg₂+ + 2e → 2 Ham +0.85 Aga) + →. → Age +0.80 Fe³+ (aq) + → Fe²(a) +0.77 O2(g) + 2 H+ (aq) 2 e →→ H₂O₂) +0.68 +0.59 MnO4 (aq) + 2 H₂O + 3 e→MnO₂ +4 OH* () 12() +2e → 2 (0) +0.53 O2(g) + 2 H₂O + 4e →→ 4 OH(aq) +0.40 Cu²+ (aq) + 2 e→→ Cu(s) +0.34 AgCl) + e→→ Ag(s) + Cl(a) +0.22 SO4 (aq) + 4 H*(aq) + 2 e SO2) + 2H₂O સ) +0.20 Cu²+ +e → Cu (aq) +0.15 Sn (aq) +2 e Sna (aq) +0.13 2 H+ 0.00 +2 e² → H₂(g) Pb²+2 e Pb) (aq) →>> -0.13 Sn²+ (aq) -0.14 NI2+ +2 e* → Sn(s) +2e → Nl(s) (aq) + 2 e →→ CO() -0.25 Coz -0.28 PbSO4+2 e→→ Pb + SO4² -0.31 Ca²+ +2e → Cd) (34) -0.40 Fe²+ (0) -0.44 Cr³+ Zn²+ -0.74 +2e →>> Fe(s) +3e →→ Cr(s) +2 e→ Zn) (aq) -0.76 2 H₂O +2 eH₂ + 2 OH -0.83 Mn²+ (4) -1.18 +2€ → M ->> AP) + 3 e Al) -1.66 (39) strong

(aq) +2H₂Om MnO₂) +4 H*() +2 e→Mn²+) O2 +4 H*)+4 e Br20+2 e 2 H₂Om 2 Br*(aq) NO3(aq) + 4H+ (aq) + 3 e→NO) + 2 H₂O 2 Hg²+2 e→ Hg₂²*09) 2+ 2+ Hg₂+ + 2e → 2 H (aq) Agte + e → Ags) Fe³+ (aq) + e→→ Fe²+ (aq) O2(g) + 2 H+ (aq) 2 e →>> H₂O2(aq) MnO4 (aq) + 2 H₂O +3 e MnO2(s) + 4 OH*(aq) 12(s) + 2e → 2 (aq) O2(g) + 2 H₂O + 4e →→ 4 OH(aq) Cu() +2 e→→ Cu(s) (aq) AgCl) + e→→ Ag() + Cl(aq) SO4 (aq) +4 H*(aq) + 2 e SO2) + 2 H₂O0) +e→ Cu Cu2+ Sn +2e → Sn² (aq) (aq) +2e → H₂) 2 H*(a) Pb²+ + 2e → Pb(s) *(aq) + 2e → Sn(s) +2e → Nis) Sn²+ N12+ CO² (aq) +2 e' →→ CO(s) PbSO4)+2 e→→ Pb(s) + SO4²00) Cd2+ *(aq) + 2 e → Cd(s) Fe2+ (aq) +2e →→ Fe(s) Cr³+ (aq) + 3 e* → Cr(s) Zn²+ +2 e→→ Zn(s) 2 H₂O +2 eH₂ + 2 OH Mn²+ + 2 € → Mn AP+ +3e → A) +2e → Bez (aq) Mg²+ + 2 € → Mg(s) Nat +e → Na(s) 2009) Ca²+ *(aq) + 2e → Ca(s) (aq) + 2e → Sr(s) +2e → Ba (ag) (9) Be(s) Sr2²+ Ba2+ (aq) + K* (aq) + → K(s) Li*(aq) + →→ Ls) +1 23 +1.23 +1.07 +0.96 +0.92 +0.85 +0.80 +0.77 +0.68 +0.59 +0.53 +0.40 +0.34 +0.22 +0.20 +0.15 +0.13 0.00 -0.13 -0.14 -0.25 -0.28 -0.31 -0.40 -0.44 -0.74 -0.76 -0.83 -1.18 -1.66 -1.85 -2.37 -2.71 -2.87 -2.89 -2.90 -2.93 -3.05 strong reducing agents