Explore relative reducing/oxidizing ability.Use the half-reactions shown below to answer the following questions.Half-reactionCl2(g) + 2e->>2Cl(aq)E° (V)1.360VNi2+(aq) + 2e-→Ni(s)-0.250VMn2+(aq) + 2e-→Mn(s) -1.180V(a) Identify the strongest oxidizing agent and the weakest oxidizing agent.Enter formulas:Strongest OA Weakest OA(b) Identify the strongest reducing agent and the weakest reducing agent.Strongest RA Weakest RA (b) Identify the strongest reducing agent and the weakest reducing agent.Enter formulas:Strongest RA Weakest RA(c) Will Cl2(g) oxidize Mn(s) to Mn2+(aq✓yesnoD(d) Identify all species that can be oxidized by Ni²+(aq).If none, leave box blank.

Answered: Explore relative reducing/oxidizing…

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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Examine the following half-reactions and select the strongest reducing agent among the species listed. Cu+(aq) + e– → Cu(s) E° = 0.52 V Ni2+(aq) + 2e– → Ni(s) E° = –0.23 V Pb2+(aq) + 2e– → Pb(s) E° = –0.13 V Select one: Ni2+(aq) Cu+(aq) Pb(s) Pb2+(aq) Cu(s) Ni(s)
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From the standard reduction potentials given below, which of the following pairs of substances will react spontaneously? Sn² (aq) + 2 e→ Sn(s) 2 H*(aq) +2 e → H₂ (g) Cd2+ (aq) + 2 e →→ Cd(s) E = -0.14 V E = 0.00 V Eº = -0.40 V a) Cd2+(aq) with H*(g) b) Cd2+ (aq) with H₂(g) O c) Sn(s) with Cd²+(aq) Cd(s) with Sn2+(aq)
Given the following standard reduction potentials, determine K for the following reaction at 25°C. Report your answer to 3 significant figures in scienitific notation using the format of 6.022E23 for 6.022 × 1023. Pb2+(aq) + SO42−(aq) → PbSO4 (s) E°red Pb2+(aq) + 2e− → Pb (s) -0.126 V PbSO4 (s) + 2e− → Pb (s) + SO42−(aq) -0.356 V
For the following two reduction half-reactions, which will occur at the cathode? a) Fe3+(aq) + e- --> Fe2+(aq) Eo = +0.771 V b) Pt2+(aq) + 2e- --> Pt(s) Eo = +1.20 V
Balance the following Redox reaction equation, and find oxidation reagent and reduction reagent. Cr2O72-(aq) + I-(aq)--> Cr3+(aq) + IO3-(aq)
Use the half-reactions shown below to answer the following questions. Half-reaction E° (V) Br,(1) + 2e-2Br (aq) 1.080 V Cu*(aq) + 2e >Cu(s) 0.337 V Zn*(aq) + 2e- Zn(s) -0.763 V (a) Identify the strongest oxidizing agent and the weakest oxidizing agent. Strongest OA Weakest OA Enter formulas: (b) Identify the strongest reducing agent and the weakest reducing agent. Strongest RA Weakest RA Enter formulas: (c) Will Bra(t) oxidize Zn(s) to Zn2*(aq)? (d) Identify all species that can be oxidized by Cu"(aq). If none, leave box blank.
Table 20.2 Half-reaction Ee (V) Cr3+ (aq) + 3e- ¬ Cr (s) -0.74 Fe2+ (aq) + 2e- - Fe (s) -0.440 Fe3+ (aq) + e- ¬ Fe2+ (s) +0.771 Sn4+ (aq) + 2e- - Sn2+ (aq) +0.154 ?Which of the following reactions will occur spontaneously as written Sn4+ (aq) + Fe2+ (aq) – Sn2+ (aq) + Fe (s) .a 3FE2+ (aq) - Fe (s) + 2Fe3+ (aq) .b O 3Fe (s) + 2Cr3+ (aq) - 2Cr (s) + 3FE2+ (aq) .c O 3Sn4+ (aq) + 2Cr (s) - 2Cr3+ (aq) + 3Sn2+ (aq) .d O Sn4+ (aq) + Fe3+ (aq) - Sn2+ (aq) + Fe2+ (aq) .e O
Complete and balance the following half-reaction in acidic solution NH_3(g)->NO_3(aq)
Complete and balance the following redox reaction in acidic solution MnO4-(aq) + N2O3 (aq) --> Mn2+ (aq) + NO3- (aq)
Both O2 + 2H2O + 4e− → 4OH− and O2(g) + 2H2O (I) → 4OH− (aq)
Examine the following half-reactions and select the strongest reducing agent among the species listed. AuBr4(aq) + 3e– → Au(s) + 4Br–(aq) E° = 0.854 V Mn2+(aq) + 2e– → Mn(s) E° = –1.185 V K+(aq) + e– → K(s) E° = –2.931 V F2O(aq) + 2H+(aq) + 4e– → 2F–(aq) + H2O(l) E° = 2.153 V Group of answer choices K K+ F2O F–

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