(а) 2103 (ад) + 10 Cu" (aq) + 10 н"(ад) — 10 Cu"** (ag) + la (ag) + 5 H-0()O P() | Cut (ag), Cu?* (аq) || IOз (ад), н* (аq), I (ag) | Pt(s)O Pel(o) | Cu* (ag), IOз (ад), н* (аg) || Cu?* (ag), I, (ag) | Pt(8)O Pt(s) | IO3 (ag), H† (aq), I2 (aq) || Cu* (aq), Cu²+ (aq) | Pt(s)О Pe(6) | Cu?* (ag), I3(ag) || Cu" (аg), 10; (аg), н* (ад) | Pt()(b) Zn(s) + 2 Ag* (aq) = Zn²+ (aq) + 2 Ag(s)O Zn(s) | Zn²+Zn(s) | Ag* (ag) || Zn²+ (aq) | Ag(s)O Ag(s) | Ag* (aq) || Zn²+ (ag) | Zn(s)O Ag(s) | Zn²+ (aq) || Ag* (aq) | Zn(s)(aq) || Ag*(aq) | Ag(s)(с) НаО(ад) + 2 H* (аq) + 2 е — 2 H:0()E° = 1.78 VОэ (9) + 2 H* (ад) + 2 е НаОz(аg)Е 3 0.68 VO Pt(s) | O2(g) | H2O2 (aq), H* (aq) || H2O2 (ag), H* (ag) | Pt(s)O Pt(s) | H2O2 (ag), H* (ag) || 02(9) | H2O2 (aq), H* (aq) | Pt(s)O Pt(s) | H2O2 (aq) | O2(9) || H† (aq) | Pt(s)O Pt(s) | H2O2(aq) | Pt(s)(d) Mn'* (aq) +2 е — Mn(s)Е 3D - 1.18 VFe+ (aq) + 3 e → Fe(s)Е 3D -0.036VO Mn(s) | Mn²+ (ag) || Fe*+ (aq) | Fe(s)O Fe(8) | Mn²+ (aq) || Fe* (aq) | Mn(8)O Fe(s) | Fe³* (aq) || Mn²* (aq) | Mn(s)О Mn(8) | Fe* (аq) || Mn?* (aq) | Fe(s)3+2+2+

Redox reaction is process in which both oxidation and reduction takes place simultaneously in a…

O Pt(s) | Cu* (aq), Cu2+ (ag) || IO3 (ag), H* (aq), I2 (ag) | Pt(s) O Pt(s) | Cu* (ag), IO, (ag), H* (aq) || Cu²+ (ag), I2 (aq) | Pt(s) Pt(s) | IO3 (ag), H* (aq), I2 (aq) || Cu* (aq), Cu²+ (aq) | Pt(s) O Pt(8) | Cu²+ (aq), I2 (ag) || Cu* (ag), I0, (ag), H* (aq) | Pt(s) (b) Zn(s) +2 Ag* (aq) = Zn?+ (aq) + 2 Ag(s) O Zn(s) | Zn2+ (ag) || Ag* (aq) | Ag(s) Zn(s) | Ag* (ag) || Zn2+ (ag) | Ag(s) O Ag(s) | Ag* (aq) || Zn²+ (aq) | Zn(s) Ag(s) | Zn2+ (aq) || Ag* (ag) | Zn(s) (c) H2 O2 (ag) + 2 H* (ag) + 2 e → 2 H20(1) E = 1.78 V O2 (9) + 2 H* (ag) + 2 e- → H2O2(aq) E = 0.68 V O Pt(s) | O2 (9) | H2O2 (aq), H* (aq) || H2 O2 (aq), Ht (ag) | Pt(s) O Pt(s) | H2O2 (ag), H* (ag) || O2(9) | H2O2 (aq), H* (aq) | Pt(s) O Pt(s) | H2O2 (aq) | O2 (g) || H* (aq) | Pt(s)

O Pt(s) | Cu* (aq), Cu2+ (ag) || IO3 (ag), H* (aq), I2 (ag) | Pt(s) O Pt(s) | Cu* (ag), IO, (ag), H* (aq) || Cu²+ (ag), I2 (aq) | Pt(s) Pt(s) | IO3 (ag), H* (aq), I2 (aq) || Cu* (aq), Cu²+ (aq) | Pt(s) O Pt(8) | Cu²+ (aq), I2 (ag) || Cu* (ag), I0, (ag), H* (aq) | Pt(s) (b) Zn(s) +2 Ag* (aq) = Zn?+ (aq) + 2 Ag(s) O Zn(s) | Zn2+ (ag) || Ag* (aq) | Ag(s) Zn(s) | Ag* (ag) || Zn2+ (ag) | Ag(s) O Ag(s) | Ag* (aq) || Zn²+ (aq) | Zn(s) Ag(s) | Zn2+ (aq) || Ag* (ag) | Zn(s) (c) H2 O2 (ag) + 2 H* (ag) + 2 e → 2 H20(1) E = 1.78 V O2 (9) + 2 H* (ag) + 2 e- → H2O2(aq) E = 0.68 V O Pt(s) | O2 (9) | H2O2 (aq), H* (aq) || H2 O2 (aq), Ht (ag) | Pt(s) O Pt(s) | H2O2 (ag), H* (ag) || O2(9) | H2O2 (aq), H* (aq) | Pt(s) O Pt(s) | H2O2 (aq) | O2 (g) || H* (aq) | Pt(s)

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 values from the table of standard reduction potentials, calculate the cell potential (in V) of the following cells. 2+ + (a) Fe(s) | Fe (aq) || Ag (aq) | Ag(s) V 2+ (b) Cd(s) | Cd²+ (aq) || Cr³+ (aq) | Cr(s) 2- 2+ (c) Cd(s), CdS(s) | S (aq) || Sn (aq) | Sn(s) V
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