Give the standard line notation for each cell. (а) 2 I03 (ад) + 10 Cr?+ (aq) + 10 H* (аq) — 10 Cr+ (aд) + Iz(аq) + 5 H2О(1) O Pe(s) | Cr (ag), I (aq) || Cr?* (аg), IO; (ад), Н* (аg) | Pt(s) O P(s) | Cr+ (ag), Cr* (ag) || IОз (ад), Н* (ад), I2 (аq) | Pt(8) O Pt(s) | IO3 (ag), H* (ag), I2 (aq) || Cr²+ (ag), Cr³+ (aq) | Pt(s) O P(s) | Cr* (aд), IOз (ад), Н*(ад) || Ст** (ag), I>(аq) | Pt(8) (b) Zn(s) + 2 Ag* (ag) = Zn²+ (ag) + 2 Ag(s) Ag(s) Zn?+ (ag) || Ag* (ag) | Zn(s) Zn(s) | Ag* (aq) || Zn²+ (aq) | Ag(s) Zn(s)| Zn²+ (aq) || Ag* (aq) | Ag(s) O Ag(s) | Ag* (aq) || Zn²+ (aq) | Zn(s) (с) Н2О2(ад) + 2 H' (ад) + 2 е — 2 Н2О(1) Е' — 1.78 V О(9) + 2 H (аq) + 2 е Н20: (ад) E° = 0.68 V O P(8) | H2О2(ад) | Pt(8) O Pe(s:) | HО2(aд), H* (ад) || О?(9) | H2О2(ад), Н* (aд) | Pt(s) O Pt(s) | O2(9) | H2 O2 (ag), H† (ag) || H2O2 (aq), H† (ag) | Pt(s) O Pe(s) | H-О2(aq) | O- (9) || H* (аg) | Pt(s)

Give the standard line notation for each cell. (а) 2 I03 (ад) + 10 Cr?+ (aq) + 10 H* (аq) — 10 Cr+ (aд) + Iz(аq) + 5 H2О(1) O Pe(s) | Cr (ag), I (aq) || Cr?* (аg), IO; (ад), Н* (аg) | Pt(s) O P(s) | Cr+ (ag), Cr* (ag) || IОз (ад), Н* (ад), I2 (аq) | Pt(8) O Pt(s) | IO3 (ag), H* (ag), I2 (aq) || Cr²+ (ag), Cr³+ (aq) | Pt(s) O P(s) | Cr* (aд), IOз (ад), Н*(ад) || Ст** (ag), I>(аq) | Pt(8) (b) Zn(s) + 2 Ag* (ag) = Zn²+ (ag) + 2 Ag(s) Ag(s) Zn?+ (ag) || Ag* (ag) | Zn(s) Zn(s) | Ag* (aq) || Zn²+ (aq) | Ag(s) Zn(s)| Zn²+ (aq) || Ag* (aq) | Ag(s) O Ag(s) | Ag* (aq) || Zn²+ (aq) | Zn(s) (с) Н2О2(ад) + 2 H' (ад) + 2 е — 2 Н2О(1) Е' — 1.78 V О(9) + 2 H (аq) + 2 е Н20: (ад) E° = 0.68 V O P(8) | H2О2(ад) | Pt(8) O Pe(s:) | HО2(aд), H* (ад) || О?(9) | H2О2(ад), Н* (aд) | Pt(s) O Pt(s) | O2(9) | H2 O2 (ag), H† (ag) || H2O2 (aq), H† (ag) | Pt(s) O Pe(s) | H-О2(aq) | O- (9) || H* (аg) | Pt(s)

Chemistry: An Atoms First Approach

2nd Edition

ISBN:9781305079243

Author:Steven S. Zumdahl, Susan A. Zumdahl

Publisher:Steven S. Zumdahl, Susan A. Zumdahl

Chapter17: Electrochemistry

Section: Chapter Questions

Problem 2RQ: Galvanic cells harness spontaneous oxidationreduction reactions to produce work by producing a...

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For each of the reactions, calculate E from the table of standard potentials, and state whether the reaction is spontaneous as written or spontaneous in the reverse direction under standard conditions. (a) Zn(s)+Fe2+(aq)Zn2+(aq)+Fe(s) (b) AgCl(s)+Fe2+(aq)Ag(s)+Fe3+(aq)+Cl(aq) (c) Br2(l)+2Cl(aq)Cl2(g)+2Br(aq)
For each of the following reactions, determine the overall balanced electrochemical reaction, its standard electric potential, and the standard Gibbs energy of the reaction. aCo+F2Co2++2F bZn+Fe2+Zn2++Fe c Zn+Fe3+Zn2++Fe d Hg2++HgHg22+
Table 17-1 lists common half-reactions along with the standard reduction potential associated with each half-reaction. These standard reduction potentials are all relative to some standard. What is the standard (zero point)? lf is positive for a half-reaction, what does it mean? If is negative for a half-reaction, what does it mean? Which species in Table 17-1 is most easily reduced? Least easily reduced? The reverse of the half-reactions in Table 17-1 are the oxidation half-reactions. How are standard oxidation potentials determined? In Table 17-1, which species is the best reducing agent? The worst reducing agent? To determine the standard cell potential for a redox reaction, the standard reduction potential is added to the standard oxidation potential. What must be true about this sum if the cell is to be spontaneous (produce a galvanic cell)? Standard reduction and oxidation potentials are intensive. What does this mean? Summarize how line notation is used to describe galvanic cells.
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