(d) Mg?+ (aq) + 2 e¯ → Mg(s)E° = - 2.37 VFe+ (ag) + 3 e → Fe(s)E°= -0.036 VO Fe(s) | Mg²+ (aq) || Fe*+ (ag) | Mg(s)O Mg(s) | Mg²+ (aq) || Fe³+O Mg(s) | Fe³+ (aq) || Mg²+ (ag) | Fe(s)O Fe(s) | Fe+(aq) || Mg²+ (aq) | Mg(8)(aq) | Fe(s) Give the standard line notation for each cell.(а) 2 IOз (аq) + 10 Cr (аq) + 10 H* (аq) — 10 Cr" (ag) + I2(ад) + 5 Нә0(1)O P(:) | Cr* (a), I> (aq) || Cr?* (аg), IO; (ад), н (аg) | Pt(s)O Pe(s) | Cr* (ag), IO; (ад), Н* (аq) | Cr* (aq), Iz (aq) І Pt(s)"(aд), I2 (aд) | Pt(8)O P(6) | 10; (aд), н* (аq), 1ә(аq) | Cr?* (ag), Cr** (ag) | Pt(6)Pe(s) | Cr* (aq), Сr* (aq) || IOз (aд), H* (ад), I2 (ад) | Pt(8)(b) Zn(s) +2 Ag* (aq) = Zn?+ (aq) + 2 Ag(s)O Ag(s)| Zn²+(aq) || Ag* (aq) | Zn(s)O Ag(s)| Ag*(aq) || Zn²+ (aq) | Zn(s)Zn(s) Ag* (ag) || Zn?+ (ag) | Ag(s)Zn(s) | Zn²+ (aq) || Ag* (aq) | Ag(s)(c) Н;О2(ад) + 2 H* (аq) + 2 е 2 Hә0(1)E°1.78 VО:(9) + 2 H (аq) + 2 е — Н,O%(аq)E° = 0.68 VO P(8) | H2О2(ад) | Pt(8)O Pt(s) | O2(9) | H,O2 (aq), H† (aq) || H,O2 (aq), H† (aq) | Pt(s)Pt(:) | H>О2(аq) | 02(9) || н* (аq) | Pt(8)O Pe(8) | H2О2(аg), H* (ад) || О2 (9) | Н-О2(ад), Н* (ад) | Pt(s)

Since you have posted a question with multiple sub-parts, we will solve the first three subparts for…

Give the standard line notation for each cell. (a) 2 103 (аq) + 10 Cr** (ag) + 10 H* (аq) — 10 Cr* (aq) + Iz(ag) + 5 H20(1) O Pt(s)| Cr³+ (aq), I2 (aq) || Cr²+ (ag), IO3¬(ag), H† (aq) | Pt(s) O Pt(s)| Cr²+ (aq), IO3¬(aq), H† (ag) || Cr³+ (ag), I2 (aq) | Pt(s) O Pt(s) | IO3¬(aq), H† (aq), I2 (aq) || Cr²+ (aq), Cr³+ (aq) | Pt(s) O Pt(s) | Cr²+(aq), Cr³+ (aq) || IO3¬(aq), H† (aq), I (aq) | Pt(s) (b) Zn(s)+2 Ag*(aq) = Zn²+ (aq) + 2 Ag(s) O Ag(s) | Zn²+ (aq) || Ag* (aq) | Zn(s) Ag(s) | Ag*(aq) || Zn²+ (aq) | Zn(s) Zn(s) | Ag*(aq) || Zn²+ (aq) | Ag(s) O Zn(s) | Zn²+ (ag) || Ag* (ag) | Ag(s) (c) H2O2(aq) +2 H* (aq) + 2 e¯ → 2 H2O(1) E° = 1.78 V О:(9) + 2 H* (аg) + 2 е > НәО:(аg) E° = 0.68 V O Pt(s)| H2O2(aq) | Pt(s) O Pt(s) | O2(9) | H2O2(aq), H† (aq) || H2O2 (aq), H* (aq) | Pt(s) O Pt(s) | H2O2(aq) | O2 (g) || H† (aq) | Pt(s) O Pt(s) | H2O2(aq), H† (aq) || O2(g) | H2O2(aq), H† (aq) | Pt(s)

Give the standard line notation for each cell. (a) 2 103 (аq) + 10 Cr** (ag) + 10 H* (аq) — 10 Cr* (aq) + Iz(ag) + 5 H20(1) O Pt(s)| Cr³+ (aq), I2 (aq) || Cr²+ (ag), IO3¬(ag), H† (aq) | Pt(s) O Pt(s)| Cr²+ (aq), IO3¬(aq), H† (ag) || Cr³+ (ag), I2 (aq) | Pt(s) O Pt(s) | IO3¬(aq), H† (aq), I2 (aq) || Cr²+ (aq), Cr³+ (aq) | Pt(s) O Pt(s) | Cr²+(aq), Cr³+ (aq) || IO3¬(aq), H† (aq), I (aq) | Pt(s) (b) Zn(s)+2 Ag(aq) = Zn²+ (aq) + 2 Ag(s) O Ag(s) | Zn²+ (aq) || Ag (aq) | Zn(s) Ag(s) | Ag(aq) || Zn²+ (aq) | Zn(s) Zn(s) | Ag(aq) || Zn²+ (aq) | Ag(s) O Zn(s) | Zn²+ (ag) || Ag* (ag) | Ag(s) (c) H2O2(aq) +2 H* (aq) + 2 e¯ → 2 H2O(1) E° = 1.78 V О:(9) + 2 H* (аg) + 2 е > НәО:(аg) E° = 0.68 V O Pt(s)| H2O2(aq) | Pt(s) O Pt(s) | O2(9) | H2O2(aq), H† (aq) || H2O2 (aq), H* (aq) | Pt(s) O Pt(s) | H2O2(aq) | O2 (g) || H† (aq) | Pt(s) O Pt(s) | H2O2(aq), H† (aq) || O2(g) | H2O2(aq), 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

Chapter18: Electrochemistry

Section: Chapter Questions

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

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Similar questions

A 0.0712-g sample of a purified organic acid was dissolved in an alcohol-water mixture and titrated with coulometrically generated hydroxide ions. With a current of 0.0392 A, 241 s was required to reach aphenolphthalein end point. Calculate the equivalent mass of the acid.
Halide ions can he deposited at a silver anode, the reaction being Ag(s) + X- AgX(s) +e- Suppose that a cell was formed by immersing a silver anode in an analyte solution that was 0.0250 M Cl-,Br-, and I -ions and connecting the half-cell to a saturated calomel cathode via a salt bridge. (a) Which halide would form first and at what potential? Is the cell galvanic or electrolytic? (b) Could I- and Br- be separated quantitatively? (Take 1.00 l0-5 M as the criterion for quantitative removal of an ion.) If a separation is feasible, what range of cell potential could he used? (c) Repeat part (b) for I- and Cl-. (d) Repeat part (b) for Br- and Cl-.
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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Consider the reaction low at 25°C: 3SO42(aq)+12H+(aq)+2Cr(s)3SO2(g)+2Cr3+(aq)+6H2O Use Table 17.1 to answer the following questions. Support your answers with calculations. (a) Is the reaction spontaneous at standard conditions? (b) Is the reaction spontaneous at a pH of 3.00 with all other ionic species at 0.100 M and all gases at 1.00 atm? (c) Is the reaction spontaneous at a pH of 8.00 with all other ionic species at 0.100 M and all gases at 1.00 atm? (d) At what pH is the reaction at equilibrium with all other ionic species at 0.100 M and all gases at 1.00 atm?
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What cathode potential (versus SCE) would be required to lower the total Hg(II) concentration of the following solutions to 1.00 10-6 M (assume reaction product in each case is elemental Hg): (a) an aqueous solution of Hg2+? (b) a solution with an equilibrium SCN- concentration of 0.100 M? Hg2+ + 2SCN- Hg(SCN)2(aq) = Kf = 1.8 107 c) a solution with an equilibrium Br- concentration of 0.100 M? HgBr42++ 2e- Hg(l) + 4Br- E0= 0.223 V
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Give the standard line notation for each cell. (а) 2 IOз (ад) + 10 Ст** (аq) + 10 H"(ад) — 10 Cr (аq) + I2(аq) + 5 Н2О(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 P(6) | H2О2(аg) | O2 (9) || н* (аq) | Pt(8)
Give the standard line notation for each cell. (а) 2 IO3 (аф) + 10 Ст2+ (ад) + 10 H* (ад) — 10 Сr+ (аg) + I2 (аq) + 5 Н2O() Pe(6) | Cr3+ (aq), Iz (aq) || Cr (ag), IО; (ад), н* (ад) | Рt (s) O Pt(s) | IO3 (ag), H* (ад), 12(аg) || Cr?+ (ag), Cr3+ (aq) | Pt(8) O Pt(s) | Cr²+ О Pt(s) | Cr?* (ag), IOз (ад), Н* (ад) || Cr* (ag), I2(aq) | Pt(s) (aq), Сr* (aq) || I0з (aq), H* (aд), 12 (aq) | Pt(s) (b) Со(s) + 2 Аg* (aq) — Cо?+ (aq) + 2 Ag(s) Ag(s) | Cо* (ад)|| Ag" (aq) | Co(s) Co(s) | Со* (ag) || Ag" (ag) | Ag(8) О Ag(8) | Ag* (ag) || Со?* (ад) | Со(s) о Со(8) | Ag* (ag) || Со** (аg) | Ag(s) 2+ 2+ 2+ (с) НаО2(ад) +2 H" (ад) + 2 е 2 HаО() Е — 1.78 V Оp(9) + 2 H* (аg) + 2 е Н2О2 (ag) E° = 0.68 V O Pt(s) | H2O2 (ag) | Pt(s) Pt(s) | H2O2(aq) | 02(g) || H* (aq) | Pt(s) О Pe(:) | О2(9) | Н-0- (аq), Н* (аq) || H,О2(аq), Н* (aq) | Pt(8) O Pt(s) | H2O2(aq), H† (aq) || O2 (9) | H2O2(aq), H† (aq) | Pt(s) (d) Mn+ (ag) +2е — Mn(s) Е— — 1.18 V = - Fe+ (aq) + 3 e → Fe(s) E° -0.036 V O Fe(s) | Mn2+ (ag) ||…
Give the standard line notation for each cell. (а) 2 IO3 (ад) + 10 Cr*+ (аg) + 10 H+(ад) — 10 Cr3+ (ад) + I2(ад) + 5 H20(1) O P(8) | Cr2+ (aq), Cr'+ (ag) || IOз (ад), Н* (аq), І, (ag) | Pt(8) O Pe(s:) | Cr* (ag), IOз (ад), н* (ag) || Cr* (ag), I> (aq) | Pt(8) O P($) | Cr* (aq), I, (aq) || Cr?* (aq), I0; (ад), Н* (аq) | Pt() O Pt(s) | IO3-(ag), H* (aq), I2(aq) || Cr²+ (ag), Cr³+ (aq) | Pt(s) 3+ 2+ (b) Со(8) + 2 Аgt (ag) — Cо?+ (ag) + 2 Ag(s) O Co(s) | Co+ (ag) || Ag* (aq) | Ag(s) O Ag(s) | Ag* (ag) || Со+ (aq) | Со(s) O Ag(s) | Co²+ (aq) || Ag* (ag) Co(s) O Co(s) | Ag*(ag) || Co2+ (ag) | Ag(s) (с) Н2О2(ад) +2H"(ад) + 2 е → 2 H20(1) E° 1.78 V Оp(9) + 2 H* (ад) + 2 е — Hа02 (аg) Е — 0.68 V O Pe(:) | О- (9) | H-02(аq), H* (ад) I| H-О2(aд), Н* (ад) | Pt(s) O Pt(s) | H2O2(ag), H† (aq) || O2(9) | H2O2(aq), H† (aq) | Pt(s) Pt(s) | H2O2(ag) | Pt(s) O Pt(s) | H2O2(ag) | O2 (9) || H† (ag) | Pt(s)