Consider the following half-reactions:Half-reactionE° (V)Hg-"(aq) + 2e"Hg(1) 0.855V2+,Pb2*(aq) + 2e → Pb(s)-0.126VZn*(aq) + 2e" – Zn(s) -0.763V(1) The weakest oxidizing agent is:enter formula(2) The strongest reducing agent is:(3) The strongest oxidizing agent is:(4) The weakest reducing agent is:(5) Will Zn(s) reduce Hg*"(aq) to Hg(1?(6) Which species can be reduced by Pb(s)?If none, leave box blank.

These questions are based on oxidation and reduction potentials . Reaction will be spontaneous if…

Answered: Consider the following half-reactions:…

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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Consider the following unbalanced oxidation-reductionreactions in aqueous solution:Ag+(aq) + Li(s)----> Ag(s) + Li+(aq)Fe(s) + Na+(aq)----> Fe2+ (aq) + Na(s)K(s) + H2O(l)---->KOH(aq) + H2(g)(a) Balance each of the reactions. (b) By using data inAppendix C, calculate ΔH° for each of the reactions.(c) Based on the values you obtain for ΔH°, which of the reactionswould you expect to be thermodynamically favored?(d) Use the activity series to predict which of these reactionsshould occur. Are these results in accordwith your conclusion in part (c) of this problem?
Consider the following cell. Ag(s)|AgCI(s)|NaCI(aq)|Hg2Cl2(s)|Hg(/)|Pt(s) (a) Write the half-cell reactions. (Include states-of-matter under the given conditions in your answer.) Cathode: chemPad Help Greek - Anode: chemPad O Help X.X"| Greek - (b) The standard emfs of the cell at several temperatures are as follows. T/K 291 298 303 311 E°/mV 43.0 45.4 47.1 50.1 Calculate the values of A,G°, A,Sº, and A,H° for the reaction at 303 K. A,G°: A,S° kJ•mol-1 J-mol -1.к-1 %3D A,H° kJ•mol-1
Using the Table of Standard Electrode Potentials (Appendix L, page 1251), calculate the E°cell for each of the following reactions and predict whether each redox reaction is spontaneous or non-spontaneous. 2. 3+, (a) Au(s) + NO; (aq) + 4H*(aq) → Au³*(aq) + NO(g) + 2H2O(); (b) Сu's) + 2Fe?" (ag) —> Сu?"(aq) + Fe(s) ; (c) 2Fe" (ag) + 21 (aд) —> I2(ад) + 2Fe?"(aq); 2+ (d) Zn(OH)2(s) + 4NH3(aq) → Zn(NH3)4*(aq) + 20H (aq);
Calculate AG° f( in kJ) or the reaction of iron(II) ions with permanganate ions. (F =96500 C) MnO4 (aq) + 8H*(aq) + 5e → Mn2+(aq) + 4H20(1) E° = 1.51 V Fe3+ (aq) + e → Fe2*(aq) E°= 0.77 V
Consider the following half-reactions: Half-reaction E° (V) 2+ Hg"(aq) + 2e → Hg(1) 0.855V Co**(aq) + 2e → Co(s) -0.280V 2+ Fe"(aq) + 2e → Fe(s) |-0.440v (1) The strongest oxidizing agent is: enter formula (2) The weakest oxidizing agent is: (3) The weakest reducing agent is: (4) The strongest reducing agent is: (5) Will Hg*(aq) oxidize Fe(s) to Fe2*(aq)?| (6) Which species can be oxidized by Co2*(aq)? If none, leave box blank.
Consider the following half-reactions: Half-reaction E° (V) F2(g) + 2e → 2F*(aq) 2.870V Co2+*(aq) + 2e → Co(s) |-0.28OV 2+ Mg"(aq) + 2e → Mg(s) -2.37OV (1) The weakest oxidizing agent is: enter formula (2) The strongest reducing agent is: (3) The strongest oxidizing agent is: (4) The weakest reducing agent is: (5) Will Mg(s) reduce F2(g) to F"(aq)? (6) Which species can be reduced by Co(s)? If none, leave box blank.
3:19 PM Thu May 4 * 8 J ↑ M ● ( 9 K 8 H x H₂O O O 9 L cmd = (aq) P H3O+ "' X 0 : ; { [ 300 option ? 1 50 69% Ï Submit 1 delete 1
Give the standard line notation for each cell. (a) 2 IO3 (aq) + 10 Fe2+ (ag) + 10 H* (aq) = 10 Fet (ag) + I2 (aq) + 5 H2O(1) O Pt(s) | Fe?+ (aq), Fe+ (ag) || IO3 (ag), Ht (ag), I2 (ag) | Pt(s) O Pt(s) | Fet (aq), I2 (ag) || Fe2+ (ag), IO3 (ag), H* (ag) | Pt(s) Pt(s) | IO3 (ag), H* (ag), I2 (aq) || Fe2+ (ag), Fet (ag) | Pt(s) Pt(s) | Fe2+ (ag), IO3 (ag), H* (aq) || Fet (aq), I2 (ag) | Pt(s) (b) Zn(s) + 2 Ag* (ag) = Zn?+ (aq) + 2 Ag(s) O Zn(s) | Zn?+ (aq) || Ag* (aq) | Ag(s) O Zn(s) | Ag* (aq) || Zn?+ (ag) | Ag(s) Ag(s) | Ag* (ag) || Zn2+ (aq) | Zn(s) O Ag(s) | Zn?+ (aq) || Ag* (aq) | Zn(s) (c) H2O2 (aq) + 2 H* (ag) + 2 e → 2 H2O(1) E = 1.78 V 02 (9) + 2 H* (ag) + 2 e + H2O2 (ag) E = 0.68 V O Pt(s) | O2(9) | H2O2 (aq), H* (ag) || H2O2 (ag), H* (ag) | Pt(s) Pt(s) | H2O2 (aq), H* (ag) || O2 (9) | H2O2 (ag), H* (ag) | Pt(s) Pt(s) | H2O2 (aq) | O2(9) || H* (aq) | Pt(s) O Pt(s) | H2O2(aq) | Pt(s) (d) Mn2+ (aq) + 2 e → Mn(s) E° = - 1.18 V Fe+ (aq) + 3 e → Fe(s) E - -0.036 V O Mn(s) | Mn²+ (ag)…
(19) Consider the following redox reaction that occurs in a voltaic cell: Cr2+ (aq) + Cu²+ (aq) → Cr³+ (aq) + Cut (aq) If the cell is operating at 25°C, what is the value of the equilibrium constant (Keq)? (A) 1.41 x 10¹1 1.19 x 1018 5.53 x 105 2.79 x 1033 1.81 x 10-6 (B) (C) (D) (E)
An electrochemical cell consists of a silver metal electrode immersed in a solution with Ag* = 1.0 M separated by a porous disk from a copper metal electrode. If the copper electrode is placed in a solution of 5.0 MNH3 that is also 0.0080M in Cu(NH3),+, what is the cell potential at 25°C? Cu?+ (ag) + 4 NH3 (aq) = Cu(NH3)4²* (aq) K = 1.0 × 1013 Cell potential V
(a) A silver wire is placed in a solution of CuCl₂. Does this reaction occur under standard conditions? O The reaction occurs. No reaction occurs. (b) Cl2 gas is bubbled into a solution of Nal. Write a balanced net-ionic equation. (Use the lowest possible coefficients. Specify states such as (aq) or (s). If a box is not needed, leave it blank.) 21 (aq) +C1₂(g) Calculate E, AG, and K. E = 0.82 AG = -158.235 K =7.345x10^13 →2Cl(aq) + 1,(s) The reaction occurs. O No reaction occurs. V kj Does this reaction occur, under standard conditions?
What is the balanced equation for the galvanic cell reaction expressed using the following shorthand notation? Mg (s) | Mg2+ (aq) || Cl2 (g) | Cl– (aq) | C (s)

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