Sub O Previous Page 9 of 10 Next. Consider the following reaction in acidic solution, along with the half-reactions: I(ag) + ClO (ag) I,(ag) + CI (ag) Half-reactions: CiO + CI After determining the half-reactions, the next step in balancing oxidation-reduction equations using the half-reaction method is to balance each half-reaction. Select the correctly balanced half-reactions.for the reaction above: (Select all that apply) O CIO (ag) + CI (aq) + H20(1) O CIO (ag) 2H (aq) + CIO (aq) + CI (ag) + H20(1) O 2e + 2H* (ag) + CIO (ag) CI (ag) + H20(1) O 31 (ag) →5(ag) + 2e O 31 (aq) +5(aq) CI (ag) + H20(1) + 2H* (ag) https://ais-asp.cengage.info/als-asp/take Save and Exit

Sub O Previous Page 9 of 10 Next. Consider the following reaction in acidic solution, along with the half-reactions: I(ag) + ClO (ag) I,(ag) + CI (ag) Half-reactions: CiO + CI After determining the half-reactions, the next step in balancing oxidation-reduction equations using the half-reaction method is to balance each half-reaction. Select the correctly balanced half-reactions.for the reaction above: (Select all that apply) O CIO (ag) + CI (aq) + H20(1) O CIO (ag) 2H (aq) + CIO (aq) + CI (ag) + H20(1) O 2e + 2H* (ag) + CIO (ag) CI (ag) + H20(1) O 31 (ag) →5(ag) + 2e O 31 (aq) +5(aq) CI (ag) + H20(1) + 2H* (ag) https://ais-asp.cengage.info/als-asp/take Save and Exit

Chemistry: Principles and Reactions

8th Edition

ISBN:9781305079373

Author:William L. Masterton, Cecile N. Hurley

Publisher:William L. Masterton, Cecile N. Hurley

Chapter17: Electrochemistry

Section: Chapter Questions

Problem 101QAP: Use Table 17.1 to answer the following questions. Use LT (for is less than), GT (for is greater...

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Consider a salt bridge cell in which the anode is a manganese rod immersed in an aqueous solution of manganese(II) sulfate. The cathode is a chromium strip immersed in an aqueous solution of chromium(III) sulfate. Sketch a diagram of the cell, indicating the flow of the current throughout. Write the half-equations for the electrode reactions, the overall equation, and the abbreviated notation for the cell.
Consider the following standard reduction potentials: Tl+(aq)+eTl(s)Ered=0.34VTl3+(aq)+3eTl(s)Ered=0.74VTl3+(aq)+2eTl+(aq)Ered=1.28V and the following abbreviated cell notations: (1) Tl|Tl+Tl3+,Tl+|Pt (2) Tl|Tl3+Tl3+,Tl+|Pt (3) Tl|Tl+Tl3+|Tl (a) Write the overall equation for each cell. (b) Calculate E° for each cell. (c) Calculate G° for each overall equation. (d) Comment on whether G° and/or E° are state properties. (Hint: A state property is path-independent.)
Consider a voltaic cell in which the following reaction occurs. Zn(s)+Sn2+(aq)Zn2+(aq)+Sn(s) (a) Calculate E° for the cell. (b) When the cell operates, what happens to the concentration of Zn2+? The concentration of Sn2+? (c) When the cell voltage drops to zero, what is the ratio of the concentration of Zn2+ to that of Sn2+? (d) If the concentration of both cations is 1.0 M originally, what are the concentrations when the voltage drops to zero?
Consider three metals, X, Y, and Z, and their salts, XA, YA, and ZA. Three experiments take place with the following results: • X+hotH2Obubbles • X+YAnoreaction • X+ZAXdiscolored+Z Rank metals X, Y, and Z, in order of decreasing strength as reducing agents.
Consider only the species (at standard conditions) Na+, Cl, Ag+, Ag, Zn2+, Zn, Pb in answering the following questions. Give reasons for your answers. (Use data from Table 17-1.) a. Which is the strongest oxidizing agent? b. Which is the strongest reducing agent? c. Which species can be oxidized by SO42 (aq) in acid? d. Which species can be reduced by Al(s)?
Why is a salt bridge necessary in galvanic cells like the one in Figure 17.4?
In biological systems, acetate ion is converted to ethyl alcohol in a two-step process: CH3COO(aq)+3H+(aq)+2eCH3CHO(aq)+H2OE=0.581V CH3CHO(aq)+2H+(aq)+2eC2H5OH(aq)E=0.197V (E°' is the standard reduction voltage at 25°C and pH of 7.00.) (a) Calculate G°' for each step and for the overall conversion. (b) Calculate E°' for the overall conversion.
Given the following pairs of balanced half-reactions, determine the balanced reaction for each pair of half-reactions in an acidic solution. (a) CaCa2++2e,F2+2e2F (b) LiLi++e,Cl2+2e2Cl (c) FeFe3++3e,Br2+2e2Br (d) AgAg++e,MnO4+4H++3eMnO2+2H2O
Which of the following statement(s) is/are true? a. Copper metal can be oxidized by Ag+ (at standard conditions). b. In a galvanic cell the oxidizing agent in the cell reaction is present at the anode. c. In a cell using the half reactions Al3+ + 3e Al and Mg2+ + 2e Mg, aluminum functions as the anode. d. In a concentration cell electrons always flow from the compartment with the lower ion concentration to the compartment with the higher ion concentration. e. In a galvanic cell the negative ions in the salt bridge flow in the same direction as the electrons.
Use Table 17.1 to answer the following questions. Use LT (for is less than), GT (for is greater than), EQ (for is equal to), or MI (for more information required). (a) For the half reaction 12Br2(l)+eBr(aq)Ered1.077 v. (b) For the reaction 2Br(aq)+Co2+(aq)Br2(l)+Co(s)E0. (c) If the half reaction Co2+(aq)+2eCo(s) is designated as the new standard where Ered is 0.00, then Ered for 2H+(aq)+2eH2(g) is 0. (d) For the reaction 2Cr3+(aq)+3Co(s)2Cr(s)+3Co2+(aq) the number of electrons exchanged is6. (e) For the reaction described in (d), the number of coulombs that passes through the cell is9.648104 .
Balance the following reactions and write the reactions using cell notation. Ignore any inert electrodes, as they are never part of the half-reactions. (a) Al(s)+Zr4+(aq)Al3+(aq)+Zr(s) (b) Ag+(aq)+No(g)Ag(s)+NO3(aq) (acidic solution). (C) SiO32(aq)+Mg(s)Si(s)+Mg(OH)2(s) (basic solution). (d) CIO3(aq)+MnO2(s)CI(aq)+MnO4(aq) (basic solution)
Calculate E° for the following voltaic cells: (a) 2Na(s)+Fe2+(aq)2Na+(aq)+Fe(s) (b) 3SO42(aq)+12H+(aq)+2Al(s)3SO2(g)+2Al3+(aq)+6H2O (c) 2S(s)+4OH(aq)O2(g)+2S2(aq)+2H2O (basic)