Consider the following half-reactions:Half-reactionAg+(aq) + eE° (V)Ag(s) 0.799V2H+(aq) + 2eAl3+(aq) + 3e¯→H2(g) 0.000VAl(s) -1.660V(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 Ag*(aq) oxidize Al(s) to Al3+(aq)?(6) Which species can be reduced by H2(g)?If none, leave box blank. Consider the following half-reactions:Half-reactionF2(g) + 2e2F˜(aq)Pb2+(aq) + 2eMg2+(aq) + 2eE° (V)2.870VPb(s) -0.126VMg(s)-2.370V(1) The strongest oxidizing agent is:(2) The weakest oxidizing agent is:(3) The weakest reducing agent is:(4) The strongest reducing agent is:(5) Will Mg2+(aq) oxidize F*(aq) to F2(g)?(6) Which species can be reduced by Pb(s)?|If none, leave box blank.enter formula

Answered: Consider the following half-reactions:…

Principles of Modern Chemistry

8th Edition

ISBN:9781305079113

Author:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler

Publisher:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler

Chapter17: Electrochemistry

Section: Chapter Questions

Problem 77AP

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Question

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Consider the following half-reactions:
Half-reaction
Ag+(aq) + e
E° (V)
Ag(s) 0.799V
2H+(aq) + 2e
Al3+(aq) + 3e¯
→H2(g) 0.000V
Al(s) -1.660V
(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 Ag*(aq) oxidize Al(s) to Al3+(aq)?
(6) Which species can be reduced by H2(g)?
If none, leave box blank.

Consider the following half-reactions:
Half-reaction
F2(g) + 2e2F˜(aq)
Pb2+(aq) + 2e
Mg2+(aq) + 2e
E° (V)
2.870V
Pb(s) -0.126V
Mg(s)-2.370V
(1) The strongest oxidizing agent is:
(2) The weakest oxidizing agent is:
(3) The weakest reducing agent is:
(4) The strongest reducing agent is:
(5) Will Mg2+(aq) oxidize F*(aq) to F2(g)?
(6) Which species can be reduced by Pb(s)?|
If none, leave box blank.
enter formula

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The following two half-reactions arc involved in a voltaic cell. At standard conditions, what species is produced at each electrode? Ag++eAgE=0.80VNi2++2eNiE=0.25V
What is the standard cell potential you would obtain from a cell at 25C using an electrode in which Hg22+(aq) is in contact with mercury metal and an electrode in which an aluminum strip dips into a solution of Al3+(aq)?
Calculate the standard cell potential at 25C for the following cell reaction from standard free energies of formation (Appendix C). Mg(s)+2Ag+(aq)Mg2+(aq)+2Ag(s)
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At 298 K, the solubility product constant for Pb(IO3)2 is 2.6 1013, and the standard reduction potential of the Pb2+(aq) to Pb(s) is 0.126 V. (a) Find the standard potential of the half-reaction Pb(IO3)2(s)+2ePb(s)+2IO3(aq) (Hint: The desired half-reaction is the sum of the equations for the solubility product and the reduction of Pb2+. Find G for these two reactions, and add them to find G for their sum. Convert the G to the potential of the desired half-reaction.) (b) Calculate the potential of the Pb/Pb(IO3)2 electrode in a 3.5 103 M solution of NaIO3.
For the following half-reactions, answer these questions. Ce4+(aq)+eCe3+(aq)E=+1.61VAg+(aq)+eAg(s)E=+0.80VHg22+(aq)+2e2Hg(l)E=+0.80VSn2+(aq)+2eSn(s)E=0.14VNi2+(aq)+2eNi(s)E=0.24VAl3+(aq)+3eAl(s)E=1.68V (a) Which is the weakest oxidizing agent? (b) Which is the strongest oxidizing agent? (c) Which is the strongest reducing agent? (d) Which is the weakest reducing agent? (e) Will Sn(s) reduce Ag+(aq) to Ag(s)? (f) Will Hg(l) reduce Sn2+(aq) to Sn(s)? (g) Which ion(s) can be reduced by Sn(s)? (h) Which metal(s) can be oxidized by Ag+(aq)?
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For the following half-reactions, answer the questions below. Co3+(aq)+eCo2+(aq)E=+1.953VFe3+(aq)+eFe2+(aq)E=+0.769VI2(aq)+2e2I(aq)E=+0.534VPb2+(aq)+2ePb(s)E=0.127VCd2+(aq)+2eCd(s)E=0.402VMn2+(aq)+2eMn(s)E=1.182V (a) Which is the weakest reducing agent? (b) Which is the strongest reducing agent? (c) Which is the strongest oxidizing agent? (d) Which is the weakest oxidizing agent? (e) Will Pb(s) reduce Fe3+(aq) to Fe2+(aq)? (f) Will I-(aq) reduce Pb2+(aq) to Pb(s)? (g) Which ion(s) can be reduced by Pb(s)? (h) Which if any metal(s) can be oxidized by Fe3+(aq)?
A solution of copper(II) sulfate is electrolyzed by passing a current through the solution using inert electrodes. Consequently, there is a decrease in the Cu2+ concentration and an increase in the hydronium ion concentration. Also, one electrode increases in mass and a gas evolves at the other electrode. Write half-reactions that occur at the anode and at the cathode.
Consider the following cell running under standard conditions: Fe(s)Fe2+(aq)Al3+(aq)Al(s) a Is this a voltaic cell? b Which species is being reduced during the chemical reaction? c Which species is the oxidizing agent? d What happens to the concentration of Fe3+(aq) as the reaction proceeds? e How does the mass of Al(s) change as the reaction proceeds?
Follow the directions of Question 39 for the following half-reactions: 1. I2(s)+2e2I(aq) 2. Co3+(aq)+eCo2+(aq) 3. Cr2O72(aq)+14H+(aq)+6e2Cr3+(aq)+7H2O

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