Balance the following half-reactions by adding the appropriate number of electrons (e-). Then, classify each reaction as an oxidation or reduction half-reaction. Note that for each of the four reactions, one of the gray boxes will be left blank and the other will be filled with electron(s). Use the symbol e- to represent an electron. Part 4 + 12(s) + 6H2O(I) > 2I0-3 + 12H+(aq) + - - --

Balance the following half-reactions by adding the appropriate number of electrons (e-). Then, classify each reaction as an oxidation or reduction half-reaction. Note that for each of the four reactions, one of the gray boxes will be left blank and the other will be filled with electron(s). Use the symbol e- to represent an electron. Part 4 + 12(s) + 6H2O(I) > 2I0-3 + 12H+(aq) + - - --

Fundamentals Of Analytical Chemistry

9th Edition

ISBN:9781285640686

Author:Skoog

Publisher:Skoog

Chapter18: Introduction To Electrochemistry

Section: Chapter Questions

Problem 18.11QAP

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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)?
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?
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)?
Atomic masses can be determined by electrolysis. In one hour, a current of 0.600 A deposits 2.42 g of a certain metal, M, which is present in solution as M+ ions. What is the atomic mass of the metal?
At 298 K, the solubility product constant for PbC2O4 is 8.5 1010, 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 PbC2O4(s)+2ePb(s)+C2O42(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/PbC2O4 electrode in a 0.025 M solution of Na2C2O4.
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
The iron content of hemoglobin is determined by destroying the hemoglobin molecule and producing small water-soluble ions and molecules. The iron in the aqueous solution is reduced to iron(II) ion and then titrated against potassium permanganate. In the titration, iron(ll) is oxidized to iron(III) and permanganate is reduced to manganese(II) ion. A 5.00-g sample of hemoglobin requires 32.3 mL of a 0.002100 M solution of potassium permanganate. The reaction with permanganate ion is MnO4(aq)+8H+(aq)+5Fe2+(aq)Mn2+(aq)+5Fe3+(aq)+4H2O What is the mass percent of iron in hemoglobin?
Balance the following skeleton equations. The reactions occur in acidic or basic aqueous solution, as indicated. a MnO4+S2MnO2+S8(basic) b IO3+HSO3I+SO42(acidic) c Fe(OH)2+CrO42Fe(OH)3+Ce(OH)4(basic) d Cl2Cl+ClO(basic)
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)?
An active (metal) electrode was found to gain mass as the oxidation-reduction reaction was allowed to proceed. Was the electrode part of the anode or cathode? Explain.
An electrolysis experiment is performed to determine the value of the Faraday constant (number of coulombs per mole of electrons). In this experiment, 28.8 g of gold is plated out from a AuCN solution by running an electrolytic cell for two hours with a current of 2.00 A. What is the experimental value obtained for the Faraday Constant?

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