2. Use the half reaction method to balance the reaction below in an acidicenvironment. (5 marks)a. Correct oxidation numbersb. Correct oxidation half reactionc. Correct reduction half reactiond. Correct number of water and hydrogen ions addede. Correct balance redox reactionOF + I →F2(aq)(aq)+(aq)3 (aq)

Part 2: Explanation:Step 1: Determine oxidation numbers:The oxidation number of oxygen (O) in OF2 is…

Answered: 2. Use the half reaction method to…

Chemistry: An Atoms First Approach

2nd Edition

ISBN:9781305079243

Author:Steven S. Zumdahl, Susan A. Zumdahl

Publisher:Steven S. Zumdahl, Susan A. Zumdahl

Chapter17: Electrochemistry

Section: Chapter Questions

Problem 17RORR: Specify which of the following equations represent oxidation reduction reactions, and indicate the...

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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?
(a) Rank the following metals in their ability to function as reducing agents: Hg, Sn, and Pb. (b) Which halogens will oxidize mercury to mercury(II)?
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)?
Specify which of the following equations represent oxidation reduction reactions, and indicate the oxidizing agent, the reducing agent, the species being oxidized, and the species being reduced. a. CH4(g)+H2O(g)CO(g)+3H2(g) b. 2AgNO3(aq)+Cu(s)Cu(NO3)2(aq)+2Ag(s) c. Zn(s)+2HCl(aq)ZnCl2(aq)+H2(g) d. 2H+(aq)+2CrO42-(aq)Cr2O72-(aq)+H2O(l)
Four metals, A, B, C, and D, exhibit the following properties: (a) Only A and C react with 1.0 M hydrochloric acid to give H2(g). (b) When C is added to solutions of the ions of the other metals, metallic B, D, and A are formed. (c) Metal D reduces Bn+ to give metallic B and Dn+. Based on this information, arrange the four metals in order of increasing ability to act as reducing agents.
One of the few industrial-scale processes that produce organic compounds electrochemically is used by the Monsanto Company to produce1,4-dicyanobutane. The reduction reaction is 2CH2CHCH+2H++2eNC(CH2)4CN The NC(CH2)4CN is then chemically reduced using hydrogen gas to H2N(CH2)6NH2, which is used in the production of nylon. What current must be used to produce 150.kg NC(CH2)4CN per hour?

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