< Part B.: Determination of Oxidation NumberChanges for Reducing Agents >If you use [KMnO4] = 0.0252 M,Concentration of FeSO4*7 H2O = 5.70 g/LUsing a 100-mL graduated cylinder, 50 mL sample ofFeSO4*7 H2O will be measured out.To each sample of FeSO4*7 H2O, add 10.0 mL ofH2SO4 and 10 mL of H3PO4Concentration of SnCl2 2 H2O = 2.85 g/mLUsing a 100-mL graduated cylinder, 50.0 mLsample of SnCl2 + 2 H2O will be measured out.No additional acid is needed.•#1#1KMnOKMnOSampl44e #InitialFinalburet,buret,mLmLFeSO4• 712.05 21.51H2OSnCl20.079.542 H₂OQuestion) Answer the following questions.b) Determine mol of electron lost per mol of Sn ion.

the equilibrium constant (Kc) for the reaction between chromium(III) ions (Cr³⁺) and thiocyanate…

Answered: < Part B.: Determination of Oxidation…

Chemistry

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Chapter18: Electrochemistry

Section: Chapter Questions

Problem 36E: Consider the following galvanic cell: a. Label the reducing agent and the oxidizing agent, and...

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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)
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?
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?
. To obtain useful electrical energy from an oxidation-reduction process, we must set up the reaction in such a way that the Oxidation half-reaction and the reduction half-reaction are physically one _____another.
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 it not possible for hydroxide ion (OH-) to appear in either of the half-reactions or the overall equation when balancing oxidation—reduction reactions in acidic solution?
Consider the following galvanic cell: a. Label the reducing agent and the oxidizing agent, and describe the direction of the electron flow. b. Determine the standard cell potential. c. Which electrode increases in mass as the reaction proceeds, and which electrode decreases in mass?
In some old European churches, the stained-glass windowshave so darkened from corrosion and age that hardly anylight comes through. Microprobe analysis showed that tinycracks anddefects on the glass surface were enriched ininsoluble Mn(III) and Mn(IV) compounds. From AppendixE, suggest a reducing agent and conditions that might successfullyconvert thesecompounds to soluble Mn(II) withoutsimultaneously reducing Fe(III) (which gives the glassits colors) to Fe(II). Take MnO2 as representative of theinsoluble Mn(III) and Mn(IV) compounds.
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.
Which of the following are oxidation-reduction reactions’? Explain. a.PCl3+Cl2PCl5b.Cu+2AgNO3Cu( NO3)2+2Agc.CO2+2LiOHLi2CO3+H2Od.FeCl2+2NaOHFe(OH)2+2NaCIe.MnO2+4HClCl2+2H2O+MnCl2

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