Letter J only 1. Balance the following reactions in both acidic and basic media, identify the oxidation andreduction reactions, and identify the oxidizing and reducing agents.a. The oxidation of iodide ion I- by permanganate ion Mn0, in basic solution to yieldmolecular iodine I2 and manganese (IV) oxide Mn02.b. Fe2+ + Mn0,c. Sn + NO3 → Sn02 + NO2d. Zn + N03→ Fe3+ + Mn²+Zn2+ + NHf. Sn|Sniag)||Pbiag)|Pb(s)2+2+3+(aq)h. Pt|Cutag), Cuaq)||Mgaq)|Mg(s)i. Pt|Criag), Cr20aq)||C103(aq9), Clag)|Ptj. Mn(s)|Mnag)||Haq)|H2C9) |Pt2+

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Answered: I. i. Pt|Cra), Cr,0ag)||CLO3(aq),…

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Chemistry

I. i. Pt|Cra), Cr,0ag)||CLO3(aq), Cliag)|Pt j. Mn(s)|Mnaq)||Htaq)\H2c9) \Pt

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter18: Electrochemistry

Section: Chapter Questions

Problem 31Q: Consider the electrolysis of a molten salt of some metal. What information must you know to...

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Consider the electrolysis of a molten salt of some metal. What information must you know to calculate the mass of metal plated out in the electrolytic cell?
In the electrolysis of a solution containing Ag+(aq), metallic Ag(s) deposits on the cathode. Using a current of 1.12 A for 2.40 hours, what mass of silver forms?
Order the following oxidizing agents by increasing strength under standard-state conditions: O2(g); MnO4(aq); NO3 (aq) (in acidic solution ).
Order the following oxidizing agents by increasing strength under standard-state conditions: Ag+(aq); Cd2+(aq); MnO4(aq) (in acidic solution).
Use Table 17.1 to select (a) a reducing agent in acidic solution that converts ClO3- to Cl2 but not Cr2O72- to Cr3+. (b) an oxidizing agent that converts Mg to Mg2+ but not Mn to Mn2+. (c) a reducing agent in basic solution that converts NO2- to NO3- but not OH- to O2.
Consider the following electrochemical cell: a. If silver metal is a product of the reaction, is the cell a galvanic cell or electrolytic cell? Label the cathode and anode, and describe the direction of the electron flow. b. If copper metal is a product of the reaction, is the cell a galvanic cell or electrolytic cell? Label the cathode and anode, and describe the direction of the electron flow. c. If the above cell is a galvanic cell, determine the standard cell potential. d. If the above cell is an electrolytic cell, determine the minimum external potential that must be applied to cause the reaction to occur.
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?
Order the following oxidizing agents by increasing strength under standard-state conditions: Mg2+(aq), Hg2+(aq), Pb2+(aq).
A factory wants to produce 1.00 103 kg barium from the electrolysis of molten barium chloride. What current must be applied for 4.00 h to accomplish this?
Using Table 17.1, calculate E° for the reaction between (a) chromium(II) ions and tin(IV) ions to produce chromium(III) ions and tin(II) ions. (b) manganese(II) ions and hydrogen peroxide to produce solid manganese dioxide (MnO2)
What is electrochemistry? What are redox reactions? Explain the difference between a galvanic and an electrolytic cell.
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)