Write down the balanced redox equations (including the chemical equations for the oxidation and reduction halfreactions). Write down all ions with their counterions in the final equation. Stellen Sie die ausgeglichenen Reaktionsgleichungen auf (inklusive der Halbreaktionsgleichungen für Oxidation und Reduktion). Schreiben Sie alle lonen inklusive der dazugehörenden Gegenionen in der Gesamtgleichung auf. (a) Aluminiumtribromide reacts with potassium permanganate in diluted sulfuric acid and manganese(II) and elemental bromine are formed. Aluminiumtribromide reagiert mit Kaliumpermanganat in verdünnter Schwefelsäure und bildet dabei Mangan(II) und elementares Brom. (b) Potassium dichromate (which is only stable under acidic conditions) reacts with hydrogen peroxide and chromium(III) and oxygen are formed. Kaliumdichromat (das nur im Sauren stabil ist) reagiert mit Wasserstoffperoxid und bildet dabei Chrom(III) und Sauerstoff.

Write down the balanced redox equations (including the chemical equations for the oxidation and reduction halfreactions). Write down all ions with their counterions in the final equation. Stellen Sie die ausgeglichenen Reaktionsgleichungen auf (inklusive der Halbreaktionsgleichungen für Oxidation und Reduktion). Schreiben Sie alle lonen inklusive der dazugehörenden Gegenionen in der Gesamtgleichung auf. (a) Aluminiumtribromide reacts with potassium permanganate in diluted sulfuric acid and manganese(II) and elemental bromine are formed. Aluminiumtribromide reagiert mit Kaliumpermanganat in verdünnter Schwefelsäure und bildet dabei Mangan(II) und elementares Brom. (b) Potassium dichromate (which is only stable under acidic conditions) reacts with hydrogen peroxide and chromium(III) and oxygen are formed. Kaliumdichromat (das nur im Sauren stabil ist) reagiert mit Wasserstoffperoxid und bildet dabei Chrom(III) und Sauerstoff.

Fundamentals Of Analytical Chemistry

9th Edition

ISBN:9781285640686

Author:Skoog

Publisher:Skoog

Chapter20: Applications Of Oxidation/reduction Titrations

Section: Chapter Questions

Problem 20.28QAP

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Why is it not possible for hydrogen ion (H+) to appear in either of the half-reactions or the overall equation when balancing oxidationreduction reactions in basic solution?
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.
Using data from Table 17-1, place the following in order of increasing strength as reducing agents (all under standard conditions). Cu+,F,H,H2O,I2,K
Use Table 17.1 to answer the following questions. Use LT (for is less than), GT (for is greater than), EQ (for is equal to), or MI (for more information required). (a) For the half reaction 12Br2(l)+eBr(aq)Ered1.077 v. (b) For the reaction 2Br(aq)+Co2+(aq)Br2(l)+Co(s)E0. (c) If the half reaction Co2+(aq)+2eCo(s) is designated as the new standard where Ered is 0.00, then Ered for 2H+(aq)+2eH2(g) is 0. (d) For the reaction 2Cr3+(aq)+3Co(s)2Cr(s)+3Co2+(aq) the number of electrons exchanged is6. (e) For the reaction described in (d), the number of coulombs that passes through the cell is9.648104 .
Give balanced equations for the overall reaction in the electrolysis of molten lithium chloride and for the reactions occurring at the electrodes. You may wish to review the Chapter on electrochemistry for relevant examples.
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?
Based on the cell potential measured for the cells Co(s)|Co2+(aq) Cu 2+( aq)|Cu( s)E=0.614VFe(s)|Fe2+(aq) Cu 2+( aq)|Cu( s)E=0.777V what potential should you expect to find for the following cell? Fe(s)|Fe2+(aq)Co2+(aq)|Co(s)
Consider a salt bridge cell in which the anode is a manganese rod immersed in an aqueous solution of manganese(II) sulfate. The cathode is a chromium strip immersed in an aqueous solution of chromium(III) sulfate. Sketch a diagram of the cell, indicating the flow of the current throughout. Write the half-equations for the electrode reactions, the overall equation, and the abbreviated notation for the cell.
Electrochemical Cells II Consider this cell running under standard conditions: Ni(s)Ni2(aq)Cu+(aq)Cu(s) a Is this cell a voltaic or an electrolytic cell? How do you know? b Does current flow in this cell spontaneously? c What is the maximum cell potential for this cell? d Say the cell is connected to a voltmeter. Describe what you might see for an initial voltage and what voltage changes, if any, you would observe as time went by. e What is the free energy of this cell when it is first constructed? f Does the free energy of the cell change over time as the cell runs? If so, how does it change?
What is electrochemistry? What are redox reactions? Explain the difference between a galvanic and an electrolytic cell.
An aqueous solution of an unknown salt of vanadium is electrolyzed by a current of 2.50 amps for 1.90 hours. The electroplating is carried out with an efficiency of 95.0%, resulting in a deposit of 2.850 g of vanadium. a How many faradays are required to deposit the vanadium? b What is the charge on the vanadium ions (based on your calculations)?
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

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