Write a balanced half-reaction for the reduction of CrO 4 2–(aq) to Cr(OH) 3(s) in a basic solution. Write a balanced half-reaction for the reduction of CrO 4 2-(aq) to Cr(OH) 3(S) in a basic solution.А) CrO, (aq) +3 ОН (аq) + 3 е — Сr(ОН)3(s) + 2 Oz(g)CrO, (аq) + 3 н (аq) + 3 е- — Cr(ОН)3(9)(с) Сrо,(аq) +3 н (аq) — Сr(ОН)3(9) + 2 е-DCrog (aq) + 4 H-0()+ 3 е — Cr(ОH);(S) + 5 ОН (аq)E) CrOД (aq) +3 ОН (аq) — Cr(ОH)3(8) + 2 0-(g)

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Answered: balanced half-reaction

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balanced half-reaction

Chemistry & Chemical Reactivity

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ISBN:9781337399074

Author:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel

Publisher:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel

Chapter22: The Chemistry Of The Transistion Elements

Section: Chapter Questions

Problem 18PS

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1. If you wish to convert 0.0100 mol of Au3+ (aq) ions into Au(s) in a “gold-plating” process, how long must you electrolyze a solution if the current passing through the circuit is 2.00 amps? 483 seconds 4.83 104 seconds 965 seconds 1450 seconds
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)?
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?
A galvanic cell is based on the following half-reactions: In this cell, the copper compartment contains a copper electrode and [Cu2+] = 1.00 M, and the vanadium compartment contains a vanadium electrode and V2+ at an unknown concentration. The compartment containing the vanadium (1.00 L of solution) was titrated with 0.0800 M H2EDTA2, resulting in the reaction H2EDTA2(aq)+V2+(aq)VEDTA2(aq)+2H+(aq)K=? The potential of the cell was monitored to determine the stoichiometric point for the process, which occurred at a volume of 500.0 mL H2EDTA2 solution added. At the stoichiometric point, was observed to be 1 .98 V. The solution was buffered at a pH of 10.00. a. Calculate before the titration was carried out. b. Calculate the value of the equilibrium constant, K, for the titration reaction. c. Calculate at the halfway point in the titration.
Write balanced net ionic equations for the following reactions in acid solution. (a) Liquid hydrazine reacts with an aqueous solution of sodium bromate. Nitrogen gas and bromide ions are formed. (b) Solid phosphorus (P4) reacts with an aqueous solution of nitrate to form nitrogen oxide gas and dihydrogen phosphate (H2PO4-) ions. (c) Aqueous solutions of potassium sulfite and potassium permanganate react. Sulfate and manganese(II) ions are formed.
Answer the following questions by referring to standard electrode potentials at 25C. a Will oxygen, O2, oxidize iron(II) ion in solution under standard conditions? b Will copper metal reduce 1.0 M Ni2(aq) to metallic nickel?
An electrochemical cell consists of a standard hydrogen electrode and a copper metal electrode. If the copper electrode is placed in a solution of 0.10 M NaOH that is saturated with Cu(OH)2, what is the cell potential at 25C? [For Cu(OH)2, Ksp = 1.6 1019.]
The overall reaction for the production of Cu(OH)2 from Cu in oxygenated water can be broken into three steps: an oxidation half-reaction, a reduction half-reaction, and a precipitation reaction. a. Complete and balance the two missing half-reactions to give the overall equation for the oxidation of cooper in seawater. Oxidation half-reaction: ? Reduction half-reaction: ? Precipitation:Cu2+(aq)+2OH(aq)Cu(OH)2(s)Overall:Cu(s)+12O2(g)+H2O(l)Cu(OH)2(s) b. Determine the equilibrium constant for the overall reaction at 25 C using standard reduction potentials and the solubility product constant (Ksp) of Cu(OH)2(s).
Copper(I) ion disproportionates to copper metal and copper(ll) ion. (See Study Question 99.) 2 Cu+(aq) Cu(s) + Cu2 + (aq) (a) What two half-reactions make up the disproportionation reaction? (b) Use values of the standard reduction potentials for the two half-reactions in part (a) to determine whether this disproportionation reaction is product-favored at equilibrium. (c) What is the equilibrium constant for this reaction? If you have a solution that initially contains 0.10 mol of Cu+ in 1.0 L of water, what are the concentrations of Cu+ and Cu2+ at equilibrium?
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Although there are a number of magnesium-containing minerals, the commercial source of this metal is seawater. Treatment of seawater with Ca(OH)2 gives insoluble Mg(OH)2. This reacts with HCI to produce MgCl2, which is dried, and the metal is obtained by electrolysis of the molten salt. Write balanced net ionic equations for the three reactions described here.
Complete and balance the following oxidation–reductionreaction in basic solution:Cr(OH)3(s) + ClO-(aq)---->CrO42-(aq) + Cl2(g)

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