GENERAL CHEMISTRY-MOD.MASTERINGCHEM.
11th Edition
ISBN: 9780134193601
Author: Petrucci
Publisher: PEARSON
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Chapter 19, Problem 91IAE
Interpretation Introduction
Interpretation:
Whether the color of solution appears blue or not if
Concept introduction:
In an
The half-cell reaction with the lowest reduction potential reduces 1st in electrolysis process.
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The formation constant for the mercury acetate complex is
Hg2+ + 2OAc- ....................> Hg(OAc)2(aq) Kf=2.7*10^8
<.......................
calculate the standard potential for half-reaction
Hg(OAc)2(aq) + 2e- ...........> Hg(l) + 2OAc-
The standard reduction potential for the reaction [Co(H2 O)6]3+(aq) + e− ⟶ [Co(H2 O)6]2+(aq) is about 1.8 V. The reduction potential for the reaction [Co(NH3)6]3+(aq) + e− ⟶ [Co(NH3)6]2+(aq) is +0.1 V. Calculate the cell potentials to show whether the complex ions, [Co(H2O)6]2+ and/or [Co(NH3)6]2+, can be oxidized to the corresponding cobalt(III) complex by oxygen.
(TRUE OR FALSE)
In the electrolysis of aqueous KBr, the two competing reactions in the anode are the oxidation of K+ ion and the oxidation of H2O.
[Pt(py)4][Pt(CN)6] and [Pt(py)4(CN)2][Pt(CN)4] are a pair of ionization isomers.
A very large Kf value indicates that the dissociation of the complex is strongly favored.
Chapter 19 Solutions
GENERAL CHEMISTRY-MOD.MASTERINGCHEM.
Ch. 19 - From the observations listed, estimate the value...Ch. 19 - You must estimate E for e half-cell reaction...Ch. 19 - Ecol=0.201V for the reaction...Ch. 19 - Ascorbic acid ( C6H6C6 , also commonly known as...Ch. 19 - Given that Ecol for the aluminum-air batter is...Ch. 19 - The theoretical Ecol for the methane-oxygen fuel...Ch. 19 - The following sketch is of a voltaic cell...Ch. 19 - Given these half-cell reactions and associated...Ch. 19 - Prob. 9ECh. 19 - Use standard reduction potentials to predict which...
Ch. 19 - Assume that all reactants and products are in...Ch. 19 - For the readuction half-cell reactions...Ch. 19 - Use date from Table 19.1 to predict whether, to...Ch. 19 - Prob. 14ECh. 19 - Dihromate ion (C2I72-) in acidic solution is a...Ch. 19 - Prob. 16ECh. 19 - Prob. 17ECh. 19 - Predict whether, to any significant extent. a....Ch. 19 - Write cell reactions for the electrochemical cells...Ch. 19 - Write the half-cell reactions and the balanced...Ch. 19 - Prob. 21ECh. 19 - In each of the following examples, sketch a...Ch. 19 - Use the data in Appendix D to calculate the...Ch. 19 - Write a cell diagram and call diagram the value of...Ch. 19 - Determine the values of tG for the following...Ch. 19 - Prob. 26ECh. 19 - Prob. 27ECh. 19 - Consider the voltaic cell below....Ch. 19 - Prob. 29ECh. 19 - Prob. 30ECh. 19 - Prob. 31ECh. 19 - The theoretical voltage of the aluminum-air...Ch. 19 - Prob. 33ECh. 19 - Prob. 34ECh. 19 - Prob. 35ECh. 19 - Prob. 36ECh. 19 - Prob. 37ECh. 19 - Use the Nernst equation and data from Appendix D...Ch. 19 - Prob. 39ECh. 19 - Prob. 40ECh. 19 - If [Zn2+] is maintained at 1.0 M, a. what the...Ch. 19 - Prob. 42ECh. 19 - Prob. 43ECh. 19 - Prob. 44ECh. 19 - Consider the voltaic cell Mg Mg(s)Mg2+ (satd Mg2(...Ch. 19 - Prob. 46ECh. 19 - For the voltaic cell,...Ch. 19 - For the voltaic cell,...Ch. 19 - Prob. 49ECh. 19 - Derive e balanced equation for the reaction...Ch. 19 - Prob. 51ECh. 19 - Prob. 52ECh. 19 - Prob. 53ECh. 19 - Prob. 54ECh. 19 - Prob. 55ECh. 19 - Prob. 56ECh. 19 - Prob. 57ECh. 19 - Prob. 58ECh. 19 - Refer to Figure 19-20, . end describe en words or...Ch. 19 - Prob. 60ECh. 19 - Natural gas transmission pipes are sometimes...Ch. 19 - Prob. 62ECh. 19 - How many gram of metal are deposited at the...Ch. 19 - A quantity of electric charge brings about the...Ch. 19 - Which of the blowing reactions occur spontaneously...Ch. 19 - An aqueous solution of K2SO4 , is electrolyzed by...Ch. 19 - Prob. 67ECh. 19 - Prob. 68ECh. 19 - Calculate the quantity indicated for each of the...Ch. 19 - Calculate the quantity indicated for each of the...Ch. 19 - Prob. 71ECh. 19 - Prob. 72ECh. 19 - Prob. 73ECh. 19 - A solution containing a mixture of a platinum(H)...Ch. 19 - Prob. 75IAECh. 19 - Suppose that a fully charged lead-acid battery...Ch. 19 - Prob. 77IAECh. 19 - For the half-cell reaction...Ch. 19 - Prob. 79IAECh. 19 - Prob. 80IAECh. 19 - Describe a laboratory experiment that you co...Ch. 19 - Prob. 82IAECh. 19 - Prob. 83IAECh. 19 - Prob. 84IAECh. 19 - Prob. 85IAECh. 19 - Prob. 86IAECh. 19 - Prob. 87IAECh. 19 - A common reference electrode consists of a silver...Ch. 19 - The electrodes in the following electrochemical...Ch. 19 - Prob. 90IAECh. 19 - Prob. 91IAECh. 19 - A solution is prepared by saturating 1000 mL of...Ch. 19 - Prob. 93IAECh. 19 - Prob. 94IAECh. 19 - Prob. 95IAECh. 19 - Prob. 96IAECh. 19 - Prob. 97IAECh. 19 - Prob. 98IAECh. 19 - Prob. 99IAECh. 19 - Prob. 100IAECh. 19 - Consider the following electrochemical cell:...Ch. 19 - Prob. 102FPCh. 19 - Prob. 103FPCh. 19 - Prob. 104FPCh. 19 - Prob. 105FPCh. 19 - Consider two cells involving two metals X and Y...Ch. 19 - Prob. 107FPCh. 19 - Prob. 108FPCh. 19 - Some electrochemical cells employ large biological...Ch. 19 - Prob. 110FPCh. 19 - Prob. 111SAECh. 19 - Prob. 112SAECh. 19 - Explain the important distinctions between each...Ch. 19 - Prob. 114SAECh. 19 - Prob. 115SAECh. 19 - Prob. 116SAECh. 19 - Prob. 117SAECh. 19 - The gas evolved at e anode when K2SO4(aq) is...Ch. 19 - Prob. 119SAECh. 19 - Prob. 120SAECh. 19 - Prob. 121SAECh. 19 - The following voltaic cell registers an...Ch. 19 - Prob. 123SAECh. 19 - For each of the following combination of...Ch. 19 - Prob. 125SAECh. 19 - Prob. 126SAECh. 19 - Prob. 127SAECh. 19 - Construct a concept map illustrating the...
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Need a deep-dive on the concept behind this application? Look no further. Learn more about this topic, chemistry and related others by exploring similar questions and additional content below.Similar questions
- The formation constant for the mercury(II) acetate complex is Hg2++ 2OAc- Hg(OAc)2(aq) Kf = 2.7 108 Calculate the standard potential for the half-reaction Hg(OAc)2(aq) + 2e- Hg(l) + 2OAc-arrow_forwardUse the formation constant of [Au(CN)2] in Appendix K to determine the equilibrium concentration of Au+(aq) in a solution that is 0.0071 M CN and 1.1 104 M [Au(CN)2]. Is it reasonable to conclude that 100% of the gold in solution is present as the [Au(CN)2] complex ion? Explain.arrow_forwardThe standard reduction potential for the reaction [Co( H 2 O)6]3+(aq)+e[CO( H 2 O)6]2+(aq) is about 1.8 V. The reduction potential for the reaction [Co( NH 3 )6]3+(aq)+e[Co( NH 3 )6]2+(aq) is +0.1 V. Calculate the cell potentials to show whether the complex ions,. [Co( H 2 O)6]2+ and or [Co( NH 3 )6]2+, can be oxidized to the corresponding Cobalt (III) complex by oxygen.arrow_forward
- 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)?arrow_forwardAnswer 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?arrow_forwardThe photographs below (a) show what occurs when a solution of iron(III) nitrate is treated with a few drops of aqueous potassium thiocyanate. The nearly colorless iron(III) ion is converted to a red [Fe(H2O)5SCN)2+ ion. (This is a classic test for the presence of iron(III) ions in solution.) [Fe(H2O)6]3+(aq) + SCN(aq) [Fe(H2O)5SCN]2+(aq) + H2O() (a) As more KSCN is added to the solution, the color becomes even more red. Explain this observation. (b) Silver ions form a white precipitate with SCN ions. What would you observe on adding a few drops of aqueous silver nitrate to a red solution of [Fe(H2O)5 SCN]+ ions? Explain your observation.arrow_forward
- Consider the following half-reactions: IrCl63-+3e-Ir+6Cl-E=0.77VPtCl42-+2e-Pt+4Cl-E=0.73VPdCl42-+2e-Pd+4Cl-E=0.62V A hydrochloric acid solution contains platinum, palladium, and iridium as chloro-complex ions. The solution is a constant 1.0 M in chloride ion and 0.020 M in each complex ion. Is it feasible to separate the three metals from this solution by electrolysis? (Assume that 99% of a metal must be plated out before another metal begins to plate out.)arrow_forwardIn 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.arrow_forwardBased on the reaction, Sn + Cu2+ ⇌ Sn2+ + Cu+ (in acidic medium) Calculate the following values: K E (when [Cu2+] = 0.0200 M, [Sn2+] = 0.0100 M, and [Cu+] = 0.0300 M)arrow_forward
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