f 0.060 faraday is passed through an electrolytic cell containing a solution of In³* ions, the maximum number of moles of In that could be deposited at the cathode is O 0.010 moles O 0.020 moles O 0.060 moles O 0.18 moles

f 0.060 faraday is passed through an electrolytic cell containing a solution of In³* ions, the maximum number of moles of In that could be deposited at the cathode is O 0.010 moles O 0.020 moles O 0.060 moles O 0.18 moles

Principles of Modern Chemistry

8th Edition

ISBN:9781305079113

Author:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler

Publisher:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler

Chapter17: Electrochemistry

Section: Chapter Questions

Problem 3P

See similar textbooks

Similar questions

A galvanic cell is constructed in which the overall reactionis Cr2O72(aq)+14H2O+(aq)+6I(aq)2Cr3+(aq)+3I2(s)+21H2O(l) Calculate E for this cell. At pH 0, with [Cr2O72]=1.5M and [I]=0.40M, the cell potential is found to equal 0.87 V. Calculatethe concentration of Cr3+(aq) in the cell.
Consider the following galvanic cell at 25C: Pt|Cr2+(0.30M),Cr3+(2.0M)||Co2+(0.20M)|Co The overall reaction and equilibrium constant value are 2Cr2+(aq)+Co2+(aq)2Cr3+(aq)+Co(s)K=2.79107 Calculate the cell potential, for this galvanic cell and G for the cell reaction at these conditions.
Determine the overall reaction and its standard cell potential at 25 C for this reaction. Is the reaction spontaneous at standard conditions? Cu(s)|Cu2+(aq)Au3+(aq)|Au(s)
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)?
Consider a galvanic cell for which the anode reaction is 3 Pb(s)Pb2+(1.0102M)+2e and the cathode reaction is VO2+(0.10M)+2H3O+(0.10M)+eV3+(1.0105M)+3H2O(l) The measured cell potential is 0.640 V. Calculate E for the VO2+V3+ half-reaction, usingE(Pb2+Pb) from Appendix E. Calculate the equilibrium constant (K) at 25°C for thereaction Pb(s)+2VO2+(aq)+4H3O+(aq)Pb2+(aq)+2V3+(aq)+6H2O(l)
An aqueous solution of an unknown salt of gold is electrolyzed by a current of 2.75 amps for 3.39 hours. The electroplating is carried out with an efficiency of 93.0%, resulting in a deposit of 21.221 g of gold. a How many faradays are required to deposit the gold? b What is the charge on the gold ions (based on your calculations)?
Determine the overall reaction and its standard cell potential at 25 C for the reaction involving the galvanic cell made from a half-cell consisting of a silver electrode in 1 M silver nitrate solution and a half-cell consisting of a zinc electrode in 1 M zinc nitrate. Is the reaction spontaneous at standard conditions?
A standard galvanic cell is constructed so that the overall cell reaction is 2A13++(aq)+3M(s)3M2+(aq)+2A1(s) Where M is an unknown metal. If G = 411 kJ for the overall cell reaction, identify the metal used to construct the standard cell.
Determine the overall reaction and its standard cell potential at 25 C for these reactions. Is the reaction spontaneous at standard conditions? Assume the standard reduction for Br2(l) is the same as for Br2(aq).. Pt(s)|H2(g)|H+(aq)Br2(aq),Br(aq)|Pt(s)
Consider the galvanic cell based on the following half-reactions: a. Determine the overall cell reaction and calculate b. Calculate G and K for the cell reaction at 25C. c. Calculate at 25C when [Au3+] = 1.0 102 M and [Tl+] = 1.0 104 M.
Determine the overall reaction and its standard cell potential at 25 C for the reaction involving the galvanic cell in which cadmium metal is oxidized to 1 M cadmium(II) ion and a half—cell consisting of an aluminum electrode in 1 M aluminum nitrate solution. 15 the reaction spontaneous at standard conditions?
The mass of three different metal electrodes, each from a different galvanic cell, were determined before and after the current generated by the oxidation-reduction reaction in each cell was allowed to flow for a few minutes. The first metal electrode, given the label A, was found to have increased in mass; the second metal electrode, given the label B, did not change in mass; and the third metal electrode, given the label C, was found to have lost mass. Make an educated guess as to which electrodes were active and which were inert electrodes, and which were anode(s) and which were the cathode(s).