Voltaic cells are. Select the correct answer below: electrochemical cells in which spontaneous oxidation-reduction reactions convert chemical energy to electrical O C C energy. electrochemical cells in which spontaneous oxidation-reduction reactions convert mechanical energy to electrical force. electrochemical cells in which spontaneous oxidation-reduction reactions convert electrical energy to chemical reactions. electrochemical cells in which nonspontaneous oxidation-reduction reactions convert electrical energy to chemical energy.

Voltaic cells are. Select the correct answer below: electrochemical cells in which spontaneous oxidation-reduction reactions convert chemical energy to electrical O C C energy. electrochemical cells in which spontaneous oxidation-reduction reactions convert mechanical energy to electrical force. electrochemical cells in which spontaneous oxidation-reduction reactions convert electrical energy to chemical reactions. electrochemical cells in which nonspontaneous oxidation-reduction reactions convert electrical energy to chemical energy.

Fundamentals Of Analytical Chemistry

9th Edition

ISBN:9781285640686

Author:Skoog

Publisher:Skoog

Chapter18: Introduction To Electrochemistry

Section: Chapter Questions

Problem 18.3QAP

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Similar questions

Give the notation for a voltaic cell whose overall cell reaction is Mg(s)+2Ag+(aq)Mg2+(aq)+2Ag(s) What are the half-cell reactions? Label them as anode or cathode reactions. What is the standard cell potential of this cell?
a Calculate G for the following cell reaction: Tl(s)Tl+(aq)Pb2+(aq)Pb(s) The Gf for Tl+(aq) is 32.4 kJ/mol. b From G, calculate the standard cell potential for the cell reaction and from this, determine the standard potential for Tl2+(aq)+eTl(s).
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).
A potassium chloride solution is electrolyzed by passing a current through the solution using inert electrodes. A gas evolves at each electrode, and there is a large increase in pH of the solution. Write the half-reactions that occur at the anode and at the cathode.
Calculate the standard cell potential of the cell corresponding to the oxidation of oxalic acid, H2C2O4, by permanganate ion. MnO4. 5H2C2O4(aq)+2MnO4(aq)+6H+(aq)10CO2(g)+2Mn2+(aq)+8H2O(l) See Appendix C for free energies of formation: Gf for H2C2O4(aq) is 698 kJ.
Consider a voltaic cell at 25°C in which the following reaction takes place. 3H2O2(aq)+6H+(aq)+2Au(s)2Au3+(aq)+6H2O (a) Calculate E°. (b) Write the Nernst equation for the cell. (c) Calculate E when [Au3+]=0.250M,[H+]=1.25M,[H2O2]=1.50M .
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
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)?
Calculate the standard cell potential of the following cell at 25C. Sn(s)Sn2+(aq)I2(aq)I(aq)
Consider a voltaic cell in which the following reaction takes place. 2F2+(aq)+H2O2(aq)+2H+(aq)2Fe3+(aq)+2H2O (a) Calculate E°. (b) Write the Nernst equation for the cell. (c) Calculate E at 25°C under the following conditions: [Fe2+]=0.00813M,[H2O2]=0.914M,[Fe3+]=0.199M,ph=2.88 .

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