7 Help please show all work and correct sig figs in calculation of needed to better understand thanks. Construct a well-illustrated sketch for a voltaic cell using the following redox reaction:Mn + CaCa + Mn. Your illustration should include:Identify which metal is will be the anode and which the cathode.The direction of electron flow.а.b.с.The direction of anions and cations.d.What (specify) balanced half-reaction occurs at the anode., What (specify) balanced half-reaction occurs at the cathode.Total number of electrons involved in the transfer isInclude a salt bridge (no need to specify a particular ionic compound to be used).е.f.g.

Given: Electrolytic cell: Mn2+ + Ca ------> Ca2+ + Mn

Construct a well-illustrated sketch for a voltaic cell using the following redox reaction: Mn + Ca - Ca + Mn. Your illustration should include: Identify which metal is will be the anode and which the cathode. The direction of electron flow. a. b. The direction of anions and cations. d. What (specify) balanced half-reaction occurs at the anode. , What (specify) balanced half-reaction occurs at the cathode. Total number of electrons involved in the transfer is Include a salt bridge (no need to specify a particular ionic compound to be used). е. f. g.

Construct a well-illustrated sketch for a voltaic cell using the following redox reaction: Mn + Ca - Ca + Mn. Your illustration should include: Identify which metal is will be the anode and which the cathode. The direction of electron flow. a. b. The direction of anions and cations. d. What (specify) balanced half-reaction occurs at the anode. , What (specify) balanced half-reaction occurs at the cathode. Total number of electrons involved in the transfer is Include a salt bridge (no need to specify a particular ionic compound to be used). е. f. g.

Chemistry: An Atoms First Approach

2nd Edition

ISBN:9781305079243

Author:Steven S. Zumdahl, Susan A. Zumdahl

Publisher:Steven S. Zumdahl, Susan A. Zumdahl

Chapter17: Electrochemistry

Section: Chapter Questions

Problem 41E

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Similar questions

Consider a galvanic cell based on the following half-reactions: a. What is the expected cell potential with all components in their standard states? b. What is the oxidizing agent in the overall cell reaction? c. What substances make up the anode compartment? d. In the standard cell, in which direction do the electrons flow? e. How many electrons are transferred per unit of cell reaction? f. If this cell is set up at 25C with [Fe2+] = 2.00 104 M and [La3+] = 3.00 103 M, what is the expected cell potential?
Consider a voltaic cell in which the following reaction occurs. Zn(s)+Sn2+(aq)Zn2+(aq)+Sn(s) (a) Calculate E° for the cell. (b) When the cell operates, what happens to the concentration of Zn2+? The concentration of Sn2+? (c) When the cell voltage drops to zero, what is the ratio of the concentration of Zn2+ to that of Sn2+? (d) If the concentration of both cations is 1.0 M originally, what are the concentrations when the voltage drops to zero?
Is it reasonable to conclude that a potential could be assigned to each half-cell in a voltaic cell, based on these data for three voltaic cells? Explain. Zn(s)|Zn2+(aq)||Cu2+(aq)|Cu(s) cell potential=1.10 V Zn(s)|Zn2+(aq)||Ag+(aq)|Ag(s) cell potential=1.56 V Cu(s)|Cu2+(aq)||Ag+(aq)|Ag(s) cell potential=0.46 V
Consider a voltaic cell in which the following reaction takes place in basic medium at 25°C. 2NO3-(aq)+3S2(aq)+4H2O3S(s)+2NO(g)+8OH(aq) (a) Calculate E°. (b) Write the Nernst equation for the cell E. (c) Calculate E under the following conditions: PNO=0.994atm,ph=13.7,[S2]=0.154M,[NO3-]=0.472M, .
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 .
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 .
A mercury battery, used for hearing aids and electric watches, delivers a constant voltage (1.35 V) for long periods. The half-reactions are HgO(s)+H2O(l)+2eHg(l)+2OH(aq)Zn(s)+2OH(aq)Zn(OH)2(s)+2e Which half-reaction occurs at the anode and which occurs at the cathode? What is the overall cell reaction?
A galvanic cell is based on the following half-reactions at 25C: Ag++eAg H2O2+2H++2e2H2O Predict whether is larger or smaller than for the following cases. a. [Ag+]=1.0M,[H2O2]=2.0M,[H+]=2.0M b. [Ag+]=2.0M,[H2O2]=1.0M,[H+]=1.0107M
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 metallurgist wants to gold-plate an object with a surface area of 17.21 in2. The gold plating must be 0.00200 in. thick (assume uniform thickness). (a) How many grams of gold (d=10.5g/cm3) are required? (b) How many minutes will it take to plate the object from a solution of AuCN using a current of 7.00 A? Assume 100% efficiency.
You have 1.0 M solutions of Al(NO3)3 and AgNO3 along with Al and Ag electrodes to construct a voltaic cell. The salt bridge contains a saturated solution of KCl. Complete the picture associated with this problem by a writing the symbols of the elements and ions in the appropriate areas (both solutions and electrodes). b identifying the anode and cathode. c indicating the direction of electron flow through the external circuit. d indicating the cell potential (assume standard conditions, with no current flowing). e writing the appropriate half-reaction under each of the containers. f indicating the direction of ion flow in the salt bridge. g identifying the species undergoing oxidation and reduction. h writing the balanced overall reaction for the cell.

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