Use the References to access important values if needed for this question.A standard galvanic cell is constructed with H* | H2 and Cd 2+ | Cd half cell compartments connected by a salt bridge. Which of the following statementsare correct?Hint: Refer to a table of standard reduction potentials.(Choose all that apply.)As the cell runs, anions will migrate from the H* | H₂ compartment to the Cd2+ | Cd compartment.Cd2+ is reduced at the cathode.The cathode compartment is the Cd2+ | Cd compartment.The anode compartment is the Cd2+ | Cd compartment.In the external circuit, electrons flow from the H+ | H2 compartment to the Cd 2+ | Cd compartment.Submit AnswerRetry Entire Group8 more group attempts remaining

Based on the information provided, the following statements are correct:Cd2+ is reduced at the…

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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 135CWP: Consider a galvanic cell based on the following half-reactions: a. What is the expected cell...

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Consider the following standard reduction potentials: Tl+(aq)+eTl(s)Ered=0.34VTl3+(aq)+3eTl(s)Ered=0.74VTl3+(aq)+2eTl+(aq)Ered=1.28V and the following abbreviated cell notations: (1) Tl|Tl+Tl3+,Tl+|Pt (2) Tl|Tl3+Tl3+,Tl+|Pt (3) Tl|Tl+Tl3+|Tl (a) Write the overall equation for each cell. (b) Calculate E° for each cell. (c) Calculate G° for each overall equation. (d) Comment on whether G° and/or E° are state properties. (Hint: A state property is path-independent.)
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 salt bridge cell in which the anode is a manganese rod immersed in an aqueous solution of manganese(II) sulfate. The cathode is a chromium strip immersed in an aqueous solution of chromium(III) sulfate. Sketch a diagram of the cell, indicating the flow of the current throughout. Write the half-equations for the electrode reactions, the overall equation, and the abbreviated notation for the cell.
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?
Consider a galvanic cell based on the following half-reactions: a. What is the standard potential for this cell? b. A nonstandard cell is set up at 25C with [Mg2+] = 1.00 105 M. The cell potential is observed to be 4.01 V. Calculate [Au3+] in this cell.
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, .
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).
For each reaction listed, determine its standard cell potential at 25 C and whether the reaction is spontaneous at standard conditions. (a) Mn(s)+Ni2+(aq)Mn2+(aq)+Ni(s) (b) 3Cu2+(aq)+2Al(s)2Al3+(aq)+3Cu(s) (c) Na(s)+LiNO3(aq)NaNO3(aq)+Li(s) (d) Ca(NO3)2(aq)+Ba(s)Ba(NO3)2(aq)+Ca(s)

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